Choice Based Creditsystem (Cbcs)

CHOICE BASED CREDIT SYSTEM

(CBCS)

Syllabus for Chemistry

B. Sc. (HONOURS, GENERIC ELECTIVE), M. Sc & Ph. D.

ABOUT THE DEPARTMENT Department of Chemistry, IGNTU, Amarkantak

The Department of Chemistry was started in 2008, and has now grown into a major department for teaching and research within the Faculty of Science at IGNTU. The department offer vibrant atmosphere to students and faculty to encourage the spirit of scientific inquiry and to pursue cutting-edge research in a highly encouraging environment. The key objective of our department is to create good quality human resource through competitive yet inspiring environment for developing their careers. Currently, the department comprises more than hundred students, five research scholar and seven faculties and a dedicate team of staff members. The department offers three years undergraduate B.Sc. courses in Chemistry (Hons.) in the University. In addition it also offers two years M. Sc. and PhD programme. At present the Department consists of about seven research groups working in the areas of material chemistry (Functional Hybrid Nanomaterials), coordination/ supramolecular chemistry, bioinorganic chemistry, asymmetric synthesis, catalysis, nanomagnetism and Single Molecule Magnets (SMMs), as major thrust areas. The department is doing well in research activities and published good numbers of research papers. The faculty has been undertaking research projects sponsored by different national agencies such as DST, UGC, etc. The most important achievement of the University is the first Department of Chemistry has succeeded “DST-FIST Program – 2017” recognition from Govt. of India, Department of Science & Technology, New Delhi. Many students have been qualified National Eligibility Test (NET) and Joint Admission Test (JAM) Examination for pursuing PhD and M. Sc. Program in different prestigious IIT, NIT and Central Universities. The most of the students of our department is tribal and our mission is that the department of Chemistry can be reached at highest level in the country for its teaching and research activities and produced number of best quality of students in India.

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At a Glance Department of Chemistry, IGNTU Faculty Profile

Presentation Name & Designation Research Area Awards and Honors

Dr. Tanmay K Ghorai Nanoscience, BOYSCAST Associate Professor & Catalysis & Single Fellowship & Young Head Molecule Magnets Scientist Award PhD: IIT-KGP (DST)

Dr. Subrata Jana Molecular Radhika Panda Associate Professor Recognition & Memorial Award, PhD: IIEST-Shibpur Supramolecular UrFU PDF Award Chemistry

Dr. Khemchand Nanostructure BSR-UGC Start-Up Dewangan Transition Metal Grant Assistant Professor Oxides & Nitrides PhD: IIT-Kanpur

Dr. Adhish Jaiswal Dieletrics, Best Research Assistant Professor Magnetism & Solar- Scholar Award in PhD: NCL-Pune cell NCL Pune

Dr. Biswajit Maji Asymmetric INSPIRE Faculty Assistant Professor Synthesis and Award, President PhD: IIT-KGP Catalysis INSPIRE Teacher Recognition

Dr. Sadhu Charan Metal Nano Best Poster Award Mallick Particles, Polymer at IICT Hyderabad Assistant Professor Composites & Bio PhD: IITGuwahati applications

Dr. Ajay Shankar Nano- Post- Doctoral Assistant Professor magnetism fellowship Award at PhD: NPL, Delhi Germany

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Members of the Board of Studies

For

Revised the Chemistry Syllabus of B. Sc. (HONOURS, GENERIC ELECTIVE), M. Sc & Ph. D. Courses

According

CHOICE BASED CREDIT SYSTEM

(CBCS)

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(Chemistry-Major) Course Structure Details of courses under B.Sc. (Honours) Course *Credits Theory+ Practical Theory + Tutorial ======I. Core Course (14 Papers) 14×4= 56 14×5=70 Core Course Practical / Tutorial* (14 Papers) 14×2=28 14×1=14 II. Elective Course (8 Papers) A.1. Discipline Specific Elective 4×4=16 4×5=20 (4 Papers) A.2. Discipline Specific Elective Practical/Tutorial* 4×2=8 4×1=4 (4 Papers) B.1. Generic Elective/ Interdisciplinary 4×4=16 4×5=20 (4 Papers) B.2. Generic Elective Practical/ Tutorial* 4×2=8 4×1=4 (4 Papers)

 Optional Dissertation or project work in place of one Discipline Specific th Elective paper (6 credits) in 6 Semester   III. Ability Enhancement Courses 1. Ability Enhancement Compulsory (2 Papers of 4 credit each) 2×4=8 2×4=8 Environmental Science English/MIL Communication 2. Ability Enhancement Elective (Skill Based) (Minimum 2) 2×4=8 2×4=8 (2 Papers of 4 credit each) ______Total credit 148 148

* wherever there is a practical there will be no tutorial and vice-versa

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PROPOSED SCHEME FOR CHOICE BASED CREDIT SYSTEM IN B. Sc. Honours (Chemistry)

SEM CORE COURSE (14) Ability Ability Elective: Elective: Enhancement Enhancement Discipline Generic Compulsory Course Elective Specific (GE) (4) (AECC) (2) Course (AEEC) DSE (4) (2) (Skill Based) I Inorganic I: Atomic (English Structure & Chemical Communication/MIL) Bonding–I (4+2) /Environmental GE – I Physical I: States of Matter Science & Ionic Equilibrium (4+2) II Organic I: Basics & (English Hydrocarbons (4+2) Communication/MIL) Physical II: Chemical /Environmental GE – II Thermodynamics & Science Chemical Equilibrium (4+2) III Inorganic II: Radioactivity & s- and p-Block Elements (4+2) Organic II: Oxygen Containing Functional SEC – I GE – III Groups (4+2) Physical III: Phase Equilibria, Solution & Chemical Kinetics (4+2) IV Inorganic III: Coordination Chemistry (4+2) Organic III: Heterocyclic Chemistry (4+2) SEC – II GE – IV Physical IV: Catalysis, Electro and Photo- Chemistry (4+2) V Organic IV: Biomolecules DSE – I (4+2) Physical V: Quantum Chemistry & Spectroscopy DSE – II (4+2) VI Inorganic IV: Organometallic Chemistry DSE – III (4+2) Organic V: Spectroscopy DSE – IV (4+2)

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Course Structure for B.Sc. CHEMISTRY HONORS 1 credit = 1 hour per week for Theory and 2 hours per week for Laboratory Course Code Course Structure Course Name Credit SEMESTER-I Ability Enhancement English Communications/Environmental 4 Compulsory Course – I Science (offered by respective Department) Inorganic Chemistry I: Atomic Structure & CHM T 111 Core Course – I 4 Chemical Bonding CHM P 111 Core Course – I Practical Inorganic Chemistry - I Lab 2 Physical Chemistry I: States of Matter & Ionic CHMT 112 Core Course-II 4 Equilibrium CHM P 112 Core Course – I Practical Physical Chemistry - I Lab 2 CHM T 113 GE - I (Opted subject from Table GE offered Generic Elective – I 4 ***GE - (A-G) by Department) CHM P 113 Generic Elective – I GE Chemistry Practical – I Lab 2 ***GE - (A-G) Practical SEMESTER-II Ability Enhancement English Communications/Environmental 4 Compulsory Course – II Science (offered by respective Department) Organic Chemistry – I: Basics and CHM T 121 Core Course – III 4 Hydrocarbons CHM P 121 Core Course – III Practical Organic Chemistry – I Lab 2 Physical Chemistry – II: Chemical CHM T 122 Core Course – IV 4 Thermodynamics and Chemical Equilibrium CHM P 122 Core Course – IV Practical Physical Chemistry – II Lab 2 CHM T 123 GE - II (Opted subject from Table GE offered Generic Elective – II 4 ***GE - (A-G) by Department) CHM P 123 Generic Elective – II GE Chemistry Practical – II Lab 2 ***GE - (A-G) Practical SEMESTER-III Inorganic Chemistry – II : Radioactivity & s- CHM T 211 Core Course – V 4 and p-Block Elements CHM P 211 Core Course – V Practical Inorganic Chemistry – II Lab 2 Organic Chemistry – II: Oxygen Containing CHM T 212 Core Course – VI 4 Functional Groups CHM P 212 Core Course – VI Practical Organic Chemistry – II Lab 2 Physical Chemistry – III: Phase Equilibria, CHM T 213 Core Course – VII 4 Solution and Chemical Kinetics Core Course – VII CHM P 213 Physical Chemistry – III Lab 2 Practical

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CHM T 214 Skill Enhancement Course SEC-I (Opted subject from Table SEC offered 4 **SEC - (A-H) – I by Department) CHM T 215 GE - III (Opted subject from Table GE offered Generic Elective – III 4 ***GE - (A-G) by Department) CHM P 215 Generic Elective – III GE Chemistry Practical – III Lab 2 ***GE - (A-G) Practical SEMESTER-IV Inorganic Chemistry III: Coordination CHM T 221 Core Course – VIII 4 Chemistry Core Course – VIII CHM P 221 Inorganic Chemistry – III Lab 2 Practical Organic Chemistry – III: Introduction of N – CHM T 222 Core Course – IX Containing Functional Group Towards 4 Heterocyclic Chemistry CHM P 222 Core Course – IX Practical Organic Chemistry – III Lab 2 Physical Chemistry – IV: Catalysis, Electro CHM T 223 Core Course – X 4 and Photo-Chemistry CHM P 223 Core Course – X Practical Physical Chemistry – IV Lab 2 CHM T 224 Skill Enhancement Course SEC-II (Opted subject from Table SEC 4 **SEC - (A-H) – II offered by Department) CHM T 225 GE – IV (Opted subject from Table GE Generic Elective – IV 4 ***GE - (A-G) offered by Department) CHM P 225 Generic Elective – IV GE Chemistry Practical –IV Lab 2 ***GE - (A-G) Practical SEMESTER-V CHM T 311 Core Course – XI Organic Chemistry – IV: Biomolecules 4 CHM P 311 Core Course – XI Practical Organic Chemistry – IV Lab 2 Physical Chemistry – V: Quantum Chemistry CHM T 312 Core Course – XII 4 & Spectroscopy CHM P 312 Core Course – IX Practical Physical Chemistry – V Lab 2 CHM T 313 Discipline Specific DSE – I (Opted subject from Table DSE 4 *DSE - (A - M) Elective – I offered by Department) CHM P 313 Discipline Specific DSE – I Lab 2 *DSE - (A - M) Elective – I Practical CHM T 314 Discipline Specific DSE – II (Opted subject from Table DSE 4 *DSE - (A - M) Elective – II offered by Department) CHM P 314 Discipline Specific DSE – II Lab 2 *DSE - (A - M) Elective – II Practical SEMESTER-VI Inorganic Chemistry – IV: Organometallic CHM T 321 Core Course – XIII 4 Chemistry Core Course – XIII CHM P 321 Inorganic Chemistry – IV Lab 2 Practical CHM T 322 Core Course – XIV Organic Chemistry – V: Spectroscopy 4

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Core Course – XIV CHM P 322 Organic Chemistry – V Lab 2 Practical CHM T 323 Discipline Specific DSE – III (Opted subject from Table DSE 4 *DSE - (A - M) Elective – III offered by Department) CHM P 323 Discipline Specific DSE – III Lab 2 *DSE - (A - M) Elective – III Practical CHM T 324 Discipline Specific DSE – IV (Opted subject from Table DSE 4 *DSE - (A - M) Elective – IV offered by Department) CHM P 324 Discipline Specific DSE – IV Lab 2 *DSE - (A - L) Elective – IV Practical Grand Total 148 * Discipline Specific Elective (A – M) referred in Table DSE **Skill Enhancement Course (A – H) referred in Table SEC *** General Elective Course (A – G) referred in Table GE

Core Courses: (Credit: 06 each)

(1 period/week for tutorials or 4 periods/week for practical)

1. Inorganic Chemistry – I : Atomic Structure & Chemical Bonding (4 + 2) 2. Physical Chemistry – I : States of Matter & Ionic Equilibrium (4 + 2) 3. Organic Chemistry – I : Basics and Hydrocarbons (4 + 2) 4. Physical Chemistry – II : Chemical Thermodynamics and (4 + 2) 5. Inorganic Chemistry – II : Radioactivity & s- and p-Block Elements (4 + 2) 6. Organic Chemistry – II : Oxygen Containing Functional Groups (4 + 2) 7. Physical Chemistry – III : Phase Equilibria, Solution and Chemical Kinetics (4+2) 8. Inorganic Chemistry – III : Coordination Chemistry (4 + 2) 9. Organic Chemistry – III : Heterocyclic Chemistry (4 + 2) 10. Physical Chemistry – IV : Catalysis, Electro and Photo-chemistry (4 + 2) 11. Organic Chemistry – IV : Biomolecules (4 + 2) 12. Physical Chemistry – V : Quantum Chemistry & Spectroscopy (4 + 2) 13. Inorganic Chemistry – IV : Organometallic Chemistry (4 +2) 14. Organic Chemistry – V : Spectroscopy (4 + 2)

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Table DSE *Discipline Specific Elective (DSE)

Course Title of Paper Credit Code

DSE – A Applications of Computers in Chemistry 4

DSE – B Analytical Methods in Chemistry 4

DSE – C Basics of Drug Design & Medicinal Chemistry 4

DSE – D Novel Inorganic Solids 4

DSE – E Polymer Chemistry 4

DSE – F Green Chemistry 4

DSE – G Industrial Chemicals & Environment 4

DSE – H Inorganic Materials of Industrial Importance 4

DSE – I Instrumental Methods of Chemical Analysis 4

DSE – J Basic of Nanomaterials 4

DSE – K Advanced Organic Chemistry 4

5 + 1(Tutori DSE – L Research Methodology for Chemistry al)

5 + DSE – M Crystalline Material and Properties 1(Tutori al)

5+1(Tut DSE – N Basic Mathematical Concept for Chemist orial)

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Table SEC

**Skill Enhancement Course (SEC)

Course Title of Paper Credit Code SEC – A IT Skills for Chemists 4 SEC – B Basic Analytical Chemistry 4 SEC – C Chemical Technology & Environmental Aspects for Society 4 SEC – D Chemoinformatics 4 SEC – E Green Methods in Chemistry 4 SEC – F Cosmetics, Perfumes &Pharmaceutical Chemistry 4 SEC – G Pesticide & Fuel Chemistry 4 Computer Science/Sports/NCC/NSS/Yoga etc. offered by SEC – H 4 respective Department

Table GE

*Generic Elective Course (GE)

Course Title of Paper Credit Code Atomic Structure, Bonding, General Organic Chemistry & GE – A 4 Aliphatic Hydrocarbons Kinetic Theory of Gases, Chemical Energetics, Equilibria & GE – B 4 Functional Group Organic Chemistry Solutions, Phase Equilibrium, Conductance and Chemistry of GE – C 4 s-, p- and d- block elements Electrochemistry, Chemical Kinetics, Co-ordination GE – D 4 compounds, Organometallics and Molecules of life GE – E Analytical Chemistry, Quantum Chemistry and Spectroscopy 4 Chemistry of f-block elements, Bioinorganic Chemistry, GE – F 4 Polynuclear hydrocarbons and UV, IR Spectroscopy GE – G Polymer Chemistry, Nuclear and Materials Chemistry 4

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SEMESTER – I

CHM T 111: Inorganic Chemistry– I: Atomic Structure & Chemical Bonding (Credits: Theory - 04, Practical - 02) Theory: 60 Hours Unit –1: Atomic Structure

Bohr’s theory, its limitations and atomic spectrum of hydrogen atom. Wave mechanics: de Broglie equation, Heisenberg’s Uncertainty Principle and its significance, Schrödinger’s wave equation, significance of ψ and ψ2. Quantum numbers and their significance. Normalized and orthogonal wave functions. Sign of wave functions. Radial and angular wave functions for hydrogen atom. Radial and angular distribution curves. Shapes of s, p, d and f orbitals. Contour boundary and probability diagrams.

Pauli’s Exclusion Principle, Hund’s rule of maximum multiplicity, Aufbau’s principle and its limitations, Variation of orbital energy with atomic number. (14 Hours) Unit – 2: Periodicity of Elements s, p, d, f block elements, the long form of periodic table. Detailed discussion of the following properties of the elements, with reference to s & p-block.

(a) Effective nuclear charge, shielding or screening effect, Slater rules, variation of effective nuclear charge in periodic table.

(b) Atomic radii (van der Waals) (c) Ionic and crystal radii. (d) Covalent radii (octahedral and tetrahedral) (e) Ionization enthalpy, Successive ionization enthalpies and factors affecting ionization energy. Applications of ionization enthalpy.

(f) Electron gain enthalpy, trends of electron gain enthalpy. (g) Electronegativity, Pauling’s/ Mulliken’s/ Allred Rachow’s/ and Mulliken-Jaffé’s electronegativity scales. Variation of electronegativity with bond order, partial charge, hybridization, group electronegativity. Sanderson’s electron density ratio. (14 Hours) Unit – 3: Chemical Bonding

(i) lonic bond: General characteristics, types of ions, size effects, radius ratio rule and its limitations. Packing of ions in crystals. Born-Landé equation with derivation and importance of Kapustinskii expression for lattice energy. Madelung constant, Born-Haber cycle and its application, Solvation energy

(ii) Covalent bond: Lewis structure, Valence Bond theory (Heitler-London approach). Formal

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Covalent character in ionic compounds, polarizing power and polarizability. Fajan’s rules and consequences of polarization.

Ionic character in covalent compounds: Bond moment and dipole moment. Percentage ionic character from dipole moment and electronegativity difference.

(iii) Metallic Bond: Qualitative idea of valence bond and band theories. Semiconductors and insulators, defects in solids.

(iv) Weak Chemical Forces: van der Waals forces, ion-dipole forces, dipole-dipole interactions, induced dipole interactions, Instantaneous dipole-induced dipole interactions. Repulsive forces, Hydrogen bonding (theories of hydrogen bonding, valence bond treatment) Effects of chemical force, melting and boiling points, solubility energetics of dissolution process. (20 Hours) Unit – 4: Non-aqueous solvents

Physical properties of a solvent, types of solvents and their general characteristics, reactions in non-aqueous solvents with reference to liquid NH3, liquid SO2 and liquid HF. (4 Hours) Unit – 5: Oxidation-Reduction

Redox equations, Standard electrode potentials, redox potentials and formal potentials, Nernst equation, redox potentials to explore the feasibility of reaction and calculation of values of equilibrium constant, redox potential as a function of pH, precipitation and complex formation, redox titrations and redox indicators, Frost and Latimer diagrams of redox potentials. (8 Hours) Reference Books: • Lee, J.D. Concise Inorganic Chemistry, ELBS, 1991. • Douglas, B.E. and Mc Daniel, D.H., Concepts & Models of Inorganic Chemistry, Oxford, 1970 • Atkins, P.W. & Paula, J. Physical Chemistry, Oxford Press, 2006. • Day, M.C. and Selbin, J. Theoretical Inorganic Chemistry, ACS Publications 1962. • Wahid U. Malic, G. D. Tuli, R. D. Madan, Inorganic Chemistry, S. Chand & Co. Ltd • R. Sarkar and N. Saha, General & Inorganic Chemistry, New Central Book Agency • Puri, Sharma and Kalia, Principle of Inorganic Chemistry, Milestone publishers & distributors

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CHM P 111: Inorganic Chemistry – I Lab: (60 Hours) (A) Titrimetric Analysis

(i) Calibration and use of apparatus (ii) Preparation of solutions of different Molarity/Normality of titrants

(B) Acid-Base Titrations

(i) Estimation of carbonate and hydroxide present together in mixture. (ii) Estimation of carbonate and bicarbonate present together in a mixture. (iii) Estimation of free alkali present in different soaps/detergents

(i) Estimation of Fe(II) and oxalic acid using standardized KMnO4 solution. (ii) Estimation of oxalic acid and sodium oxalate in a given mixture. (iii) Estimation of Fe(II) with K2Cr2O7 using internal (diphenylamine, anthranilic acid) and external indicator.

Reference text:

1. Vogel, A.I. A Textbook of Quantitative Inorganic Analysis, ELBS.

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CHM T 112: Physical Chemistry- I: States of Matter & Ionic Equilibrium (Credits: Theory-04, Practical-02) Theory: 60 Hours Unit – 1: Gaseous State – I Kinetic molecular model of a gas: postulates and derivation of the kinetic gas equations; deduction of gas laws from kinetic gas equation. Behavior of real gases: Deviations from ideal gas behavior, compressibility factor, Z, and its variation with pressure for different gases. Causes of deviation from ideal behavior; van der Waals equation of state, its derivation and application in explaining real gas behavior, mention of other equations of state (Berthelot, Dietrici); virial equation of state; van der Waals equation expressed in virial form and calculation of Boyle temperature. Isotherms of real gases and their comparison with van der Waals isotherms, continuity of states, critical state, relation between critical constants and van der Waals constants, law of corresponding states. (9 Hours) Unit – 2: Gaseous State – II

Maxwell Boltzmann distribution laws of molecular velocity and molecular energies (graphic representation – derivation not required) and its use in evaluating molecular velocities

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(average, root mean square, and most probable) and average kinetic energy, law of equipartition of energy, degrees of freedom and molecular basis of heat capacities. Collision frequency, collision diameter, and mean free path including their temperature and pressure dependence; viscosity of gases, relation between mean free path and coefficient of viscosity; calculation of collision diameter from coefficient of viscosity; variation of viscosity with temperature and pressure. (9 Hours) Unit – 3: Liquid State

Qualitative treatment of the structure of the liquid state; Radial distribution function; physical properties of liquids; vapor pressure, surface tension and coefficient of viscosity, and their determination. Effect of addition of various solutes on surface tension and viscosity. Explanation of cleansing action of detergents. Temperature variation of viscosity of liquids and comparison with that of gases. Qualitative discussion of structure of water. (6 Hours) Unit – 4: Solid State

Nature of the solid state, definition of space lattice, unit cell; laws of crystallography – (i) law of constancy of interfacial angles, (ii) law of rational indices (Miller indices ) and, (iii) law of symmetry, elementary ideas of symmetry, symmetry elements and symmetry operations. qualitative idea of point and space groups, seven crystal systems and fourteen Bravais lattices; X-ray diffraction, Bragg’s law, a simple account of rotating crystal method and powder pattern method. Analysis of powder diffraction patterns of NaCl, CsCl and KCl. Defects in crystals. Glasses and liquid crystals. (16 Hours) Unit – 5: Ionic Equilibria

Arrhenius theory of electrolytic dissociation: strong, moderate, and weak electrolytes, degree of ionization, factors affecting degree of ionization, ionization constant and ionic product of water. Ionization of weak acids and bases, pH scale, common ion effect; dissociation constants of mono-, di-and triprotic acids (exact treatment). Salt hydrolysis – calculation of hydrolysis constant, degree of hydrolysis and pH for different salts. Buffer solutions, derivation of Henderson-Hasselbalch equation and its applications; buffer capacity, buffer range, buffer action and applications of buffers in analytical chemistry and biochemical processes in the human body. Multistage equilibria in polyelectrolyte systems; hydrolysis and hydrolysis constants. Theory of acid–base indicators; selection of indicators and their limitations. Solubility and solubility product of sparingly soluble salts – applications of solubility product principle. Qualitative treatment of acid – base titration curves (calculation of pH at various stages).

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(20 Hours) Reference Books:

 Atkins, P. W. & Paula, J. de Atkin’s: Physical Chemistry 10th Ed., Oxford University Press (2006).  Ball, D. W.: Physical Chemistry, Thomson Press, India (2007).  Castellan, G. W.: Physical Chemistry 4th Ed. Narosa (2004).  Mortimer, R. G. Physical Chemistry 3rd Ed. Elsevier: NOIDA, U.P. (2009).  Puri, B. R., Sharma L. R., and Pathania M. S.: Principle of Physical Chemistry, Eds. 44th, Vishal Publishing Co., Jalandhar, (2010).  Kotz J. C., Treichel P. M. & Townsend J. R.: General Chemistry, Cengage Lening India Pvt. Ltd., New Delhi (2009).  Crow, D. R: Principles and Applications of Electrochemistry, Eds. 4th, Blackie Academic & Professional, Madras, (1994).

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CHM P 112: Physical Chemistry – I Lab (60 Hours)

1. Surface tension measurements. a. Determine the surface tension by (i) drop number (ii) drop weight method. b. Study the variation of surface tension of detergent solutions with concentration. c. Viscosity composition curve for a binary liquid mixture.

2. Viscosity measurement using Ostwald’s viscometer. a. Determination of viscosity of aqueous solutions of (i) polymer (ii) ethanol and (iii) sugar at room temperature. b. Study the variation of viscosity of sucrose solution with the concentration of solute. c. Surface tension composition curve for a binary liquid mixture.

3. Indexing of a given powder diffraction pattern of a cubic crystalline system.

4. pH metry a. Study the effect on pH of addition of HCl/NaOH to solutions of acetic acid, sodium acetate and their mixtures. b. Preparation of buffer solutions of different pH (i) Sodium acetate-acetic acid (ii) Ammonium chloride-ammonium hydroxide c. pH metric titration of (i) strong acid versus strong base, (ii) weak acid versus strong base. d. Determination of dissociation constant of a weak acid. e. To study the dissociation constant of amino acid (glycine) and hence the isoelectirc point of the acid.

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Any other experiment carried out in the class if permit. Reference Books:

 Khosla, B. D.; Garg, V. C. & Gulati, A. Senior Practical Physical Chemistry, R. Chand & Co.: New Delhi (2011).  Garland, C. W.; Nibler, J. W. & Shoemaker, D. P. Experiments in Physical Chemistry 8th Ed.; McGraw-Hill: New York (2003).  Halpern, A. M. & McBane, G. C. Experimental Physical Chemistry 3rd Ed.; W.H. Freeman & Co.: New York (2003).  Elias A. J., A collection of Interesting General Chemistry Experiments, University Press, India.

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SEMESTER – II

CHM T 121: Organic Chemistry-I: Basics and Hydrocarbons (Credits: Theory-04, Practicals-02) Theory: 60 Hours Unit – 1: Basics of Organic Chemistry

Organic Compounds: Classification, and Nomenclature, Hybridization, Shapes of molecules, Influence of hybridization on bond properties.

Electronic Displacements: Inductive, electromeric, resonance and mesomeric effects, hyperconjugation and their applications; Dipole moment; Organic acids and bases; their relative strength.

Homolytic and Heterolytic fission with suitable examples. Curly arrow rules, formal charges; Electrophiles and Nucleophiles; Nucleophlicity and basicity; Types, shape and their relative stability of Carbocations, Carbanions, Free radicals and Carbenes.

Introduction to types of organic reactions and their mechanism: Addition, Elimination and Substitution reactions. (6 Hours)

Unit -2: Stereochemistry

Fischer Projection, Newmann and Sawhorse Projection formulae and their interconversions; Geometrical isomerism: cis–trans and, syn-anti isomerism E/Z notations with C.I.P rules.

Optical Isomerism: Optical Activity, Specific Rotation, Chirality/Asymmetry, Enantiomers, Molecules with two or more chiral-centres, Distereoisomers, meso structures, Racemic mixture and resolution. Relative and absolute configuration: D/L and R/S designations. (14 Hours)

Unit – 3: Chemistry of Aliphatic Hydrocarbons

A. Carbon-Carbon sigma bonds

Chemistry of alkanes: Formation of alkanes, Wurtz Reaction, Wurtz-Fittig Reactions, Free radical substitutions: Halogenation -relative reactivity and selectivity.

B. Carbon-Carbon pi bonds:

Formation of alkenes and alkynes by elimination reactions, Mechanism of E1, E2, E1cb reactions. Saytzeff and Hofmann eliminations.

Reactions of alkenes: Electrophilic additions their mechanisms (Markownikoff/ Anti Markownikoff addition), mechanism of oxymercuration-demercuration, hydroboration- oxidation, ozonolysis, reduction (catalytic and chemical), syn and anti-hydroxylation (oxidation).

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1,2-and 1,4-addition reactions in conjugated dienes and, Diels-Alder reaction; Allylic and benzylic bromination and mechanism, e.g. propene, 1-butene, toluene, ethyl benzene. Reactions of alkynes: Acidity, Electrophilic and Nucleophilic additions. Hydration to form carbonyl compounds, Alkylation of terminal alkynes.

C. Cycloalkanes and Conformational Analysis

Types of cycloalkanes and their relative stability, Baeyer strain theory, Conformation analysis of alkanes: Relative stability: Energy diagrams of cyclohexane: Chair, Boat and Twist boat forms; Relative stability with energy diagrams. (20 Hours) Unit – 4: Aromatic Hydrocarbons

Aromaticity: Hückel’s rule, aromatic character of arenes, cyclic carbocations/carbanions and heterocyclic compounds with suitable examples. Electrophilic aromatic substitution: halogenation, nitration, sulphonation and Friedel-Craft’s alkylation/acylation with their mechanism. Directing effects of the groups. (12 Hours) Unit – 5: Polunuclear Hydrocarbons

Reactions of naphthalene phenanthrene and anthracene Structure, Preparation and structure elucidation and important derivatives of naphthalene and anthracene; Polynuclear hydrocarbons.

(8 Hours) Reference Books:

• Morrison, R. N. & Boyd, R. N. Organic Chemistry, Dorling Kindersley (India) Pvt. Ltd. (Pearson Education). • Finar, I. L. Organic Chemistry (Volume 1), Dorling Kindersley (India) Pvt. Ltd. (Pearson Education). • Finar, I. L. Organic Chemistry (Volume 2: Stereochemistry and the Chemistry of Natural Products), Dorling Kindersley (India) Pvt. Ltd. (Pearson Education). • Eliel, E. L. & Wilen, S. H. Stereochemistry of Organic Compounds; Wiley: London, 1994. • Kalsi, P. S. Stereochemistry Conformation and Mechanism; New Age International, 2005.

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CHM P 121: Organic Chemistry – I Lab (60 Hours)

1. Checking the calibration of the thermometer

2. Purification of organic compounds by crystallization using the following solvents:

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a. Water b. Alcohol c. Alcohol-Water

3. Determination of the melting points of above compounds and unknown organic compounds (Kjeldahl method and electrically heated melting point apparatus)

4. Effect of impurities on the melting point – mixed melting point of two unknown organic compounds

5. Determination of boiling point of liquid compounds. (boiling point lower than and more than 100 °C by distillation and capillary method)

6. Chromatography

a. Separation of a mixture of two amino acids by ascending and horizontal paper chromatography b. Separation of a mixture of two sugars by ascending paper chromatography c. Separation of a mixture of o-and p-nitrophenol or o-and p-aminophenol by thin layer chromatography (TLC)

Reference Books

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CHM T 122: Physical Chemistry – II: Chemical Thermodynamics and Chemical Equilibrium (Credits: Theory-04, Practicals-02) Theory: 60 Hours Unit – 1: Chemical Thermodynamics – I Introduction of different terms and processes in thermodynamics: [systems (isolated, closed, open) and surrounding, macroscopic properties (extensive and intensive), kinds of processes], state and path functions and their differentials. Zeroth law of thermodynamics. First Law: concept of heat, q, work, w, internal energy, U, sign convention for heat and work; statement of first law; enthalpy, H; heat capacities (Cv, Cp) and relation between them for ideal gases. Reversible and irreversible processes, maximum work; calculations of q, w, U and H for reversible, irreversible and free expansion of gases (ideal and van der Waals) under isothermal and adiabatic conditions. Ideal gas law for adiabatic reversible expansion, comparison of adiabatic and isothermal reversible expansion. Joule-Thomson effect, Joule-Thomson coefficient in ideal and real (van der Waals) gases, inversion temperature.

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(10 Hours) Unit – 2: Thermochemistry Standard state, standard enthalpy of formation, Hess’s Laws of constant heat summation and its application. Change in internal energy (∆U) and enthalpy (∆H) of chemical reactions, relation between ∆U and ∆H, variation of heat of reaction with temperature (Kirchhoff’s equation). Enthalpy of neutralization. Bond Energy – Bond dissociation energy and its calculation from thermo-chemical data. Adiabatic flame temperature and explosion temperature. (8 Hours) Unit – 3: Chemical Thermodynamics – II

Second Law: Limitation of first Law, spontaneous processes and different statement of second law of thermodynamics, Carnot cycle and its efficiency, Carnot theorem; thermodynamic scale of temperature. Concept of Entropy: Entropy changes in reversible and irreversible processes and of universe, physical concept of entropy (molecular and statistical interpretation of entropy), Calusius inequality; entropy as a function of V & T, and P & T; entropy changes of an ideal gas in different processes, entropy change in mixing of gases. Free Energy Functions: Free energy and its concept, Gibbs (G) and Helmholtz (A) free energies as thermodynamic quantities and their relationship; variation of free energy with temperature and pressure. Maxwell’s relations, thermodynamic equation of state; criteria for reversible and irreversible processes (spontaneity); Gibbs-Helmholtz equations, its application of the determination of ∆G, ∆H, ∆S of a reversible cell reaction. Third Law: Variation of entropy with temperature (Nernst heat theorem), statement of third law, the concept of residual entropy. Applications of third law for determination of absolute entropies of liquid and gases. (18 Hours) Unit – 4: Thermodynamic of Open System (Systems of Variable Composition) Partial molal quantities, dependence of thermodynamic parameters on composition;, the Gibbs- Duhem equation, chemical potential, variation of chemical potential with temperature and pressure, chemical potential in case of a system of ideal gases, chemical potential of real gases; concept and physical significance of fugacity, activity and activity coefficient, reference and standard states, thermodynamic functions of mixing (Gmix, Smix, Vmix, and Hmix) of ideal gases. (10 Hours) Unit – 5: Chemical Equilibrium Criteria of thermodynamic equilibrium, degree of advancement of reaction, chemical equilibria in ideal gases. Thermodynamic derivation of relation between Gibbs free energy of reaction and reaction quotient. Coupling of exoergic and endoergic reactions. Equilibrium constants and their quantitative dependence on temperature, pressure and concentration; thermodynamic derivation of relations between the various equilibrium constants Kp, Kc and Kx. Le Chatelier principle (quantitative treatment); equilibrium between ideal gases and a pure condensed phase.

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(14 Hours) Reference Books:

 Samuel Glasstone, Thermodynamics for Chemistry, Affiliated East-West Press, NewDelhi (2003).  Atkins, P. W. & Paula, J. de Atkin’s: Physical Chemistry 10th Ed., Oxford University Press (2006).  Castellan, G. W. Physical Chemistry 4th Ed., Narosa (2004).  Engel, T. & Reid, P. Physical Chemistry 3rd Ed., Prentice-Hall (2012).  McQuarrie, D. A. & Simon, J. D. Molecular Thermodynamics Viva Books Pvt. Ltd.: New Delhi (2004).  Assael, M. J.; Goodwin, A. R. H.; Stamatoudis, M.; Wakeham, W. A. & Will, S. Commonly Asked Questions in Thermodynamics. CRC Press: NY (2011).  Metz, C.R. 2000 Solved problems in chemistry, Schaum Series (2006).

------CHM P 122: Physical Chemistry – II Lab (60 Hours) Thermochemistry:

 Determination of heat capacity of a calorimeter for different volumes using change of enthalpy data of a known system (method of back calculation of heat capacity of calorimeter from known enthalpy of solution or enthalpy of neutralization).  Determination of heat capacity of the calorimeter and enthalpy of neutralization of hydrochloric acid with sodium hydroxide.  Calculation of the enthalpy of ionization of ethanoic acid.  Determination of heat capacity of the calorimeter and integral enthalpy (endothermic and exothermic) solution of salts.  Determination of basicity/proticity of a poly-protic acid by the thermo-chemical method in terms of the changes of temperatures observed in the graph of temperature versus time for different additions of a base. Also calculate the enthalpy of neutralization of the first step.  Determination of enthalpy of hydration of copper sulphate.  Study of the solubility of benzoic acid in water and determination of ∆H.

Chemical Equilibrium:

 Equilibrium constant of methyl acetate hydrolysis reaction. Any other experiment carried out in the class if permit. Reference Books:

 Khosla, B. D.; Garg, V. C. & Gulati, A. Senior Practical Physical Chemistry, R. Chand & Co.: New Delhi (2011).  Athawale, V. D. & Mathur, P. Experimental Physical Chemistry New Age International: New Delhi (2001).

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SEMESTER – III

CHM T 211: Inorganic Chemistry – II: Radioactivity & Chemistry of s-and p-Block elements (Credits: Theory-04, Practicals-02) Theory: 60 Hours Unit – 1: Radioactivity

Radioactive decay, half life and average life of radio elements, units of radioactivity, natural radioactive disintegration series, Instrumental analysis of radioactive elements, radioactive equilibrium, group displacement law, isotope, isotone, isobars and nuclear isomerism. Application of isotope in medicine, agriculture, reaction mechanism (isotope as tracer), age of minerals, age of earth, radio carbon dating, nuclear particles, nuclear forces: meson exchange theory. Nuclear models (elementary idea), nuclear stability, nuclear binding energy, nuclear reactions, magic numbers, mass defect, proton-neutron ratio, packing fraction, Artificial radioactivity, transmutation of elements, fission, fusion and spallation reaction. Nuclear energy, hazards of nuclear radiations and safety measures. (14 Hours) Unit – 2: Acid and Bases

Brönsted-Lowry concept of acid-base reactions, solvated proton, relative strength of acids, types of acid-base reactions, levelling solvents, Lewis acid-base concept, Classification of Lewis acids, Hard and Soft Acids and Bases (HSAB) Application of HSAB principle. (8 Hours) Unit – 3: Chemistry of s and p Block Elements

Inert pair effect, Relative stability of different oxidation states, diagonal relationship and anomalous behaviour of first member of each group. Allotropy and catenation. Complex formation tendency of s and p block elements.

Hydrides and their classification ionic, covalent and interstitial. Basic beryllium acetate and nitrate. Study of the following compounds with emphasis on structure, bonding, preparation, properties and uses. Boric acid and borates, boron nitrides, borohydrides (diborane) carboranes and graphitic compounds, silanes, Oxides and oxoacids of nitrogen, Phosphorus and chlorine. Peroxo acids of sulphur, interhalogen compounds, polyhalide ions, pseudohalogens and basic properties of halogens. (20 Hours) Unit – 4: Noble Gases

Occurrence and uses, rationalization of inertness of noble gases, Clathrates; preparation and properties of XeF2, XeF4 and XeF6; Nature of bonding in noble gas compounds (Valence bond reatment and MO treatment for XeF2). Molecular shapes of noble gas compounds (VSEPR theory).

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(10 Hours) Unit – 5: Inorganic Polymers

Types of inorganic polymers, comparison with organic polymers, synthesis, structural aspects and applications of silicones and siloxanes. Borazines, silicates and phosphazenes, and polysulphates. (8 Hours) Reference Books:

• Lee, J.D. Concise Inorganic Chemistry, ELBS, 1991. • Douglas, B.E; Mc Daniel, D.H. & Alexander, J.J. Concepts & Models of Inorganic Chemistry 3rd Ed., John Wiley Sons, N.Y. 1994. • Greenwood, N.N. & Earnshaw. Chemistry of the Elements, Butterworth- Heinemann. 1997. • Cotton, F.A. & Wilkinson, G. Advanced Inorganic Chemistry, Wiley, VCH, 1999. • Miessler, G. L. & Donald, A. Tarr. Inorganic Chemistry 4th Ed., Pearson, 2010. • Shriver & Atkins, Inorganic Chemistry 5th Ed.

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CHM P 211: Inorganic Chemistry – II Lab (60 Hours) (A) Iodo / Iodimetric Titrations

(i) Estimation of Cu(II) and K2Cr2O7 using sodium thiosulphate solution (Iodimetrically). (ii) Estimation of (i) arsenite and (ii) antimony in tartar-emetic iodimetrically (iii) Estimation of available chlorine in bleaching powder iodometrically.

(B) Gravimetric Analysis:

i. Estimation of nickel (II) using Dimethylglyoxime (DMG). ii. Estimation of copper as CuSCN iii. Estimation of iron as Fe2O3 by precipitating iron as Fe(OH)3. iv. Estimation of Al (III) by precipitating with oxine and weighing as Al(oxine)3 (aluminium oxinate).

(i) Cuprous Chloride, Cu2Cl2 (ii) Preparation of Manganese(III) phosphate, MnPO4.H2O (iii) Preparation of Aluminium potassium sulphate KAl(SO4)2.12H2O (Potash alum) or Chrome alum.

Reference Books:

• Vogel, A.I. A Textbook of Quantitative Inorganic Analysis, ELBS. 1978

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CHM T 212: Organic Chemistry-II: Oxygen Containing Functional Groups (Credits: Theory-04, Practicals-02) Theory: 60 Hours Unit – 1: Chemistry of Halogenated Hydrocarbons

1 2 i Alkyl halides: Methods of preparation, nucleophilic substitution reactions – SN , SN and SN mechanisms with stereochemical aspects and effect of solvent etc.; nucleophilic substitution vs. elimination.

Aryl halides: Preparation, including preparation from diazonium salts. nucleophilic aromatic substitution; SNAr, Benzyne mechanism.

Relative reactivity of alkyl, allyl/benzyl, vinyl and aryl halides towards nucleophilic substitution reactions.

Organometallic compounds of Mg and Li – Use in synthesis of organic compounds. (16 Hours) Unit – 2: Alcohols, Phenols, Ethers and Epoxides

Alcohols: preparation, properties and relative reactivity of 1°, 2°, 3° alcohols, Bouvaelt-Blanc Reduction; Preparation and properties of glycols: Oxidation by periodic acid and lead tetraacetate, Pinacol-Pinacolone rearrangement: Phenols: Preparation and properties; Acidity and factors effecting it, Ring substitution reactions, Reimer–Tiemann and Kolbe’s–Schmidt Reactions, Fries and Claisen rearrangements with mechanism;

Ethers and Epoxides: Preparation and reactions with acids. Reactions of epoxides with alcohols, ammonia derivatives and LiAlH4 (16 Hours)

Unit – 3: Carbonyl Compounds

Structure, reactivity and preparation

Nucleophilic additions, Nucleophilic addition-elimination reactions with ammonia derivatives with mechanism; Mechanisms of Aldol and Benzoin condensation, Knoevenagel condensation, Claisan-Schmidt, Perkin, Cannizzaro and Wittig reaction, Beckmann and Benzil-Benzilic acid rearrangements, haloform reaction and Baeyer Villiger oxidation, α-substitution reactions, oxidations and reductions (Clemmensen, Wolff-Kishner, LiAlH4, NaBH4, MPV, PDC and PGC)

Addition reactions of unsaturated carbonyl compounds: Michael addition. Active methylene compounds: Keto-enol tautomerism. Preparation and synthetic applications of diethyl malonate and ethyl acetoacetate. (14 Hours) Unit – 4: Carboxylic Acids and their Derivatives

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Preparation, physical properties and reactions of monocarboxylic acids: Typical reactions of dicarboxylic acids, hydroxy acids and unsaturated acids: succinic/phthalic, lactic, malic, tartaric, citric, maleic and fumaric acids

Preparation and reactions of acid chlorides, anhydrides, esters and amides; Comparative study of nucleophilic sustitution at acyl group -Mechanism of acidic and alkaline hydrolysis of esters, Claisen condensation, Dieckmann and Reformatsky reactions, Hofmann-bromamide degradation and Curtius rearrangement. (10 Hours) Unit – 5: Sulphur containing compounds

Preparation and reactions of thiols, thioethers and sulphonic acids.

(4 Hours) Reference Books: • Morrison, R. T. & Boyd, R. N. Organic Chemistry, Dorling Kindersley (India) Pvt. Ltd. (Pearson Education). • Finar, I. L. Organic Chemistry (Volume 1), Dorling Kindersley (India) Pvt. Ltd. (Pearson Education). • Graham Solomons, T.W. Organic Chemistry, John Wiley & Sons, Inc.

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CHM P 212: Organic Chemistry – II Lab (60 Hours)

1. Functional group tests for alcohols, phenols, carbonyl and carboxylic acid group. 2. Organic preparations: i. Acetylation of one of the following compounds: amines (aniline, o-, m-, p- toluidines and o-, m-, p-anisidine) and phenols (β-naphthol, vanillin, salicylic acid) by any one method: a. Using conventional method. b. Using green approach ii. Benzolyation of one of the following amines (aniline, o-, m-, p- toluidines and o-, m-, p-anisidine) and one of the following phenols (β-naphthol, resorcinol, p-cresol) by Schotten-Baumann reaction. iii. Oxidation of ethanol/ isopropanol (Iodoform reaction). iv. Bromination of any one of the following: a. Acetanilide by conventional methods b. Acetanilide using green approach (Bromate-bromide method) v. Nitration of any one of the following: a. Acetanilide/nitrobenzene by conventional method b. Salicylic acid by green approach (using ceric ammonium nitrate). vi. Selective reduction of meta dinitrobenzene to m-nitroaniline. vii. Reduction of p-nitrobenzaldehyde by sodium borohydride. viii. Hydrolysis of amides and esters.

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ix. Semicarbazone of any one of the following compounds: acetone, ethyl methyl ketone, cyclohexanone, benzaldehyde. x. S-Benzylisothiouronium salt of one each of water soluble and water insoluble acids (benzoic acid, oxalic acid, phenyl acetic acid and phthalic acid). xi. Aldol condensation using either conventional or green method. xii. Benzil-Benzilic acid rearrangement. xiii. Beckman Rearrangement The above derivatives should be prepared using 0.5-1g of the organic compound. The solid samples must be collected and may be used for recrystallization, melting point and TLC.

Reference Books

• Mann, F.G. & Saunders, B.C. Practical Organic Chemistry, Pearson Education (2009) • Furniss, B.S.; Hannaford, A.J.; Smith, P.W.G.; Tatchell, A.R. Practical Organic Chemistry, 5th Ed., Pearson (2012) • Ahluwalia, V.K. & Aggarwal, R. Comprehensive Practical Organic Chemistry: Preparation and Quantitative Analysis, University Press (2000). • Ahluwalia, V.K. & Dhingra, S. Comprehensive Practical Organic Chemistry, Qualitative Analysis, University Press (2002).

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CHM P 213: Physical Chemistry-III: Phase Equilibria, Solution and Chemical Kinetics (Credits: Theory-04, Practicals-02) Theory: 60 Hours Unit – 1: Phase Equilibriam Concept of phases, components and degrees of freedom, derivation of Gibbs Phase Rule for nonreactive and reactive systems; Phase diagrams with applications for one-component systems (water and sulfur) and two component systems involving eutectics, congruent, incongruent melting points and solid solution (lead-silver, FeCl3-H2O and Na-K etc.). Three Component System: Graphical representation of three component system; system of three liquids: having partial miscibility. Type-I Formation of one pair of partially miscible liquids Type-II Formation of two pairs of partially miscible liquids Type-III Formation of three pairs of partially miscible liquids (15 Hours) Unit – 2: Phase Transformation

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Stability of phases; Clapeyron equation; Clasius-Clapeyron equation and its applications to solid- liquid, liquid-vapor and solid-vapor equilibria. Thermodynamics of phase transition; classification of phases - bubbles, cavities and droplets-Kelvin equation. (8 Hours)

Unit – 3: Solutions and Colligative Properties The chemical potential of liquids; ideal solutions; lowering of vapor pressure, Raoult’s and Henry’s Laws and their applications. Excess thermodynamic functions. Thermodynamic derivation using chemical potential to derive relations between the four colligative properties [(i) relative lowering of vapor pressure, (ii) elevation of boiling point, (iii) Depression of freezing point, (iv) osmotic pressure] and amount of solute. Applications in calculating molar masses of normal, dissociated, and associated solutes in solution. Binary solutions: Gibbs-Duhem-Margules equation, its derivation and applications to fractional distillation of binary miscible liquids (ideal and non-ideal), vapor pressure-composition and temperature-composition curves of ideal and non-ideal solution; distillation of solution, Lever rule, azeotropes. Partial miscibility of liquids, CST, miscible pairs, Immiscibility of liquids – Principle of steam distillation. Nernst distribution law: its derivation and applications. (19 Hours)

Unit – 4: Chemical Kinetics The concept of reaction rate, order and molecularity of a reaction, rate laws in terms of the advancement of a reaction, differential and integrated form of rate expressions up to second order reactions, experimental methods of the determination of rate laws; half life of a reaction. Temperature dependence of reaction rates; Arrhenius equation; activation energy. Collision theory of reaction rates, qualitative treatment of the theory of absolute reaction rates. (10 Hours) Unit – 5: Complex Reactions Kinetics of complex reactions (integrated rate expressions up to first order only): (i) opposing reactions (ii) parallel reactions and (iii) consecutive reactions and their differential rate equations (steady-state approximation in reaction mechanisms) (iv) chain reactions (v) uni molecular gas reaction (Lindemann mechanism) (8 Hours) Reference Books:

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 Rajaram, J. and Kuriacose, J. C.; Kinetics and Mechanisms of Chemical Transformations Applications of Femto-chemistry, MacMillan, New Delhi, 2011.  McQuarrie, D. A. & Simon, J. D. Molecular Thermodynamics Viva Books Pvt. Ltd.: New Delhi (2004).  Assael, M. J.; Goodwin, A. R. H.; Stamatoudis, M.; Wakeham, W. A. & Will, S. Commonly Asked Questions in Thermodynamics. CRC Press: NY (2011).  Levine, I .N. Physical Chemistry 6th Ed., Tata Mc Graw Hill (2010).  Metz, C.R. 2000 solved problems in chemistry, Schaum Series (2006).  Zundhal, S.S. Chemistry concepts and applications Cengage India (2011).

CHM P 213: Physical Chemistry – III Lab (60 Hours) 1. Determination of critical solution temperature and composition of the phenol-water system and to study the effect of impurities on it. 2. Phase equilibria: Construction of the phase diagram using cooling curves or ignition tube method: a. simple eutectic and b. congruently melting systems 3. Distribution of acetic/ benzoic acid between water and cyclohexane. 4. Study the equilibrium of at least one of the following reactions by the distribution method:

- - I2(aq) + I (aq) ⇌ I3 (aq) 2+ 2+ Cu (aq) + nNH3(aq) ⇌ [Cu(NH3)n]

5. Study the kinetics of the following reactions. a. Initial rate method: Iodide-persulphate reaction. + b. Order of reaction of I2 – acetone – H ion. c. Integrated rate method: (i) Acid hydrolysis of methyl acetate with hydrochloric acid (ii) Saponification of ethyl acetate. d. Compare the strengths of HCl and H2SO4 by studying kinetics of hydrolysis of methyl acetate.

Reference Books:

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 Halpern, A. M. & McBane, G. C. Experimental Physical Chemistry 3rd Ed.; W.H. Freeman & Co.: New York (2003).  Rose, J.: Advanced Physico-Chemical Experiments, Sir Isaac Pitman & Sons Ltd, London.

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SEMESTER – IV

CHM T 221: Inorganic Chemistry – III: Coordination Chemistry (Credits: Theory-04, Practicals-02) Theory: 60 Hours Unit – 1: Coordination Chemistry

Werner’s theory, IUPAC nomenclature of coordination compounds, Types of isomerism in coordination compounds: Constitutional, geometrical and optical isomerism in respect of coordination numbers 4 and 6, Determination of configuration of cis-, trans-isomers by chemical methods. Valence bond theory (inner and outer orbital complexes), electroneutrality principle and back bonding. Crystal field theory, measurement of 10 Dq (o), CFSE in weak and strong fields, pairing energies, factors affecting the magnitude of 10 Dq ( o, t). Octahedral vs. tetrahedral coordination, tetragonal distortions from octahedral geometry Jahn-Teller theorem, square planar geometry. Qualitative aspect of Ligand field and MO Theory, Chelate effect, polynuclear complexes. (20 Hours) Unit – 2: Electronic Spectra of Transition Metal Complex

Introduction to electronic spectra of transition metal complexes, Orgel diagrams for 3d1-3d9 ions, selection rules, d-d/charge transfer spectra, Colour, spectrochemical series, Nephelauxetic effect, trans effect, (example and applications) labile and inert complexes. Difference between the first, second and third transition series.

Chemistry of Ti, V, Cr Mn, Fe and Co in various oxidation states (excluding their metallurgy)

(10 Hours) Unit – 3: Magnetic Properties of Transition Metal Complex

Types of magnetic behaviour, methods of determining magnetic susceptibility, spin only formula, L-S coupling, Orbital contribution to magnetic moments, quenching of magnetic moment, super-exchange, antiferromagnetic interaction (elementary idea with examples only), application of spin only values of magnetic moments to determine valency and stereochemistry of coordination compounds (based on VBT and CFT). (10 Hours) Unit – 4: Chemistry of Lanthanoids and Actinoids

Electronic configuration, oxidation states, colour, spectral and magnetic properties, lanthanide contraction, separation of lanthanides and actinides (ion-exchange method only), important lanthanide compounds, similarities the later actinides and lanthanides elements. (6 Hours) Unit – 5: Bioinorganic Chemistry

Elements of life: essential major, trace and ultratrace elements. Basic chemical reactions in the biological systems and the role of metal ions (specially Na+, K+, Mg+2,Ca+2, Fe3+/2+, Cu+2, and

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Zn+2). Haemoglobin, myoglobin, chlorophyll, cytochromes, ferredoxins and carbonic anhydrase- their structural features and functions in living system. Toxic metal ions and their effects, lead, mercury, cadmium and arsenic poisoning, organomercury compounds; Use of chelating agents in medicine: Wilson diseases, detoxification of metal ions – chelation therapy (simple idea with some examples of chelating drugs). Pt and Au complexes as drugs (examples only), metal dependent diseases. (14 Hours) Reference Books:

• Purcell, K.F & Kotz, J.C. Inorganic Chemistry W.B. Saunders Co, 1977. • Huheey, J.E., Inorganic Chemistry, Prentice Hall, 1993. • Lippard, S.J. & Berg, J.M. Principles of Bioinorganic Chemistry Panima Publishing Company 1994. • Cotton, F.A. & Wilkinson, G, Advanced Inorganic Chemistry. Wiley-VCH, 1999 • Basolo, F, and Pearson, R.C., Mechanisms of Inorganic Chemistry, John Wiley & Sons, NY, 1967. • Greenwood, N.N. & Earnshaw A., Chemistry of the Elements, Butterworth-Heinemann, 1997. ------

CHM P 221: Inorganic Chemistry – III Lab (60 Hours) (A) Inorganic Preparations:

i. Tetraamminecopper (II) sulphate, [Cu(NH3)4]SO4.H2O ii. Cis and trans K[Cr(C2O4)2. (H2O)2] Potassium dioxalatodiaquachromate (III) iii. Tetraamminecarbonatocobalt (III) ion iv. Potassium tris(oxalate)ferrate(III)

(B) Quantitative Estimation of Metal Ions in Binary Mixture

i. Estimation of Iron (II/III) and Calcium (II) in a Mixture ii. Estimation of Fe(III) and Mn (II) in a Mixture iii. Estimation of Fe(III) and Cu(II) in a Mixture iv. Estimation of Fe(III) and Zn(II) in a Mixture

Principles involved in chromatographic separations. Paper chromatographic separation of following metal ions: i. Ni (II) and Co (II) ii. Fe (III) and Al (III)

Reference Book: 1. Vogel, A.I. A text book of Quantitative Analysis, ELBS 1986.

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CHM T 222: Organic Chemistry-III: Introduction of N – Containing Functional Group Towards Heterocyclic Chemistry (Credits: Theory-04, Practicals-02) Theory: 60 Hours

Unit – 1: Nitrogen Containing Functional Groups

Preparation and important reactions of nitro and compounds, nitriles and isonitriles

Amines: Effect of substituent and solvent on basicity; Preparation and properties: Gabriel phthalimide synthesis, Carbylamine reaction, Mannich reaction, Hoffmann’s exhaustive methylation, Hofmann-elimination reaction; Distinction between 1°, 2° and 3° amines with Hinsberg reagent and nitrous acid.

Diazonium Salts: Preparation and their synthetic applications. (18 Hours)

Unit – 2: Heterocyclic Compounds

Classification and nomenclature, Structure, aromaticity in 5-numbered and 6-membered rings containing one heteroatom; Synthesis, reactions and mechanism of substitution reactions of: Furan, Pyrrole (Paal-Knorr synthesis, Knorr pyrrole synthesis, Hantzsch synthesis), Thiophene, Pyridine (Hantzsch synthesis), Pyrimidine, Structure elucidation of indole, Fischer indole synthesis and Madelung synthesis), Structure elucidation of quinoline and isoquinoline, Skraup synthesis, Friedlander’s synthesis, Knorr quinoline synthesis, Doebner-Miller synthesis, Bischler-Napieralski reaction, Pictet-Spengler reaction, Pomeranz-Fritsch reaction

Derivatives of furan: Furfural and furoic acid. (22 Hours) Unit – 3: Alkaloids

Natural occurrence, General structural features, Isolation and their physiological action

Hoffmann’s exhaustive methylation, Emde’s modification, Structure elucidation and synthesis of Hygrine and Nicotine. Medicinal importance of Nicotine, Hygrine, Quinine, Morphine, Cocaine, and Reserpine. (10 Hours) Unit – 4: Terpenes

Occurrence, classification, isoprene rule; Elucidation of stucture and synthesis of Citral, Neral and α-terpineol. (10 Hours) Reference Books: • Morrison, R. T. & Boyd, R. N. Organic Chemistry, Dorling Kindersley (India) Pvt. Ltd. (Pearson Education). • Finar, I. L. Organic Chemistry (Volume 1), Dorling Kindersley (India) Pvt. Ltd. (Pearson Education).

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• Finar, I. L. Organic Chemistry (Volume 2: Stereochemistry and the Chemistry of Natural Products), Dorling Kindersley (India) Pvt. Ltd. (Pearson Education). • Acheson, R.M. Introduction to the Chemistry of Heterocyclic compounds, John Welly & Sons (1976). • Graham Solomons, T.W. Organic Chemistry, John Wiley & Sons, Inc. • Kalsi, P. S. Textbook of Organic Chemistry 1st Ed., New Age International (P) Ltd. Pub. • Clayden, J.; Greeves, N.; Warren, S.; Wothers, P.; Organic Chemistry, Oxford University Press. • Singh, J.; Ali, S.M. & Singh, J. Natural Product Chemistry, Prajati Parakashan (2010

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CHM P 222: Organic Chemistry – III Lab (60 Hours) 1. Detection of extra elements. 2. Functional group test for nitro, amine and amide groups. 3. Qualitative analysis of unknown organic compounds containing simple functional groups (alcohols, carboxylic acids, phenols and carbonyl compounds)

Reference Books

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CHM T 223: Physical Chemistry-IV: Catalysis, Electro & Photo-Chemistry (Credits: Theory-04, Practicals-02) Theory: 60 Hours Unit – 1: Catalysis Type of catalysts, specificity and selectivity, mechanism of catalyzed reaction at solid surface; effect of temperature on surface reaction, promoters and poisons, effect of particle size and efficiency of nanoparticles as catalysts; enzyme catalysis, Michaelis-Menten mechanism, effect of temperature and pH on enzyme catalysis; acid-base catalysis. (10 Hours) Unit – 2: Surface and Colloidal Chemistry Physical adsorption, chemisorptions, nature of adsorbed state, adsorption isotherm; Langmuir and Freundlich adsorption isotherms. Multi layer adsorption-BET equation (no derivation) and its application to surface area measurement. Colloidal state; definition of colloids, classification of colloids. Solids in liquids (sols); properties– kinetic, optical and electrical, stability of colloids, protective action; Hardy-Schulze law, gold number. Liquids in liquids (Emulsions): types of emulsions (micelles and reverse micelles), preparation, emulsifier. Liquid in solid (gels): classification, preparation, and properties, general application of colloids. (10 Hours) Unit – 3: Conductance Conductivity, equivalent and molar conductivity and their variation with dilution for weak and strong electrolytes (Kohlrausch square root law). Molar conductivity at infinite dilution. Kohlrausch law of independent migration of ions. Debye-Hückel-Onsager equation, Wien effect, Debye-Falkenhagen effect, Walden’s rules. Ionic velocities, mobilities and their determinations, transference numbers and their relation to ionic mobilities, determination of transference numbers using Hittorf and Moving Boundary methods. Applications of conductance measurement: (i) degree of dissociation of weak electrolytes, (ii) ionic product of water (iii) solubility and solubility product of sparingly soluble salts, (iv) conductometric titrations, and (v) hydrolysis constants of salts.

(15 Hours)

Unit – 4: Electrochemistry Quantitative aspects of Faraday’s laws of electrolysis, rules of oxidation/reduction of ions based on half-cell potentials, applications of electrolysis in metallurgy and industry. Chemical cells, reversible and irreversible cells with examples. Electromotive force of a cell and its measurement, Nernst equation; Single electrode potential, its measurement and sign convention. Standard electrode (reduction) potential, and its application to different kinds of half-cells. Application of EMF measurements in determining (i) free energy, enthalpy and

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(15 Hours) Unit – 4: Photochemistry

Characteristics of electromagnetic radiation and interaction of radiation with matter, difference between thermal and photochemical processes. Laws of photochemistry: Grothus-Drapper law, Stark-Einstein law, Jablonski diagram depicting various processes occurring in the excited state, qualitative description of fluorescence, phosphorescence, non-radiative processes (internal conversion, intersystem crossing). Lambert-Beer’s law and its limitation, physical significance of absorption coefficient; quantum efficiency, reasons for low and high quantum efficiency. Kinetics of photochemical reactions (H2 + Br2 = HBr and 2HI = H2 + I2), photostationary state. Chemical actinometers (ferri-oxalate, uranyl oxalate, MGL [malachite green leucocyanide)] and Reinecke’s salt); chemiluminescence, role of photochemical reactions in biological process. (10 Hours) Reference Books:

 Peter, A. & Paula, J. de. Physical Chemistry 9th Ed., Oxford University Press (2011).  Castellan, G. W. Physical Chemistry 4th Ed., Narosa (2004).  Engel, T. & Reid, P. Physical Chemistry 3rd Ed., Prentice-Hall (2012).  Barrow, G. M., Physical Chemistry 5th Ed., Tata McGraw Hill: New Delhi (2006).  Mortimer, R. G. Physical Chemistry 3rd Ed., Elsevier: NOIDA, UP (2009).  Rogers, D. W. Concise Physical Chemistry Wiley (2010).  Silbey, R. J.; Alberty, R. A. & Bawendi, M. G. Physical Chemistry 4th Ed., John Wiley & Sons, Inc. (2005).  Laidler, K. J.; Chemical Kinetics, Eds: 3rd, Pearson, New Delhi, 2011.  Crow, D. R: Principles and Applications of Electrochemistry, Eds. 4th, Blackie Academic & Professional, Madras, 1994.

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CHM P 223: Physical Chemistry – IV Lab (60 Hours) Catalysis: 1. Kinetics of enzymation reaction (starch-amylase system). 2. Kinetics of catalytic decomposition of H2O2

Surface Chemistry:

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 Verify the Freundlich and Langmuir isotherms for adsorption of acetic acid on activated charcoal.

Conductometry:

 Determination of cell constant.  Determination of equivalent conductance, degree of dissociation and dissociation constant of a weak acid.  Perform the following conductometric titrations: (i) Strong acid versus strong base (ii) Weak acid versus strong base (iii) Dibasic acid versus strong base (iv) Potassium dichromate versus Mohr's salt

Potentiometry:

 Perform the following potentiometric titrations: (i) Strong acid versus strong base (ii) Weak acid versus strong base (iii) Dibasic acid versus strong base (iv) Potassium dichromate versus Mohr's salt

Photochemistry:

 Photochemical reduction of ferric oxalate in cyanotype blue printing.

Reference Books:

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SEMESTER – V

CHM T 311: Organic Chemistry – IV: Biomolecules (Credits: Theory-04, Practical-02) Theory: 60 Hours Unit – 1: Nucleic Acids

Components of nucleic acids, Nucleosides and nucleotides

Structure, synthesis and reactions of: Adenine, Guanine, Cytosine, Uracil and Thymine Structure of polynucleotides. (9 Hours) Unit – 2: Amino Acids, Peptides and Proteins

Amino acids, Peptides and their classification.

α-Amino Acids - Synthesis, ionic properties and reactions. Zwitterions, pKa values, isoelectric point and electrophoresis

Study of peptides: determination of their primary structures-end group analysis, methods of peptide synthesis. Synthesis of peptides using N-protecting, C-protecting and C-activating groups -Solid-phase synthesis

(16 Hours) Unit – 3: Enzymes

Introduction, classification and characteristics of enzymes. Salient features of active site of enzymes. Mechanism of enzyme action (taking trypsin as example), factors affecting enzyme action, coenzymes and cofactors and their role in biological reactions, specificity of enzyme action (including stereospecificity), enzyme inhibitors and their importance, phenomenon of inhibition (competitive, uncompetitive and non-competitive inhibition including allosteric inhibition). (8 Hours) Unit – 4: Lipids

Introduction to oils and fats; common fatty acids present in oils and fats, Hydrogenntion of fats and oils, Saponification value, acid value, iodine number. Reversion and rancidity.

(8 Hours) Unit – 5: Concept of Energy in Biosystems

Cells obtain energy by the oxidation of foodstuff (organic molecules). Introduction to metabolism (catabolism, anabolism). ATP: The universal currency of cellular energy, ATP hydrolysis and free energy change. Agents + for transfer of electrons in biological redox systems: NAD , FAD.

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Conversion of food to energy: Outline of catabolic pathways of carbohydrate- glycolysis, fermentation, Krebs cycle. Overview of catabolic pathways of fat and protein. Interrelationship in the metabolic pathways of protein, fat and carbohydrate. Caloric value of food, standard caloric content of food types. (7 Hours) Unit – 6: Pharmaceutical Compounds: Structure and Importance

Classification, structure and therapeutic uses of antipyretics: Paracetamol (with synthesis), Analgesics: Ibuprofen (with synthesis), Antimalarials: Chloroquine (with synthesis). An elementary treatment of Antibiotics and detailed study of chloramphenicol, Medicinal values of curcumin (haldi), azadirachtin (neem), vitamin C and antacid (ranitidine).

(12 Hours)

Reference Books:

• Berg, J.M., Tymoczko, J.L. and Stryer, L. (2006) Biochemistry. VIth Edition. W.H. Freeman and Co. • Nelson, D.L., Cox, M.M. and Lehninger, A.L. (2009) Principles of Biochemistry. IV Edition. W.H. Freeman and Co. • Murray, R.K., Granner, D.K., Mayes, P.A. and Rodwell, V.W. (2009) Harper’s Illustrated Biochemistry. XXVIII edition. Lange Medical Books/ McGraw-Hill.

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CHM P 311: Organic Chemistry – IV Lab (60 Hours) 1. Estimation of glycine by Sorenson’s formalin method. 2. Study of the titration curve of glycine. 3. Estimation of proteins by Lowry’s method. 4. Study of the action of salivary amylase on starch at optimum conditions. 5. Effect of temperature on the action of salivary amylase. 6. Saponification value of an oil or a fat. 7. Determination of Iodine number of an oil/ fat. 8. Isolation and characterization of DNA from onion/ cauliflower/peas.

Reference Books:

• Manual of Biochemistry Workshop, 2012, Department of Chemistry, University of Delhi. • Arthur, I. V. Quantitative Organic Analysis, Pearson.

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CHM T 312: Physical Chemistry – V: Quantum Chemistry and Spectroscopy (Credits: Theory-04, Practicals-02) Theory: 60 Hours Unit – 1: Quantum Chemistry – I A review of quantum mechanics versus classical mechanics, (black body radiation, photoelectric effect, Compton’s effect), wave nature of electron; wave particle duality; Heisenberg’s uncertainty principle.

Schrödinger wave equation: wave function and interpretation, wave functions and probabilities; normalization and orthogonality of wave functions; time-independent Schrödinger equations.

Operators and their algebra, linear and Hermitian operators, quantum mechanical operators for the dynamic variables; eigenfunctions, eigenvalues and eigen value equation, average value and the expectation value of the physical quantities; expansion of arbitrary state in term of complete set; postulates of quantum mechanics.

Schrödinger equation and its application to free particle and “particle-in-a-box” (rigorous treatment), quantization of energy levels, zero-point energy and Heisenberg Uncertainty principle; wavefunctions, probability distribution functions, nodal properties, Extension to two and three dimensional boxes, separation of variables, degeneracy.

Qualitative treatment of simple harmonic oscillator model of vibrational motion: Setting up of Schrödinger equation and discussion of solution and wavefunctions. Vibrational energy of diatomic molecules and zero-point energy. Rigid rotator model of rotation of diatomic molecule. Schrödinger equation, transformation to spherical polar coordinates. Separation of variables. Spherical harmonics. Discussion of solution. Angular momentum: Commutation rules, quantization of square of total angular momentum and z-component. (12 Hours) Unit – 2: Quantum Chemistry – II Qualitative treatment of hydrogen and hydrogen like atoms, setting up of Schrödinger wave equation in spherical polar coordinate; separation into three equation of variables, R, theta and phi (without derivation), introduction of the four quantum numbers and their interdependence on the basis of the solutions of the three equations, total wave function, expression for the energy, probability density function, radial and angular plots., expressions for the total wave function for 1s, 2s, 2p and 3d orbitals of hydrogen. Application of the Schrödinger equation to two or more (many) electron systems, limitations of the equation, need for the approximate solutions, methods of obtaining the approximate solution of the Schrödinger wave equation. The variation principle (particle-in-a-box, harmonic oscillator, hydrogen atom), electron spin, Pauli antisymmetry principle; application to the two electron system for ground and exited state He atom. (12 Hours)

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Unit – 3: Molecular Spectroscopy – I Interaction of electromagnetic radiation with molecules and various types of spectra; Born- Oppenheimer approximation. Rotation spectroscopy: Selection rules, intensities of spectral lines, determination of bond lengths of diatomic and linear triatomic molecules, isotopic substitution. Vibrational spectroscopy: Classical equation of vibration, computation of force constant, amplitude of diatomic molecular vibrations, anharmonicity, Morse potential, dissociation energies, fundamental frequencies, overtones, hot bands, degrees of freedom for polyatomic molecules, modes of vibration, concept of group frequencies. Vibration-rotation spectroscopy: diatomic vibrating rotator, P, Q, R branches. Raman spectroscopy: Qualitative treatment of Rotational Raman effect; Effect of nuclear spin, Vibrational Raman spectra, Stokes and anti-Stokes lines; their intensity difference, rule of mutual exclusion.

(12 Hours) Unit – 4: Molecular Spectroscopy – II Electronic spectroscopy: Franck-Condon principle, electronic transitions, singlet and triplet states, fluorescence and phosphorescence, dissociation and predissociation, calculation of electronic transitions of polyenes using free electron model. Nuclear Magnetic Resonance (NMR) spectroscopy: Principles of NMR spectroscopy, Larmor precession, chemical shift and low resolution spectra, different scales, spin-spin coupling and high resolution spectra, interpretation of PMR spectra of organic molecules. Electron Spin Resonance (ESR) spectroscopy: Its principle, hyperfine structure, ESR of simple radicals. (12 Hours) UNIT – 5: Electrical & Magnetic Properties of Atoms and Molecules Basic ideas of electrostatics, Electrostatics of dielectric media, Clausius-Mosotti equation, Lorenz-Laurentz equation, Dipole moment and molecular polarizabilities and their measurements. Diamagnetism, paramagnetism, magnetic susceptibility and its measurement, molecular interpretation. (12 Hours) Reference Books:

 Atkins, P. and Friedman, R.; Molecular Quantum Mechanics, Eds: 5th, Oxford University Press, 2011.  Chandra, A. K.: Introductory Quantum Chemistry, Eds: 4th, Tata McGraw Hill, New Delhi, 1994.  Levine, I. N.: Quantum Chemistry, Eds: 5th, PHI, 2000.  Engel, T. and Reid, P.: Quantum Chemistry and Spectroscopy, Pearson, 2011, New Delhi.

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 Prasad, R. K.: Quantum Chemistry, Eds: 4th, New Age Inter. Pub., 2010.  Banwell, C. N. and McCash, E. M.: Fundamentals of Molecular Spectroscopy, Ed. 4th, Tata McGraw-Hill, 1994.  G. M. Barrow: Introduction to Molecular Spectroscopy  Kakkar, R. Atomic & Molecular Spectroscopy, Cambridge University Press (2015)

------CHM P 312: Physical Chemistry – V Lab (60 Hours)

UV/Visible spectroscopy:

 Study the 200-500 nm absorbance spectra of KMnO4 and K2Cr2O7 (in 0.1 M H2SO4) and determine the λmax values. Calculate the energies of the two transitions in different units (J molecule-1, kJ mol-1, cm-1, eV).  Study the pH-dependence of the UV-Vis spectrum (200-500 nm) of K2Cr2O7.  Record the 200-350 nm UV spectra of the given compounds (acetone, acetaldehyde, 2- propanol, acetic acid) in water. Comment on the effect of structure on the UV spectra of organic compounds. Colorimetry:

 Verify Lambert-Beer’s law and determine the concentration of CuSO4/KMnO4/K2Cr2O7 in a solution of unknown concentration.  Determine the concentrations of KMnO4 and K2Cr2O7 in a mixture.  Study the kinetics of iodination of propanone in acidic medium.  Determine the amount of iron present in a sample using 1,10-phenathroline.  Determine the dissociation constant of an indicator (phenolphthalein).  Study the kinetics of interaction of crystal violet/phenolphthalein with sodium hydroxide.  Analysis of the given vibration-rotation spectrum of HCl(g)

Reference Books:

 Garland, C. W.; Nibler, J. W. & Shoemaker, D. P. Experiments in Physical Chemistry 8th Ed.; McGraw-Hill: New York (2003).  Khosla, B. D.; Garg, V. C. & Gulati, A. Senior Practical Physical Chemistry, R. Chand & Co.: New Delhi (2011).  Halpern, A. M. & McBane, G. C. Experimental Physical Chemistry 3rd Ed.; W.H. Freeman & Co.: New York (2003).  Elias A. J.: A collection of Interesting General Chemistry Experiments, University Press, India.  Yadav J. B.: Advanced Practical Physical Chemistry, Krishna Prakashan Media (P) Ltd. Meerut.

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SEMSETER – VI

CHM T 321: Inorganic Chemistry-IV: Organometallic Chemistry (Credits: Theory-04, Practicals-02) Theory: 60 Hours

Unit – 1: Theoretical Principles in Qualitative Analysis (H2S Scheme)

Basic principles involved in analysis of cations and anions and solubility products, common ion effect. Principles involved in separation of cations into groups and choice of group reagents. Interfering anions (fluoride, borate, oxalate and phosphate) and need to remove them after Group II. (10 Hours) Unit – 2: Organometallic Compounds

Definition and classification of organometallic compounds on the basis of bond type. Concept of hapticity of organic ligands. Metal carbonyls: 18 electron rule, electron count of mononuclear, polynuclear and substituted metal carbonyls of 3d series. General methods of preparation (direct combination, reductive carbonylation, thermal and photochemical decomposition) of mono and binuclear carbonyls of 3d series. Structures of mononuclear and binuclear carbonyls of Cr, Mn, Fe, Co and Ni using VBT. π-acceptor behaviour of CO (MO diagram of CO to be discussed), synergic effect and use of IR data to explain extent of back bonding. Zeise’s salt: Preparation and structure, evidences of synergic effect and comparison of synergic effect with that in carbonyls. Metal Alkyls: Important structural features of methyl lithium (tetramer) and trialkyl aluminium (dimer), concept of multicentre bonding in these compounds. Role of triethylaluminium in polymerisation of ethene (Ziegler – Natta Catalyst). Species present in ether solution of Grignard reagent and their structures, Schlenk equilibrium. Ferrocene: Preparation and reactions (acetylation, alkylation, metallation, Mannich Condensation). Structure and aromaticity. Comparison of aromaticity and reactivity with that of benzene. (22 Hours) Unit – 3: Reaction Kinetics and Mechanism

Introduction to inorganic reaction mechanisms. Substitution reactions in square planar complexes, Trans- effect, theories of trans effect, Mechanism of nucleophilic substitution in square planar complexes, Thermodynamic and Kinetic stability, Kinetics of octahedral substitution, Ligand field effects and reaction rates, Mechanism of substitution in octahedral complexes. (10 Hours)

Unit – 4: Catalysis by Organometallic Compounds

Study of the following industrial processes and their mechanism: 1. Alkene hydrogenation (Wilkinsons Catalyst)

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2. Hydroformylation (Co salts) 3. Wacker Process 4. Synthetic gasoline (Fischer Tropsch reaction) 5. Synthesis gas by metal carbonyl complexes (10 Hours)

Unit – 5: Complexometric Titration

Complexones, masking and demasking interactions, metallochrome indicators, titration of metal ions and their mixtures with EDTA, hardness of water and its determination (8 Hours)

Reference Books:

• Vogel, A.I. Qualitative Inorganic Analysis, Longman, 1972

• Svehla, G. Vogel's Qualitative Inorganic Analysis, 7th Edition, Prentice Hall, 1996- 03-07. • Cotton, F.A. G.; Wilkinson & Gaus, P.L. Basic Inorganic Chemistry 3rd Ed.; Wiley India, • Huheey, J. E.; Keiter, E.A. & Keiter, R.L. Inorganic Chemistry, Principles of Structure and Reactivity 4th Ed., Harper Collins 1993, Pearson,2006. • Sharpe, A.G. Inorganic Chemistry, 4th Indian Reprint (Pearson Education) 2005 • Douglas, B. E.; McDaniel, D.H. & Alexander, J.J. Concepts and Models in Inorganic rd Chemistry3 Ed., John Wiley and Sons, NY, 1994. • Greenwood, N.N. & Earnshaw, A. Chemistry of the Elements, Elsevier 2nd Ed, 1997 (Ziegler Natta Catalyst and Equilibria in Grignard Solution). th • Lee, J.D. Concise Inorganic Chemistry 5 Ed., John Wiley and sons 2008. • Powell, P. Principles of Organometallic Chemistry, Chapman and Hall, 1988. • Shriver, D.D. & P. Atkins, Inorganic Chemistry 2nd Ed., Oxford University Press, 1994. • Basolo, F. & Person, R. Mechanisms of Inorganic Reactions: Study of Metal Complexes in Solution 2nd Ed., John Wiley & Sons Inc; NY. • Purcell, K.F. & Kotz, J.C., Inorganic Chemistry, W.B. Saunders Co. 1977 th • Miessler, G. L. & Donald, A. Tarr, Inorganic Chemistry 4 Ed., Pearson, 2010. • Collman, James P. et al. Principles and Applications of Organotransition Metal Chemistry. Mill Valley, CA: University Science Books, 1987. • Crabtree, Robert H. The Organometallic Chemistry of the Transition Metals. j New York, NY: John Wiley, 2000. • Spessard, Gary O., &Gary L. Miessler. Organometallic Chemistry. Upper Saddle River, NJ: Prentice-Hall, 1996.

------CHM P 321: Inorganic Chemistry – IV Lab (60 Hours) Qualitative semimicro analysis of mixtures containing 3 anions and 3 cations. Emphasis should be given to the understanding of the chemistry of different reactions. The following

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2 - - 2- 2- 2 ------3- 2- 3- + + CO3 , NO2 , S , SO3 ,S2O3 , CH3COO , F ,Cl , Br , I , NO3 , BO 3 , C2O4 , PO4 , NH4 , K , Pb2+, Cu2+, Cd2+, Bi3+, Sn2+, Sb3+, Fe3+, Al3+,, Cr3+, Zn2+, Mn2+, Co2+, Ni2+, Ba2+,Sr2+, Ca2+, Mg2+

Mixtures should preferably contain one interfering anion, or insoluble component (BaSO4, 2- 2- - - - SrSO4, PbSO4, CaF2 or Al2O3) or combination of anions e.g. CO3 and SO3 , NO2 and NO3 , Cl ------and Br , Cl and I , Br and I , NO3 and Br , NO3 and I .

Spot tests should be done whenever possible

i. Measurement of 10 Dq by spectrophotometric method ii. Verification of spectrochemical series. iii. Controlled synthesis of two copper oxalate hydrate complexes: kinetic vs thermodynamic factors. 2+/ 3+ iv. Preparation of acetylacetanato complexes of Cu Fe . Find the λmax of the complex. v. Synthesis of ammine complexes of Ni(II) and its ligand exchange reactions (e.g. bidentate ligands like acetylacetone, DMG, glycine) by substitution method.

Reference Books

• Vogel’s Qualitative Inorganic Analysis, Revised by G. Svehla. • Marr & Rockett Inorganic Preparations. • Ghosal, Mahapatra and Nad, An Advanced Course in Practical Chemistry.

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CHM T 322: Organic Chemistry – V: Spectroscopy (Credits: Theory-04, Practicals-02) Theory: 60 Hours

Unit - 1: Organic Spectroscopy

General principles Introduction to absorption and emission spectroscopy.

UV Spectroscopy: Types of electronic transitions, λmax, Chromophores and Auxochromes, Bathochromic and Hypsochromic shifts, Intensity of absorption; Application of Woodward Rules for calculation of λmax for the following systems: α,β unsaturated aldehydes, ketones, carboxylic acids and esters; Conjugated dienes: alicyclic, homoannular and heteroannular; Extended conjugated systems (aldehydes, ketones and dienes); distinction between cis and trans isomers.

IR Spectroscopy: Fundamental and non-fundamental molecular vibrations; IR absorption positions of O, N and S containing functional groups; Effect of H-bonding, conjugation, resonance and ring size on IR absorptions; Fingerprint region and its significance; application in functional group analysis.

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NMR Spectroscopy: Basic principles of Proton Magnetic Resonance, chemical shift and factors influencing it; Spin – Spin coupling and coupling constant; Anisotropic effects in alkene, alkyne, aldehydes and aromatics, Interpetation of NMR spectra of simple compounds.

Applications of IR, UV and NMR for identification of simple organic molecules.

(24 Hours) Unit - 2: Carbohydrates

Occurrence, classification and their biological importance.

Monosaccharides: Constitution and absolute configuration of glucose and fructose, epimers and anomers, mutarotation, determination of ring size of glucose and fructose, Haworth projections and conformational structures; Interconversions of aldoses and ketoses; Killiani-Fischer synthesis and Ruff degradation;

Disaccharides – Structure elucidation of maltose, lactose and sucrose.

Polysaccharides – Elementary treatment of starch, cellulose and glycogen.

(16 Hours) Unit – 3: Dyes

Classification, Colour and constitution; Mordant and Vat Dyes; Chemistry of dyeing, Synthesis and applications of: Azo dyes – Methyl Orange and Congo Red (mechanism of Diazo Coupling); Triphenyl Methane Dyes -Malachite Green, Rosaniline and Crystal Violet; Phthalein Dyes – Phenolphthalein and Fluorescein; Natural dyes –structure elucidation and synthesis of Alizarin and Indigotin; Edible Dyes with examples.

(8 Hours) Unit – 4: Polymers

Introduction and classification including di-block, tri-block and amphiphilic polymers; Number average molecular weight, Weight average molecular weight, Degree of polymerization, Polydispersity Index.

Polymerisation reactions -Addition and condensation -Mechanism of cationic, anionic and free radical addition polymerization; Metallocene-based Ziegler-Natta polymerisation of alkenes; Preparation and applications of plastics – thermosetting (phenol-formaldehyde, Polyurethanes) and thermosoftening (PVC, polythene);

Fabrics – natural and synthetic (acrylic, polyamido, polyester); Rubbers – natural and synthetic: Buna-S, Chloroprene and Neoprene; Vulcanization; Polymer additives; Introduction to liquid crystal polymers; Biodegradable and conducting polymers with examples.

(12 Hours)

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Reference Books:

• Kalsi, P. S. Textbook of Organic Chemistry 1st Ed., New Age International (P) Ltd. Pub. • Morrison, R. T. & Boyd, R. N. Organic Chemistry, Dorling Kindersley (India) Pvt. Ltd. (Pearson Education). • Billmeyer, F. W. Textbook of Polymer Science, John Wiley & Sons, Inc. • Gowariker, V. R.; Viswanathan, N. V. & Sreedhar, J. Polymer Science, New Age International (P) Ltd. Pub. • Finar, I. L. Organic Chemistry (Volume 2: Stereochemistry and the Chemistry of Natural Products), Dorling Kindersley (India) Pvt. Ltd. (Pearson Education). • Graham Solomons, T.W. Organic Chemistry, John Wiley & Sons, Inc. • Clayden, J.; Greeves, N.; Warren, S.; Wothers, P.; Organic Chemistry, Oxford University Press. • Singh, J.; Ali, S.M. & Singh, J. Natural Product Chemistry, Prajati Prakashan (2010). • Kemp, W. Organic Spectroscopy, Palgrave

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CHM P 322: Organic Chemistry – V Lab (60 Hours) 1. Extraction of caffeine from tea leaves. 2. Preparation of sodium polyacrylate. 3. Preparation of urea formaldehyde. 4. Analysis of Carbohydrate: aldoses and ketoses, reducing and non-reducing sugars. 5. Qualitative analysis of unknown organic compounds containing monofunctional groups (carbohydrates, aryl halides, aromatic hydrocarbons, nitro compounds, amines and amides) and simple bifunctional groups, for e.g. salicylic acid, cinnamic acid, nitrophenols etc. 6. Identification of simple organic compounds by IR spectroscopy and NMR spectroscopy (Spectra to be provided). 7. Preparation of methyl orange.

Reference Books:

• Vogel, A.I. Quantitative Organic Analysis, Part 3, Pearson (2012). • Mann, F.G. & Saunders, B.C. Practical Organic Chemistry, Pearson Education (2009) • Furniss, B.S.; Hannaford, A.J.; Smith, P.W.G.; Tatchell, A.R. Practical Organic Chemistry, 5th Ed., Pearson (2012) • Ahluwalia, V.K. & Aggarwal, R. Comprehensive Practical Organic Chemistry: Preparation and Quantitative Analysis, University Press (2000). • Ahluwalia, V.K. & Dhingra, S. Comprehensive Practical Organic Chemistry: Qualitative Analysis, University Press (2000).

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*Discipline Specific Elective (DSE) in Chemistry

CHM T 313-314 and 323-324

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DSE – A: Applications of Computers in Chemistry (Credits: Theory-04, Practicals-02) Theory: 60 Hours Unit – 1: Basics Constants, variables, bits, bytes, binary and ASCII formats, arithmetic expressions, hierarchy of operations, inbuilt functions. Elements of the BASIC language. BASIC keywords and commands. Logical and relative operators. Strings and graphics. Compiled versus interpreted languages. Debugging. Simple programs using these concepts. Matrix addition and multiplication. Statistical analysis. (30 Hours)

Unit – 2: Numerical methods

Roots of equations: Numerical methods for roots of equations: Quadratic formula, iterative method, Newton-Raphson method, Binary bisection and Regula-Falsi.

Differential calculus: Numerical differentiation.

Integral calculus: Numerical integration (Trapezoidal and Simpson’s rule), probability distributions and mean values.

Simultaneous equations: Matrix manipulation: addition, multiplication. Gauss-Siedal method.

Interpolation, extrapolation and curve fitting: Handling of experimental data.

Conceptual background of molecular modelling: Potential energy surfaces. Elementary ideas of molecular mechanics and practical MO methods. (30 Hours)

Reference Books: th • Harris, D. C. Quantitative Chemical Analysis. 6 Ed., Freeman (2007) Chapters 3-5. • Levie, R. de, How to use Excel in analytical chemistry and in general scientific data analysis, Cambridge Univ. Press (2001) 487 pages. • Noggle, J. H. Physical chemistry on a Microcomputer. Little Brown & Co. (1985). • Venit, S.M. Programming in BASIC: Problem solving with structure and style. Jaico Publishing House: Delhi (1996).

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DSE – A Lab: Applications of Computers in chemistry (60 Hours) Computer programs based on numerical methods for

1. Roots of equations: (e.g. volume of van der Waals gas and comparison with ideal gas, pH of a weak acid). 2. Numerical differentiation (e.g., change in pressure for small change in volume of a van der Waals gas, potentiometric titrations). 3. Numerical integration (e.g. entropy/ enthalpy change from heat capacity data), probability distributions (gas kinetic theory) and mean values. 4. Matrix operations. Application of Gauss-Siedel method in colourimetry. 5. Simple exercises using molecular visualization software.

Reference Books:

• McQuarrie, D. A. Mathematics for Physical Chemistry University Science Books (2008). rd • Mortimer, R. Mathematics for Physical Chemistry. 3 Ed. Elsevier (2005). • Steiner, E. The Chemical Maths Book Oxford University Press (1996). • Yates, P. Chemical Calculations. 2nd Ed. CRC Press (2007). th • Harris, D. C. Quantitative Chemical Analysis. 6 Ed., Freeman (2007) Chapters 3-5. • Levie, R. de, How to use Excel in analytical chemistry and in general scientific data analysis, Cambridge Univ. Press (2001) 487 pages. • Noggle, J. H. Physical Chemistry on a Microcomputer. Little Brown & Co. (1985). • Venit, S.M. Programming in BASIC: Problem solving with structure and style. Jaico Publishing House: Delhi (1996).

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DSE – B: Analytical Methods in Chemistry (Credits: Theory-04, Practicals-02) Theory: 60 Hours Unit – 1: Qualitative and quantitative aspects of analysis

Sampling, evaluation of analytical data, errors, accuracy and precision, methods of their expression, normal law of distribution if indeterminate errors, statistical test of data; F, Q and t test, rejection of data, and confidence intervals.

(5 Hours) Unit – 2: Optical methods of analysis

Origin of spectra, interaction of radiation with matter, fundamental laws of spectroscopy and selection rules, validity of Beer-Lambert’s law.

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UV-Visible Spectrometry: Basic principles of instrumentation (choice of source, monochromator and detector) for single and double beam instrument;

Basic principles of quantitative analysis: estimation of metal ions from aqueous solution, geometrical isomers, keto-enol tautomers. Determination of composition of metal complexes using Job’s method of continuous variation and mole ratio method.

Infrared Spectrometry: Basic principles of instrumentation (choice of source, monochromator & detector) for single and double beam instrument; sampling techniques.

Structural illustration through interpretation of data, Effect and importance of isotope substitution.

Flame Atomic Absorption and Emission Spectrometry: Basic principles of instrumentation (choice of source, monochromator, detector, choice of flame and Burner designs. Techniques of atomization and sample introduction; Method of background correction, sources of chemical interferences and their method of removal. Techniques for the quantitative estimation of trace level of metal ions from water samples.

(25 Hours) Unit – 3: Thermal methods of analysis:

Theory of thermogravimetry (TG), basic principle of instrumentation.

Techniques for quantitative estimation of Ca and Mg from their mixture.

(5 Hours) Unit – 4: Electroanalytical methods:

Classification of electroanalytical methods, basic principle of pH metric, potentiometric and conductometric titrations. Techniques used for the determination of equivalence points. Techniques used for the determination of pKa values.

(10 Hours) Unit – 5: Separation techniques:

Solvent extraction: Classification, principle and efficiency of the technique. Mechanism of extraction: extraction by solvation and chelation. Technique of extraction: batch, continuous and counter current extractions. Qualitative and quantitative aspects of solvent extraction: extraction of metal ions from aqueous solution, extraction of organic species from the aqueous and nonaqueous media. Chromatography: Classification, principle and efficiency of the technique. Mechanism of separation: adsorption, partition & ion exchange. Development of chromatograms: frontal, elution and displacement methods.

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Qualitative and quantitative aspects of chromatographic methods of analysis: IC, GLC, GPC, TLC and HPLC.

Stereoisomeric separation and analysis: Measurement of optical rotation, calculation of Enantiomeric excess (ee)/ diastereomeric excess (de) ratios and determination of enantiomeric composition using NMR, Chiral solvents and chiral shift reagents. Chiral chromatographic techniques using chiral columns (GC and HPLC).

Role of computers in instrumental methods of analysis.

(15 Hours)

Reference Books:

• Vogel, Arthur I: A Test book of Quantitative Inorganic Analysis (Rev. by G.H. Jeffery and others) 5th Ed. The English Language Book Society of Longman . • Willard, Hobert H. et al.: Instrumental Methods of Analysis, 7th Ed. Wardsworth Publishing Company, Belmont, California, USA, 1988. • Christian, Gary D; Analytical Chemistry, 6th Ed. John Wiley & Sons, New York, 2004. • Harris, Daniel C: Exploring Chemical Analysis, Ed. New York, W.H. Freeman, 2001. • Khopkar, S.M. Basic Concepts of Analytical Chemistry. New Age, International Publisher, 2009. • Skoog, D.A. Holler F.J. and Nieman, T.A. Principles of Instrumental Analysis, Thomson Asia Pvt. Ltd. Singapore. • Mikes, O. & Chalmes, R.A. Laboratory Hand Book of Chromatographic & Allied Methods, Elles Harwood Ltd. London. • Ditts, R.V. Analytical Chemistry – Methods of separation.

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DSE – B Lab: Analytical Methods in Chemistry

(60 Hours) I. Separation Techniques

1. Chromatography:

(a) Separation of mixtures

(i) Paper chromatographic separation of Fe3+, Al3+, and Cr3+.

(ii) Separation and identification of the monosaccharides present in the given mixture (glucose & fructose) by paper chromatography. Reporting the Rf values.

(b) Separate a mixture of Sudan yellow and Sudan Red by TLC technique and identify them on the basis of their Rf values.

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II. Solvent Extractions:

(i) To separate a mixture of Ni2+ & Fe2+ by complexation with DMG and extracting the Ni2+- DMG complex in chloroform, and determine its concentration by spectrophotometery.

(ii) Solvent extraction: separation from a mixture of irons and gallium.

3. Determine the pH of the given aerated drinks fruit juices, shampoos and soaps.

4. Determination of Na, Ca, Li in cola drinks and fruit juices using fame photometric techniques.

5. Analysis of soil:

(i) Determination of pH of soil. (ii) Total soluble salt (iii) Estimation of calcium, magnesium, phosphate, nitrate

6. Quantitative Estimation of Metal Ions in Binary Mixture

(i) Estimation of Iron (II/III) and Calcium (II) in a Mixture (ii) Estimation of Fe(III) and Mn (II) in a Mixture (iii)Estimation of Fe(III) and Cu(II) in a Mixture (iv) Estimation of Fe(III) and Zn(II) in a Mixture

III Spectrophotometry

1. Determination of pKa values of indicator using spectrophotometry. 2. Structural characterization of compounds by infrared spectroscopy. 3. Determination of dissolved oxygen in water. 4. Determination of chemical oxygen demand (COD). 5. Determination of Biological oxygen demand (BOD). 6. Determine the composition of the Ferric-salicylate/ ferric-thiocyanate complex by Job’s method.

Reference Books:

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2004. • Harris, Daniel C: Exploring Chemical Analysis, Ed. New York, W.H. Freeman, 2001. • Khopkar, S.M. Basic Concepts of Analytical Chemistry. New Age, International Publisher, 2009. • Skoog, D.A. Holler F.J. and Nieman, T.A. Principles of Instrumental Analysis, Thomson Asia Pvt. Ltd. Singapore. • Mikes, O. & Chalmes, R.A. Laboratory Hand Book of Chromatographic & Allied Methods, Elles Harwood Ltd. London. • Ditts, R.V. Analytical Chemistry – Methods of separation. ------

DSE – C: Basics of Drug Design & Medicinal Chemistry (Credits: Theory-04, Practicals-02) Theory: 60 Hours Unit – 1: Basic Concept of Drug Design & Physiochemical Factors

Introduction; Basics of drug design; analog and Prodrug; Cocept of lead; Factors governing drug design; Rational approach to drug design. Physical-Chemical factors and biological activities; Factors governing ability of drug to reach active site. (12 Hours) Unit – 2: Molecular Modeling & Ligand Design Concept

Concept of structure of drug molecules and its optimization; Molecular modeling and drug design; Basic concept of Protein and its structure; Structure based drug design; Ligand receptor recognition; Active site of a target molecules; Characterization of site and design of ligands.

(12 Hours) Unit – 3: Analgesic & Antimalerial Drugs

Concept of Analgesics drug; Synthesis and use of analgesics drugs: Paracetamol, Phenacetine, Acetanilide, Aspirin, Salol, Cinchophene, and Phenazone.

Antimalerial Drugs: Synthesis and use of Chloroquine phosphate.

(12 Hours) Unit - 4: Antibacterial & Antibiotic

Sulphonamide drugs: Antibacterial properties. Synthesis and use of Sulphonamide drugs: Sulphanilide, Sulphapyridine, Sulphathiazole, Sulphadiazine, Concept of Antibiotics with its application. (12 Hours)

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Unit – 5: Herbal medicine

Herbal Drug: Its importance

Ethanobotanical survey methods; introduction to ayurveda, pharmacopia; plants as source of drugs; Indian medicinal plants and uses - Tulasi, Neem, Pili, Mango, Sarpagandhi, Gulbakavali, Shyma Haldi, Vanchana, Safed Musli, Aswagandha, Satavar, Pipalendi, Digitalis, Senna, Clove, Cardamom, Plantago, Artemisia annua, Coleus forskoli, Aloe Patal Kumhda, Banpyaz.

(12 Hours) Reference Books:

 Asutosh Kar, Medicinal Chemistry, New Age Publication.  P. D. Sethi, Dilip Charegaonkar: Identification of Drugs and Pharmaceutical Formulations by Thin Layer Chromatography –2nd Edition.  G.E. Trease, W.C. Evans: Pharmacognosy, ELBS.  Varro E.Tyler, Lynn. R.Brady, James E.Robbers: Pharmacognosy.  T.E. Wallis: Text Book of Pharmacognosy, CBS Pub. Delhi.  Kirthikar, Basu: Indian Medicinal Plants.  K.M. Nalkarni: Indian Meteria Medica  W. Dymock: Pharmacographia Indica

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DSE – C Lab: Basics of Drug Design & Medicinal Chemistry

(60 Hours) (a) Drawing of different organic molecules using ChemDraw and ChemSketech software.

(b) Synthesis and characterization of following drugs:

1. Paracetamol, 2. Acetanilide, 3. Aspirin, 4. Phenazone 5. Ibuprofen

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DSE – D: Novel Inorganic Solids (Credits: Theory-04, Practicals-02) Theory: 60 Hours

Unit – 1: Synthesis and modification of inorganic solids

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Conventional heat and beat methods, Co-precipitation method, Sol-gel methods, Hydrothermal method, Ion-exchange and Intercalation methods. (10 Hours) Unit – 2: Inorganic solids of technological importance

Solid electrolytes – Cationic, anionic, mixed Inorganic pigments – coloured solids, white and black pigments.

Molecular material and fullerides, molecular materials & chemistry – one-dimensional metals, molecular magnets, inorganic liquid crystals.

(10 Hours) Unit – 3: Nanomaterials

Overview of nanostructures and nanomaterials: classification.

Preparation of gold and silver metallic nanoparticles, self-assembled nanostructures-control of nanoarchitecture-one dimensional control. Carbon nanotubes and inorganic nanowires. Bio- inorganic nanomaterials, DNA and nanomaterials, natural and antisical nanomaterials, bionano composites.

(10 Hours) Unit – 4: Introduction to engineering materials for mechanical construction

Composition, mechanical and fabricating characteristics and applications of various types of cast irons, plain carbon and alloy steels, copper, aluminum and their alloys like duralumin, brasses and bronzes cutting tool materials, super alloys thermoplastics, thermosets and composite materials. (10 Hours) Unit – 5: Composite materials

Introduction, limitations of conventional engineering materials, role of matrix in composites, classification, matrix materials, reinforcements, metal-matrix composites, polymer-matrix composites, fibre-reinforced composites, environmental effects on composites, applications of composites. (10 Hours) Unit – 6: Polymers

Conducting polymers - Introduction, conduction mechanism, polyacetylene, polyparaphenylene and polypyrole, applications of conducting polymers, Ion-exchange resins and their applications. Ceramic & Refractory: Introduction, classification, properties, raw materials, manufacturing and applications. (10 Hours)

Reference Books:

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• Shriver & Atkins. Inorganic Chemistry, Peter Alkins, Tina Overton, Jonathan Rourke, th Mark Weller and Fraser Armstrong, 5 Edition, Oxford University Press (2011-2012) • Adam, D.M. Inorganic Solids: An introduction to concepts in solid-state structural chemistry. • Frank J. Ovens, Introduction to Nanotechnology

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DSE – D Lab: Novel Inorganic Solids (60 Hours) 1. Determination of cation exchange method 2. Determination of total difference of solids. 3. Synthesis of hydrogel by co-precipitation method. 4. Synthesis of silver and gold metal nanoparticles.

Ion exchange:

(i) Determination of exchange capacity of cation exchange resins and anion exchange resins. (ii) Separation of metal ions from their binary mixture. (iii) Separation of amino acids from organic acids by ion exchange chromatography.

Reference Book:  Fahan, Materials Chemistry, Springer (2004).  Vogel, Arthur I: A Test book of Quantitative Inorganic Analysis (Rev. by G.H. Jeffery and others) 5th Ed. The English Language Book Society of Longman.

DSE – E: Basic of Polymer Chemistry (Credits: Theory-04, Practicals-02) Theory: 60 Hours

Unit – 1: Introduction and Classification Different schemes of classification of polymers, Polymer nomenclature, Molecular forces and chemical bonding in polymers, Texture of Polymers. Functionality and its importance: Criteria for synthetic polymer formation, classification of polymerization processes, Relationships between functionality, extent of reaction and degree of polymerization. Bi- functional systems, Poly-functional systems.

(12 Lectures) Unit – 2: Kinetics of Polymerization

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Mechanism and kinetics of step growth, radical chain growth, ionic chain (both cationic and anionic) and coordination polymerizations, Mechanism and kinetics of copolymerization, polymerization techniques. (8 Lectures) Unit – 3: Crystallization and crystallinity Determination of crystalline melting point and degree of crystallinity, Morphology of crystalline polymers, Factors affecting crystalline melting point. Nature and structure of polymers-Structure Property relationships.

(8 Lectures) Unit – 4: Molecular weight and Glass Transition Temperature of polymers

(Molecular weight distribution and its significance. Polydispersity index. Mn, Mw, etc) by end group analysis, viscometry, light scattering and osmotic pressure methods. Glass transition temperature (Tg) and determination of Tg, Free volume theory, WLF equation, Factors affecting glass transition temperature (Tg). (16 Lectures)

Unit – 5: Polymer Solution

Criteria for polymer solubility, Solubility parameter, Thermodynamics of polymer solutions, entropy, enthalpy, and free energy change of mixing of polymers solutions, Flory- Huggins theory, Lower and Upper critical solution temperatures.

Properties of Polymers (Physical, thermal, Flow & Mechanical Properties).

Brief introduction to preparation, structure, properties and application of the following polymers: polyolefins, polystyrene and styrene copolymers, poly(vinyl chloride) and related polymers, poly(vinyl acetate) and related polymers, acrylic polymers, fluoro polymers, polyamides and related polymers. Phenol formaldehyde resins (Bakelite, Novalac), polyurethanes, silicone polymers, polydienes, Polycarbonates, Conducting Polymers, [polyacetylene, polyaniline, poly(p-henylene sulphide polypyrrole, polythiophene)]. (16 Lectures) Reference Books:

 Seymour’s Polymer Chemistry, Marcel Dekker, Inc.  G. Odian: Principles of Polymerization, John Wiley.  F.W. Billmeyer: Text Book of Polymer Science, John Wiley.  A Ravve: Principle of Polymer Chemistry, Eds. 3rd, Springer Science + Business Media, New York, 2012.

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 P. Ghosh: Polymer Science & Technology, Tata Mcgraw-Hill.  R.W. Lenz: Organic Chemistry of Synthetic High Polymers.

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DSE – E Lab: Basic of Polymer Chemistry

(60 Hours) 1. Polymer synthesis

(i) Free radical solution polymerization of styrene (St)/Methyl Methacrylate (MMA) / Methyl Acrylate (MA) / Acrylic acid (AA). (a) Purification of monomer (b) Polymerization using benzoyl peroxide (BPO)/2,2’-azo-bis-isobutyl-onitrile (AIBN)

(ii) Preparation of nylon 66/6 (iii) Interfacial polymerization, preparation of polyester from isophthaloyl chloride (IPC) and phenolphthalein (a) Preparation of IPC (b) Purification of IPC (c) Interfacial polymerization (iv) Redox polymerization of acrylamide (v) Precipitation polymerization of acrylonitrile (vi) Preparation of urea-formaldehyde resin (vii) Preparations of novalac resin/resold resin (viii) Microscale Emulsion Polymerization of Poly(methylacrylate)

2. Polymer characterization

(i) Determination of molecular weight by viscometry: (a) Polyacrylamide-aq.NaNO2 solution (b) (Poly vinyl proplylidine (PVP) in water (ii) Determination of the viscosity-average molecular weight of poly(vinyl alcohol) PVOH) and the fraction of “head-to-head” monomer linkages in the polymer. (iii) Determination of molecular weight by end group analysis: Polyethylene glycol (PEG) (OH group). (iv) Testing of mechanical properties of polymers. (v) Determination of hydroxyl number of a polymer using colorimetric method.

3. Polymer analysis (i) Estimation of the amount of HCHO in the given solution by sodium sulphite method (ii) Instrumental Techniques (iii) IR studies of polymers (iv) DSC analysis of polymers (v) Preparation of polyacrylamide and its electrophoresis

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*at least 7 experiments to be carried out.

Reference Books:

 Malcohm P. Stevens, Polymer Chemistry: An Introduction, 3rd Ed.  Harry R. Allcock, Frederick W. Lampe and James E. Mark, Contemporary Polymer Chemistry, 3rd ed. Prentice-Hall (2003)  Fred W. Billmeyer, Textbook of Polymer Science, 3rd ed. Wiley-Interscience (1984)  L. H. Sperling, Introduction to Physical Polymer Science, 4th ed. John Wiley & Sons  (2005)  Malcolm P. Stevens, Polymer Chemistry: An Introduction, 3rd ed. Oxford University Press (2005)  Seymour/ Carraher’s Polymer Chemistry, 9th ed. by Charles E. Carraher, Jr. (2013).  Petr Munk and Tejraj M. Aminabhavi, Introduction to Macromolecular Science, 2nd ed. John Wiley & Sons (2002)  Joel R. Fried, Polymer Science and Technology, 2nd ed. Prentice-Hall (2003)

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DSE – F: Green Chemistry (Credits: Theory-04, Practicals-02) Theory: 60 Hours

Unit – 1: Introduction to Green Chemistry

What is Green Chemistry? Need for Green Chemistry. Goals of Green Chemistry. Limitations/ Obstacles in the pursuit of the goals of Green Chemistry. (4 Hours) Unit – 2: Principles of Green Chemistry and Designing a Chemical synthesis

Twelve principles of Green Chemistry with their explanations and examples; Designing a Green Synthesis using these principles; Prevention of Waste/ byproducts; maximum incorporation of the materials used in the process into the final products (Atom Economy); prevention/ minimization of hazardous/ toxic products; designing safer chemicals – different basic approaches to do so; selection of appropriate auxiliary substances (solvents, separation agents), green solvents, solventless processes, immobilized solvents and ionic liquids; energy requirements for reactions - use of microwaves, ultrasonic energy; selection of starting materials; avoidance of unnecessary derivatization – careful use of blocking/protecting groups; use of catalytic reagents (wherever possible) in preference to stoichiometric reagents; designing of biodegradable products; prevention of chemical accidents; strengthening/ development of

62 | P a g e analytical techniques to prevent and minimize the generation of hazardous substances in chemical processes. (24 Hours) Unit – 3: Examples of Green Synthesis/ Reactions

1. Green Synthesis of the following compounds: adipic acid, catechol, BHT, methyl methacrylate, urethane, aromatic amines (4-aminodiphenylamine), benzyl bromide, acetaldehyde, citral, ibuprofen, paracetamol, furfural. 2. Microwave assisted reactions in water: Hofmann Elimination, Hydrolysis (of benzyl chloride, benzamide, n-phenyl benzamide, methylbenzoate to benzole acid), Oxidation (of toluene, alcohols). 3. Microwave assisted reactions in organic solvents: Esterification, Fries rearrangement, Orthoester Claisen Rearrangement, Diels-Alder Reaction, Decarboxylation. 4. Microwave assisted solid state reactions: Deacetylation, Deprotection. Saponification of esters, Alkylation of reactive methylene compounds, reductions, synthesis of nitriles from aldehydes; anhydrides from dicarboxylic acid; pyrimidine and pyridine derivatives; 1,2- dihydrotriazine derivatives; benzimidazoles. 5. Ultrasound assisted reactions: Esterification, saponification, substitution reactions, Alkylations, oxidation, reduction, coupling reaction, Cannizaro reaction, Strecker synthesis, Reformatsky reaction. (16 Hours) Unit – 4: Future Trends in Green Chemistry

Oxidation reagents and catalysts; Biomimetic, multifunctional reagents; Combinatorial green chemistry; Proliferation of solventless reactions; oncovalent derivatization; Green chemistry in sustainable development. (8 Hours)

Unit – 5: Green Chemistry in the Fine chemicals and Pharmaceutical Industries (8 Hours)

Reference Books:

• V.K. Ahluwalia & M.R. Kidwai: New Trends in Green Chemistry, • Anamalaya Publishers (2005). • P.T. Anastas & J.K. Warner: Oxford Green Chemistry- Theory and Practical, University Press (1998). • A.S. Matlack: Introduction to Green Chemistry, Marcel Dekker (2001). • M.C. Cann & M.E. Connely: Real-World cases in Green Chemistry, American Chemical Society, Washington (2000). • M.A. Ryan & M. Tinnesand, Introduction to Green Chemistry, American Chemical Society, Washington (2002). • Review article from Green Chemistry, Chemical Review.

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DSE – F Lab: Green Chemistry

60 Hours 1. Safer starting materials

The Vitamin C clock reaction using Vitamin C tablets, tincture of iodine, hydrogen peroxide and liquid laundry starch.

a) Effect of concentration on clock reaction b) Effect of temperature on clock reaction. (if possible)

1. Using renewable resources

Preparation of biodiesel from vegetable oil.

3. Avoiding waste

Principle of atom economy.

Use of molecular model kit to stimulate the reaction to investigate how the atom economy can illustrate Green Chemistry.

Preparation of propene by two methods can be studied

- (I) Triethylamine ion + OH → propene + trimethylpropene + water H2SO4/ (II) 1-propanol propene + water

The other types of reactions, like addition, elimination, substitution and rearrangement should also be studied for the calculation of atom economy.

4. Use of enzymes as catalysts

Benzoin condensation using Thiamine Hydrochloride as a catalyst instead of cyanide Alternative Green solvents

5. Diels Alder reaction in water

Reaction between furan and maleic acid in water and at room temperature rather than in benzene and reflux.

6. Environmentally benign extraction of Lycopene from Tomato sauces.

7. Green aqueous Wittig reaction.

8. Microwave assisted Claisen/Dieckman condensation reaction..

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Alternative sources of energy

9. Eosin Y catalyzed visible light Oxidative C-C bond formation reaction.

10. Photo reduction of benzophenone to benzopinacol in the presence of sunlight.

At least five experiments to be carried out.

Reference Books:

• Anastas, P.T & Warner, J.C. Green Chemistry: Theory and Practice, Oxford University Press (1998). • Kirchoff, M. & Ryan, M.A. Greener approaches to undergraduate chemistry experiment. American Chemical Society, Washington DC (2002). • Ryan, M.A. Introduction to Green Chemistry, Tinnesand; (Ed), American Chemical Society, Washington DC (2002). • Sharma, R.K.; Sidhwani, I.T. & Chaudhari, M.K. I.K. Green Chemistry Experiment: A monograph International Publishing House Pvt Ltd. New Delhi. Bangalore CISBN 978- 93-81141-55-7 (2013). • Cann, M.C. & Connelly, M. E. Real world cases in Green Chemistry, American Chemical Society (2008). • Cann, M. C. & Thomas, P. Real world cases in Green Chemistry, American Chemical Society (2008). • Pavia, D. L. Lamponan, G. H. &Kriz, G.S. W B Introduction to organic laboratory • Journal of Chemical Education (ACS Publishers) 2014, 91, 611. • Journal of Chemical Education (ACS Publishers) 2011, 88, 1014. • Journal of Chemical Education (ACS Publishers) 2000, 85, 256.

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DSE – G: Industrial Chemicals and Environment (Credits: Theory-04, Practicals-02) Theory: 60 Hours Unit – 1: Industrial Gases and Inorganic Chemicals

Industrial Gases: Large scale production, uses, storage and hazards in handling of the following gases: oxygen, nitrogen, argon, neon, helium, hydrogen, acetylene, carbon monoxide, chlorine, fluorine, sulphur dioxide and phosgene.

Inorganic Chemicals: Manufacture, application, analysis and hazards in handling the following chemicals: hydrochloric acid, nitric acid, sulphuric acid, caustic soda, common salt, borax, bleaching powder, sodium thiosulphate, hydrogen peroxide, potash alum, chrome alum, potassium dichromate and potassium permanganate. (10 Hours) Unit – 2: Industrial Metallurgy

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Preparation of metals (ferrous and nonferrous) and ultrapure metals for semiconductor technology. (4 Hours) Unit – 3: Environment and its segments

Ecosystems. Biogeochemical cycles of carbon, nitrogen and sulphur. Air Pollution: Major regions of atmosphere. Chemical and photochemical reactions in atmosphere. Air pollutants: types, sources, particle size and chemical nature; Photochemical smog: its constituents and photochemistry. Environmental effects of ozone, Major sources of air pollution.

Pollution by SO2 , CO2, CO, NOx, H2S and other foul smelling gases. Methods of estimation of CO, NOx, SOx and control procedures.

Effects of air pollution on living organisms and vegetation. Greenhouse effect and Global warming, Ozone depletion by oxides of nitrogen, chlorofluorocarbons and Halogens, removal of sulphur from coal. Control of particulates.

Water Pollution: Hydrological cycle, water resources, aquatic ecosystems, Sources and nature of water pollutants, Techniques for measuring water pollution, Impacts of water pollution on hydrological and ecosystems.

Water purification methods. Effluent treatment plants (primary, secondary and tertiary treatment). Industrial effluents from the following industries and their treatment: electroplating, textile, tannery, dairy, petroleum and petrochemicals, agro, fertilizer, etc. Sludge disposal.

Industrial waste management, incineration of waste. Water treatment and purification (reverse osmosis, electro dialysis, ion exchange). Water quality parameters for waste water, industrial water and domestic water. (30 Hours) Unit – 4: Energy & Environment

Sources of energy: Coal, petrol and natural gas. Nuclear Fusion / Fission, Solar energy, Hydrogen, geothermal, Tidal and Hydel, etc.

Nuclear Pollution: Disposal of nuclear waste, nuclear disaster and its management.

(10 Hours) Unit – 5: Biocatalysis

Introduction to biocatalysis: Importance in “Green Chemistry” and Chemical Industry.

(6 Hours) Reference Books:

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• E. Stocchi: Industrial Chemistry, Vol-I, Ellis Horwood Ltd. UK. • R.M. Felder, R.W. Rousseau: Elementary Principles of Chemical Processes, Wiley Publishers, New Delhi. • J. A. Kent: Riegel’s Handbook of Industrial Chemistry, CBS Publishers, New Delhi. • S. S. Dara: A Textbook of Engineering Chemistry, S. Chand & Company Ltd. New Delhi. • K. De, Environmental Chemistry: New Age International Pvt., Ltd, New Delhi. • S. M. Khopkar, Environmental Pollution Analysis: Wiley Eastern Ltd, New Delhi. • S.E. Manahan, Environmental Chemistry, CRC Press (2005). • G.T. Miller, Environmental Science 11th edition. Brooks/ Cole (2006). • A. Mishra, Environmental Studies. Selective and Scientific Books, New Delhi (2005). ------

DSE – G Lab: Industrial Chemicals & Environment (60 Hours)

1. Determination of dissolved oxygen in water. 2. Determination of Chemical Oxygen Demand (COD) 3. Determination of Biological Oxygen Demand (BOD) 4. Percentage of available chlorine in bleaching powder. 5. Measurement of chloride, sulphate and salinity of water samples by simple titration method (AgNO3 and potassium chromate). 2- - 6. Estimation of total alkalinity of water samples (CO3 , HCO3 ) using double titration method. 7. Measurement of dissolved CO2. 8. Study of some of the common bio-indicators of pollution. 9. Estimation of SPM in air samples. 10. Preparation of borax/ boric acid.

Reference Books:

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DSE – H: Inorganic Materials of Industrial Importance (Credits: Theory-04, Practicals-02) Theory: 60 Hours

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Unit – 1: Silicate Industries

Glass: Glassy state and its properties, classification (silicate and non-silicate glasses). Manufacture and processing of glass. Composition and properties of the following types of glasses: Soda lime glass, lead glass, armoured glass, safety glass, borosilicate glass, fluorosilicate, coloured glass, photosensitive glass.

Ceramics: Important clays and feldspar, ceramic, their types and manufacture. High technology ceramics and their applications, superconducting and semiconducting oxides, fullerenes carbon nanotubes and carbon fibre.

Cements: Classification of cement, ingredients and their role, Manufacture of cement and the setting process, quick setting cements.

(16 Hours) Unit – 2: Fertilizer

Different types of fertilizers. Manufacture of the following fertilizers: Urea, ammonium nitrate, calcium ammonium nitrate, ammonium phosphates; polyphosphate, superphosphate, compound and mixed fertilizers, potassium chloride, potassium sulphate.

(8 Hours) Unit – 3: Surface Coatings

Objectives of coatings surfaces, preliminary treatment of surface, classification of surface coatings. Paints and pigments-formulation, composition and related properties. Oil paint, Vehicle, modified oils, Pigments, toners and lakes pigments, Fillers, Thinners, Enamels, emulsifying agents. Special paints (Heat retardant, Fire retardant, Eco-friendly paint, Plastic paint), Dyes, Wax polishing, Water and Oil paints, additives, Metallic coatings (electrolytic and electroless), metal spraying and anodizing.

(10 Hours) Unit – 4: Batteries

Primary and secondary batteries, battery components and their role, Characteristics of Battery. Working of following batteries: Pb acid, Li-Battery, Solid state electrolyte battery. Fuel cells, Solar cell and polymer cell.

(6 Hours) Unit – 5: Alloys

Classification of alloys, ferrous and non-ferrous alloys, Specific properties of elements in alloys. Manufacture of Steel (removal of silicon decarbonization, demanganization, desulphurization dephosphorisation) and surface treatment (argon treatment, heat treatment, nitriding, carburizing). Composition and properties of different types of steels. (10 Hours)

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Unit – 6: Catalysis & Chemical explosives

General principles and properties of catalysts, homogenous catalysis (catalytic steps and examples) and heterogenous catalysis (catalytic steps and examples) and their industrial applications, Deactivation or regeneration of catalysts.

Phase transfer catalysts, application of zeolites as catalysts.

Origin of explosive properties in organic compounds, preparation and explosive properties of lead azide, PETN, cyclonite (RDX). Introduction to rocket propellants. (10 Hours) Reference Books:

• E. Stocchi: Industrial Chemistry, Vol-I, Ellis Horwood Ltd. UK. • R. M. Felder, R. W. Rousseau: Elementary Principles of Chemical Processes, Wiley Publishers, New Delhi. • W. D. Kingery, H. K. Bowen, D. R. Uhlmann: Introduction to Ceramics, Wiley Publishers, New Delhi. • J. A. Kent: Riegel’s Handbook of Industrial Chemistry, CBS Publishers, New Delhi. • P. C. Jain, M. Jain: Engineering Chemistry, Dhanpat Rai & Sons, Delhi. • R. Gopalan, D. Venkappayya, S. Nagarajan: Engineering Chemistry, Vikas Publications, New Delhi. • B. K. Sharma: Engineering Chemistry, Goel Publishing House, Meerut

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DSE – H Lab: Inorganic Materials of Industrial Importance (60 Hours) 1. Determination of free acidity in ammonium sulphate fertilizer. 2. Estimation of Calcium in Calcium ammonium nitrate fertilizer. 3. Estimation of phosphoric acid in superphosphate fertilizer. 4. Electroless metallic coatings on ceramic and plastic material. 5. Determination of composition of dolomite (by complexometric titration). 6. Analysis of (Cu, Ni); (Cu, Zn ) in alloy or synthetic samples. 7. Analysis of Cement. 8. Preparation of pigment (zinc oxide).

Reference Books:

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• J. A. Kent: Riegel’s Handbook of Industrial Chemistry, CBS Publishers, New Delhi. • P. C. Jain, M. Jain: Engineering Chemistry, Dhanpat Rai & Sons, Delhi. • R. Gopalan, D. Venkappayya, S. Nagarajan: Engineering Chemistry, Vikas Publications, New Delhi. • B. K. Sharma: Engineering Chemistry, Goel Publishing House, Meerut

DSE – I: Instrumental Methods of Chemical Analysis (Credits: Theory-04, Practicals-02) Theory: 60 Hours Unit – 1: Introduction to spectroscopic methods of analysis

Recap of the spectroscopic methods covered in detail in the core chemistry syllabus: Treatment of analytical data, including error analysis. Classification of analytical methods and the types of instrumental methods. Consideration of electromagnetic radiation. (4 Hours) Unit – 2: Molecular spectroscopy

Infrared spectroscopy: Interactions with molecules: absorption and scattering. Means of excitation (light sources), separation of spectrum (wavelength dispersion, time resolution), detection of the signal (heat, differential detection), interpretation of spectrum (qualitative, mixtures, resolution), advantages of Fourier Transform (FTIR). Samples and results expected. Applications: Issues of quality assurance and quality control, Special problems for portable instrumentation and rapid detection.

UV-Visible/ Near IR – emission, absorption, fluorescence and photoaccoustic. Excitation sources (lasers, time resolution), wavelength dispersion (gratings, prisms, interference filters, laser, placement of sample relative to dispersion, resolution), Detection of signal (photocells, photomultipliers, diode arrays, sensitivity and S/N), Single and Double Beam instruments, Interpretation (quantification, mixtures, absorption vs. fluorescence and the use of time, photoaccoustic, fluorescent tags). (16 Hours) Unit – 3: Separation techniques

Chromatography: Gas chromatography, liquid chromatography, supercritical fluids, Importance of column technology (packing, capillaries), Separation based on increasing number of factors (volatility, solubility, interactions with stationary phase, size, electrical field), Detection: simple vs. specific (gas and liquid), Detection as a means of further analysis (use of tags and coupling to IR and MS), Electrophoresis (plates and capillary) and use with DNA analysis.

Immunoassays and DNA techniques

Mass spectroscopy: Making the gaseous molecule into an ion (electron impact, chemical ionization), Making liquids and solids into ions (electrospray, electrical discharge, laser desorption, fast atom bombardment), Separation of ions on basis of mass to charge ratio,

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Magnetic, Time of flight, Electric quadrupole. Resolution, time and multiple separations, Detection and interpretation (how this is linked to excitation). (16 Hours) Unit – 4: Elemental analysis

Mass spectrometry (electrical discharges).

Atomic spectroscopy: Atomic absorption, Atomic emission, and Atomic fluorescence. Excitation and getting sample into gas phase (flames, electrical discharges, plasmas), Wavelength separation and resolution (dependence on technique), Detection of radiation (simultaneous/scanning, signal noise), Interpretation (errors due to molecular and ionic species, matrix effects, other interferences). (8 Hours) Unit – 5:

NMR spectroscopy: Principle, Instrumentation, Factors affecting chemical shift, Spin- coupling, Applications. Electroanalytical Methods: Potentiometry & Voltammetry

Radiochemical Methods

X-ray analysis and electron spectroscopy (surface analysis) (16 Hours)

Reference books:

• Principles of Instrumental Analysis - 6th Edition by Douglas A. Skoog, F. James Holler, and Stanley Crouch (ISBN 0-495-01201-7). • Instrumental Methods of Analysis, 7th ed, Willard, Merritt, Dean, Settle. • P.W. Atkins: Physical Chemistry. • G.W. Castellan: Physical Chemistry. • C.N. Banwell: Fundamentals of Molecular Spectroscopy. • Brian Smith: Infrared Spectral Interpretations: A Systematic Approach. • W.J. Moore: Physical Chemistry.

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DSE – I Lab: Instrumental Methods of Chemical Analysis (60 Hours) 1. Safety Practices in the Chemistry Laboratory 2. Determination of the isoelectric pH of a protein. 3. Titration curve of an amino acid. 4. Determination of the void volume of a gel filtration column. 5. Determination of a Mixture of Cobalt and Nickel (UV/Vis spec.) 6. Study of Electronic Transitions in Organic Molecules (i.e., acetone in water)

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7. IR Absorption Spectra (Study of Aldehydes and Ketones) 8. Determination of Calcium, Iron, and Copper in Food by Atomic Absorption 9. Quantitative Analysis of Mixtures by Gas Chromatography (i.e., chloroform and carbon tetrachloride) 10. Separation of Carbohydrates by HPLC 11. Determination of Caffeine in Beverages by HPLC Potentiometric Titration of a Chloride- Iodide Mixture 12. Cyclic Voltammetry of the Ferrocyanide/Ferricyanide Couple 13. Nuclear Magnetic Resonance 14. Use of fluorescence to do “presumptive tests” to identify blood or other body fluids. 15. Use of “presumptive tests” for anthrax or cocaine 16. Collection, preservation, and control of blood evidence being used for DNA testing 17. Use of capillary electrophoresis with laser fluorescence detection for nuclear DNA (Y chromosome only or multiple chromosome) 18. Use of sequencing for the analysis of mitochondrial DNA 19. Laboratory analysis to confirm anthrax or cocaine 20. Detection in the field and confirmation in the laboratory of flammable accelerants or explosives 21. Detection of illegal drugs or steroids in athletes 22. Detection of pollutants or illegal dumping 23. Fibre analysis

At least 10 experiments to be performed.

Reference Books:

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DSE – J: Basic of Nanomaterials (Credits: Theory-04, Practicals-•02) Theory: 60 Hours Unit – 1: Introduction and Classification

What is nanotechnology?; Why nano? Classification of nanostructures, nanoscale architecture; summary of the electronic properties of atoms and solids; the isolated atom, bonding between atoms, giant molecular solids, the free electron model and energy bands of crystalline solids, periodicity of crystal lattices; electronic conduction; effects of the nanometre length scale, changes to the system total energy, changes to the system structure; how nanoscale dimensions affect properties. (electronic conduction, system classification confined to one, two or three dimension and their effect on properties). (15 Lectures)

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Unit – 2: Properties of Nanomaterials

Introductory discussion of size and shape dependable properties of nanomaterials like melting point, magnetism, optical, conductivity (conductor and semi-conductivity), catalytic and electrochemical aspect. (10 Lectures) Unit – 3: Synthesis of Nanomaterials Common methods of top down and bottom approaches of the preparation of nanomaterials. Special interest on the synthesis of metal nanoparticles, metal oxides, and carbon nanotube (CNT) etc. A brief discussion of biological synthesis of nanomaterials. (10 Lectures) Unit – 4: Characterization of Nanomaterials A brief historical overview of common instrumental techniques used for characterization of nanomaterials such as, X-ray diffraction, electron microscopy (SEM, TEM, including EDX technique), XPS with respect to working principle, instrumentation and applications. Differential scanning calorimeter (DSC), Thermogravimetric / Diffferential (TG/DTA), UV-Visible Spectrophotometer, and FTIR –Principle and Applications. (15 Lectures) Unit – 5: Applications of Nanomaterials

Use of nanomaterials in daily life with examples (solar cell, GMR read heads, NEMS goniometers, health care, energy materials, etc). Societal aspects of nanotechnology: health, environment, hype and reality. (10 Lectures)

Reference Books:

 Hornyak, G. L.; Moore, J. J.; Tibbals, H. F. and Dutta, J. Fundamentals of Nanotechnology, CRC Press, 2009.  Pradeep, T. A Textbook of Nanoscience and Nanotechnology, McGraw Hill Edu. New Delhi, (2015).  Cao, G. Nanostructures and Nanomaterials Synthesis, Properties and Appli-cations, Imperial College Press, London, 2004.  Klabunde, K. J. Nanoscale materials in Chemistry, Wiley-Interscience, (2001).  Knauth, P. and Schoonman, J. Nanostructured Materials: Selected Synthesis Methods, Properties and Applications, Kluwer Academic Publishers, New York, (2002).  Cullity, B. D., Elements of X-ray Diffraction, Eds: 2nd, Addison-Wesley, USA, 1959.  Williams, D. B. and Carter C. B., Transmission Electron Microscopy: A Textbook for Materials Science, Plenum Press, New York, 1996.  Brugel W., in Introduction to Infrared Spectroscopy, John Wiley and Sons, New York, 1962.  S. Hüfner, in Photoelectron Spectroscopy: Principles and Applications, Springer-Verlog, Germany, 1995.

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DSE – J Lab: Basic of Nanomaterials (60 Hours)  Verification of the Beer-Lambert law using gold/silver nanoparticles.  Determination of the band gap of semiconductor nanomaterials.  Nanochemistry of silver nanoparticles in converting p-nitrophenol to p-aminophenol.  Study of surface enhanced Raman scattering activity of silver nanostructures.  Removal of Mercury by supported nanoparticles.  Synthesis and characterization of core-shell nanocomposite (bimetallic and oxides)  Preparation and characterization of nanomaretials by wet chemical routes (sol-gel, reverse micelles, hydrothermal, co-precipitation, etc.)

Reference Books:

 Pradeep, T. A Textbook of Nanoscience and Nanotechnology, McGraw Hill Edu. New Delhi, (2015).

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DSE – K : Advanced Organic Chemistry (Credits: Theory-04, Practicals-•02) Theory: 60 Hours Unit – 1: Nomenclature

Basic nomenclature of bicyclic compounds: Spirocyclic, Polycyclic compounds and heterocyclic compounds. (3 Hours) Unit – 2: Stereochemistry

Definition of Stereochemistry, Properties of stereoisomers, Tartaric acid and it’s various isomers, Enantiomeric purity, How do we measure enantiomeric purity, Definition of d.r.; e.r.; ee. Topism, Diastereotopic, Enantiotopic. Prochirality, Making compounds Chiral, Prochiral at sp2 carbon. (10 Hours) Unit – 3: Reaction Mechanism

SN2, SN1 Rate equation, Eyring equation, Linear free Energy relationship. Determining the mechanism of a reaction: Detection and trapping of intermediates, Cross-over experiments, kinetic isotopic effect-primary kinetic and secondary kinetic isotopic effect. (7 Hours) Unit – 4: Introduction of Pericyclic Reaction and Free radical Chemistry

Definition of Pericyclic reaction. classification of Pericyclic reactions. Cycloaddition reaction (Diels-Alder reaction and it’s application to the natural products), Sigmatropic rearrangements. Free radical initiation, Barton Reaction, Hoffmann-Loffler-Freytag reaction, Deoxygenation reaction, dehalogenation reaction.

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(10 Hours) Unit – 5: Functional Group Interconversions

Functional Groups, Oxidation state, Markonikov-Antimarkonikov addition, Hydration, Acetal/ketal or thioketal formation, Selective reduction, Oxidation of alcohols (Swern oxidation, DMP-oxidation), Stereoselective oxidation and reduction. (10 Hours) Unit – 6: Stereoselective C-C bond formation reaction

Carbon nucleophile and electrophile, LDA to make enolate, Carbonyl compound reactions, Enolate and pka, The aldol reaction. Claisen and Dieckmen condensastion reaction, Michael addition and Robinson annulations reaction. Acid Promoted reaction (Prins reaction, F-C alkylation and acylation reaction). Benzoin and acylanion equivalent. Retrosynthetic analysis for DA and Robinson annulations reaction. (10 Hours) Unit – 7: NMR Spectroscopy

Chemical shift, Spin-spin coupling, determining stereochemistry and regiochemistry by 1H-NMR spectroscopy, 13C-NMR: 2D NMR COSY, HMBC, HMQC. (10 Hours) References:

 Advanced Organic Chemistry –by J. March 6th Edition  Advance Organic Chemistry (part A) –by A. Carey and R.J. Sundberg  Stereochemistry of carbon compound-by E.L. Eliel  Stereochemistry of organic compound-by Nasipuri  J. Singh & J.Singh, Photochemistry and Pericyclic Reactions,  W. Carruthers, Some Modern Methods of Organic Synthesis, Cambridge University, Press, 1993.  Bessler and Silverstein, Spectroscopy of Organic Compounds, JOHN WILEY, 2001.  D. C. Pavia, G. M. Lampman, G. S. Kriz, Introduction to Spectroscopy, 3rd Edition, 2007.  Organic Spectroscopy III Edition–by William Kemp

------DSE – K Lab: Advanced Organic Chemistry (60 Hours) 1. Hands on experiences:

a) To determine the enantiomeric purity (ee/er) by HPLC chromatogram. b) To determine the diastereoisomers ratio from NMR Spectra. c) Analyze the 1H-NMR Spectra of any organic molecules. d) Analyze the 2D-13C-NMR spectra of any organic molecules.

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2. Synthesis of an Imidazolidinone Oraganocatalyst and its application in a DA Reaction: Multistep Synthesis.

a) Catalyst synthesis b) Diels-Alder reaction. c) Purification step d) Spectral data analysis (1H-NMR and 13C-NMR)

3. Robinson annulations

a) Two step synthesis of Wieland-Miescher ketone from 1,3-diketone and enones. b) Asymmetric synthesis by chiral proline catalyst c) HPLC Chromatogram and spectral data interpretation.

4. Rearrangement of trans-stilbene Oxide with Bi(OTf)3 and other metal triflates.

5. Oxidation and Reduction

a) Oxidation of secondary alcohol to ketone b) Oxidation of primary alcohol to aldehyde c) Reduction of aldehyde/ketone by NaBH4 d) Reduction of Ester by using LialH4

References:

 Bessler and Silverstein, Spectroscopy of Organic Compounds, JOHN WILEY, 2001.  J. Chem. Edu. DOI: 10.1021/acs.jchemed.5b00812  J. Chem. Edu. 2008, 85, 1531.  J. Chem. Edu. 2011, 88, 1014.  J. Chem. Edu. 2008, 85, 1274.  Practical Organic Chemistry by A. I. Vogel.  Practical Organic Chemistry by F. G. Mann and B. C. Saunders.

------DSE• – L : Research Methodology for Chemistry (Credits: Theory-05, Tutorials-01) Theory: 75 Hours Unit – 1: Literature Survey

Print: Sources of information: Primary, secondary, tertiary sources; Journals: Journal abbreviations, abstracts, current titles, reviews, monographs, dictionaries, text-books, current contents, Introduction to Chemical Abstracts and Beilstein, Subject Index, Substance Index, Author Index, Formula Index, and other Indices with examples.

Digital: Web resources, E-journals, Journal access, TOC alerts, Hot articles, Citation index, Impact factor, H-index, E-consortium, UGC infonet, E-books, Internet discussion groups

76 | P a g e andcommunities, Blogs, Preprint servers, Search engines, Scirus, Google Scholar, ChemIndustry, Wiki- Databases, ChemSpider, Science Direct, SciFinder, Scopus.

Information Technology and Library Resources: The Internet and World Wide Web. Internet resources for chemistry. Finding and citing published information. (20 Hours) Unit – 2: Methods of Scientific Research and Writing Scientific Papers

Reporting practical and project work. Writing literature surveys and reviews. Organizing a poster display. Giving an oral presentation.

Writing scientific papers – justification for scientific contributions, bibliography, description of methods, conclusions, the need for illustration, style, publications of scientific work. Writing ethics. Avoiding plagiarism. (20 Hours) Unit – 3: Chemical Safety and Ethical Handling of Chemicals

Safe working procedure and protective environment, protective apparel, emergency procedure and first aid, laboratory ventilation. Safe storage and use of hazardous chemicals, procedure for working with substances that pose hazards, flammable or explosive hazards, procedures for working with gases at pressures above or below atmospheric – safe storage and disposal of waste chemicals, recovery, recycling and reuse of laboratory chemicals, procedure for laboratory disposal of explosives, identification, verification and segregation of laboratory waste, disposal of chemicals in the sanitary sewer system, incineration and transportation of hazardous chemicals. (12 Hours) Unit – 4: Data Analysis

The Investigative Approach: Making and Recording Measurements. SI Units and their use.Scientific method and design of experiments.

Analysis and Presentation of Data: Descriptive statistics. Choosing and using statistical tests. Chemometrics. Analysis of variance (ANOVA), Correlation and regression, Curve fitting, fitting of linear equations, simple linear cases, weighted linear case, analysis of residuals, General polynomial fitting, linearizing transformations, exponential function fit, r and its abuse. Basic aspects of multiple linear regression analysis. (13 Hours) Unit – 5: Electronics Basic fundamentals of electronic circuits and their components used in circuits of common instruments like spectrophotometers, typical circuits involving operational amplifiers for electrochemical instruments. Elementary aspects of digital electronics. (10 Hours) Reference Books

• Dean, J. R., Jones, A. M., Holmes, D., Reed, R., Weyers, J. & Jones, A. (2011) 77 | P a g e

Practical skills in chemistry. 2nd Ed. Prentice-Hall, Harlow. • Hibbert, D. B. & Gooding, J. J. (2006) Data analysis for chemistry. Oxford University Press. • Topping, J. (1984) Errors of observation and their treatment. Fourth Ed., Chapman Hall, London. • Harris, D. C. Quantitative chemical analysis. 6th Ed., Freeman (2007) Chapters 3-5. • Levie, R. de, How to use Excel in analytical chemistry and in general scientific data analysis. Cambridge Univ. Press (2001) 487 pages. • Chemical safety matters – IUPAC – IPCS, Cambridge University Press, 1992.

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DSE• – L Tutorial: Research Methodology for Chemistry (Credits: Tutorials-01) 1. Seminar 2. Short Project 3. Literature review

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DSE• – M : Crystalline Material and Properties (Credits: Theory-05, Tutorials-01) Theory: 75 Hours Unit – 1: Introduction Crystalline and non-crystalline solids; space lattice and primitive and non-primitive lattice, crystal structure, unit cell, symmetry in crystal, seven crystal system, Bravais lattice, a qualitative ideas of point and space group; crystal planes and Miller indices, reciprocal lattice. Cubic lattice: lattice point in cubic crystals, coordination number, Packing density, separation between crystal planes (10 Hours) Unit – 2: Bonding and Crystal Structure of Crystalline Materials Closed packed structure- hcp and ccp, packing efficiency, voids, limiting radius ratio; description of solid structure of rack salt (NaCl), Wurzite and zinc blend of ZnS, Fluoride (CaF2) and antifluoride (Na2O), Rutile (TiO2). Bonding between atoms in solid: ionic bonds, covalent bonds, metallic bonds, van der Waals bonds; cohesive energy of an ionic crystal, Madelung constant and lattice energy. (10 Hours) Unit – 3: Determination of Crystal Structure X-ray diffraction by crystal, Bragg’s law, a simple description of rotating crystal method and powder pattern methods. Analysis of powder pattern of simple cubic systems. A brief overview of determination of crystal structure by electron microscope (TEM, SAED, and HRTEM) (15 Hours) Unit – 4: Thermal and Electrical Properties of Solids

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Thermal Properties: Specific heat of solids, classical theory – Dulong-Petit’s law, Einstein- Debye theory, vibrational modes of one dimensional lattice – dispersion relation and Brillouin zones. Electronic Properties: Free electron theory of metals; solution of one dimensional Schrödinger equation in constant potential; density of state; Fermi energy; Energy band in a solid, explanations of Kronig-Penney model (without derivation), refinement of simple band formation in solid, k-space and Brillouin Zones, band structure of metals, insulators and semiconductors, intrinsic and extrinsic semiconductors, doped semiconductors, p-n junctions. Hall effect- definition, Hall potential Hall coefficient. Superconductivity- qualitative discussion, critical temperature, Meissner effect, and Josephson Tunnelling. (15 Hours) Unit – 5: Magnetic Properties of Solids concept of dia- para- and ferro- magnetism; magnetic moment due to orbital and spin motion of electron, effect of temperature, Langevin’s theory of dia- and paramagnetism; Curie-Weiss law, qualitative description of ferro-magnetism (magnetic domains), B-H curve, hysteresis loop, retentivity, coercivity, hysteresis loss, soft and hard magnets. (10Hours) Reference Books

 A. R. West: Solid State Chemistry and Its Applications, John Wiley & Sons, 1989.  L. Smart and E. Moore: Solid State Chemistry, Chapman and Hall, 1992.  L. V. Azaroff Introduction to Solid, Tata Mcgraw Hill  Cullity, B. D., Elements of X-ray Diffraction, Eds: 2nd, Addison-Wesley, USA, 1959.  Williams, D. B. and Carter C. B., Transmission Electron Microscopy: A Textbook for Materials Science, Plenum Press, New York, 1996.

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DSE – M Tutorial: Crystalline Material and Properties (Credits: Tutorials-01)  Indexing of powder XRD pattern and calculation of lattice parameter for crystals.  Analyzing of TEM images and Indexing of SAED pattern and HRTEM images.

Reference Books

 Cullity, B. D., Elements of X-ray Diffraction, Eds: 2nd, Addison-Wesley, USA, 1959.  Williams, D. B. and Carter C. B., Transmission Electron Microscopy: A Textbook for Materials Science, Plenum Press, New York, 1996.

------DSE – N: Basic Mathematical Concept for Chemist Credits: Theory-05, Tutorial-01) (75 Hours) Unit – 1: Logatithmic Relations, Numbers, and Vectors

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Logarithmic Relations. Numbers; Real and Complex number. Vectors: Vectors, dot, cross and triple product etc. The gradient, divergence and curl. Vector calculus, Gauss’ theorem, divergence theorem etc. (15 Hours) Unit – 2: Matrix Algebra Addition and multiplication; inverse, adjoint and transpose of matrices, special matrices (symmetric, screw-symmetric, Hermitian, screw-Hermitian, unit, diagonal, unitary etc.) and their properties. Matrix equations; homogeneous, non-homogeneous linear equation and conditions for the solution, linear dependence and independence. Introduction of vector spaces, matrix eigenvalues and eigenvectors, digonalization, determinants. (15 Hours) Unit – 3: Differential and Calculus

Differential: Functions, continuity and differentiability, rules for differentiation, application of differential calculus including maxima and minima, exact and inexact differentials, their application to related to chemistry syllabus.

Partial Differential: Function of several variables, partial differentiation, co-ordinate transformation (e.g. Cartesian to spherical polar). Integral calculus: Basic rules for integration, integration by parts, partial fraction and substitution, reduction formulae, applications of integral calculus. (15 Hours) Unit – 4: Elementary Differential Equations Ordinary first- and second-order differential equations. Partial differential equations. Solution of inexact differential equations by the method of integrating factors. Power series and extended power series solutions. (15 Hours) Unit – 5: Probability and Curve Sketching Permutation & Combination. Factorial and probability. Curve sketching linear graphs and calculation of slopes, and curve fitting. (15 Hours) Reference Books:

 The Chemistry Maths Book, Oxford University Press, New Delhi (2011)  R. G. Mortimer: Mathematics for Physical Chemistry, Academic Press  F. Diniels: Mathematical Preparation for Physical chemistry, McGraw Hill.

------DSE – N Tutorial: Basic Mathematical Concept for Chemistry (Credits: Tutorials-01)  Solving neumerical problems related to chemistry syllabus especially related to quantum mechanics, thermodynamics, kinetics etc. .

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**Skill Enhancement Course (SEC) in Chemistry Skill Enhancement Course (any two) (Credit: 04 each)- SEC1 to SEC2

CHM T 214 and CHM T 224

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SEC – A: IT Skill for Chemists (Credits: 04) Theory: 60 Hours Unit – 1: Mathematics

Fundamentals, mathematical functions, polynomial expressions, logarithms, the exponential function, units of a measurement, interconversion of units, constants and variables, equation of a straight line, plotting graphs.

Uncertainty in experimental techniques: Displaying uncertainties, measurements in chemistry, decimal places, significant figures, combining quantities.

Uncertainty in measurement: types of uncertainties, combining uncertainties. Statistical treatment. Mean, standard deviation, relative error. Data reduction and the propagation of errors. Graphical and numerical data reduction. Numerical curve fitting: the method of least squares (regression).

Algebraic operations on real scalar variables (e.g. manipulation of van der Waals equation in different forms).Roots of quadratic equations analytically and iteratively (e.g. pH of a weak acid). Numerical methods of finding roots (Newton-Raphson, binary –bisection, e.g. pH of a weak acid not ignoring the ionization of water, volume of a van der Waals gas, equilibrium constant expressions).

Differential calculus: The tangent line and the derivative of a function, numerical differentiation (e.g., change in pressure for small change in volume of a van der Waals gas, potentiometric titrations).

Numerical integration (Trapezoidal and Simpson’s rule, e.g. entropy/enthalpy change from heat capacity data). (10 Hours) Unit – 2: Computer programming

Constants, variables, bits, bytes, binary and ASCII formats, arithmetic expressions, hierarchy of operations, inbuilt functions. Elements of the BASIC language. BASIC keywords and commands. Logical and relative operators. Strings and graphics. Compiled versus interpreted languages. Debugging. Simple programs using these concepts. Matrix addition and multiplication. Statistical analysis.

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BASIC programs for curve fitting, numerical differentiation and integration (Trapezoidal rule, Simpson’s rule), finding roots (quadratic formula, iterative, Newton-Raphson method).

(10 Hours) HANDS ON Unit – 3: Introductory writing activities

Introduction to word processor and structure drawing (ChemSketch) software. Incorporating chemical structures, chemical equations, expressions from chemistry (e.g. Maxwell-Boltzmann distribution law, Bragg’s law, van der Waals equation, etc.) into word processing documents.

(10 Hours) Unit – 4: Handling numeric data

Spreadsheet software (Excel), creating a spreadsheet, entering and formatting information, basic functions and formulae, creating charts, tables and graphs. Incorporating tables and graphs into word processing documents. Simple calculations, plotting graphs using a spreadsheet (Planck’s distribution law, radial distribution curves for hydrogenic orbitals, gas kinetic theory- Maxwell- Boltzmann distribution curves as function of temperature and molecular weight), spectral data, pressure-volume curves of van der Waals gas (van der Waals isotherms), data from phase equilibria studies. Graphical solution of equations.

(10 Hours)

Unit – 5: Numeric modeling

Simulation of pH metric titration curves. Excel functions LINEST and Least Squares. Numerical curve fitting, linear regression (rate constants from concentration-time data, molar extinction coefficients from absorbance data), numerical differentiation (e.g. handling data from potentiometric and pH metric titrations, pKa of weak acid), integration (e.g. entropy/enthalpy change from heat capacity data). (10 Hours)

Unit – 6: Statistical analysis

Gaussian distribution and Errors in measurements and their effect on data sets. Descriptive statistics using Excel. Statistical significance testing: The t test. The F test.

Presentation: Presentation graphics (10 Hours)

Reference Books: • McQuarrie, D. A. Mathematics for Physical Chemistry University Science Books (2008). rd • Mortimer, R. Mathematics for Physical Chemistry. 3 Ed. Elsevier (2005). • Steiner, E. The Chemical Maths Book Oxford University Press (1996). nd • Yates, P. Chemical calculations. 2 Ed. CRC Press (2007). • Harris, D. C. Quantitative Chemical Analysis. 6th Ed., Freeman (2007) Chapters 3-5. • Levie, R. de, How to use Excel in analytical chemistry and in general scientific data

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analysis, Cambridge Univ. Press (2001) 487 pages. • Noggle, J. H. Physical chemistry on a Microcomputer. Little Brown & Co. (1985). • Venit, S.M. Programming in BASIC: Problem solving with structure and style. Jaico Publishing House: Delhi (1996).

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SEC – B: Basic Analytical Chemistry (Credits: 04) Theory: 60 Hours Unit – 1: Introduction

Introduction to Analytical Chemistry and its interdisciplinary nature. Concept of sampling. Importance of accuracy, precision and sources of error in analytical measurements. Presentation of experimental data and results, from the point of view of significant figures.

(10 Hours) Unit – 2: Volumetric Titration Standard solution, primary standard and secondary standard, titration, end point, indicator, concentration of standard solution- moles, Normality, molarity, Molality, parts per million(PPM), volumetric calculation, acid base titration and use of indicators,titration curves for strong acid vs strong base, weak acid with strong base, weak base with strong acid, theory of acid base indicator, Redox titration- titration of Mohr salt against KMnO4, Titration of Oxalic acid against KMnO4, Titration of FeSO4 against K2Cr2O7, Iodometric and iodimetric titration, Internal and external indicator, complexometric titration- EDTA titration, Eriochrome black T indicator, complexometric titration curve, direct and back titration, masking and demasking of cations, precaution in volumetric titration. (15 Hours) Unit – 3: Qualitative Analysis of Inorganic Radicals

Introduction to salt analysis, dry and wet test for acid and basic radicals, Principle and chemistry of qualitative analysis of inorganic salt; chemistry involved in qualitative analysis of mixture containing interfering radicals and insolubles. (10 Hours) Unit – 3: Chromatography

Definition, general introduction on principles of chromatography, paper chromatography, TLC etc. a) Paper chromatographic separation of mixture of metal ion (Fe3+ and Al3+). b) To compare paint samples by TLC method.

Solvent Extraction: Distribution Coefficient, distribution ratio, percent extracted, solvent extraction of metals ions, extraction of ion association complex, extraction of metal chelates, multiple batch extraction and applications.

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Ion-exchange: Column, ion-exchange chromatography etc. Determination of ion exchange capacity of anion / cation exchange resin (using batch procedure if use of column is not feasible). (10 Hours) Unit – 4: Suggested Applications (Any one):

a) To study the use of phenolphthalein in trap cases. b) To analyze arson accelerants. c) To carry out analysis of gasoline. (5 Hours)

Unit – 5: Suggested Instrumental demonstrations:

a) Estimation of macro nutrients: Potassium, Calcium, Magnesium in soil samples by flame photometry. b) Spectrophotometric determination of Iron in Vitamin / Dietary Tablets. c) Spectrophotometric Identification and Determination of Caffeine and Benzoic Acid in Soft Drink.

(10 Hours) Reference Books:

1. Willard, H. H. Instrumental Methods of Analysis, CBS Publishers. 2. Skoog & Lerry. Instrumental Methods of Analysis, Saunders College Publications, New York. 3. Skoog, D.A.; West, D.M. & Holler, F.J. Fundamentals of Analytical Chemistry 6th Ed., Saunders College Publishing, Fort Worth (1992). 4. Harris, D. C. Quantitative Chemical Analysis, W. H. Freeman. 5. Dean, J. A. Analytical Chemistry Notebook, McGraw Hill. 6. Day, R. A. & Underwood, A. L. Quantitative Analysis, Prentice Hall of India. 7. Freifelder, D. Physical Biochemistry 2nd Ed., W.H. Freeman and Co., N.Y. USA (1982). 8. Cooper, T.G. The Tools of Biochemistry, John Wiley and Sons, N.Y. USA. 16 (1977). 9. Vogel, A. I. Vogel’s Qualitative Inorganic Analysis 7th Ed., Prentice Hall. 10. Vogel, A. I. Vogel’s Quantitative Chemical Analysis 6th Ed., Prentice Hall. 11. Robinson, J.W. Undergraduate Instrumental Analysis 5th Ed., Marcel Dekker, Inc., New York (1995). ------

SEC – C: Chemical Technology & Environmental Aspects for Society (Credits: 04) Theory: 60 Hours Unit – 1: Chemical Technology

Basic principles of distillation, solvent extraction, solid-liquid leaching and liquid-liquid extraction, separation by absorption and adsorption. An introduction into the scope of

84 | P a g e different types of equipment needed in chemical technology, including reactors, distillation columns, extruders, pumps, mills, emulgators. Scaling up operations in chemical industry. Introduction to clean technology.

(20 Hours) Unit – 2: Society

Exploration of societal and technological issues from a chemical perspective. Chemical and scientific literacy as a means to better understand topics like air and water (and the trace materials found in them that are referred to as pollutants); energy from natural sources (i.e. solar and renewable forms), from fossil fuels and from nuclear fission; materials like plastics and polymers and their natural analogues, proteins and nucleic acids, and molecular reactivity and interconversions from simple examples like combustion to complex instances like genetic engineering and the manufacture of drugs.

(20 Hours) Unit – 3: Uses of Hazard Chemical in Laboratory

Sodium metal, Sodium Azide, Grignard reagent, Concentrated H2SO4, HNO3 & HCl, Arsenic oxide,

(10 Hours) Unit – 4: Effect of Disposal Materials from Industry

Waste water, Skin effect, Fertilizer activity of Soil, Impact of polythine in river or Ocean etc.

(10 Hours)

Reference Book:

 John W. Hill, Terry W. McCreary & Doris K. Kolb, Chemistry for changing times 13th Ed.  A. K. Dey, Environmental Chemistry

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SEC – D: Cheminformatics (Credits: 04) Theory: 60 Hours Unit – 1: Introduction to Chemoinformatics

History and evolution of chemoinformatics, Use of chemoinformatics, Prospects of chemoinformatics, Molecular Modelling and Structure elucidation.

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(10 Hours)

Unit – 2: Representation of molecules and chemical reactions

Nomenclature, Different types of notations, SMILES coding, Matrix representations, Structure of Molfiles and Sdfiles, Libraries and toolkits, Different electronic effects, Reaction classification.

(10 Hours) Unit – 3: Searching chemical structures

Full structure search, sub-structure search, basic ideas, similarity search, three dimensional search methods, basics of computation of physical and chemical data and structure descriptors, data visualization. (10 Hours) Unit – 4: Applications

Prediction of Properties of Compounds; Linear Free Energy Relations; Quantitative Structure- Property Relations; Descriptor Analysis; Model Building; Modeling Toxicity; Structure-Spectra correlations; Prediction of NMR, IR and Mass spectra; Computer Assisted Structure elucidations; Computer Assisted Synthesis Design, Introduction to drug design; Target Identification and Validation; Lead Finding and Optimization; Analysis of HTS data; Virtual Screening; Design of Combinatorial Libraries; Ligand-Based and Structure Based Drug design; Application of Chemoinformatics in Drug Design. (20 Hours)

Unit – 5: Hands-on Exercises (10 Hours)

Reference Books: • Andrew R. Leach & Valerie, J. Gillet (2007) An introduction to Chemoinformatics. Springer: The Netherlands. • Gasteiger, J. & Engel, T. (2003) Chemoinformatics: A text-book. Wiley-VCH. • Gupta, S. P. (2011) QSAR & Molecular Modeling. Anamaya Pub.: New Delhi.

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SEC – E: Green Methods in Chemistry (Credits: 04) Theory: 60 Hours

Unit – 1: Short Introduction to Green Chemistry

What is Green Chemistry? Need for Green Chemistry. Goals of Green Chemistry. Limitations/ Obstacles in the pursuit of the goals of Green Chemistry.

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(10 Hours)

Unit – 2: Principles

Tools of Green chemistry, Twelve principles of Green Chemistry, with examples. (10 Hours)

Unit – 3: Prevention of Byproducts

The following Real world Cases in Green Chemistry should be discussed:

1 A green synthesis of ibuprofen which creates less waste and fewer byproducts (Atom economy). 2 Surfactants for Carbon Dioxide – replacing smog producing and ozone depleting solvents with CO2 for precision cleaning and dry cleaning of garments. 3 Environmentally safe antifoulant. 4 CO2 as an environmentally friendly blowing agent for the polystyrene foam sheet packaging market. 5 Using a catalyst to improve the delignifying (bleaching) activity of hydrogen peroxide. 6 A new generation of environmentally advanced preservative: getting the chromium and arsenic out of pressure treated wood. 7 Rightfit pigment: synthetic azopigments to replace toxic organic and inorganic pigments. 8 Development of a fully recyclable carpet: cradle to cradle carpeting.

(40 Hours)

Reference Books:

1. Manahan S.E. (2005) Environmental Chemistry, CRC Press 2. Miller, G.T. (2006) Environmental Science 11th edition. Brooks/Cole 3. Mishra, A. (2005) Environmental Studies. Selective and Scientific Books, New

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SEC – F: Cosmetics, Perfumes & Pharmaceutical Chemistry (Credits: 04) Theory: 60 Hours

Unit – 1: Introduction of Cosmetics & perfumes chemistry

History of Cosmetics & perfumes chemistry, a general study including preparation and uses of the following: Hair dye, hair spray, shampoo, suntan lotions, face powder, lipsticks, talcum powder, nail enamel, creams (cold, vanishing and shaving creams), antiperspirants and artificial flavours. Essential oils and their importance in cosmetic industries with reference to Eugenol,

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Geraniol, sandalwood oil, eucalyptus, rose oil, 2-phenyl ethyl alcohol, Jasmone, Civetone, Muscone. (20 Hours)

Unit – 2: Synthesis procedure

1. Preparation of talcum powder. 2. Preparation of shampoo. 3. Preparation of enamels. 4. Preparation of hair remover. 5. Preparation of face cream. 6. Preparation of nail polish and nail polish remover.

(10 Hours)

Unit – 3: Drugs & Pharmaceuticals

Drug discovery, design and development; Basic Retrosynthetic approach. Synthesis of the representative drugs of the following classes: analgesics agents, antipyretic agents, anti- inflammatory agents (Aspirin, paracetamol, lbuprofen); antibiotics (Chloramphenicol); antibacterial and antifungal agents (Sulphonamides; Sulphanethoxazol, Sulphacetamide, Trimethoprim); antiviral agents (Acyclovir), Central Nervous System agents (Phenobarbital, Diazepam),Cardiovascular (Glyceryl trinitrate), antilaprosy (Dapsone), HIV-AIDS related drugs (AZT- Zidovudine).

(20 Hours) Unit – 4: Fermentation

Aerobic and anaerobic fermentation. Production of (i) Ethyl alcohol and citric acid, (ii) Antibiotics; Penicillin, Cephalosporin, Chloromycetin and Streptomycin, (iii) Lysine, Glutamic acid, Vitamin B2, Vitamin B12 and Vitamin C. (10 Hours) Reference Books:

• E. Stocchi: Industrial Chemistry, Vol -I, Ellis Horwood Ltd. UK. • P.C. Jain, M. Jain: Engineering Chemistry, Dhanpat Rai & Sons, Delhi. • B.K. Sharma: Industrial Chemistry, Goel Publishing House, Meerut. • G.L. Patrick: Introduction to Medicinal Chemistry, Oxford University Press, UK. • Hakishan, V.K. Kapoor: Medicinal and Pharmaceutical Chemistry, Vallabh Prakashan, Pitampura, New Delhi. • William O. Foye, Thomas L., Lemke , David A. William: Principles of Medicinal Chemistry, B.I. Waverly Pvt. Ltd. New Delhi.

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SEC – G: Pesticide & Fuel Chemistry (Credits: 04) Theory: 60 Hours Unit – 1: Introduction of Pesticide Chemistry & Preparation Procedure

General introduction to pesticides (natural and synthetic), benefits and adverse effects, changing concepts of pesticides, structure activity relationship, synthesis and technical manufacture and uses of representative pesticides in the following classes: Organochlorines (DDT, Gammexene,); Organophosphates (Malathion, Parathion ); Carbamates (Carbofuran and carbaryl); Quinones ( Chloranil), Anilides (Alachlor and Butachlor). (20 Hours) Unit – 2: Introduction and Industrial Manufacture of Fuel Energy Sources

Review of energy sources (renewable and non-renewable). Classification of fuels and their calorific value. Coal: Uses of coal (fuel and nonfuel) in various industries, its composition, carbonization of coal.Coal gas, producer gas and water gas—composition and uses. Fractionation of coal tar, uses of coal tar bases chemicals, requisites of a good metallurgical coke, Coal gasification (Hydro gasification and Catalytic gasification), Coal liquefaction and Solvent Refining.

Petroleum and Petrochemical Industry: Composition of crude petroleum, Refining and different types of petroleum products and their applications.

Fractional Distillation (Principle and process), Cracking (Thermal and catalytic cracking), Reforming Petroleum and non-petroleum fuels (LPG, CNG, LNG, bio-gas, fuels derived from biomass), fuel from waste, synthetic fuels (gaseous and liquids), clean fuels. Petrochemicals: Vinyl acetate, Propylene oxide, Isoprene, Butadiene, Toluene and its derivatives Xylene.

Lubricants: Classification of lubricants, lubricating oils (conducting and non-conducting) Solid and semisolid lubricants, synthetic lubricants.

Properties of lubricants (viscosity index, cloud point, pore point) and their determination.

(40 Hours) Reference Books: • E. Stocchi: Industrial Chemistry, Vol -I, Ellis Horwood Ltd. UK. • P.C. Jain, M. Jain: Engineering Chemistry, Dhanpat Rai & Sons, Delhi. • B.K. Sharma: Industrial Chemistry, Goel Publishing House, Meerut.

Reference Book:

• R. Cremlyn: Pesticides, John Wiley.

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------SEC – H: Computer Science/Sports/NCC/NSS/Yoga etc. offered by respective

Department (Credits: 04) Theory: 60 Hours

*Course Structure for SEC – H to be offered by respective Department

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Generic Elective Course (GE) (Minor-Chemistry) (any four) for other Departments/Disciplines: ------

GE – A: Atomic Structure, Bonding, General Organic Chemistry & Aliphatic Hydrocarbons (Credits: Theory-04, Practicals-02) Theory: 60 Hours Section – A: Inorganic Chemistry – 1

Unit – 1: Atomic Structure

Review of: Bohr’s theory and its limitations, dual behaviour of matter and radiation, de-Broglie’s relation, Heisenberg Uncertainty principle. Hydrogen atom spectra. Need of a new approach to Atomic structure.

What is Quantum mechanics? Time independent Schrodinger equation and meaning of various terms in it. Significance of ψ and ψ2, Schrödinger equation for hydrogen atom. Radial and angular parts of the hydogenic wavefunctions (atomic orbitals) and their variations for 1s, 2s, 2p, 3s, 3p and 3d orbitals (Only graphical representation). Radial and angular nodes and their significance. Radial distribution functions and the concept of the most probable distance with special reference to 1s and 2s atomic orbitals. Significance of quantum numbers, orbital angular momentum and quantum numbers ml and ms. Shapes of s, p and d atomic orbitals, nodal planes. Discovery of spin, spin quantum number (s) and magnetic spin quantum number (ms).

Rules for filling electrons in various orbitals, Electronic configurations of the atoms. Stability of half-filled and completely filled orbitals, concept of exchange energy. Relative energies of atomic orbitals, Anomalous electronic configurations. (12 Hours)

Unit – 2: Chemical Bonding

Ionic Bonding: General characteristics of ionic bonding. Energy considerations in ionic bonding, lattice energy and solvation energy and their importance in the context of stability and solubility of ionic compounds. Statement of Born-Landé equation for calculation of lattice energy, Born- Haber cycle and its applications, polarizing power and polarizability. Fajan’s rules, ionic character in covalent compounds, bond moment, dipole moment and percentage ionic character.

Covalent bonding: VB Approach: Shapes of some inorganic molecules and ions on the basis of VSEPR and hybridization with suitable examples of linear, trigonal planar, square planar, tetrahedral, trigonal bipyramidal and octahedral arrangements, such as BeCl2, BF3, SiF4, PCl5, + – + – + SF6, NH3, H2O, OF2, CIF3, SF4, XeF4, XeF6, H3O , I3 , I3 , ICl2 , XeF5 .

Concept of resonance and resonating structures in various inorganic and organic compounds.

(10Hours)

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Unit – 3: Molecular Orbital Theory

MO Approach: Rules for the LCAO method, bonding and antibonding MOs and their characteristics for s-s, s-p and p-p combinations of atomic orbitals, nonbonding combination of orbitals, MO treatment of homonuclear diatomic molecules of 1st and 2nd periods (including idea of s-p mixing) and heteronuclear diatomic molecules such as CO, NO and NO+. Comparison of VB and MO approaches. (8 Hours)

Section – B: Organic Chemistry – 1

Unit – 1: Fundamentals of Organic Chemistry

Physical Effects, Electronic Displacements: Inductive Effect, Electromeric Effect, Resonance and Hyperconjugation. Cleavage of Bonds: Homolysis and Heterolysis.

Structure, shape and reactivity of organic molecules: Nucleophiles and electrophiles. Reactive Intermediates: Carbocations, Carbanions and free radicals.

Strength of organic acids and bases: Comparative study with emphasis on factors affecting pK values. Aromaticity: Benzenoids and Hückel’s rule. (8 Hours) Unit – 2: Stereochemistry

Conformations with respect to ethane, butane and cyclohexane. Interconversion of Wedge Formula, Newmann, Sawhorse and Fischer representations. Concept of chirality (upto two carbon atoms). Configuration: Geometrical and Optical isomerism; Enantiomerism, Diastereomerism and Meso compounds). Threo and erythro; D and L; cis - trans nomenclature; CIP Rules: R/ S (for upto 2 chiral carbon atoms) and E / Z Nomenclature (for upto two C=C systems). (10 Hours) Unit – 3: Aliphatic Hydrocarbons

Functional group approach for the following reactions (preparations & reactions) to be studied in context to their structure.

Alkanes: (Upto 5 Carbons). Preparation: Catalytic hydrogenation, Wurtz reaction, Kolbe’s synthesis, from Grignard reagent. Reactions: Free radical Substitution: Halogenation.

Alkenes: (Upto 5 Carbons) Preparation: Elimination reactions: Dehydration of alkenes and dehydrohalogenation of alkyl halides (Saytzeff’s rule); cis alkenes (Partial catalytic hydrogenation) and trans alkenes (Birch reduction). Reactions: cis-addition (alk. KMnO4) and trans-addition (bromine), Addition of HX (Markownikoff’s and anti-Markownikoff’s addition), Hydration, Ozonolysis, oxymecuration-demercuration, Hydroboration-oxidation.

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Alkynes: (Upto 5 Carbons) Preparation: Acetylene from CaC2 and conversion into higher alkynes; by dehalogenation of tetra halides and dehydrohalogenation of vicinal-dihalides.

Reactions: formation of metal acetylides, addition of bromine and alkaline KMnO4, ozonolysis and oxidation with hot alk. KMnO4. (12 Hours) Reference Books:

• J. D. Lee: A new Concise Inorganic Chemistry, E L. B. S. • F. A. Cotton & G. Wilkinson: Basic Inorganic Chemistry, John Wiley. • Douglas, McDaniel and Alexader: Concepts and Models in Inorganic Chemistry, John Wiley. • James E. Huheey, Ellen Keiter and Richard Keiter: Inorganic Chemistry: Principles of Structure and Reactivity, Pearson Publication. • T. W. Graham Solomon: Organic Chemistry, John Wiley and Sons. • Peter Sykes: A Guide Book to Mechanism in Organic Chemistry, Orient Longman. • E. L. Eliel: Stereochemistry of Carbon Compounds, Tata McGraw Hill. • I. L. Finar: Organic Chemistry (Vol. I & II), E. L. B. S. • R. T. Morrison & R. N. Boyd: Organic Chemistry, Prentice Hall. • Arun Bahl and B. S. Bahl: Advanced Organic Chemistry, S. Chand

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GE – A Lab: Atomic Structure, Bonding, General Organic Chemistry & Aliphatic Hydrocarbons (60 Hours) Section – A: Inorganic Chemistry - Volumetric Analysis

1. Estimation of sodium carbonate and sodium hydrogen carbonate present in a mixture.

2. Estimation of oxalic acid by titrating it with KMnO4.

3. Estimation of water of crystallization in Mohr’s salt by titrating with KMnO4.

4. Estimation of Fe (II) ions by titrating it with K2Cr2O7 using internal indicator.

5. Estimation of Cu (II) ions iodometrically using Na2S2O3.

Section – B: Organic Chemistry

1. Detection of extra elements (N, S, Cl, Br, I) in organic compounds (containing upto two extra elements)

2. Separation of mixtures by Chromatography: Measure the Rf value in each case (combination of two compounds to be given)

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(a) Identify and separate the components of a given mixture of 2 amino acids (glycine, aspartic acid, glutamic acid, tyrosine or any other amino acid) by paper chromatography

(b) Identify and separate the sugars present in the given mixture by paper chromatography.

Reference Books:

• Textbook of Practical Organic Chemistry, A.I. Vogel , Prentice Hall, 5th edition. • Practical Organic Chemistry, F. G. Mann. & B. C. Saunders, Orient Longman, 1960. • Vogel’s Qualitative Inorganic Analysis, A.I. Vogel, Prentice Hall, 7th Edition. • Vogel’s Quantitative Chemical Analysis, A.I. Vogel, Prentice Hall, 6th Edition. • A. K. Nad, B. Mahapatra and A. Ghosal, An Advanced Course in Practical Chemistry, New Central Book Agency Priv. Ltd, 2011

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GE – B: Kinetic Theory of Gases, Chemical Energetics, Equilibria & Functional Group Organic Chemistry

(Credits: Theory-04, Practicals-02) Theory: 60 Hours Section – A: Physical Chemistry – 1

Unit – 1: Kinetic Theory of Gases

Postulates of Kinetic Theory of Gases and derivation of the kinetic gas equation.

Deviation of real gases from ideal behaviour, compressibility factor, causes of deviation. van der Waals equation of state for real gases. Boyle temperature (derivation not required). Critical phenomena, critical constants and their calculation from van der Waals equation. Andrews isotherms of CO2.

Maxwell Boltzmann distribution laws of molecular velocities and molecular energies (graphic representation – derivation not required) and their importance.

Temperature dependence of these distributions. Most probable, average and root mean square velocities (no derivation). Collision cross section, collision number, collision frequency, collision diameter and mean free path of molecules. Viscosity of gases and effect of temperature and pressure on coefficient of viscosity (qualitative treatment only).

(10 Hours)

Unit – 2: Chemical Energetics

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Chemical Energetics: Introduction of different terms and processes in thermodynamics: [systems (isolated, closed, open) and surrounding, macroscopic properties, state and path functions and their differentials.

First Law: concept of heat, q, work, w, internal energy, U, sign convention for heat and work, nature of work, path dependence of work and heat; statement of first law; enthalpy, H, heat changes at constant volume and constant pressure; heat capacities (Cv, Cp) and relation between them for ideal gases. Reversible and irreversible processes, maximum work, thermodynamic quantities (w, q, ∆U, ∆H) and its calculation for isothermal and adiabatic reversible expansion of ideal gases. Ideal gas law for adiabatic reversible expansion, comparison of adiabatic and isothermal reversible expansion. Joule-Thomson effect, JouleThomson coefficient in ideal and real (van der Waal) gases, inversion temperature.

Thermo-chemistry: Standard state, standard enthalpy of formation, Hess’s Laws of constant heat summation and its application. Change in internal energy (∆U) and enthalpy (∆H) of chemical reactions, relation between ∆U and ∆H, variation of heat of reaction with temperature (Kirchhoff’s equation). Enthalpy of neutralization. Bond Energy – Bond dissociation energy and its calculation from thermo-chemical data.– Kirchhoff’s equation.

Second law of thermodynamics, concept of entropy, free energy work functions, Gibbs Helmholtz equation and its applications

Statement of Third Law of thermodynamics and calculation of absolute entropies of substances.

(12 Hours) Unit – 3: Chemical and Ionic Equilibrium

Free energy change in a chemical reaction. Thermodynamic derivation of the law of chemical o equilibrium. Distinction between G and G , Le Chatelier’s principle. Relationships between Kp, Kc and Kx for reactions involving ideal gases.

Strong, moderate and weak electrolytes, degree of ionization, factors affecting degree of ionization, ionization constant and ionic product of water. Ionization of weak acids and bases, pH scale, common ion effect. Salt hydrolysis-calculation of hydrolysis constant, degree of hydrolysis and pH for different salts. Buffer solutions. Solubility and solubility product of sparingly soluble salts – applications of solubility product principle.

(8 Hours) Section – B: Organic Chemistry – 2

Functional group approach for the following reactions (preparations & reactions) to be studied in context to their structure.

Unit – 1: Aromatic Hydrocarbons & Alkyl and Aryl Halides

Aromatic Hydrocarbons: Preparation (Case benzene): from phenol, by decarboxylation,

95 | P a g e from acetylene, from benzene sulphonic acid. Reactions: (Case benzene): Electrophilic substitution: nitration, halogenation and sulphonation. Friedel-Craft’s reaction (alkylation and acylation) (upto 4 carbons on benzene). Side chain oxidation of alkyl benzenes (upto 4 carbons on benzene); aromatic hydrocarbon side chain reactions.

Alkyl Halides (upto 5 Carbons): Types of Nucleophilic Substitution (SN2, SN1, SNi) reactions. Preparation: from alkenes and alcohols. Reactions: hydrolysis, nitrite & nitro formation, nitrile & isonitrile formation. Williamson’s ether synthesis: Elimination vs substitution.

Aryl Halides: Preparation: (Chloro, bromo and iodo-benzene case): from phenol, Sandmeyer & Gattermann reactions. Reactions (Chlorobenzene): Aromatic nucleophilic substitution (replacement by –OH group) and effect of nitro substituent. Benzyne Mechanism: KNH2/NH3 or NaNH2/NH3 reagent system. Reactivity and Relative strength of C-Halogen bond in alkyl, allyl, benzyl, vinyl and aryl halides.

(10 Hours) Unit – 2: Alcohols, Phenols, Ethers, Aldehydes and Ketones (Upto 5 Carbons)

Alcohols: Preparation: Preparation of 1°, 2° and 3° alcohols: using Grignard reagent, Ester hydrolysis, Reduction of aldehydes, ketones, carboxylic acid and esters. Reactions: With sodium, HX (Lucas test), esterification, oxidation (with PCC, alk. KMnO4, acidic dichromate, conc.HNO3). Oppeneauer oxidation Diols: (Upto 6 Carbons) oxidation of diols. Pinacol-Pinacolone rearrangement.

Phenols: (Phenol case) Preparation: Cumene hydroperoxide method, from diazonium salts. Reactions: Electrophilic substitution: Nitration, halogenation and sulphonation. Reimer-Tiemann Reaction, Gattermann-Koch Reaction, Houben–Hoesch Condensation, Schotten–Baumann Reaction. Ethers (Aliphatic and Aromatic): Cleavage of ethers with HI.

Aldehydes and Ketones (Aliphatic and Aromatic): (Formaldehye, acetaldehyde, acetone and benzaldehyde); Preparation: from acid chlorides and from nitriles. Reactions -Reaction with HCN, ROH, NaHSO3, NH-G derivatives. Iodoform test. Aldol Condensation, Cannizzaro’s reaction, Wittig reaction, Benzoin condensation. Clemensen reduction and Wolff Kishner reduction. Meerwein-Pondorff Verley reduction. (12 Hours)

Unit – 3: Carboxylic acids and their derivatives & Amines salt

Carboxylic acids (aliphatic and aromatic): Preparation: Acidic and Alkaline hydrolysis of esters. Reactions: Hell – Vohlard - Zelinsky Reaction. Preparation: Acid chlorides, Anhydrides, Esters and Amides from acids and their interconversion. Reactions: Comparative study of nucleophilicity of acyl derivatives. Reformatsky Reaction, Perkin condensation.

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Amines and Diazonium Salts: Amines (Aliphatic and Aromatic): (Upto 5 carbons), Preparation: from alkyl halides, Gabriel’s Phthalimide synthesis, Hofmann Bromamide reaction. Reactions: Hofmann vs. Saytzeff elimination, Carbylamine test, Hinsberg test, with HNO2, Schotten – Baumann Reaction. Electrophilic substitution (case aniline): nitration, bromination, sulphonation.

Diazonium salts: Preparation: from aromatic amines. Reactions: conversion to benzene, phenol, dyes.

(8 Hours) Reference Books:

• T. W. Graham Solomons: Organic Chemistry, John Wiley and Sons. • Peter Sykes: A Guide Book to Mechanism in Organic Chemistry, Orient Longman. • R. T. Morrison & R. N. Boyd: Organic Chemistry, Prentice Hall. • Arun Bahl and B. S. Bahl: Advanced Organic Chemistry, S. Chand. • G. M. Barrow: Physical Chemistry Tata McGraw-Hill (2007). • G. W. Castellan: Physical Chemistry 4th Edn. Narosa (2004). • J. C. Kotz, P. M. Treichel & J. R. Townsend: General Chemistry Cengage Lening India Pvt. Ltd., New Delhi (2009). • Morrison, R. T. & Boyd, R. N. Organic Chemistry, Dorling Kindersley (India) Pvt. Ltd. (Pearson Education). • Finar, I. L. Organic Chemistry (Volume 1), Dorling Kindersley (India) Pvt. Ltd. (Pearson Education). • Finar, I. L. Organic Chemistry (Volume 2), Dorling Kindersley (India) Pvt. Ltd. (Pearson Education). • B. H. Mahan: University Chemistry 3rd Ed. Narosa (1998). • R. H. Petrucci: General Chemistry 5th Ed. Macmillan Publishing Co.: New York (1985).

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GE – B Lab: Kinetic Theory of Gases, Chemical Energetics, Equilibria & Functional Group Organic Chemistry (60 Hours) (Practicals : 02)

Section – A: Physical Chemistry

Thermochemistry

1. Determination of heat capacity of calorimeter for different volumes. 2. Determination of enthalpy of neutralization of hydrochloric acid with sodium hydroxide. 3. Determination of enthalpy of ionization of acetic acid. 4. Determination of integral enthalpy of solution of salts (KNO3, NH4Cl).

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5. Determination of enthalpy of hydration of copper sulphate. 6. Study of the solubility of benzoic acid in water and determination of H.

Ionic Equilibria pH measurements

a) Measurement of pH of different solutions like aerated drinks, fruit juices, shampoos and soaps (use dilute solutions of soaps and shampoos to prevent damage to the glass electrode) using pH-meter. b) Preparation of buffer solutions: (i) Sodium acetate-acetic acid

(ii) Ammonium chloride-ammonium hydroxide

Measurement of the pH of buffer solutions and comparison of the values with theoretical values.

Section – B: Organic Chemistry

I Systematic Qualitative Organic Analysis of Organic Compounds possessing monofunctional groups (-COOH, phenolic, aldehydic, ketonic, amide, nitro, amines) and preparation of one derivative.

II 1. Criteria of Purity: Determination of melting and boiling points. 2. Purification of organic compounds by crystallization (from water and alcohol) and distillation. 3. Preparations: Mechanism of various reactions involved to be discussed. Recrystallisation, determination of melting point and calculation of quantitative yields to be done. (a) Bromination of Phenol/Aniline (b) Benzoylation of amines/phenols (c) Oxime and 2,4 dinitrophenylhydrazone of aldehyde/ketone

Reference Books • A.I. Vogel: Textbook of Practical Organic Chemistry, 5th edition, Prentice-Hall. • F. G. Mann & B. C. Saunders, Practical Organic Chemistry, Orient Longman (1960). • Ahluwalia, V.K. & Aggarwal, R. Comprehensive Practical Organic Chemistry, Universities Press • B.D. Khosla, Senior Practical Physical Chemistry, R. Chand & Co. • A. K. Nad, B. Mahapatra and A. Ghosal, An Advanced Course in Practical Chemistry, New Central Book Agency Priv. Ltd, 2011

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GE – C: Solid, Solutions, Phase Equilibrium, Conductance, Periodic Properties and Chemistry of s-, p-, and d- block elements (Credits: Theory-04, Practicals-02) Theory: 60 Hours Section – A: Physical Chemistry – 2

Unit – 1: Solids

Forms of solids. Symmetry elements, unit cells, crystal systems, Bravais lattice types and identification of lattice planes. Laws of Crystallography - Law of constancy of interfacial angles, Law of rational indices. Miller indices. X–Ray diffraction by crystals, Bragg’s law. Structures of NaCl, KCl and CsCl (qualitative treatment only). Defects in crystals. Glasses and liquid crystals.

(10 Hours)

Unit – 2: Solutions & Phase Equilibrium

Thermodynamics of ideal solutions: Ideal solutions and Raoult’s law, deviations from Raoult’s law – non-ideal solutions. Vapour pressure-composition and temperature-composition curves of ideal and non-ideal solutions. Distillation of solutions. Lever rule. Azeotropes.

Partial miscibility of liquids: Critical solution temperature; effect of impurity on partial miscibility of liquids. Immiscibility of liquids- Principle of steam distillation. Nernst distribution law and its applications, solvent extraction.

Phases, components and degrees of freedom of a system, criteria of phase equilibrium. Gibbs Phase Rule and its thermodynamic derivation. Derivation of Clausius – Clapeyron equation and its importance in phase equilibria. Phase diagrams of one-component systems (water and sulphur) and two component systems involving eutectics, congruent and incongruent melting points (lead-silver, FeCl3-H2O and Na-K only). (12 Hours)

Unit – 3: Conductance

Conductivity, equivalent and molar conductivity and their variation with dilution for weak and strong electrolytes. Kohlrausch law of independent migration of ions.

Transference number and its experimental determination using Hittorf and Moving boundary methods. Ionic mobility. Applications of conductance measurements: determination of degree of ionization of weak electrolyte, solubility and solubility products of sparingly soluble salts, ionic product of water, hydrolysis constant of a salt. Conductometric titrations (only acid-base). (8 Hours)

Section – B: Inorganic Chemistry – 2

Unit – 1: Periodic Properties & Acid-Base Concepts

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Periodic Properties: Division of elements into s, p, d, and f blocks, covalent radii, van der Waals radii and ionic radii; ionization enthalpy, electron gain enthalpy, and electronegativity (Pauling, Mulliken, and Alfred-Rochow scales: Definition, methods of determination, trends in periodic table, and applications in predicting and explaining chemical behavior).

Acids and Bases: Arrhenius, Brønsted-Lowry, Lux-Flood and Lewis concepts of acids and bases. Factors affecting strengths of Lewis acids and bases, Classification of acids and bases as hard and soft, Pearsons HSAB concept, acid-base strength and hardness and softness, symbiosis, application of HSAB theory. (10 Hours)

Unit – 2: Oxidation-Reduction

Redox equations, Standard electrode potentials, Ellingham diagrams for reduction of metal oxides using carbon as reducing agent, Nernst equation, redox potentials to explore the feasibility of reaction and calculation of values of equilibrium constant,

(6 Hours)

Unit – 3: Chemistry of s-, p- and d- Block Elements s-Block Elements: General characteristic properties, complexes of alkali metals, comparative study of hydrides, oxides, hydroxides, halides, carbonates and bicarbonates of group I and II, Diagonal relationship, Biological role of alkali and alkaline earth metals. p-Block Elements: General characteristic properties, comparative study (including diagonal relationship and inert pair effect) of groups 13-17 (B, C, N, O, F) elements and group trends of compounds like hydrides, oxides, halides, and oxy acids; preparation properties and structure, of diborane, borazine, alkalimetal borohydrides, fullerenes, silicates and silicones, inter-halogens and polyhalides.

Chemistry of Noble Gases: Isolation and separation of noble gases from air, chemical properties of noble gases, chemistry of xenon, structure and bonding in xenon compounds. d-Block Elements: Characteristic properties of d-block elements. Properties of the elements of the first transition series, their binary compounds and complexes illustrating relative stability of their oxidation states, coordination number and geometry. Comparative treatment with their 3d-analogues in respect of ionic radii, oxidation states and stereochemistry.

(14 Hours)

Reference Books:

• G. M. Barrow: Physical Chemistry Tata McGraw-Hill (2007). • G. W. Castellan: Physical Chemistry 4th Ed. Narosa (2004). • J. C. Kotz, P. M. Treichel, J. R. Townsend, General Chemistry, Cengage Learning India

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Pvt. Ltd.: New Delhi (2009). • B. H. Mahan: University Chemistry, 3rd Edn. Narosa (1998). • R. H. Petrucci, General Chemistry, 5th Edn., Macmillan Publishing Co.: New York (1985). • E. S. Gilreath, Fundamental Concepts of Inorganic Chemistry, Mc Graw Hill Edu. Pvt. Ltd. • R. Sarkar (Part-I & II), General & Inorganic Chemistry, Central. • R. L. Dutta (Part-I & II), Inorganic Chemistry, The New Book Stall. • J. D. Lee: A New Concise Inorganic Chemistry, E.L.B.S. • F.A. Cotton & G. Wilkinson: Basic Inorganic Chemistry, John Wiley. • D. F. Shriver and P. W. Atkins: Inorganic Chemistry, Oxford University Press. • Gary Wulfsberg: Inorganic Chemistry, Viva Books Pvt. Ltd.

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GE – C Lab: Solid, Solutions, Phase Equilibrium, Conductance & Periodic Properties and Chemistry of s-, p-, and d- block elements (60 Hours) Section – A: Physical Chemistry

Distribution

Study of the equilibrium of one of the following reactions by the distribution method:

- - I2(aq) + I (aq) ⇌ I3 (aq) 2+ 2+ Cu (aq) + xNH3(aq) ⇌ [Cu(NH3)x]

Phase equilibria

a) Construction of the phase diagram of a binary system (simple eutectic) using cooling curves. b) Determination of the critical solution temperature and composition of the phenol water system and study of the effect of impurities on it. c) Study of the variation of mutual solubility temperature with concentration for the phenol water system and determination of the critical solubility temperature.

Conductance

a) Determination of cell constant b) Determination of equivalent conductance, degree of dissociation and dissociation constant of a weak acid. c) Perform the following conductometric titrations: i. Strong acid vs. strong base ii. Weak acid vs. strong base

Potentiometry

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Perform the following potentiometric titrations: a) Strong acid vs. strong base b) Weak acid vs. strong base c) Potassium dichromate vs. Mohr's salt

Section – B: Inorganic Chemistry

Semi-micro qualitative analysis using H2S of mixtures- not more than four ionic species (two anions and two cations and excluding insoluble salts) out of the following:

Cations : NH4+, Pb2+, Ag+, Bi3+, Cu2+, Cd2+, Sn2+, Fe3+, Al3+, Co2+, Cr3+, Ni2+, Mn2+, Zn2+, 2+ 2+ 2+ + 2– 2– 2– 2– – – – – – 2- 3- Ba , Sr , Ca , K , Anions : CO3 , S , SO , S2O3 , NO3 , NO2 , Cl , Br , I , SO4 , PO4 , 3- 2- - BO3 , C2O4 , F

(Spot tests should be carried out wherever feasible)

Reference Books: • B.D. Khosla: Senior Practical Physical Chemistry, R. Chand & Co. • A.I. Vogel, Qualitative Inorganic Analysis, Prentice Hall, 7th Edn. • A.I. Vogel, Quantitative Chemical Analysis, Prentice Hall, 6th Edn. • A. K. Nad, B. Mahapatra and A. Ghosal, An Advanced Course in Practical Chemistry, New Central Book Agency Priv. Ltd, 2011 • V. K. Ahluwalia, S. Dhingra & A. Gulati, College Practical Chemistry, University Press, Delhi.

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GE – D: Electrochemistry, Chemical Kinetics, Co-ordination compounds, Organometallics and Molecules of life

(Credits: Theory-04, Practicals-02) Theory: 60 Hours Section – A: Physical Chemistry – 3

Unit – 1: Electrochemistry

Reversible and irreversible cells. Concept of EMF of a cell. Measurement of EMF of a cell. Nernst equation and its importance. Types of electrodes. Standard electrode potential. Electrochemical series. Thermodynamics of a reversible cell, calculation of thermodynamic properties: G, H and S from EMF data. Calculation of equilibrium constant from EMF data. pH determination using hydrogen electrode and glass electrode. Potentiometric titrations -qualitative treatment (acid-base and oxidation-reduction only).

(10 Hours)

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Unit – 2: Chemical Kinetics

The concept of reaction rates. Effect of temperature, pressure, catalyst and other factors on reaction rates. Order and molecularity of a reaction. Derivation of integrated rate equations for zero, first and second order reactions (both for equal and unequal concentrations of reactants). Half–life of a reaction. General methods for determination of order of a reaction. Concept of activation energy and its calculation from Arrhenius equation.

Theories of Reaction Rates: Collision theory and Activated Complex theory of bimolecular reactions. Comparison of the two theories (qualitative treatment only).

(10 Hours) Section – B: Inorganic Chemistry – 3

Unit – 1: Coordination Compounds

Werner's coordination theory and its experimental verification, effective atomic number concept, chelats, nomenclature of co-ordination compounds, isomerism in coordination compounds.

Crystal Field Theory: Crystal field effect, octahedral symmetry. Crystal field stabilization energy (CFSE), Crystal field effects for weak and strong fields. Tetrahedral symmetry. Factors affecting the magnitude of D. Spectrochemical series. Comparison of CFSE for Oh and Td complexes, Tetragonal distortion of octahedral geometry. Jahn-Teller distortion, Square planar coordination.

(10 Hours) Unit – 2: Organometallics

Definition and Classification with appropriate examples based on nature of metal-carbon bond (ionic, s, p and multi centre bonds). Structures of methyl lithium, Zeiss salt and ferrocene. EAN rule as applied to carbonyls. Preparation, structure, bonding and properties of mononuclear and polynuclear carbonyls of 3d metals. p-acceptor behaviour of carbon monoxide. Synergic effects (VB approach)- (MO diagram of CO can be referred to for synergic effect to IR frequencies).

(10 Hours) Section – C: Organic Chemistry – 3

Molecules of Life

Unit – 1: Carbohydrates

Classification of carbohydrates, reducing and non reducing sugars, and General Properties, Glucose and Fructose, their open chain structure. Epimers, mutarotation and anomers,

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Determination of configuration of monosaccharides, absolute configuration of Glucose and Fructose, Mutarotation, ascending and descending in monosaccharides. Structure of disacharrides (sucrose, cellobiose, maltose, lactose) and polysacharrides (starch and cellulose) excluding their structure elucidation. (8 Hours) Unit – 2: Amino Acids, Peptides, Proteins and Nucleic Acids

Preparation of Amino Acids: Strecker synthesis using Gabriel’s phthalimide synthesis. Zwitterion, Isoelectric point and Electrophoresis.

Reactions of Amino acids: ester of –COOH group, acetylation of –NH2 group, complexation with 2+ Cu ions, ninhydrin test. Overview of Primary, Secondary, Tertiary and Quaternary structure of proteins. Determination of primary structure of peptides, determination of N-terminal amino acid (by DNFB and Edman method) and C–terminal amino acid (by thiohydantoin and with carboxypeptidase enzyme). Synthesis of simple peptides (upto dipeptides) by N-protection (t-butyloxycarbonyl and phthaloyl) & C-activating groups and Merrifield solid phase synthesis.

Components of Nucleic acids: Adenine, guanine, thymine and Cytosine (Structure only), other components of nucleic acids, Nucleosides and nucleotides (nomenclature), Structure of polynucleotides; Structure of DNA (Watson-Crick model) and RNA(types of RNA), Genetic Code, Biological roles of DNA and RNA: Replication, Transcription and Translation.

(12 Hours) Reference Books:

• G. M. Barrow: Physical Chemistry Tata McGraw-Hill (2007). • G. W. Castellan: Physical Chemistry 4th Edn. Narosa (2004). • J. C. Kotz, P. M. Treichel & J. R. Townsend: General Chemistry Cengage Lening India Pvt. Ltd., New Delhi (2009). • B. H. Mahan: University Chemistry 3rd Ed. Narosa (1998). • R. H. Petrucci: General Chemistry 5th Ed. Macmillan Publishing Co.: New York (1985). • J. D. Lee: A New Concise Inorganic Chemistry, E.L.B.S. • F.A. Cotton & G. Wilkinson: Basic Inorganic Chemistry, John Wiley. • D. F. Shriver and P. W. Atkins: Inorganic Chemistry, Oxford University Press. • R. L. Dutta (Part-I & II), Inorganic Chemistry, The New Book Stall. • Gary Wulfsberg: Inorganic Chemistry, Viva Books Pvt. Ltd. • S. Chand. Morrison, R. T. & Boyd, R. N. Organic Chemistry, Dorling Kindersley (India) Pvt. Ltd. (Pearson Education). • Finar, I. L. Organic Chemistry (Volume 1), Dorling Kindersley (India) Pvt. Ltd. (Pearson Education). • Finar, I. L. Organic Chemistry (Volume 2), Dorling Kindersley (India) Pvt. Ltd. (Pearson Education). • Nelson, D. L. & Cox, M. M. Lehninger’s Principles of Biochemistry 7th Ed., W. H. Freeman.

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• Berg, J. M., Tymoczko, J. L. & Stryer, L. Biochemistry 7th Ed., W. H. Freeman

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GE – D Lab: Electrochemistry, Chemical Kinetics, Co-ordination compounds, Organometallics and Molecules of life (60 Hours)

Section – A: Physical Chemistry

(I) Surface tension measurement (use of organic solvents excluded).

a) Determination of the surface tension of a liquid or a dilute solution using a stalagmometer. b) Study of the variation of surface tension of a detergent solution with concentration.

(II) Viscosity measurement (use of organic solvents excluded).

a) Determination of the relative and absolute viscosity of a liquid or dilute solution using an Ostwald’s viscometer. b) Study of the variation of viscosity of an aqueous solution with concentration of solute.

(III) Chemical Kinetics

Study the kinetics of the following reactions. 1. Initial rate method: Iodide-persulphate reaction 3. Integrated rate method: c. Acid hydrolysis of methyl acetate with hydrochloric acid. b. Saponification of ethyl acetate. c. Compare the strengths of HCl and H2SO4 by studying kinetics of hydrolysis of methyl acetate

Section – B: Inorganic Chemistry

1. Separation of mixtures by chromatography: Measure the Rf value in each case. (Combination of two ions to be given) Binary mixture of nickel and cobalt, copper and nickel, zinc and magnesium, iron and copper; aluminium and nickel.

2. Preparation of any two of the following complexes:

(a) tetraaammine copper (II) sulphate

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(b) tetraamminecarbonatocobalt (III) nitrate (c) potassium trioxalatochromate (III) (d) potassium trioxalatoferrate (III) (e) sodium hexanitritocabaltate (III) (f) prussin blue

Section – C: Organic Chemistry

1. Determination of the concentration of glycine solution by formylation method. 2. Titration curve of glycine 3. Action of salivary amylase on starch 4. Effect of temperature on the action of salivary amylase on starch. 5. Determination of the saponification value of an oil/fat. 6. Determination of the iodine value of an oil/fat 7. Differentiation between a reducing/nonreducing sugar. 8. Extraction of DNA from onion/ cauliflower

Reference Books: • B.D. Khosla, Senior Practical Physical Chemistry, R. Chand & Co. • A.I. Vogel, Qualitative Inorganic Analysis, Prentice Hall, 7th Edn. • A.I. Vogel, Quantitative Chemical Analysis, Prentice Hall, 6th Edn. • A. K. Nad, B. Mahapatra and A. Ghosal, An Advanced Course in Practical Chemistry, New Central Book Agency Priv. Ltd, 2011 • V. K. Ahluwalia, S. Dhingra & A. Gulati, College Practical Chemistry, University Press, Delhi.

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GE – E: Analytical Chemistry, Quantum Chemistry & Spectroscopy (Credits: Theory-04, Practicals-02) Theory: 60 Hours Section – A: Inorganic Chemistry – 4

Unit – 1: Introduction

Introduction to Analytical Chemistry and its interdisciplinary nature. Balances, burettes, volumetric flasks, pipettes, calibration of tools, sampling. Errors and Statistics: significant figures, rounding off, accuracy and precision, determinate and indeterminate errors, standard deviation, propagation of errors, confidence limit, test of significance, rejection of a result.

(8 Hours) Unit – 2: Volumetric Titration

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Standard solution, primary standard and secondary standard, titration, end point, indicator, concentration of standard solution- moles, Normality, molarity, Molality, parts per million(PPM), volumetric calculation, acid base titration and use of indicators,titration curves for strong acid vs strong base, weak acid with strong base, weak base with strong acid, theory of acid base indicator, Redox titration- titration of Mohr salt against KMnO4, Titration of Oxalic acid against KMnO4, Titration of FeSO4 against K2Cr2O7, Iodometric and iodimetric titration, Internal and external indicator, complexometric titration- EDTA titration, Eriochrome black T indicator, complexometric titration curve, direct and back titration, masking and demasking of cations, precaution in volumetric titration and Gravimetric methods. (10 Hours) Unit – 3: Chromatography

Chromatographic Techniques: classification, theory of chromatographic separation, distribution coefficient, retention, sorption, efficiency and resolution. - Column, ion exchange, paper, TLC & HPTLC chromatography etc.

Ion-exchange: Column, ion-exchange chromatography etc. Determination of ion exchange capacity of anion / cation exchange resin (using batch procedure if use of column is not feasible).

Gas Chromatography: retention time or volume, capacity ratio, partition coefficient, theoretical plate and number, separation efficiency and resolution, instrumentation and application. (12 Hours)

Section – B: Physical Chemistry – 4

Unit – 1: Quantum Chemistry & Spectroscopy

Spectroscopy and its importance in chemistry. Wave-particle duality. Link between spectroscopy and quantum chemistry. Electromagnetic radiation and its interaction with matter. Types of spectroscopy. Difference between atomic and molecular spectra. Born-Oppenheimer approximation: Separation of molecular energies into translational, rotational, vibrational and electronic components.

Postulates of quantum mechanics, quantum mechanical operators.

Free particle. Particle in a 1-D box (complete solution), quantization, normalization of wavefunctions, concept of zero-point energy.

Rotational Motion: Schrödinger equation of a rigid rotator and brief discussion of its results (solution not required). Quantization of rotational energy levels. Microwave (pure rotational) spectra of diatomic molecules. Selection rules. Structural information derived from rotational spectroscopy.

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Vibrational Motion: Schrödinger equation of a linear harmonic oscillator and brief discussion of its results (solution not required). Quantization of vibrational energy levels. Selection rules, IR spectra of diatomic molecules. Structural information derived from vibrational spectra. Vibrations of polyatomic molecules. Group frequencies. Effect of hydrogen bonding (inter- and intramolecular) and substitution on vibrational frequencies.

Electronic Spectroscopy: Electronic excited states. Free Electron model and its application to electronic spectra of polyenes. Colour and constitution, chromophores, auxochromes, bathochromic and hypsochromic shifts. (24 Hours) Unit – 2: Photochemistry

Laws of photochemistry. Lambert-Beer’s law. Fluorescence and phosphorescence. Quantum efficiency and reasons for high and low quantum yields. Primary and secondary processes in photochemical reactions. Photochemical and thermal reactions. Photoelectric cells.

(6 Hours)

Reference Books:

• Skoog, D.A.; West, D.M. & Holler, F.J. Fundamentals of Analytical Chemistry 6th Ed., Saunders College Publishing, Fort Worth (1992). • Dean, J. A. Analytical Chemistry Notebook, McGraw Hill. • Vogel, A. I. Vogel’s Qualitative Inorganic Analysis 7th Ed., Prentice Hall. • Vogel, A. I. Vogel’s Quantitative Chemical Analysis 6th Ed., Prentice Hall. • G. M. Barrow: Physical Chemistry Tata McGraw-Hill (2007). • G. W. Castellan: Physical Chemistry 4th Edn. Narosa (2004). • J. C. Kotz, P. M. Treichel & J. R. Townsend: General Chemistry, Cengage Lening India Pvt. Ltd., New Delhi (2009). • B. H. Mahan: University Chemistry 3rd Ed. Narosa (1998). • R. H. Petrucci: General Chemistry 5th Ed. Macmillan Publishing Co.: New York (1985). • J. D. Lee: A New Concise Inorganic Chemistry, E.L.B.S. • F.A. Cotton & G. Wilkinson: Basic Inorganic Chemistry, John Wiley. • D. F. Shriver and P. W. Atkins: Inorganic Chemistry, Oxford University Press. • Gary Wulfsberg: Inorganic Chemistry, Viva Books Pvt. Ltd.

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GE – E Lab: Analytical Chemistry, Quantum Chemistry & Spectroscopy

(60 Hours) Section – A: Inorganic Chemistry

1. Estimation of the amount of nickel present in a given solution as

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bis(dimethylglyoximato) nickel(II) or aluminium as oxinate in a given solution gravimetrically. 2. Estimation of (i) Mg2+ or (ii) Zn2+ by complexometric titrations using EDTA. 3. Estimation of total hardness of a given sample of water by complexometric titration. 4. To draw calibration curve (absorbance at λmax vs. concentration) for various concentrations of a given coloured compound and estimate the concentration of the same in a given solution. 5. Determination of the composition of the Fe3+ - salicylic acid complex / Fe2+ - phenanthroline complex in solution by Job’s method. 6. Determination of concentration of Na+ and K+ using Flame Photometry.

Section – B: Physical Chemistry

UV/Visible spectroscopy

I. Study the 200-500 nm absorbance spectra of KMnO4 and K2Cr2O7 (in 0.1 M H2SO4) and determine the λmax values. Calculate the energies of the two transitions in different units (J molecule-1, kJ mol-1, cm-1, eV). II. Study the pH-dependence of the UV-Vis spectrum (200-500 nm) of K2Cr2O7. III. Record the 200-350 nm UV spectra of the given compounds (acetone, acetaldehyde, 2- propanol, acetic acid) in water. Comment on the effect of structure on the UV spectra of organic compounds.

Colourimetry

I. Verify Lambert-Beer’s law and determine the concentration of CuSO4/KMnO4/K2Cr2O7 in a solution of unknown concentration II. Analyses the given vibration-rotation spectrum of HCl(g)

Reference Books: • A.I. Vogel, Qualitative Inorganic Analysis, Prentice Hall, 7th Edn. • A.I. Vogel, Quantitative Chemical Analysis, Prentice Hall, 6th Edn. • B.D. Khosla, Senior Practical Physical Chemistry, R. Chand & Co.

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GE – F: Chemistry of f-Block Elements, Bio-inorganic Chemistry, Polynuclear Hydrocarbons and UV, IR Spectroscopy

(Credits: Theory-04, Practicals-02) Theory: 60 Hours Section – A: Inorganic Chemistry – 5

Unit – 1: Chemistry of f- Block Elements

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Chemistry of Lanthanide: Comparative study with respect to Electronic configuration, Oxidation states, atomic and ionic radii and complex formation, Lanthanide contraction, occurrence and isolation (ion exchange and solvent extraction methods), important lanthanide compounds.

Chemistry of Actinides: General features and chemistry of actinides, chemistry of separation of Np, Pu and Am from U. trans-uranium elements. Similarities between the later actinides and the later lanthanides.

(10 Hours) Unit – 1: Radioactivity

Radioactive decay, half-life and average life of radio elements, units of radioactivity, natural radioactive disintegration series, Instrumental analysis of radioactive elements, radioactive equilibrium, group displacement law, isotope, isotone, isobars and nuclear isomerism. Application of isotope in medicine, agriculture, reaction mechanism (isotope as tracer), age of minerals, age of earth, radio carbon dating, nuclear particles, nuclear forces: meson exchange theory.

Unit – 1: Bio-Inorganic Chemistry

A brief introduction to bio-inorganic chemistry. Role of metal ions present in biological systems with special reference to Na+, K+ and Mg2+ ions: Na/K pump; Role of Mg2+ ions in energy production and chlorophyll. Role of Ca2+ in blood clotting, stabilization of protein structures and structural role (bones). (10 Hours)

Section – B: Organic Chemistry – 4

Unit – 1: Polynuclear and heteronuclear aromatic compounds:

Properties of the following compounds with reference to electrophilic and nucleophilic substitution: Naphthalene, Anthracene , Furan, Pyrrole, Thiophene, and Pyridine.

Active methylene compounds: Preparation: Claisen ester condensation. Keto-enol tautomerism. Reactions: Synthetic uses of ethylacetoacetate (preparation of non-heteromolecules having upto 6 carbon). (10 Hours) Unit – 2: Concept of Energy in Biosystems

Calorific value of food. Standard caloric content of carbohydrates, proteins and fats. Oxidation of foodstuff (organic molecules) as a source of energy for cells. Introduction to Metabolism (catabolism, anabolism), ATP: the universal currency of cellular energy, ATP hydrolysis and free energy change.

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Conversion of food into energy. Outline of catabolic pathways of Carbohydrate- Glycolysis, Fermentation, Krebs Cycle. Overview of catabolic pathways of Fats and Proteins. Interrelationships in the metabolic pathways of Proteins, Fats and Carbohydrates.

Unit – 3: Application of Spectroscopy to Simple Organic Molecules

Application of visible, ultraviolet and Infrared spectroscopy in organic molecules. Electromagnetic radiations, electronic transitions, λmax & εmax, chromophore, auxochrome, bathochromic and hypsochromic shifts. Application of electronic spectroscopy and Woodward rules for calculating l max of conjugated dienes and α,β – unsaturated compounds.

Infrared radiation and types of molecular vibrations, functional group and fingerprint region. IR spectra of alkanes, alkenes and simple alcohols (inter and intramolecular hydrogen bonding), aldehydes, ketones, carboxylic acids and their derivatives (effect of substitution on >C=O stretching absorptions).

(18 Hours)

Reference Books:

• B. R. Puri, L. R. Sharma, and K. C. Kalia: Principle of Inorganic Chemistry, Milestone Publisher, New Delhi 2010. • W. U. Malik, G. D. Tuli, and R. D. Madan: Selected Topic in Inorganic Chemistry, S. Chand & Company Ltd, New Delhi, 1998. • I.L. Finar: Organic Chemistry (Vol. I & II), E.L.B.S. • H. J. Arnikar: Essentials of Nuclear Chemistry. • A. K. Das, Bioinorganic Chemistry, Books & Allied Ltd. • John R. Dyer: Applications of Absorption Spectroscopy of Organic Compounds, Prentice Hall. • R.M. Silverstein, G.C. Bassler & T.C. Morrill: Spectroscopic Identification of Organic Compounds, John Wiley & Sons. • R.T. Morrison & R.N. Boyd: Organic Chemistry, Prentice Hall. • Peter Sykes: A Guide Book to Mechanism in Organic Chemistry, Orient Longman. • Arun Bahl and B. S. Bahl: Advanced Organic Chemistry. • Nelson, D. L. & Cox, M. M. Lehninger’s Principles of Biochemistry 7th Ed., W. H. Freeman. • Berg, J. M., Tymoczko, J. L. & Stryer, L. Biochemistry 7th Ed., W. H. Freeman. •

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GE – F Lab: Chemistry of f-Block Elements, Bio-inorganic Chemistry, Polynuclear Hydrocarbons and UV, IR Spectroscopy (60 Hours)

Section – A: Inorganic Chemistry

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1. Separation of mixtures by chromatography: Measure the Rf value in each case. (Combination of two ions to be given)

Paper chromatographic separation of Fe3+, A13+ and Cr3+ or

Paper chromatographic separation of Ni2+, Co2+, Mn2+ and Zn2+

2. Gravimetric estimation of Cations/ Anions. Estimation of zinc, aluminium and barium given in ore. Chloride, fluoride and sulphate in given sample.

Section – B: Organic Chemistry

1. Separation of amino acids by paper chromatography 2. Study of titration curve of glycine 3. Effect of temperature on the action of salivary amylase on starch. 4. To determine the saponification value of an oil/fat. 5. To determine the iodine value of an oil/fat 6. Differentiate between a reducing/ nonreducing sugar. 7. Extraction of DNA from onion/cauliflower 8. To synthesize aspirin by acetylation of salicylic acid and compare it with the ingredient of an aspirin tablet by TLC.

Reference Books:

• A.I. Vogel: Qualitative Inorganic Analysis, Prentice Hall, 7th Edn. • A.I. Vogel: Quantitative Chemical Analysis, Prentice Hall, 6th Edn. • A.I. Vogel: Textbook of Practical Organic Chemistry, Prentice Hall, 5th Edn. • F. G. Mann & B. C. Saunders: Practical Organic Chemistry, Orient Longman (1960).

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GE - G: Polymer, Nuclear and Materials Chemistry (Credits: Theory-04, Practicals-02) Theory: 60 Hours Section – A: Polymer Chemistry

Unit – 1: Organic Polymers

Definition of monomers and polymers. Classification of polymers. Different types of processes for polymerization and their mechanisms (ionic, free radical and Ziegler-Natta catalyst). Preparation and uses of some polymers viz., nylons, polyesters, polyvinyl chloride, Teflon, Bakelite, urea and melamineformaldehyde, resins. Natural rubber (isolation, structure and vulcanization). Synthetic elastomers – buna S, butyl rubber and polyurethane. Development of biodegradable polymers viz., polylactic acid and polyhydroxybutyric acid.

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Unit – 2: Inorganic and Physical Polymers

Comparison between inorganic and organic polymers. Synthesis, structural aspects and applications of borazine, silicates and silicones.

Different schemes of classification of polymers. Molar mass of polymers. Number average and mass, average molar masses. Methods of determining molar mass by osmotic pressure and viscosity measurements.

Unit – 3: Mechanisms of Polymerisation

Types of polymers and polymerisation process, addition polymers, stereo controlled polymers, condensation poymers, radical, ionic and coordination mechanism of polymers : (i) Natural and synthetic rubber (ii) synthetic fibres, polyester, polyamides, Polyacrylartes, and rayons. (iii) Plastic: Polyolefines and Polyurethanes (iv) Fooming agent plasaticiser (v) Biodegradable polymers.

Section – B: Nuclear and Materials Chemistry

Unit – 1: Nuclear Forces, Energy and Fuels

Nuclear Forces: Nuclear Radiation, forces in nucleus, nuclear stability, neutron proton ratio and binding energy, packing fraction Nuclear Energy: Energy releasing fission, chain reactions, controlled release of fission energy, use of moderators, energy release in fusion reactions, principle of atomic and hydrogen bombs Nuclear Feuls (Uranium & Thorium): Distribution in nature, production as nuclear fuels, enrichment of uranium, extraction of thorium and uranium from their ores.

Unit – 2: Extraction of Metals and Non-Metals

Techniques and application of extraction of elements from their important ores – bauxite, lime stones other ores of the region.

Unit – 3: Chemistry of Nano-Materials

Nanoscience – principles, structure determination, Synthesis, photo-physical properties and applications of nano particles consisting of gold, silver and iron.

Recommended Texts:

• Principles of Polymer Chemistry, Ravve, A. 2nd ed.,

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• Malcolm P. Stevens, Polymer Chemistry: An Introduction, 3rd ed. Oxford University Press (2005) • Seymour/ Carraher’s Polymer Chemistry, 9th ed. by Charles E. Carraher, Jr. (2013). • Petr Munk and Tejraj M. Aminabhavi, Introduction to Macromolecular Science, 2nd ed. John Wiley & Sons (2002) • Joel R. Fried, Polymer Science and Technology, 2nd ed. Prentice-Hall (2003) • Essentials of Nuclear Chemistry by H. J. Arnikar • Chemistry of Materials by Rao

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GE – G Lab: Polymer, Nuclear and Materials Chemistry (60 Hours)

Section – A: Polymer Chemistry

4. Polymer synthesis

(ix) Free radical solution polymerization of styrene (St)/Methyl Methacrylate (MMA) / Methyl Acrylate (MA) / Acrylic acid (AA). (c) Purification of monomer (d) Polymerization using benzoyl peroxide (BPO)/2,2’-azo-bis-isobutyl-onitrile (AIBN)

(x) Preparation of nylon 66/6 (xi) Interfacial polymerization, preparation of polyester from isophthaloyl chloride (IPC) and phenolphthalein (d) Preparation of IPC (e) Purification of IPC (f) Interfacial polymerization (xii) Redox polymerization of acrylamide (xiii) Precipitation polymerization of acrylonitrile (xiv) Preparation of urea-formaldehyde resin (xv) Preparations of novalac resin/resold resin (xvi) Microscale Emulsion Polymerization of Poly(methylacrylate)

Section – B: Materials Chemistry

 Verification of the Beer-Lambert law using gold/silver nanoparticles.  Metal based nanoparticles are examined by converting p-nitrophenol to p-aminophenol.  Synthesis and characterization of mixed metal oxide (bimetallic and oxides)  Preparation and characterization of nanomaretials by wet chemical routes (sol-gel, reverse micelles, hydrothermal, co-precipitation, etc.)

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Recommended Texts:

• Malcolm P. Stevens, Polymer Chemistry: An Introduction, 3rd ed. Oxford University Press (2005) • Seymour/ Carraher’s Polymer Chemistry, 9th ed. by Charles E. Carraher, Jr. (2013). • Petr Munk and Tejraj M. Aminabhavi, Introduction to Macromolecular Science, 2nd ed. John Wiley & Sons (2002) • Joel R. Fried, Polymer Science and Technology, 2nd ed. Prentice-Hall (2003) • Furniss, B.S.; Hannaford, A.J.; Rogers, V.; Smith, P.W.G.; Tatchell, A.R. Vogel’s Textbook of Practical Organic Chemistry, ELBS. • Pradeep, T. A Textbook of Nanoscience and Nanotechnology, McGraw Hill Edu. New Delhi, (2015).

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Course Structure for M.Sc. CHEMISTRY 1 credit = 1 hour per week for Theory and 2 hours per week for Laboratory Course Course Title of Paper Credit Code Structure SEMESTER-I CHM T 411 Core Catalysis-, Surface-, Electro- Chemistry & Chemical Kinetics 4 CHM T 412 Core Transition and Inner Transition Metal Chemistry 4 CHM T 413 Core Organic Reaction Mechanism and Stereochemistry 4 CHM P 411 Core Inorganic Chemistry Practical - I 2 CHM P 412 Core Organic Chemistry Practical - I 2 Generic/Open Elective Course – I (any one course from GE/OE – I 3 elective section offered by Dept. of Chemistry) SEMESTER-II CHM T 421 Core Quantum-, Statistical-Mechanics, Symmetry & Group Theory 4 CHM T 422 Cora Chemistry of Organmetallics 4 CHM T 423 Core Principle of Organic Synthesis and Organic Spectroscopy 4 CHM P 421 Core Physical Chemistry Practical - I 2 CHM P 422 Core Organic Chemistry Practical - II 2 Generic/Open Elective Course – II (any one course from GE/OE – II 3 elective section offered by Dept. of Chemistry) SEMESTER-III Chemical Bonding, Non-equilibrium Thermodynamics and Solid CHM T 511 Core 4 State Chemistry CHM T 512 Core Bio-Inorganic & Nuclear Chemistry 4 Pericyclic Reaction, Photochemistry and Free Radical CHM T 513 Core 4 Chemistry Discipline Specific Elective Paper – I (any one course from DSE – I 3 elective section offered by Dept. Of Chemistry) CHM P 511 Core Physical Chemistry Practical – II 2 CHM P 512 Core Inorganic Chemistry Practical – II 2 SEMESTER-IV CHM T 521 Core Molecular Spectroscopy 4 Discipline Specific Elective Paper – II (any one course from DSE – II 3 elective section offered by Dept. Of Chemistry) Discipline Specific Elective Paper – III (any one course from DSE – III 3 elective section offered by Dept. Of Chemistry) CHM P 522 Core Project and Dissertation 8 Grand Total (Semester I – IV) 75

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GE: Generic Elective; OE: Open Elective; DSE: Discipline Specific Elective *Generic/Open Elective Course opted by the Other Department students

Elective Course

Course Course Title of Paper Credit Code Structure CHM T 601 Elective Mathematics for Chemist 3 CHMT 602 Elective Biology for Chemist 3 CHM T 603 Elective Industrial Chemistry 3 CHM T 604 Elective Instrumental Methods of Analysis 3 CHM T 605 Elective Basic of Materials Chemistry 3 CHM T 606 Elective Introduction to Nanomaterials and Nanotechnology 3 CHM T 607 Elective Polymers Chemistry 3 CHM T 608 Elective Bioorganic and Drug Chemistry 3 CHM T 609 Elective Advanced Heterocyclic Chemistry 3 CHM T 610 Elective Chemistry of Natural Products 3 CHM T 611 Elective Solid State Chemistry 3 CHM T 612 Elective Advanced Synthetic Organic Chemistry 3

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SEMESTER – I CHM T 411: Catalysis-, Surface-, Electro- Chemistry & Chemical Kinetics Credits: Theory-04 Theory: 60 Hours Unit – 1: Heterogeneous Catalysis

Heterogeneous Catalysis (Surface Reactions): Kinetics of uni-molecular reactions- inhibition and activation energy. Bimolecular surface reactions - reactions between a gas molecule and an adsorbed molecule, reaction between two adsorbed molecules. Effect of temperature on surface reaction promoters and poisons. (10 Hours) Unit – 2: Homogeneous Catalysis Kinetics Homogeneous Catalysis: Nature of surface, concept of active centers. Kinetics of enzymatic reactions: Michaelis-Menten equation, Lineweaver-Burk and Eadie Analyses, enzyme inhibition (competitive, non-competitive and uncompetitive inhibition), effect of temperature and pH of enzymatic reaction; acid – base catalysis and their mechanism. (10 Hours) Unit – 3: Electrochemistry

Electrochemistry of Solution: Debye-Hückel treatment for mean ionic activity coefficient and and its extension, ion solvent interaction and Debye-Hückel-Baerrum model. Thermodynamic of electrified interfaces, electrocapillary measurement of interfacial tension, derivations Lippmann equation (surface excess) and determination of surface excess. Structure of electrified interfaces, Helmholtz-Perrin, Gouy-Chapmann, Stern models, Graham-Devanathan Mottwatts, Tobin, Bockris, Devanathan Models.

Over Potential: Exchange current density, derivation of Butler-Volmer equation, Tofel plot. Quantum aspect of charge transfer at electrodes-solution interfaces, quantization of charge transfer, tunneling.

Corrosion: Introduction to corrosion, homogeneous theory, forms of corrosion, corrosion monitoring and prevention method. (12 Hours) Unit – 4: Surface Chemistry

Surface Tension: Capillary action, pressure difference across curved surface (Laplace equation), vapor pressure of droplets (Kelvin equation), Gibbs adsorption isotherm, estimation of surface area (BET equation), surface film and liquids (electro-kinetic phenomenon), catalytic activities at surface.

Surface Active Agents: Classification of surface active agents. Micellization, hydrophobic interaction, critical micellar concentration (CMC), factor affecting the CMC of surfactants, counter ion binding to micelles, thermodynamics of micellization-phase separation and mass action models, solubilization, micro-emulsion reverse micelles.

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(12 Hours) Unit – 5: Chemical Kinetics

Rate law, method of determining rate laws, General feature of fast reactions, study of fast reaction by flow method, relaxation method, flash photolysis and the nuclear magnetic resonance method.

Reactions in Gas Phase: Theories of Reaction Rates- Arrhenius theory, collision theory and transition state theory, potential energy surface, enthalpy, free energy and entropy of activation, correlation of steric factor in collision theory and entropy of activation (Thermodynamic parameter). Uni-molecular reactions: Lindeman-Hinshelwood theory, Rice-Ramsperger-Kasssel (RRK) theory, Rice- Ramsperger-Kassel- Marcus(RRKM) theory.

Elementary Reactions in Solution: Comparison between gas-phase and solution-phase reactions, factor determining reaction rates in solution; ionic reaction [influence of solvent, influence of ionic strength (salt effect)] ; Linear Free Energy Relationships, (LFER), Effect of substituent on reaction rates (Hammet relationships). Kinetics of isotopic effect.

Dynamic of Molecular Motion: probing the transition state, dynamics of barrier-less chemical reaction in solution.

Chain Dynamic: (hydrogen-bromine reaction, pyrolysis of acetaldehyde, decomposition of ethane), photochemical (hydrogen-bromine and hydrogen-chlorine reaction), and Oscillatory reaction, autocatalysis (Belousov-Zhabotinsky reaction). (16 Hours) Reference Books:

 K. J. Laidler, Chemical Kinetics, Eds: 3rd, Pearson, 2011.  J Rajaram and J. C. Kuriacose: Kinetics and Mechanisms of Chemical Transformations Applications of Femto-chemistry, MacMillan, New Delhi, 2011.  B. R. Puri, L. R. Sharma and M. S. Pathania: Principle of Physical Chemistry, Eds. 44th, Vishal Publishing Co., Jalandhar, 2010.  P. Atkins and J. D. Paula: Physical Chemistry, Eds. 7th, Oxford University Press, New Delhi, 2002.  R. S. Berry, S. A. Rice and J. Ross: Physical Chemistry, Eds: 2nd, Oxford University Press, New Delhi, 2007.  J. O’M Bockris, A. K. N. Reddy and M. Gamboa-Aldeco: Modern Electrochemistry Vol- 1 and Vol-2, Springer, 2006.  D. R Crow: Principles and Applications of Electrochemistry, Eds. 4th, Blackie Academic & Professional, Madras, 1994.  V. S. Bagotsky: Fundamental of Electrochemistry, Wiley-Interscience, 2006.

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CHM T 412: Transition and Inner Transition Metal Chemistry

Credits: Theory-04 Theory: 60 Hours Unit – 1: Coordination Chemistry

Experimental evidence of metal-ligand overlap, spin orbit coupling constant and interelectronic coupling parameters in complex ion terms-vs-free ion terms, Nephelauxetic effect, d-orbital splitting in octahedral, Jahn-Teller distortd octahedral, square planar, square pyramidal, trigonal bipyramidal, and tetrahedral complexes, CFSE for d1 to d10 systems, pairing energy, low-spin and high-spin complexes and magnetic properties, Crystal field activation energy, hole formalism, Tetrahedral distortion and Jahn Teller effect, Static and Dynamic Jahn-Teller effect, Effect of crystal field stabilization on ionic radii, lattice energy, hydration enthalpy and stabilization of complexes (Irving Williams order). Colour and spectra, Kinetic aspects of crystal field stabilization. adjusted CFT, Limitations of CFT, Labile and inert complexes. (12 Hours) Unit – 2: Electronic Spectra of Transition Metal Complexes

Microstates, Russell-sander’s terms, determination of ground and excited state terms of dn ions; Orgel diagrams (qualitative approach) and Tanabe-Sugano diagram, selection rules for spectral transitions, d-d spectra of dn ions and crystal field parameters, nephelauxetic series, Electronic Spectra UV-Vis, charge transfer, colors, intensities and origin of spectra. MOT to rationalize σ and π interactions in octahedral, square planar and tetrahedral metal complexes. Symmetry designations of LGOs and MOs. Simplified MO diagrams. (12 Hours) Unit – 3: Magneto Chemistry

Basic principles of magnetism, Magnetic properties, paramagnetism, ferro- and antiferro magnetism, diamagnetism, Pascal constants, Currie equation, determination of magnetic susceptibility, application of Van Vleck susceptibility equation, Magnetic properties and coordination compounds Spin and orbital moments, spin – orbit coupling, quenching of orbital moment, spin only formula, room temperature and variable temperature magnetic moments and spin crossover. Magnetic properties of first transition series metal ions, lanthanides and actinides, Lanthanide and actinide contractions and their consequences, separation of lanthanides and actinides and their applications (examples). magnetic exchange interactions. ESR spectroscopy, Basic concept of Single Molecule Magnets (SMM), properties, examples and application of SMMs. (12 Hours)

Unit – 4: Inorganic Reaction Mechanism Mechanism of substitution reactions, solvent exchange, aquation, anation, base hydrolysis, acid catalyzed aquation, pseudo-substitution. Energy profile diagram of ligand substitution reactions- associative (A), dissociative (D), interchange (I) etc. type pathways, relation between intimate and stoichiometric mechanisms of ligand substitution, some important rate laws, activation parameters (∆S#, ∆H#, ∆V#), mechanism of isomerization reaction-linkage isomerism, cis-trans

120 | P a g e isomerism, intramolecular and intermolecular racimization, Ray-Dutta and Bailar twist mechanisms, substitution in octahedral complexes- the Eigen-Wilkins mechanism, the Fuoss- Eigen equation, linear free energy relation (LFER) etc. Mechanism of electron transfer reactions: General characteristics and classification of redox reactions, self-exchange reactions. Frank- condon principle (non mathematical treatment). Outer sphere and Inner sphere reactions, applications of Marcus expression (simple form), redox catalyzed substitution reactions. (12 Hours) Unit - 5: Chemistry of Elements d-Block Elements: Electronic configuration, oxidation states; aqueous, redox and coordination chemistry, spectral and magnetic properties of compounds in different oxidation states, horizontal and vertical trends in respect of 3d, 4d, and 5d elements with references to Ti-Zr- Hf , V-Nb-Ta, Cr- Mo- W, Mn-Tc-Re and Pt group metals. Occurrence and isolation in respect of V, Mo, W, Re, Pt. Iso-and heteropolyoxometalates with respect to V, Mo, and W: synthesis, reactions, structures, uses, metal-metal bonded dinuclear d-metal complexes (examples), Bonding in dirhenium complexes. Qualitative Analysis of Inorganic Radicals Introduction to salt analysis, dry and wet test for acid and basic radicals, Principle and chemistry of qualitative analysis of inorganic salt; chemistry involved in qualitative analysis of mixture containing interfering radicals and insolubles.

(12 Lectures) Reference Books:

 J. D. Lee: A new Concise Inorganic Chemistry, E L. B. S.  D. F. Shriver and P. W. Atkins: Inorganic Chemistry, Oxford University Press.  Douglas, McDaniel and Alexander: Concepts and Models in Inorganic Chemistry, John Wiley.  B. R. Puri, L. R. Sharma, and K. C. Kalia: Principle of Inorganic Chemistry, Milestone Publisher, New Delhi 2010.  W. U. Malik, G. D. Tuli, and R. D. Madan: Selected Topic in Inorganic Chemistry, S. Chand & Company Ltd, New Delhi, 1998.  J. E. Huheey, E. A. Keiter, R. L. Keiter, and O. K. Medhi: Inorganic Chemistry Principle of Structure and Reactivity, Eds: 4th Pearson, New Delhi, 2006.  F. A Cotton, G. Wilkinson, C. A. Murillo, and M. Bochmann: Advanced Inorganic Chemistry, Eds: 6th, Wiley-India, New Delhi, 2010.

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CHM T 413: Organic Reaction Mechanism and Stereochemistry

Credits: Theory-04 Theory: 60 Hours Unit – 1: Physical Organic Chemistry

(i) Thermodynamic and kinetic requirements of a reaction: Transition state theory, Hammond’s postulate, Kinetic vs Thermodynamic control (ii) Acids and Bases (iii) Determining the mechanism of a reaction: Detection and trapping of intermediates, Cross-over experiments, kinetic isotopic effect-primary kinetic and secondary kinetic isotopic effect (12 Hours)

Unit – 2: Substitution, Addition, and Elimination Reactions

Substitution Reaction: Aliphatic nucleophilic substitution- SN1, SN2, SNi mechanism, classical and nonclassical carbocations, phenonium ions, NGP-in substation reactions. Effect of solvent, structure, nucleophile and leaving group on rate of SN1, and SN2 reaction. Electrophilic aromatic substitution and Nucleophilic aromatic substitutions. Mechanism and stereo chemical aspects of substitution reactions. Addition Reaction: Addition to carbon-carbon multiple bonds, addition to carbon-heteroatom multiple bonds, electrophilic, nucleophilic and free radical addition reactions. Mechanism and stereo chemical aspects of addition reactions. Elimination Reaction: E1, E2, E1cb mechanisms, orientation and stereochemistry in elimination reaction, reactivity effect of structure, attacking and leaving group, competition between elimination and substitution, syn-eliminations. (14 Hours)

Unit – 3: Symmetry Operation and Stereoisomerism

Simple or proper axis of symmetry, plane of symmetry, centre of symmetry and improper or rotation-reflection of symmetry. Enantiomerism and diastereomerism, conventions for configurations D-L and R-S systems, Threo and erythro nomenclature. Measurement of optical purity, enantiomeric excess. Stereoselective and Stereospecific reactions. Molecules with tri- and tetra coordinated chiral centres. Molecules with two or more chiral centres. (12 Hours)

Unit – 4: Chirality and Conformations

Axial and Planar Chirality: Principles of axial and planar chirality. Stereochemistry of allenes, Stereochemistry of biphenyl derivatives and atropisomers. Stereochemistry of spiranes, Stereochemistry of molecules with planar chirality, Helicity.

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Conformations & Stereoisomerism of Acyclic and Cyclic Systems: Molecular mechanics and conformations, Conformations of a few acyclic molecules, Conformations of cyclic systems: monocyclic compounds (mono, di- and poly substituted cyclohexanes); Conformations of fused ring and bridged ring compounds. (10 Hours)

Unit – 5: Dynamic Stereochemistry

Conformation and Reactivity: Conformation, reactivity and mechanism: Cyclic systems (Nucleophilic substitution reaction at ring carbon, Addition reaction to double bonds, Elimination reactions, NGP reactions). Conformation, reactivity and mechanism: Acyclic systems (addition, Elimination and NGP participation). Formation and reaction of enols and enolates. Reduction of cyclohexanes with hydride reagents.

Stereoselective Reactions: Principle of stereoselectivity, asymmetric synthesis and asymmetric induction, Acyclic stereoselections (addition of nucleophiles to carbonyl compounds, aldol reactions, addition to allyl metal and allyl boron compound to carbonyl compounds), Diastereoselections in cyclic systems (Nucleophilic addition to cyclic ketones, alkylations, catalytic hydrogenations). (12 Hours)

Reference Books:

 J. Clayden, N. Greeves, S. Warren and P. Wothers: Organic Chemistry, Oxford  J. March: Advanced Organic Chemistry, 6th Edition  A. Carey and R.J. Sundberg: Advance Organic Chemistry (part A)  Paula Y Bruice: Organic Chemistry  E.L. Eliel: Stereochemistry of carbon compound  Nasipuri: Stereochemistry of organic compound  Peter Sykes: Guide book to Reaction Mechanism

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CHM P 411: Inorganic Chemistry Practical – I Credits: 02 Lab: 60 Hours A. Qualitative Analysis Semi-micro qualitative analysis of mixture containing eight radicals including two less common metal from among the following: (1) Basic Radicals: Ag+, Pb2+, Bi3+, Cu2+, Cd2+, As3+, Sb3+, Sn4+, Fe3+, Al3+, Cr3+, Zn2+, Mn2+, Co2+, Ni2+, Ba2+, Sr2+, Ca2+, Mg2+, Ce3+, Th4+, Zr4+, W6+, Te4+, Ti4+, Mo6+, V5+, Be2+. (2) Acid Radicals : Carbonate, Sulphite, Sulphide, Nitrite, Nitrate, Acetate, Fluoride. Chloride, Bromide, Iodide, Sulphate, Borate, Oxalate, Phosphate, Silicate, Thiosulphate, Ferrocyanide, Ferricyanide, Thiocyanide, Chromate, Arsenate and Permanganate.

B. Chromatographic Separation

 Use paper chromatography to separate and identify the metal ion components of an unknown solution.  Chromatographic separation of sugars, amino acids by paper, T.L.C. and Ion exchange.

C. Standard Deviation

 Calculation of standard deviation from the results obtained by redox titration of Fe(III) against standard solution of K2Cr2O7.  Calculation of standard deviation from the results obtained by complexometry method of hardness (Ca2+) of water using EDTA.

Reference Books:

 A.I. Vogel: Qualitative Inorganic Analysis, Prentice Hall, 7th Edn.  A.I. Vogel: Quantitative Chemical Analysis, Prentice Hall, 6th Edn.  B.D. Khosla: Senior Practical Physical Chemistry, R. Chand & Co.  P. C. Comboj: University Practical Chemistry, Vishal Publishing Co. Jalandhar.

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CHM P 412: Organic Chemistry Practical – I Credits: 02 Lab: 60 Hours Part A: Techniques of Separation and Purification

 Fractional Distillation of a mixture of liquids  Distillation under reduced pressure  Chromatographic separation (Paper chromatography and Thin Layer Chromatography)

Part B: Analysis of Organic Binary Mixture

 Separation and Identification of organic compounds from the given binary mixtures. (Complete study of determination of organic compound with melting point and preparation of a suitable derivative) Part C: Preparation of Organic Compounds (Single Stage Preparation) Representative reactions to be covered:

 Electrophilic aromatic substitution reaction (Friedel-Crafts Reaction, halogenation, nitartion and sulphonation reaction)  Acetylation reaction  Diels-Alder reaction  Condensation reaction  Cannizzaro reaction  Oxidation reaction  Reduction reaction  Rearrangement reaction  Esterification  Diazotization reaction  Sandmeyer reaction

Reference Books:

 A. I. Vogel: Practical Organic Chemistry  F. G. Mann and B. C. Saunders: Practical Organic Chemistry  J. Leonard, B. Lygo and G. Proctor: Advanced Practical Organic Chemistry.  Addison Ault: Techniques and Experiments for Organic Chemistry, University Science Book  R. L. Shriner and D. Y. Curtin: The Systematic Identification of Organic Compounds  B. S. Roa and V. Deshpande: Experimental Biochemistry, I. K. Pvt. Ltd.  V. K. Ahluwalia and Renu Aggarwal: Comprehensive Practical Organic Chemistry, Preparation and Qualitative Analysis  Ghoshal, Mahapatra and Nad: An Advanced Course in Practical Chemistry.

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SEMESTER – II

CHM T 421: Quantum-, Statistical- Mechanics, Symmetry & GroupTheory

Credits: Theory-04 Theory: 60 Hours Unit – 1: Quantum Chemistry – I

Historic Background: Important historic background of quantum mechanics versus classical mechanics, wave particle duality, Heisenberg’s uncertainty principle.

Schrödinger Wave Equation: normalization and orthogonality of wave functions; time- dependent and time-independent Schrödinger equations.

Operators: Operators and their algebra, linear and Hermitian operators, matrix representation, commutation relationship, quantum mechanical operators for position, linear momentum, angular momentum, total energy, eigenfunctions, eigenvalues and eigenvalue equation; expansion of arbitrary state in term of complete set, postulates of quantum mechanics. Solution of the Schrödinger Equations for Some Exactly Soluble Systems: particle-in-a-box; particle-in-a-ring and -sphere; harmonic oscillator; tunneling one dimensional potential barrier and well. (12 Hours) Unit – 2: Quantum Chemistry – II

Rigid Rotor, spherical coordinates Schrödinger wave equation in spherical coordinates, separation of the variables, the phi equation, wave-function, quantum number, the theta equation, wave function, quantization of rotational energy, spherical harmonics.

Hydrogen and Hydrogen Like Atoms: Radial and angular probability distributions, atomic orbitals.

Angular Momentum: Basis functions and representation of orbital angular momentum operators, eigenfunctions, and eigenvalues of orbital angular momentum operator, Ladder operator, Spin, spin angular momenta, coupling (orbital and spin) of angular momentum, Clebsch-Gordan coefficients and Wigner Eckart theorem.

Approximate Methods of Quantum Mechanics: Variational principle; time-independent perturbation theory up to second order in energy for non-degenerate and degenerate system with simple examples; application to the two electron system such as, He and He like atoms.

(12 Hours) Unit – 3: Atomic Structure and Spectroscopic

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Many electron atoms, Pauli antisymmetry principle, Hund’s rules; Slater determinant; Hatree and Hatree-Fock self consistent field model for atom; electronic term symbol (Russell-Saunders and jj coupling) for atoms and spectroscopic states (selection rules for atomic spectra). (12 Hours) Unit – 4: Statistical Thermodynamics

Concept of distribution, thermodynamic probability and most probable distribution. Ensemble averaging, postulates of ensemble averaging; conical, grand conical and micro-canonical ensembles. Boltzmann distribution laws (using Lagrange’s method of undetermined multipliers). Partition function – translational, rotational, vibrational and electronic partition functions, calculation of thermodynamic properties in term of partition function, Applications of partition functions.

Heat capacity behavior of solid – chemical equilibria and equilibrium constant in term of partition function. Fermi-Dirac statistics, distribution law and application to metal, Bose-Einstein statistics, distribution law and application to helium.

(12 Hours) Unit – 5: Symmetry & Group Theory Symmetry elements and symmetry operations; point groups, Schoenflies notation for point group, representation of group by matrix, character of a representation, reducible and irreducible representation, great orthogonality theorem and its importance. Application of group theory to atomic orbitals in ligand fields, molecular orbitals, and hybridization. Selection rules for IR and Raman spectra, procedure for determining symmetry of normal modes of vibration - hybrid orbitals in BF3, CH4, NH3, H2O and SF6. (12 Hours) Reference Books:

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CHM T 422: Chemistry of Organometallics

Credits: Theory-04 Theory: 60 Hours

Unit – 1: Organometallics – I Organo transition metal chemistry: History, Nature of metal – carbon bonding and definition and classification of organometallic compounds, classification ligands, kinetic and thermodynamic stability of organometallic compounds. Compounds with metal carbon σ and multiple bond: Heptacity complexes of Metal-alkyl, -allyl, aryl, -carbene (Fischer and Schrock type), -carbonyl, -carbines and cyclopentadienyl complexes Synthesis, bonding, stability, reactivity and decomposition pathway, Reactions in organometallic compounds. Stucture and bonding in η2- ethylenic and η3-allylic compounds with typical examples, structure and bonding of

K[Pt(C2H4)Cl3], [(Ph3P)2Pt(Ph-C≡C-Ph)]. Fluxional organometallic compounds: Fluxionality and dynamic equilibria in compounds such as η2 olefins, η3 allyl and dienyl complexes, techniques of study. (12 Hours) Unit – 2: Organometallics – II Reactions of organometallic complexes: substitution, oxidative addition, reductive elimination, insertion and elimination, electrophilic and nucleophilic reactions of coordinated ligands. Catalysis by organometallic compounds: Hydrogenation of olefins, Wilkinson’s catalyst, Tolman catalytic loop; synthesis gas, water-gas shift reaction; Hydroformylation (oxo process), Monsanto acetic acid process, Wacker process; synthetic gasoline: Fischer-Tropsch process and Mobile process, polymerization, oligomerization and metathesis reactions of alkens and alkynes, Zieglar- Natta catalysis, photo dehydrogenation catalyst (platinum POP). (12 Hours) Unit – 3: Inorganic Rings, Cages and Clusters Polymorphism of C, P and S. Structure and bonding in higher boranes and borohydrieds- Lipscomb’s topological models, Wade`s rules, carboranes and metallocenecarboranes. Metal-metal bonding (M.O. Approach), metal-metal single and multiple bonded compounds.

Low nuclearity (M3, M4) and high nuclearity (M5-M10) carbonyl clusters: skeletal electron counting, Wade-Mingos-Louher rule, Application of isolobal and isoelectronic relationships, Nb and Ta clusters, Mo and W clusters. Cluster compounds in catalysis. (12 Hours) Unit – 4: New Developments in Organometallics Chemistry Research

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Construction, structure and property of compounds with specific topology in Organometallic Chemistry: Capsules, boxes, containers, prisms or clusters, tubes, catenanes, rotaxanes, incorporation of metal atoms through metal-ligand coordination interactions, Various organic ligands containing carboxy, imidazole or pyridine groups, which can coordinate with metal atoms, have been used to generate the desired compounds (V, Cr, Mn, Fe, Co, Ni, Cu). Particularly, flexible ligands with central aromatic core and imidazol-1-ylmethyl pendant arms, e.g. 1,3,5-tris(imidazol-1-ylmethyl)-2,4,6-trimethylbenzene and its analogues, Interesting properties: olecular recognition, ion inclusion and exchange of these compounds, especially of the cage-like compounds, are described. (12 Hours) Unit – 5: Metal – ligand equilibria in solution Stability of mononuclear, polynuclear and mixed ligand complexes in solution. Stepwise and overall formation constants and their relations. Trends in stepwise formation constants, factors affecting the stability of metal complexes with reference to the nature of the metal ions and ligands. Statistical and non-statistical factors influencing stability of complexes in solution. Stability and reactivity of mixed ligand complexes with reference to chelate effect and thermodynamic considerations. Macrocyclic and template effect. Spectrophotometric and pH metric determination of binary formation constants. (12 Hours) Reference Books:

 J. E. Huheey, E. A. Keiter, R. L. Keiter, and O. K. Medhi: Inorganic Chemistry Principle of Structure and Reactivity, Eds: 4th Pearson, New Delhi, 2006.  F. A Cotton, G. Wilkinson, C. A. Murillo, and M. Bochmann: Advanced Inorganic Chemistry, Eds: 6th, Wiley-India, New Delhi, 2010.  D. F. Shriver and P. W. Atkins: Inorganic Chemistry, Oxford University Press.  Douglas, McDaniel and Alexader: Concepts and Models in Inorganic Chemistry, John Wiley.  Robert Crabtree: The Organometallic Chemistry of the Transition Metals, 3rd Edition, Wiley.  Collman, Hegedus, Norton and Finke: The Principles and Applications of Transition Metal Chemistry, 2nd Eds, University Science Books.  Christoph Elschenbroich: Organometallics, 3rd Edition,  Wei-Yin Sun, New Developments in Organometallics Chemistry, Wiley

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CHM T 423: Principle of Organic Synthesis and Organic Spectroscopy

Credits: Theory-04 Theory: 60 Hours Unit – 1: Principles of Organic Synthesis

Acid Catalyzed Carbon-Carbon Bond Formation Reaction: Principles, Self condensation of alkenes, reactions of aldehydes and ketones, Friedel-Crafts reactions, Prins reaction and Maanich reaction and Nef Reaction. Base Catalyzed Reactions (Enolate Chemistry): Enolates: structure and stability of enolates, Generation of enolates using Nucleophilic and non Nucleophilic bases. Kinetic and Thermodynamic control of regioselectivity of enolates, Reactions of enolates. Alkylation and acylation of enolates: Haloform reaction, HVZ reaction, Claisen condensation, Enolate of active methylene compounds and corresponding alkylation reactions, Michael addition, Robinson annulations reaction. (12 Hours) Unit – 2: Rearrangement and Organometallic Reactions

Rearrangement Reactions: Demjanov, Pummerer, Dienone-phenol rearrangement, Pinacol- Pinacolone rearrangement, Fries rearrangement,Wagner-Meerwein Rearrangement, Benzil- Benzilic Acid Rearrangement, Beckmann Reaction, Curtius, Schmidt, Lossen, Hoffman and Claisen rearrangement. Brook, Favorski, Neber, Von Richter, Sommelet Hauser and Wittig rearrangement. Organometallic Reagents: Organomagnesium and Lithium reagents (Preparations, uses and applications), uses of Organomercury, organocadmium, organozinc and organocopper compounds.

(12 Hours) Unit – 3: Ultraviolet and Infrared Spectroscopy

Ultraviolet Spectroscopy: Factors affecting the position and intensity of UV bands – effect of conjugation, steric factor, pH, solvent polarity. Calculation of absorption maxima by Woodward- Fieser Rules (using Woodward-Fieser tables for values for substituent’s) for the following classes of organic compounds: conjugated polyenes (cyclic and acyclic), enones and substituted benzene derivatives.

Infrared Spectroscopy: Fundamental, overtone and combination bands, vibrational coupling, important group frequencies for the common functional groups.

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Unit – 4: Nuclear Magnetic Resonance and Mass Spectroscopy

Nuclear Magnetic Resonance Spectroscopy: Chemical shift, Factors affecting chemical shift, Chemical and magnetic equivalence, Spin-spin coupling, Coupling constant J, Factors affecting J, Karplus equation, First order spectra, Geminal, vicinal and long range coupling (allylic and aromatic). 13C NMR, Heteronuclear coupling, 2D NMR spectroscopy. Mass Spectrometry: Molecular ion peak, base peak, isotopic abundance, metastable ions. Nitrogen rule, Determination of molecular formula of organic compounds based on isotopic abundance and HRMS Fragmentation pattern in various classes of organic compounds (including compounds containing hetero atoms), McLafferty rearrangement, Retro-Diels-Alder reaction, ortho effect.

(14 Hours) Unit – 5: Structure Determination of Organic Compounds

Structure determination involving individual or combined use of the above spectral techniques. (10 Hours)

Reference Books:

 J. Clayden, N. Greeves, S. Warren and P. Wothers: Organic Chemistry, Oxford  A. Carey and R.J. Sundberg: Advance Organic Chemistry (Part B).  Parikh, Parikh and Parikh: Name reactions in Organic Synthesis, Foundation Books, 2006.  G. Brahmachari: Organic Name Reactions, Narosa Publishers, 2009.  J. J. Li: Name reactions in organic synthesis, 3rd Edition, SPRINGER 2006.  Bessler and Silverstein: Spectroscopy of Organic Compounds, JOHN WILEY, 2001.  D. C. Pavia, G. M. Lampman, G. S. Kriz: Introduction to Spectroscopy, 3rd Edition, Thomson, 2007.  William Kemp: Organic Spectroscopy, III Edition

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CHM P 421: Physical Chemistry Practical – I Credits: 02 Lab: 60 Hours

(i) Chemical Kinetics (a) Kinetics of Reaction between ferric nitrate and potassium iodide using initial reaction rates. (b) Determination of the rate constant for the decomposition of hydrogen peroxide by Fe3+ and Cu2+ ions. (c) Flowing clock reactions (Experiments in physical Chemistry by Shoemaker).

(ii) Determination of CMC of the surfactant/CMC Concentration.

(iii) Determination of partial molal volume.

(iv) Determination of the isotherm for a three component system.

(v) (a) Spectrophotometric determination of acid dissociation constant. (b) Formula and stability constant using spectrophotometry.

Reference Books:

 A. M. James and F. E. Prichard: Practical Physical Chemistry, Longman.  B. P. Levi: Findley’s Practical Physical Chemistry,  R. C. Das and B. Behera: Experimental Physical Chemistry, Tata McGraw Hill.  D. P. Shoemaker, G. W. Garland and J. W. Niber: Experimental Physical chemistry, Mc Graw Hill Interscience.  A. J. Elias: A collection of Interesting General Chemistry Experiments, University Press, India.  J. Rose: Advanced Physico-Chemical Experiments, Sir Isaac Pitman & Sons Ltd, London.  J. B. Yadav: Advanced Practical Physical Chemistry, Krishna Prakashan Media (P) Ltd. Meerut.  P. C. Comboj: University Practical Chemistry, Vishal Publishing Co. Jalandhar.

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CHM P 422: Organic Chemistry Practical – II Credits: 02 Lab: 60 Hours Part A: Multi Step Synthesis of Organic Compounds Multi step organic synthesis involving the concept of protecting groups and selectivity in organic reaction. A Student must be involved to check TLC for monitoring the reaction progress and doing column chromatography for purification. Characterization of synthesized organic compoundsusing IR, UV and NMR, and mass spe ctroscopic techniques are to be studied.

 Nitrobenzene→aniline→Acetanilide (Nitration and followed by reduction)  Malonic acid→cinnamic acid→methyl cinnamate (Condensation reaction and next followed by esterification)  Benzaldehyde→benzoin→benzil→benzilic acid (Umpolung strategy, Oxidation reaction and next benzylic acid rearrangement reaction)  Aniline→benzenediazonium chloride→benzeneazo-2-naphthol (Azodye synthesis)  Skraup’s synthesis: Quinoline from o-aminophenol (Heterocyclic compound synthesis)  Acetanilide→p-acetamidobenzenesulfonylchloride→p- acetamidobenzenesulfonamide→sulfanilamide (Sulfa Drug synthesis)  cinnamaldehyde→cinnamyl alcohol→cinnamyl bromide→allyl-aryl ether synthesis (Nucleophilic substitution reaction)

Part B: Extraction Method

 Natural product extraction: Solasidine, Caffeine, Nicotine, Peptine, Rosine, Carotenoids, Computational methods of retro-synthetic analysis modeling and calculation.

Reference Books:

 A. I. Vogel: Practical Organic Chemistry  F. G. Mann and B. C. Saunders: Practical Organic Chemistry  J. Leonard, B. Lygo and G. Proctor: Advanced Practical Organic Chemistry  Addison Ault; Techniques and Experiments for Organic Chemistry, University Science Book  R. L. Shriner and D. Y. Curtin: The Systematic Identification of Organic Compounds  B. S. Roa and V. Deshpande: Experimental Biochemistry, I. K. Pvt. Ltd.  V. K. Ahluwalia and Renu Aggarwal: Comprehensive Practical Organic Chemistry, Preparation and Qualitative Analysis  Nad, Mahapatra and Ghoshal: An Advanced Course in Practical Chemistry

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SEMESTER – III

CHM T 511: Chemical Bonding, Non-equilibrium Thermodynamics and Solid State Chemistry Credits: Theory-04 Theory: 60 Hours Unit – 1: Molecular Structure

Chemical bonding in diatomic; elementary concepts of MO and VB theories; Born-Oppenheimer + approximation, MO treatment for H2 ion, MO treatment of homo- and heteronuclear diatomic molecules; comparison of MO and VB theories. Hückel MO theory for conjugated -systems. Polyatomic molecules, hybridisation and valence MOs of simple molecule like H2O, NH3, CH4, C2H6 etc.

(12 Hours) Unit – 2: Ab-initio Methods for Closed Shell Systems

Introductory treatment of semi-empirical and ab-initio calculations on molecular systems; the Hartree-Fock Self-Consistent Field Method; the generation of optimized orbitals, Koopman’s theorem (The Physical Significance of Orbital Energies), electron correlation energy; density matrix analysis of the Hartree-Fock approximation, natural orbitals, matrix solution of the Hartree-Fock equations (Roothaan’s equations); Hellman-Feynman theorem.

(12 Hours) Unit – 3: Thermodynamics

Brief resume of concepts of laws of thermodynamics, free energy, chemical potential, and entropies. Thermodynamics of open systems: partial molal properties, partial molal free energy, partial molal volume and partial molal heat content and their significances. Determination of these quantities. Concept of fugacity and determination of fugacity. Non-ideal system: excess function for non ideal solutions. Activity, activity coefficient, Debye- Hückel theory for activity coefficient of electrolytic solution; determination of activity and activity coefficients; ionic strength.

(12 Hours) Unit – 4: Non-equilibrium Thermodynamics

Thermodynamic criteria for non-equilibrium state, entropy production and entropy flow, energy balance equation for different irreversible processes (e.g. heat flow, chemical reaction etc.), transformation of the generalized fluxes and forces, non equilibrium stationary states, phenomenological equation, microscopic, reversibility and Onsager’s reciprocity relations, electrokinetic phenomena, diffusion, electric conduction, irreversible thermodynamics for biological system, coupled reactions.

(12 Hours)

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Unit – 5: Solid State Chemistry

Perfect and imperfect crystals, intrinsic and extrinsic defect, point defect, line and plane defect, vacancies, Schottky and Frankel defects; thermodynamics of Schottky and Frankel defect formation, color center, non-stochiometry defects. Metal insulators and semiconductors, electronic structure of solids-band theory, band structure of metals, insulators and semiconductors, doping semi-conductors, p-n junction; superconductors; photoelectric effects; magnetic properties. Behaviour of substances in a magnetic field, effect of temperature: Curie and Curie-Weiss law, origin of magnetic moment, ferromagnetic, antiferromagnetic and ferromagnetic ordering, super exchange, magnetic domains, hysteresis.

(12 Hours) Reference Books:

 Ira. N. Levine: Quantum Chemistry, Eds: 5th, PHI, 2000.  A. K. Chandra: Introductory Quantum Chemistry, Eds: 4th, Tata McGraw Hill, New Delhi, 1994.  P. Atkins and R. Friedman: Molecular Quantum Mechanics, Eds: 5th, Oxford University Press, 2011.  T. Engle and P. Reid: Quantum Chemistry and Spectroscopy, Pearson, New Delhi, 2011.  B. R. Puri, L. R. Sharma and M. S. Pathania, Principle of Physical Chemistry, Eds. 44th, Vishal Publishing Co., Jalandhar, 2010.  P. Atkins and J. D. Paula, Physical Chemistry, Eds. 7th, Oxford University Press, New Delhi, 2002.  R. S. Berry, S. A. Rice and J. Ross: Physical Chemistry, Eds: 2nd, Oxford University Press, New Delhi, 2007.  S. R. Degroot, P. Mazur: Non-Equilibrium Thermodynamics, North Holland Publication, Amsterdam, 1961.  C. N. R. Rao and J. Gopalakrishnan: New Direction in Solid State Chemistry, Cambridge University Press, 1997.  A. R. West: Solid State Chemistry and Its Applications, John Wiley & Sons, 1989.  L. Smart and E. Moore: Solid State Chemistry, Chapman and Hall, 1992.

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CHM T 512: Bio-Inorganic & Nuclear Chemistry

Credits: Theory-04 Theory: 60 Hours Unit – 1: Bio-inorganic Chemistry – I

Transport and storage of dioxygen: Active site structures and bio functions of O2-uptake proteins: hemoglobin, myoglobin, hemocyanin and hemerythrin; model synthetic dioxygen complexes. Chelato theraphy. Electron transfer in biology: Active site structures and functions of cytochromes, cytochrome c; iron-sulfur proteins (rubredoxin, ferredoxines), organic-redox protein cofactors – FAD, NAD, FMN, ubiquinone; blue copper proteins, HIPIP. Respiratory electron transport chain, cytochrome c oxidase. Photosynthesis and chlorophylls, photosystem-I and photosystem-II and their roles in cleavage of water. Model systems. Biological and abiological nitrogen fixing systems, model study. (12 Hours) Unit – 2: Advanced Bio-inorganic Chemistry – II Metal ion interactions with purine and pyrimidine bases, nucleosides, nucleotides and nucleic acids, DNA and RNA, metal ions in genetic information transfer. Redox enzymes: Catalase, peroxidase, super oxide dismutase (SOD), cytochrome P-450, Nitrogen cycle enzymes: NOx reductases, nitric oxide synthases (NOS), ascorbate oxidase, aldehyde oxidase, sulfite oxidase, xanthine oxidase, nitrogenase, P and M clusters in nitrogenase, transition metal dinitrogen complexes and insights into N2 binding, reduction to ammonia. (12 Hours) Unit – 3: Enzymes

Zinc enzymes, magnesium enzymes, iron enzymes, carbonic anhydrase, xanthine oxidase, aldehyde oxidase, cobalt containing enzymes, Mo and tungsten enzymes, Vitamin B-12 Zinc in Transcription: Zinc fingers, zinc thiolate clusters. Calcium Signaling Protein: Calmodulin protein and Ca2+ ion pump Biological Cycle: Nitrogen cycle, hydrogen cycle, in vivo and vitro nitrogen fixation Sensors: Iron protein as sensor, Copper sensor, protein that sense copper and zinc level Other Application: Biominiralization, cancer treatment, antiarthristis drugs Contribution of Individual Elements in Biological Function: Na, K, Li, Mg, Ca, Se, Mn, Fe, Co, Ni, Cu, Zn, Mo, W, Si, Pt, Au (12 Hours) Unit – 4: Inorganic Photochemistry

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Introduction to inorganic photochemistry, photophysical and photochemical process. Excitation modes in transition metal complexes, fate of photo-excited species, fluorescence and phosphorescence applied to Inorganic systems, intramolecular energy transfer, vibrational relaxation, internal conversion and intrasystem crossing, quantum yield, decay fluorescence. Fluorence quenching, Stern-Volmer equation. Photochemical process: photo substitution and photoelectron transfer reactions in Co, Cr, Ru and Rh complexes. (12 Hours)

Unit – 5: Nuclear Chemistry & Radiochemical Analysis Nuclear models: Nuclear stability, terrestrial abundance and distribution, relativistic effect, electronic configuration, oxidation states, aqueous-, redox- and complex- chemistry; Nuclear forces, liquid drop model, shell model, Fermi gas model; magic numbers, nuclear spin and nuclear isomerism. Nuclear reactions: Energetics, mechanism and models of nuclear reactions. Nuclear fission and nuclear fusion, fission products and fission yields. Interactions of radiation with matters, chemical effects of nuclear transmutation (elementary idea), Nuclear reactors and particle accelerators. Radioactive Techniques: Detection and measurement of radiation- GM ionization and proportional counters. Study of chemical reactions by tracer techniques, isotope exchange and kinetic isotope effect. Radiometric analysis: Isotope dilution analysis, age determination, neutron activation analysis (NAA) and their applications. Radiation hazards and safety measures.

(12 Hours) References Books:

 S. J. Lippard and J. M. Berg: Principles of Bioinorganic Chemistry, University Science Books, Mill Valley, 1994.  W. Kaim and B. Schwederski: Bioinorganic Chemistry: Inorganic Elements in the Chemistry of Life, John Wiley & Sons Inc., 1994.  D. F. Shriver and P. W. Atkins: Inorganic Chemistry, Oxford University Press.  B. R. Puri, L. R. Sharma, and K. C. Kalia: Principle of Inorganic Chemistry, Milestone Publisher, New Delhi 2010.  D. L. Nelson, & M. M. Cox: Lehninger’s Principles of Biochemistry 7 Ed., W. H. Freeman  H. J. Arnikar, Essential of Nuclear Chemistry, Wiley-Blackwell; 2nd Edition edition.  Hand Book of Nuclear Reactions, edited by Vértes, A., Nagy, S., Klencsár, Z., Lovas, R.G., Rösch, F. , Springer  J. E. Huheey, E. A. Keiter, R. L. Keiter, and O. K. Medhi: Inorganic Chemistry Principle of Structure and Reactivity, Eds: 4th Pearson, New Delhi, 2006.  A. Das and G. N. Mukherjee, Elements of Boi-inorganic Chemistry.  Ashim Kr. Das, Boi-inorganic Chemistry.

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CHM T 513: Pericyclic Reaction, Photochemistry and Free Radical

Chemistry Credits: Theory-04 Theory: 60 Hours Unit – 1: Introduction of Pericyclic Reaction

Definition, Symmetry of π molecular orbital, Filling of electrons in π molecular orbital in conjugated polyenes, conjugated ions, Frontier Molecular Orbital Theory, Classification of Pericyclic reactions (10 Hours) Unit – 2: Electrocyclic and Cycloaddition Reactions Electrocyclic Reactions: Conrotatory and disrotatory motion in ring opening and ring closing reactions, Frontier Molecular Orbital (FMO) approach for Electrocyclic reactions, Correlation diagram of the Electrocyclic reactions with 4nπ and (4n + 2)π electronic systems, Woodward – Hoffmann rule for Electrocyclic system. Cycloaddition Reactions: Theory of Cycloaddition reaction, Stereochemistry of Cycloaddition reaction, Diels-Alder reaction, 1, 3-Dipolar Cycloaddition reactions, Chelotropic reactions. Woodward – Hoffmann selection rule for Electrocyclic system. (12 Hours) Unit – 3: Sigmatropic Rearrangement and Group Transfer Reactions

Definition, Classification of Sigmatropic Rearrangement, Mechanism of Sigmatropic Rearrangement, Various types of [m, n] Sigmatropic rearrangements, Cope, Oxy-Cope and Claisen Rearrangement. Ene Reactions and Group Transfer Reactions given by Diimide. (12 Hours) Unit – 4: Photochemistry

Basic Principle of Photochemistry and Reaction with Carbonyl compounds: Introduction of Photochemistry-Jablonski Diagram, Quantum Yield calculation of photo chemical reaction, photosensitizer and quencher; α-cleavage (Norrish type I & II) and β-cleavage reactions with carbonyl compounds, Intra- and Intermolecular Hydrogen abstraction reactions with carbonyl compounds, Photocycloaddition reactions (Paterno-Bűchi Reaction).

Photo Rearrangement, Photo Reduction, and Photo Isomerization Reactions: Di- π-Methane Rearrangement, Aza-di- π-Methane Rearrangement, Photo reduction of carbonyl compounds, Cis-Trans Isomerization reactions with alkenes, Photochemistry of Dienes. (14 Hours)

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Unit – 5: Free Radical Reactions

Principles, Generation of free radicals, Formation of Carbon-Halogen bonds (Hundsdiecker reaction), Formation of Carbon-Carbon bonds (addition to carbon-carbon double bonds, Acyloin condensation reaction, Eglinton reaction). Formation of Carbon-Nitrogen bonds (Barton Recation and Hoffmann-Loeffler-Freytag Reaction). (12 Hours)

Reference Books:

 J. Singh & J. Singh: Photochemistry and Pericyclic Reactions, New Age International (P) Ltd., 2007  B. B. Woodward and Hoffman: Conservation of Orbital Symmetry, Verlag Chemie Academic Press, 1971.  W. Carruthers: Some Modern Methods of Organic Synthesis, Cambridge University, Press, 1993.

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CHM P 511: Physical Chemistry Practical – II Credits: 02 Lab: 60 Hours (i) Conductometry

(a) The measurement of electrical conductance for the determination of the equivalent conductance at infinite dilution. (b) Determination of the activity coefficient of zinc ions in the solution of 0.002 M zinc sulfate using Debye-Hückel’s limiting law. (c) To verify Debye-Hückel limiting law for strong electrolyte.

(ii) (a) Rate of the hydrolysis of sucrose using polarimeter. (b) Polarizability from refractive index measurement.

(iii) Potentiometry/pHmetry (a) Determination of pKa of poly-basic acid with the pH meter. (b) To determine the pH of various mixtures of acetic acid and sodium acetate in aqueous solutions and hence determine the dissociation constant of the acid.

(iv) Determination of the transport number by moving boundary method.

(v) IR and Raman spectroscopy of the solvent mixture.

Reference Books:

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CHM P 512: Inorganic Chemistry Practical – II Credits: 02 Lab: 60 Hours A. Analytical Chemistry:

 Analysis of Ores: Felspar , bauxite, Rocks available in that region.  Analysis of Soil sample, animal feeds, soil micronutrients, milk powder for Ca, Fe and P content.  Separation of Mixture: Chromium (III) and Mn(II) in a mixture, Iron (III) and Cu(II) in a mixture, Iron(III) and Al(III) in a mixture

At least one ore/ mineral/concentrate and one alloy should be analyzed during the laboratory session. B. Preparations of Complex (At Least eight samples)

Preparation of selected inorganic compound and their studies by I.R. electronic spectra, Mössbauer and magnetic susceptibility measurements. Handling of air and moisture sensitive compounds 1. bis(ethylene)nickel(II)thiosulphate, 2. tris(acetylacetonato)manganese(III), tris(acetylacetonato)Aluminium(III), tris(acetylacetonato)iron(II), tris(acetylacetonato)copper(II), 3. Hexaminecobalt(III)chloride, 4. Mercury tetrathiocyanatocobaltate(II), 5. Copper(II) biguanide

6. Mn12 Acetate Single Molecule Magnet 7. Preparation of copper glycine complex- cis and trans bis- (glycinato) copper (II). 8. Preparation of N, N-bis-(salicyldehyde) ethylenediamine, Co(salen), Mn(salen), determination of O2 absorption by Co(salen), reaction of oxygen adduct with CHCl3 (deoxygenation).

9. VO(acac)2

10. cis-K [Cr(C2O4)2 (H2O)2]

11. Na[Cr(NH3)2 (SCN)4]

12. K2[Fe(C2O4)3] Reference Books:

 Vogel’s Textbook of Quantitative Analysis, Revi Mendham, ELBS.  W.L. Jolly, Synthesis and Characterization of Inorganic Compounds, Prentice Hall.

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SEMESTER – IV

CHM T 521: Molecular Spectroscopy

Credits: Theory-04 Theory: 60 Hours Unit – 1: Unifying Principles

Electromagnetic radiation, interaction of electromagnetic radiation with matter, absorption, emission, transmission, reflection, refraction, dispersion, polarization, and scattering. Uncertainty relation and natural line width and natural line broadening, transition probability, result of the time dependent perturbation theory, transition moment selection rules, intensity of spectral line. Born-Oppenheimer approximation, rotational, vibrational, and electronic energy levels. Fourier Transform Spectroscopy.

(10 Hours) Unit – 2: Microwave Spectroscopy

Rotational spectroscopy: Classification of molecules, rigid rotor model, selection rule, intensity of spectral line, effect of isotopic substitution on the transition frequencies, intensities, non-rigid rotor. Stark effect nuclear and electron spin interaction and effect of external field. Applications (determination of bond lengths of diatomic and linear triatomic molecules etc.)

(10 Hours) Unit – 3: Vibrational Spectroscopy

A. Infrared Spectroscopy: Review of linear harmonic oscillator, vibrational energies of diatomic molecules, zero point energy, force constant and bond strength; anharmonicity, Morse potential energy diagram, vibration-rotation spectroscopy, P, Q, R branches. Breakdown of Oppenheimer approximation; vibration of polyatomic molecules. Selection rules, normal modes of vibration, group frequencies, overtones, hot bands, factor affecting the band positions and intensities, far IR region, metal-ligand vibrations, normal co-ordinate analysis. Fourier Transform Infra-red Spectroscopy (FTIR)

B. Raman Spectroscopy: Classical and quantum theories of Raman Effect, pure rotational, vibrational, and vibrational-rotational Raman spectra, selection rules, mutual exclusion principle. Resonance Raman spectroscopy, coherent anti-stokes Raman spectroscopy (CARS).

(10 Hours) Unit – 4: Electronic Spectroscopy

A. Atomic Spectroscopy: Energies of atomic orbitals, vector representation of momenta and vector coupling, spectra of hydrogen atom and alkali metal atoms.

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B. Molecular Spectroscopy: Energy levels, molecular orbitals, vibranic transition, vibrational progressions and geometry of excited state, Franck-Condon principle, electronic spectra of polyatomic molecules. Emission spectra; radiative and non-radiative decay, internal conversion, spectra of transition metal complex, charge transfer spectra.

C. Photoelectron Spectroscopy: Basic principle; photo-electronic effect, ionization process, Koopman’s theorem. Photoelectron spectra of simple molecules, ESCA, chemical information from ESCA, basic idea Auger electron spectroscopy.

(10 Hours) Unit – 5: Magnetic Resonance, Photoacoustic, and Mössbauer Spectroscopy

A. Nuclear Magnetic Resonance Spectroscopy: Nuclear spin, nuclear resonance, saturation, shielding of magnetic nuclei, chemical shift and its measurement, factor influencing chemical shift, deshielding, spin-spin interaction, factor influencing coupling constant ‘J’. Classification (ABX, AMX, ABC, A2B2 etc), spin decoupling; basic idea about instrument, NMR studies of nuclei other than proton – 13C, 19F, and 31P; FT NMR, advantage of FT NMR, use of NMR in medical diagnostics.

B. Electron Spin Resonance Spectroscopy: Basic principles, zero field splitting and Kramer’s degeneracy, factors affecting the ‘g’ value. Isotropic and anisotropic hyperfine coupling constants, spin Hamiltonian, spin densityies and McConnell relationship, measurement techniques, applications.

C. Nuclear Quadrupole Resonance Spectroscopy: Quatrupole nuclei, quadrupole moments, electric field gradient, coupling constant, splitting, applications.

D. Photoacoustic Spectroscopy: Basic principles of photoacoustic spectroscopy (PAS). PAS- gases and condensed system, chemical and surface applications.

E. Mössbauer Spectroscopy: Basic principles, spectral parameters and spectrum display. Application of technique to the studies of (i) bonding and structure of Fe2+ and Fe3+ compounds – nature of M-L bond, coordination number, structure and (ii) detection of oxidation state and inequivalent MB atom. (20 Hours) Reference Books:

 T. Engle and P. Reid: Quantum Chemistry and Spectroscopy, Pearson, New Delhi, 2011.  B. K. Sharma: Instrumental Methods of Chemical Analysis - 9th Edition.  William Kemp: Organic Spectroscopy –3rd Edition.  C. N. Banwell and E. M. McCash: Fundamentals of Molecular Spectroscopy, Ed. 4th, Tata McGraw-Hill, 1994.  G. M. Barrow: Introduction to Molecular Spectroscopy

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CHM P 522: Project and Dissertation

Credits: 08

Each student is assigned to a faculty supervisor to carry out a research project. They will be trained in searching research literature as well as experimental and computational work specific to the chosen research problem. On the basis of partial fulfilment of project report the student may go other University/Institute for project work. At the end of the project they will submit a report of the work done and make a presentation for evaluations.

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LIST OF ELECTIVE PAPER

S. Course Course Title of Paper Credit No. Code Structure 1 CHM T 601 Elective Mathematics for Chemist 3 2 CHM T 602 Elective Biology for Chemist 3 3 CHM T 603 Elective Industrial Chemistry 3 4 CHM T 604 Elective Instrumental Methods of Analysis 3 5 CHM T 605 Elective Basic of Materials Chemistry 3 6 CHM T 606 Elective Introduction to Nanomaterials and Nanotechnology 3 7 CHM T 607 Elective Polymers Chemistry 3 8 CHM T 608 Elective Bioorganic and Drug Chemistry 3 9 CHM T 609 Elective Advanced Heterocyclic Chemistry 3 10 CHM T 610 Elective Chemistry of Natural Products 3 12 CHM T 611 Elective Solid State Chemistry 3 13 CHM T 612 Elective Advanced Synthetic Organic Chemistry 3

Note: M.Sc. in Chemistry students have to opt total three elective papers (commonly name as Discipline Specific Elective) from the above list of elective courses from the second semester onwards. Students have to choose only that elective courses, those are offered by the Departmental faculty members in the respective semesters in the running academic years.

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CHM T 601: Mathematics for Chemist Credits: Theory-03 (45 Hours) A. Mathematics for Chemist

Unit – 1: Vectors and Matrix Algebra

Numbers: Real and Complex number Vectors: Vectors, dot, cross and triple product etc. The gradient, divergence and curl. Vector calculus, Gauss’ theorem, divergence theorem etc. (9 Hours) Unit – 2: Matrix Algebra Addition and multiplication; inverse, adjoint and transpose of matrices, special matrices (symmetric, screw-symmetric, Hermitian, screw-Hermitian, unit, diagonal, unitary etc.) and their properties. Matrix equations; homogeneous, non-homogeneous linear equation and conditions for the solution, linear dependence and independence. Introduction of vector spaces, matrix eigenvalues and eigenvectors, digonalization, determinants (examples from Hückel theory). Introduction to tensors; poarizability and magnetic susceptibility as examples. (9 Hours) Unit – 3: Differential and Calculus

Differential: Functions, continuity and differentiability, rules for differentiation, application of differential calculus including maxima and minima (examples related to maximally populated rotational energy levels, Bohr’s radius and most probable velocity from Maxwell’s distribution etc.), exact and inexact differentials with their application to the thermodynamic properties.

Partial Differential: Function of several variables, partial differentiation, co-ordinate transformation (e.g. Cartesian to spherical polar). Integral calculus: basic rules for integration, integration by parts, partial fraction and substitution, reduction formulae, applications of integral calculus. (9 Hours) Unit – 4: Elementary Differential Equations Ordinary first- and second-order differential equations. Partial differential equations. Solution of inexact differential equations by the method of integrating factors. Power series and extended power series solutions. Numerical solutions. Special functions: Hermite, Legendre and Laguerre polynomials, recursion relations. (9 Hours) Unit – 5: Probability and Curve Sketching Permutation & Combination. Probability. Stirling’s approximation. Lagrange multipliers. Curve sketching and curve fitting; Introduction to Fourier series and Fourier transforms. (9 Hours) Reference Books:

 R. G. Mortimer: Mathematics for Physical Chemistry, Academic Press.  F. Diniels: Mathematical Preparation for Physical chemistry, McGraw Hill.

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CHM T 602: Biology for Chemist Credits: Theory-03 Theory: 45 Hours Unit – 1: Cell Structure & Functions

Structure of prokaryotic and eukaryotic cells, intracellular organelles and their function, comparison of plant and animal cells. Overview of metabolic processes-catabolism and anabolism; ATP the biological energy currency. Origin of life – unique property of carbon, chemical evolution and rise of living systems. Introduction to biomolecules, building blocks of bio-molecules. (9 Hours) Unit – 2: Carbohydrates

Conformation of monosaccharides, structure and function of important derivatives of monosaccharides like glycosides, deoxy sugars, myoinsitol, amino sugars, N-acetylmuramic acid, sialic acid, disaccharides and polysaccharides. Structural polysaccharides – cellulose, and chitin; storage polysaccharides – starch and glycogen. Structure and biological functions of glucosaminoglycans or mucopolysaccharides. Carbohydrates of glycoproteins glycolipids. Role of sugar in biological recognition. Blood group substances. Ascorbic acid, carbohydrate metabolism – Krebs’ cycle, glycolysis, glycogenesis and glycogenolysis, gluconeogenesis pentose phosphate pathway. (9 Hours) Unit – 3: Lipids

Fatty acids, essential fatty acids, structure and function of triglycerols; glycerophospholipids, sphingolipids, cholesterol, bile acids, prostaglandins. Lipoproteins – composition and function, role in atherosclerosis. Properties of lipids, aggregates – micelles, bilayers, liposomes and their possible biological function. Biological membranes, fluid mosaic model of membranes structure. Lipid metabolism -oxidation of fatty acids. (9 Hours) Unit – 4: Amino Acids

Amino Acids, Peptides and Proteins: Chemical and enzymatic hydrolysis of proteins to peptides, amino acid sequencing, secondary structure of proteins, force responsible for holding of secondary structure. - helix, -sheet, super secondary structure, triple helix structure of collagen. Tertiary structure of proteins, folding and domain structure. Quaternary structure. Amino acid metabolism, degradation and biosynthesis of amino acids, sequence determination, chemical/enzymatic/mass spectral racemization detection. Chemistry of oxytocin and tryptophan releasing hormone (TRH). (9 Hours) Unit – 5: Nucleic Acids

Purine and pyrimidine bases of nucleic acids, base pairing via H-bonding. Structure of ribonucleic acids (RNA) and deoxyribonucleic acids (DNA), double helix model of DNA and forces responsible for holding it. Chemical and enzymatic hydrolysis of nucleic acids. The chemical basis of heredity, an overview of replication of DNA, transcription, translation and genetic code. Chemical synthesis of mono- and tri- nucleosides. (12 Hours) Reference Books:

 A. L. Lehninger: Principle of Biochemistry, Worth Pub. Shers.  L. Stryer and W. H. Freeman, Biochemistry  J. David Rawn: Biochemistry, Neil Patterson.

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CHM T 603: Industrial Chemistry Credits: Theory-03 Theory: 45 Hours Unit – 1: Water and Its Treatment

Sources of water, chlorinated and nonchlorinated water, chemical method of sterilization: precipitation method, Aeration, ozonisation, chlorination, chloramines process, potassium permanganate method, Physical method of sterilization: Boiling, exposure to sunlight, hard and soft water, Types of hardness, temporary and permanent hardness, water softening, cold and hot lime soda process, zeolite process, ion exchange process, removal of iron, silica, and dissolved oxygen from water for industrial purposes, water for boiler uses, water analysis. (9 Hours) Unit – 2: Glass and Rubbers Glass: physical and chemical properties of glass, constituents in glasses, raw materials, manufacturing of glasses, optical glass, borosilicate glass, lead glass, colored glass, opal glass, safety glass, fiber glass. Natural and Synthetic Rubber: classification of rubber, natural and synthetic rubber. (9 Hours) Unit – 3: Chemical Fertilizers Classification of fertilization, nitrogeneous fertilizers, method of production and its action- ammonium nitrate, ammonium sulphate, urea, calcium cyanamide, ammonium chloride, phosphate rock, normal super phosphate, triple super phosphate. (9 Hours) Unit – 4: Petroleum Classification of petroleum, composition of petroleum, mining of petroleum, refining of petroleum, octane rating, octane number and antiknock compound, cetane number, production of gases, crude naptha, benzene, kerosene oil, fuel oil, lubricating oil, paraffin wax and black tarry after refining. Cracking: thermal cracking, hydrocracking, and fluid catalytic cracking. (9 Hours) Unit – 5: Fibers and Dyes Synthetic Fibers: Preparation of fibers- Nylons, Nylon-66, Nylon-6, Nylon-11, Nylon-610, Nylon-8, polyethylene terephthalate, orlon, saran, vinyon, taflon. Synthetic Dyes and Dyeing: Requisites of true dyes, sensation of color, witt’s theory, chromophores, auxochromes: batho-, hypso-, hyper-, and hypochromic shifts; classification of dyes: acid dyes, basic dyes, adjective dyes, vat dyes, ingrain dyes, sulfur dyes, pigment dyes, nitroso dyes, nitro dyes, azo dyes, xanthenes dyes, applications of dye. (9 Hours) Reference Books:  E. Stocchi: Industrial Chemistry, Vol-I, Ellis Horwood Ltd. UK.  R.M. Felder, R.W. Rousseau: Elementary Principles of Chemical Processes, Wiley Publishers, New Delhi.  J. A. Kent: Riegel’s Handbook of Industrial Chemistry, CBS Publishers, New Delhi.  S. S. Dara: A Textbook of Engineering Chemistry, S. Chand & Company Ltd. New Delhi.

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CHM T 604: Instrumental Methods of Analysis Credits: Theory-03 Theory: 45 Hours Unit – 1: Molecular Spectroscopy

(9 Hours) Unit – 2: Atomic Spectroscopy

Flame emission spectrometry, atomic absorption spectroscopy- principle, instrumentation, Source in AAS – Hollow cathode lamp, electrode less discharge lamp, burners, nature and property of flame, interference in AAS, difference between AAS and FES, ICP. (9 Hours) Unit – 3: Thermal Analysis

(9 Hours) Unit – 4: Chromatography

Principles of chromatographic separation, classification of Chromatographic Techniques: adsorption, partition, ion exchange and size exclusion chromatography, theory of chromatographic separation, distribution coefficient, retention time, sorption, theory of column efficiency and resolution, separation factor, retention factor. – working principle and application of Column chromatography, ion exchange chromatography, paper chromatography, Thin layer chromatography (TLC) & HPTLC: techniques and application. - Gas Chromatography and high performance liquid chromatography: Van Deemter equation, retention time or volume, capacity ratio, partition coefficient, theoretical plate and number, separation efficiency and resolution, instrumentation and application. (9 Hours)

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Unit – 5: Electroanalytical Techniques

Electrochemical cells, current potential relationship, mass transfer by migration, convection and diffusion, Electrogravimetry, voltam-metry, polarography, reference electrode, working electrode, auxiliary electrode, dropping mercury electrode, current potential curve, limiting current, coulometry, conductometry methods, instrumentation, techniques and application. Amperometric titration, effect of electroactive and reagent on amperometric curve and its advantage, rotating platinum electrode, biamperometric titration and its advantage, fluorimetry and phosphorimetry.

(9 Hours) Reference Books:

 Arthur I. Vogel: A Test book of Quantitative Inorganic Analysis (Rev. by G.H. Jeffery and others) 5th Ed. The English Language Book Society of Longman .  Hobert H. Willard et al: Instrumental Methods of Analysis, 7th Ed. Wardsworth Publishing Company, Belmont, California, USA, 1988.  Gary D. Christian: Analytical Chemistry, 6th Ed. John Wiley & Sons, New York, 2004.  C. Daniel Harris: Exploring Chemical Analysis, Ed. New York, W.H. Freeman, 2001.  S. M. Khopkar: Basic Concepts of Analytical Chemistry, New Age, International Publisher, 2009.  D. A. Skoog, F. J. Holler and T. A Nieman: Principles of Instrumental Analysis, Thomson Asia Pvt. Ltd. Singapore.  O. Mikes & R. A. Chalmes: Laboratory Hand Book of Chromatographic & Allied Methods, Elles Harwood Ltd. London.  R. V. Ditts: Analytical Chemistry – Methods of separation.

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CHM T 605: Basic of Materials Chemistry

Credits: Theory-03 Theory: 45 Hours

Unit – 1: Chemical Crystallography

Introduction: Space lattice, crystal point groups, space group (working knowledge), stereographic projections, packing in solids, crystal structures of representative systems, silicates and zeolites, cements, glasses, quasicrystals, nanostructures.

Bonding in Solids and Crystal Energetics: Crystal classifications, Madelung constant and Lattice energy.

(9 Hours) Unit – 2: Characterization Techniques for Solids

X-ray diffraction, electron microscopy (SEM, TEM, AFM), thermal techniques (TG, DTA, DSC), spectroscopic techniques (Mössbauer, IR, UV-VIS), and physical property measurement techniques (magnetic moments-VSM/SQUID, electrical resistivity – two / four probe methods and thermal conductivity, optical band gap, XPES, XAS.

(9 Hours) Unit – 3: Electronic and Magnetic Properties Solids

Electronic Properties and Band Theory of Solids: Free electron theory of metals, Band theory of solids, Bloch theorem, Kroning-Penne model, refinement of simple band theory- k-space and Brillouin Zones, band structure of metals, insulators and semiconductors, intrinsic and extrinsic semiconductors, doped semiconductors, p-n junctions.

Magnetic Properties Solids: Behaviour of substances in a magnetic field, effect of temperature: Curie and Curie-Weiss law, origin of magnetic moment, ferromagnetic, antiferromagnetic and ferromagnetic ordering, super exchange, magnetic domains, hysteresis. Introduction of superconductors, Meissner effects, basic concepts of BCH theory.

Unit – 4: Defects and Phase Transitions

Defects, Nonstoichiometry and Diffusion: Point defects, dislocations, extended defects, clusters and aggregates, color centers, nonstoichiometry of compounds, diffusion mechanisms, Fick’s law, Kirkenall effect.

Phase Transitions: Critical phenomena, variety of phase transitions (ordered-disorder, Martensite-austenite, spinoidal decompositions etc), liquid crystals, structure-property relations (magnetic, electrical, superconductivity, optical and thermal).

Unit – 5: Preparative Techniques

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Reactivity of Solids: Decomposition and reactivity, solid state reactions, sintering process, reaction kinetics, organic solid reactions.

Conventional Techniques: Powder mixing, fusion, precipitation from solution, modern need for improved synthetic routes, crystal growth and thin film techniques.

Chemical Routes: Wet-chemical (Oxidation-reduction for metal nanoparticles) methods, self assembly methods, reverse micelles route, biomimetic, sonochemical, and electrochemical approaches.

Sol-Gel Synthesis: Colloids, cation hydrolysis and sol formation, gel precipitation, sol-gel process for colloids, synthesis andphysical properties of metal alkoxides, development of sol-gel process from alkoxides, derived coatings, fibers and monodispersed submicron/ nanostructured oxide powders, ormosils, sialons. Hydrothermal/Solvothermal Approach: Forced hydrolysis at elevated temperatures and pressures, hydrothermal reactions using salt solutions, metal reactants and reactions involving phase transformation.

Precursor Technique: Citrate-gel process, metallo-organic precursors, metal alkoxides.

Gas Phase Reactions: Gas-phase nucleation, flame hydrolyzed powders, direct - nitridation and carbothermic reduction, non-plasma gas phase reactions, plasma reactions, electron beam evaporation. (12 Hours)

Reference Books:

 A. R. West: Solid State Chemistry and Its Applications, John Wiley & Sons, 1989.  L. Smart and E. Moore, Solid State Chemistry, Chapman and Hall, 1992.  A. K. Cheetham and P. Day: Solid State Chemistry Compounds, Clarendon Press, Oxford 1992.  C. N. R. Rao and J. Gopalkrishanan: New Directions in Solid State Chemistry, Cambridge Univ. Press 1997.  R. E. Newnham, Structure Property Relations, Springer-Verlag, 1987

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CHM T 606: Introduction to Nanomaterials and Nanotechnology

Credits: Theory-03 Theory: 45 Hours

Unit – 1: Nanoscience and Nanotechnology

Introduction: Underlying physical principles of nanotechnology: Nanostructured Materials: Size is Everything. Fundamental physicochemical principles, size and dimensionality effects; quantum confinement; properties dependent on density of states; single electron charging, central importance of nanoscale morphology. Societal aspects of nanotechnology: health, environment, hype and reality.

Type of Nanostructures: Definition of a nano system; one dimensional (1D), two dimensional (2D), three dimensional (3D) nanostructured materials; quantum dots; quantum wire, and core/shell structures.

(9 Hours) Unit -2: The Basic Tools of Nanotechnology

Electron microscopy (SEM, TEM with EDX analysis) and X-ray diffraction, A brief historical overview of atomic force microscopy (AFM); an introduction and basic principles & applications of XPS, FTIR spectrophotometers; UV-VIS principle and application for band gap measurement.

(9 Hours) Unit – 3: Synthesis of Nanomateirals

Top down and bottom up approaches to synthesis of nanomaterils:

Chemical Routes for Synthesis of Nanomaterials: Chemical precipitation and co-precipitation; sol-gel synthesis; microemulsions or reverse micelles; solvothermal synthesis; thermolysis routes, microwave heating synthesis biomimetic and electrochemical approaches; sonochemical synthesis; photochemical synthesis; synthesis in supercritical fluids.

Physical Routes for Preparation of Nanomaterial: Inert gas condensation, arc discharge, RF plasma, plasma arc technique, ion sputtering, laser ablation, laser pyrolysis, spray pyrolysis, ball milling, molecular beam epitaxy, chemical vapour deposition method, Langmuir-Blodgett (LB) films, spin coating and electro deposition.

(9 Hours) Unit – 4: Nanomateirals and Properties

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Synthesis and size dependent properties (mechanical, physical and chemical properties) of carbon nanotubes (CNT); metals (Au, Ag); metal oxides (TiO2, CeO2, ZnO); semiconductors (Si, Ge, CdS, ZnSe); dilute magnetic semiconductor. (9 Hours) Unit -5: Applications of Nanomateirals

Basic ideas of nanodevices (molecular electronics and nanoelectronics, and quantum electronic devices); CNT based transistor and field emission display; biological applications; biochemical sensor; membrane based water purification, energy storage devices, catalysis and various related fields. (12 Hours)

Reference Books:

 T. Pradeep, Nano: The Essentials, Tata McGraw-Hill, New Delhi, 2007.  G. Cao, Nanostructures and Nanomaterials – Synthesis, Properties and Applications, Imperial College Press, London, 2004,  C. N. R. Rao, A. Muller and A. K. Cheetham, The Chemistry of Nanomaterials  G. L. Hornyak, J. J. Moore, H. F. Tibbals, and J. Dutta: Fundamentals of Nanotechnology, CRC Press, 2009

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CHM T 607: Polymers Chemistry Credits: Theory-03 Theory: 45 Hours Unit – 1: Introduction

Importance of polymers. Basic Concept: monomers, repeat units, degree of polymerization; linear, branched, and network polymers (block-copolymer, dendrimer etc.); classification of polymers. Polymerization: condensation, addition, radical, chain- ionic- and co-ordination-, and co-polymerization; polymerization condition and polymer reaction; polymerization in homogeneous and heterogeneous systems.

(9 Hours) Unit– 2: Polymer Characterization Techniques

Polydispersion-average molecular weight concept; number, weight and viscosity average molecular weights. Polydiversity and molecular weight distribution. The practical significance of molecular weight. Measurement of molecular weights. End group, viscosity, light scattering, osmotic, and ultracentrifugation methods. Analysis and testing of polymers-chemical analysis of polymers. Spectroscopic methods, X-ray diffraction, microscopy studies. Thermal analysis and physical testing tensile strength, fatigue, impact, tear resistance, hardness and abrasion resistance analysis. (9 Hours) Unit – 3: Structure and Properties

Morphology and order in crystalline polymers – configuration of polymer chains; crystal structure of polymers; morphology of crystalline polymers; strain-induced morphology; crystallization and melting polymer structure and physical properties – crystalline melting point, Tm, melting points of homogeneous series effect of chain flexibility and other steric factors, entropy and heat of fusion. The glass transition temperature, Tg, relationship between Tm and Tg, effect of molecular weight, diluents, chemical structure, chain topology, branching and cross linking. Properties requirements for polymer utilization.

(9 Hours) Unit – 4: Polymer Processing

Plastic, elastomers and fibres, compounding; processing techniques- calendaring, die casting, rotational casting, film casting, injection casting, blow moulding, extraction moulding, thermoforming, foaming, reinforcing, and fibre spinning.

(9 Hours) Unit – 5: Properties of Commercial Polymers

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Polyethylene, polyvinyl chloride, polyamide, polyester, phenolic resins, epoxy resins and silicone polymers. Functional polymers – fire retarding polymers and electrically conducting polymers. Biomedical polymers – contact lens, dental polymers, artificial heart, kidney, skin, and blood cells. (9 Hours)

Reference Books:

 Fred W. Billmeyer: Textbook of Polymer Science, Eds: 3rd, Wiley-India, New Delhi, 2012.  A Ravve: Principle of Polymer Chemistry, Eds. 3rd, Springer Science + Business Media, New York, 2012.  J. M. G. Cowie: Physics and Chemistry of Polymers, Blackie Academic and Professional.  H. R. Alcock and F. W. Iamtee: Contemporary Polymer Chemistry, Prentice Hall.  V. R. Govarikar, N. V. Viswanathan, and J. sreedhar: Polymer Science, Wieley-Eastern.

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CHM T 608: Bioorganic and Drug Chemistry

Credits: Theory-03 Theory: 45 Hours

Unit – 1: Overview of Bioorganic Chemistry

Chemistry of the Living Cell: The structure of prokaryotic and Eukaryotic cells, Composition of living cells: (9 Hours) Unit – 2: Carbohydrates, Proteins, Lipids, and Nucleic Acids

Carbohydrates: Introduction, Reactions of Monosaccharides, Interconversions, Ring structure of aldoses and ketoses, Confirmation of Monosaccharides, Disaccharides: Structure, synthesis and properties.

Proteins: General structure & classification of amino acids, Abbreviation of amino acids, Essential and non essential amino acids, Synthesis of amino acids, Isoelectric point, Acid and base properties of amino acids. Protein: Naturally occurring peptides, Modern methods of peptide synthesis with protection and deprotection, Determination of sequences and basic units of a poly peptides or proteins, C- & N-terminus detection by chemical methods, Primary, secondary, tertiary and quaternary structures of proteins, Enzyme active sites, allosteric sites, and mechanism of their actions e.g. chymotrypsin, carboxypeptidase, lipases etc.

Lipids: Lipid structure- acylglycerols, phosphoglycerides and sphingolipids, Biological importance of fatty acids and lipids, Bio- and chemical Synthesis of lipids. Nucleic Acids: Definition, structure and properties, base pairing, double helices, Genetic information storage, transmission and gene expression, Nucleotides and Nucleosides: Similarities and differentiation, Structure of DNA & RNA. Types of mRNA, tRNA and rRNA, Replication, transcription and translation, Genetic code, Protein biosynthesis.

(12 Hours) Unit – 3: Analogy Between Biochemical and Organic reactions

Introduction to metabolism (catabolism, anabolism). ATP: The universal currency of cellular energy, ATP hydrolysis and free energy change. Agents for transfer of electrons in biological redox systems: NAD+, FAD. Conversion of food to energy: Outline of catabolic pathways of

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(9 Hours) Unit – 4: Overview of Drug Chemistry and Basics of Drug Action

Definition, classification and nomenclature of drugs, Preliminary idea of drug action: Interaction (Weak interaction in drug molecules, Chirality and drug action), Receptorology (Drug-receptor interactions, Enzyme kinetics in drug action, Enzyme inhibitors (Drug action through enzyme inhibition), Nucleic acids as targets for drug actions, NA-Alkylation, NA-strand breaking and their importance in drug action, Drug metabolism, drug deactivation and elimination. (8 Hours) Unit – 5: Pharmaceutical Compounds: Structure and Importance

Reference Books:

 L. Stryer: Biochemistry, 4th Edition W. H. Freeman and Co. 1995.  S. Zubay: Biochemistry, Addison-Wesely 1983.  J. Mann; R.S. Davidson: Natural Products: Chemistry and Biological Significance  H. Dugas: Bioorganic Chemistry Frontiers Vol. 2, ed. Springer-Verlag, 1990.  E. E. Tamlen: Bioorganic Chemistry, Academic Press, 1977.  M. Bodansky: Peptide Chemistry: A Practical Textbook, Springer-Verlag 1988.  Bioorganic Chemistry: A chemical approch to enzyme action, Springer-Verlag 1989.  W. Saenger: Principles of Nucleic acid structures, Springer-Verlag 1984.  G. R. Chatwal: Medicinal Chemistry  A. Kar: Medicinal Chemistry, Wiley, 2000.  D. Lednicer: Strategies for Organic Drug Synthesis and Design, John Wiley 1998.  G. R. Chatwal: Synthetic Drugs, Himalaya, New Delhi 1995.  S. Hanessian, Total synthesis of Natural product: The chiral approach Vol.III Pergamon Press 1983.  W. D. Foye, T. L. Lemke, and D. A. Williams: Principles of Medicinal Chemistry (4th Edition)  R. B. Siwerman: Organic Chemistry of Drug Action and Design (Academic press, 1993).

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CHM T 609: Advanced Heterocyclic Chemistry Credits: Theory-03 Theory: 45 Hours Unit – 1: Introduction

Definition of heteroatom, Aromatic and non-aromatic heterocyclic compounds, Classification and nomenclature of heterocyclic compounds, important reactions with heterocyclic compounds i.e. oxidation, reduction and tertiary effect of Nitrogen in heterocyclic compound. (9 Hours) Unit – 2: Non-Aromatic Heterocycles

Different types of strains, interactions and conformational aspects of non-aromatic heterocycles. Synthesis, reactivity and importance of the following ring systems: Aziridines, Oxiranes, Thiiranes, Oxaziridines, Azetidines, Oxetanes and Thietanes. (9 Hours) Unit – 3: Five and Six Membered Heterocyclics with One Hetero Atom

Pyrrole, Furan, Thiophene, Pyridine, Indole, Quinoline, Isoquinoline - Synthesis and reactions [Advanced synthetic methods are applied]. (9 Hours) Unit – 4: Five and Six Membered Heterocyclics with Two Hetero Atoms

Synthesis, reactivity, aromatic character and importance of the following heterocycles: Pyrazole, Imidazole, Oxazole, Thiazole, Isoxazole, Isothiazole, Pyridazine, Pyrimidine. Pyrazine, Oxazine, thiazine, benzimidazole, benzoxazole and benzthiazole.

(9 Hours) Unit – 5: Larger Ring and Other Heterocycles

Synthesis, structure, stability and reactivity of Azepines, Oxepines and Thiepines. Synthesis of Benzoazepines, Benzooxepines, Benzothiepines, Azocines and Azonines. (9 Hours) Reference Books:

 T. Gilchrist: Heterocyclic Chemistry  R. M. Acheson: An Introduction to the Chemistry of Heterocyclic Compounds  J. A. Joule & K. Mills: Heterocyclic Chemistry  A. Paquette: Principles of Modern Heterocyclic Chemistry  J, A. Joule & Smith: Heterocyclic Chemistry  A .R. Katritzky: Handbook of Heterocyclic Chemistry

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CHM T 610: Chemistry of Natural Products Credits: Theory-03 Theory: 45 Hours Unit – 1: Alkaloid – I Occurrence and isolation, biological role of alkaloids, General properties, nomenclature and classification of alkaloids on the basis of amino acid origin and present core structure. Isolation, properties and structural elucidation of quinine, Morphine (structure, synthesis, molecular rearrangement, stereochemistry and biogenesis). (9 Hours) Unit – 2: Alkaloid – II

Structure and biological role of nicotine, cocaine, quinine, reserpine, vincristine, morphine, caffeine, papavarine, hyocimine. Strychnine and lysergic acid. (9 Hours) Unit – 3: Steroid

Introduction, nomenclature of steroids, absolute configuration of steroid. Occurrence, isolation, structute elucidation and chemical properties of Cholesterol. (9 Hours) Unit – 4: Terpenes

Secondary metabolites: Definition and examples; terpenes – isoprene rule; mono terpenes: structure of geraneol, limonene, alpha-pinene and camphor; sesquiterpenes: longfolene; diterpenes: abietic acid, taxol. Structure determination of Citral and Camphor. (9 Hours) Unit – 5: Vitamins

Introduction, chemical properties, structure elucidation of Vitamin A, Vitamin B, Ascorbic Acid and Vitamin D. Vitamin A and its role in vision. Biological role of Vitamin D, Ascorbic Acid, Vitamin A. (9 Hours)

Reference Books:

 I. L. Finar: Organic Chemistry Vol. II, 5th Edition  S. V. Bhat, B. A. Nagaramgagi, M. Srikumar: Chemistry of Natural Products, Alpa Science International Ltd, 2005 by  O. P. Agarwal: Chemistry of Natural Products, Vol I & Vol II, Goel publishing House, 1989  J. R. Hanson: Natural Products: The Secondary Metabolites, Wiley-Vch, 1st Ed.; 2008.

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CHM T 611: Solid State Chemistry Credits: Theory-03 Theory: 45 Hours Unit – 1: Crystal Structure

Crystalline and amorphous solids; symmetry in crystals, basic crystal systems,space lattice and unit cell, Bravais lattice,miller indices, closed packed structure- hcp and ccp, packing efficiency, limiting radius ratio and shape of ionic crystal, description of solids; structure types Rock salt (NaCl), Zinc blende (ZnS),antifluorite( Na2O), Rutile (TiO2), Wurzite (ZnS), CdCl2, nickel arsenide, CsCl, CdI2, Cs2O, perovskite ABO3, K2NiF4, spinels. (9 Hours) Unit – 2: Point Groups Symmetry operation and symmetry elements, Plane of symmetry, inversion centre, proper and improper axis of rotation, Product of symmetry operation, Relation among symmetry elements and symmetry operation, classification of symmetry, symmetry elements in octahedral and tetrahedral molecules, symmetry point group, representation of symmetry operation by matrices, reducible and irreducible representation, Character tables. (9 Hours) Unit – 3: Space Groups Thirty two point groups, Representation of point groups and selected examples like 222, mm2, mmm, 32 centrosymmetric and noncentrosymmetric point groups, space group: Triclinic P1, monoclinic C2, monoclinic C2/m, orthorhombic P2221 orthorhombic F222, Tetragonal 141 , space group and crystal structure of SrTiO3 and rutile structure of TiO2. (9 Hours) Unit – 4: Structure and Properties of Advance Materials – I Superconductors – (Ba,K)BiO3, Cuprates, LnFeAsO, MgB2, CaC6 CMR materials – La(1-x)SrxMnO3 Ferroic compounds – BaTiO3, PbTiO3, Bi4Ti3O12, SrRuO3 Peizoelectric materials- PZT, Photoluminescent materials – Lanthanide compounds Porous materials – zeolites, AlPO, MeAlPO, SAPO. (9 Hours) Unit – 5: Structure and Properties of Advance Materials – II Organic-inorganic hybrid materials – MOF compounds Ionic Conductors – NASICON, AgI, NaAl11O17 Thermoelectric materials – NaxCoO2, AgSbTe2, CoSb3, Y14MnSb11 Compounds for intercalation and redox reactions – LiCoO2, LiVS2, NASICON, Chevrel phases (9 Hours) Reference Books:

 C. N. R. Rao and J. Gopalakrishnan: New Direction in Solid State Chemistry, Cambridge University Press, 1997.  A. R. West: Solid State Chemistry and Its Applications, John Wiley & Sons, 1989.  L. Smart and E. Moore: Solid State Chemistry, Chapman and Hall, 1992.

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CHM T 612: Advanced Synthetic Organic Chemistry Credits: Theory-03 Theory: 45 Hours Unit – 1: Metal Mediated C-C and C-X Coupling Reactions

Suzuki, Heck, Stille, Sonogishira cross coupling, Buchwald-Hartwig and Negishi-Kumada coupling reactions. C=C Formation Reactions: Shapiro, Bamford-Stevens, McMurrey reactions, Julia Lythgoe olefination and Peterson’s stereoselective olefination. Olefin metathesis by Ist and IInd generation catalysts: Reaction mechanism and application in the synthesis of heterocycles. (9 Hours) Unit– 2: Reagents of Phosphorous, Sulfur, Silicon and Boron

Phosphorous Sulfur, Silicon and Boron containing compounds-preparations and their uses in organic reactions. (9 Hours) Unit – 3: Oxidation and Reduction

Oxidation: Oxidation of hydrocarbons (alkanes, aromatic hydrocarbons, alkenes), Oxidation of alcohols (Chromium reagents, Manganese reagents, Other metal and non-metal based oxidants), Oxidation of ketones ( α, β-unsaturated ketones, α-hydroxy ketones, Baeyer-Villiger oxidation of ketone) Reduction: Catalytic hydrogenation, Reduction by dissolving metals, Reduction by hydride- transfer reagents (Derivatives of lithium aluminium hydride and sodiumborohydride, mixed lithium aluminium hydride-aluminium chloride reagent, DIBAL-H, NaBH3CN, sodium triacetoxyborohydride, Borane and derivatives, other methods of reductions). (9 Hours) Unit – 4: Disconnection Approach, Umpolung Chemistry and Protection-Deprotection of Functional groups Basic principles and terminology-Target molecule, FGI, Disconnection, Synthon, Reagent and Retro-synthetic approach. One group C-C and C-X disconnection: (disconnection of alcohols, alkenes, and carbonyl compounds). Two group C-C & C-X disconnections: 1,3 and 1,5 difunctionalised compounds, α, β, unsaturated carbonyl compounds, control in carbonyl condensation, synthesis of 3,4,5 and 6 membered rings in organic synthesis. Diels- Alder reaction, connection in retro synthesis. Umpolung in organic synthesis. Protection and deprotection for functional groups as hydroxyl, amino, carboxylic and carbonyl. (9 Hours) Unit – 5: Some Important Organic Reactions

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Selective Stereoselective Organic Reactions with Alkenes: Sharpless Asymmetric Epoxidation, Asymmetric Aziridination, Dihydroxylation, Amino-hydroxylation Reactions, Oxidative cleavages of alkenes. Green Chemistry, Supramolecular chemistry (Crown ether, Cyclodextrin and Clalixerins) and multicomponent reactions (Ugi, Passerini, Biginelli, Hantzsch reactions). Chemistry of Aliphatic and Aromatic Heterocyclic Compounds: Epoxide, Aziridine, Azitidine, Oxetane, Pyrrole, Furan, Thiophene, Pyridine, Indole, Quinoline, Isoquinoline - Synthesis and reactions.

(9 Hours) References Books:

 B. F. G. Johnson: Transition Metal Cluster, Wiley, 1980.  R. H. Crabtree: The Organometallic Chemistry of the Transition Metals, Wiley- Interscience, 2005.  G. Wikinson, F. G. A. Stone, and E. Abel: Comprehensive Organometallic Chemistry, Peramon, 1980.  I. Fleming: Frontier Orbitals and Organic Chemical Reactions, Wiley, 1976.  B. B. Woodward and Hoffman: Conservation of Orbital Symmetry, Verlag Chemie Academic Press, 1971.  S. Warren: Organic Synthesis: The Disconnection Approach, John Wiley & Sons (Asia) Pte. Ltd., 2007  W. Carruthers and I. Coldham: Modern Methods of Organic Synthesis, Fourth Ed. Cambridge University Press.  T. L. Gilchrist: Heterocyclic Chemistry, Pearson Education, 3rd Ed.2007

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EVALUATION & DISTRIBUTION OF MARKS (1) Continuous Internal Assessment (CIA): Forty (40) marks (a) 1st Mid-Semester Examination: Maximum Marks 10 Duration of Examination: One Hour Pattern of Question Paper: Five (05) Objective Type Questions; each carrying one (1) mark One (01) Short Answer Type Question of five (05) marks (b) 2nd Mid-Semester: Maximum Marks 10 (as described above) (c) Assignment (minimum one): Maximum 15 Marks (d) Regularity in the Class: Maximum five (05) Marks: Award of marks based on attendance will be determined as below:

Attendance Marks 90% and above 5 Marks 85 to 89.9% 4 Marks 80 to 84.9% 3 Marks 76 to 79.9% 2 Marks 75 to 75.9% 1 Mark Below 75% Zero Note: Total Marks of CIE will be 40 (i.e., 10+10+15+5). A candidate must have to secure minimum 50% marks (i.e., 20 out of 40 marks). Failing so, s/he shall not be allowed to appear in End Semester Examination. Marks for two mid-semester examinations could either be awarded as aggregate scored by the candidate in the two exams or as best of two. The department may adopt suitable model. (2) End Semester Examination (ESE) (a) Theory Paper: Maximum Marks: 60 (Sixty) Duration of Examination-Three Hours Question Paper Pattern: The paper will be set so to cover all units/sections of the syllabus as below:

Marks for No. of questions Total Type Total No. Each to be answered Marks Question Long Answer Type 05 (one Questions (one out of question 5 (from all five 12 60 two questions from from each questions) each unit) unit) Total 60

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(b) Practical Examination: Duration of Examination: Four - Six Hours Question Paper Pattern –

Q.1. Principle/ Theory 10 Experiment Procedure 10 Results and discussion 10 Q.2 Viva-voce 10 Q.3 Record/ File 10 Total 50

(3) Total marks of each question paper will be 100 (hundred) for theory paper [i.e., 60 (ESE) + 40 (CIA)] and 50 (fifty) for practical paper (Grand Total: 150, Hundred-Fifty), irrespective of their credits.

(4) Attendance A candidate shall only be eligible to appear in the end-semester examination if s/he has secured a minimum of 75% attendance as prescribed in the university ordinance. (5) Grading Each course shall be graded (refer table below) on the basis of marks obtained, on scaled marks of 100, during a semester. There shall be absolute grading where mark obtained (out of 100) by a student in a course is converted to a Grade on a 10-point scale.

Table: Showing marks to grade conversion

Marks (%) Letter Grade Grade Points 89.5-100 O (Outstanding) 10 79.5-89.4 A+ (Excellent) 09 69.5-79.4 A (Very Good) 08 59.5-69.4 B+ (Good) 07 49.5-59.4 B (Pass) 06 0-49.4 F (Fail) 00 Ab (Absent) 00

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Course Structure for PhD Course Work CHEMISTRY

The PhD course work course comprises common courses (05 credits; A), Research theme - Common Elective Courses (04 credits; B) and Discipline Specific Elective Courses (06 Credits; C). Since PhD students come from different educational backgrounds, relevant courses will be chosen in consultation with the concerned DRC to compliment the previous education, improve specific skills required for thesis and subsequent career. The Common Courses (CHM T 700), for all PhD scholars registered in chemical science related disciplines with the Faculty of Science in the Indira Gandhi National Tribal University, Amarkantak. Research Them- Common Elective Course and Discipline Specific Elective Courses designed for individual Chemical science whereas, a research scholar will select elective courses as suggested by the concerned DRC. Evaluation of the research plan proposal and presentation, and review of literature will be done by the concerned DRC. The detailed course layout is given below.

Course Structure:

(A) Common Courses (05 credits)

Course Code Title Nature Credits

CHM T 700 Research Methodology Compulsory 04

CHM P 700 Lab. work based on CHM T 700 Compulsory 01

(B) Research Them- Common Elective Course (opt any one) (04 credits)

S. Course Course Code Title Credits No. Structure 1 CHM T 701 Elective Principles of Physical Chemistry 04 Modern Physical Methods in 2 CHM T 702 Elective 04 Chemistry Research Nanomaterials: Synthesis and 3 CHM T 703 Elective 04 Characterization Newer Methods in Organic 4 CHM T 704 Elective 04 Synthesis 5 CHM T 705 Elective Supramolecular Chemistry 04

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Discipline Specific Elective Course* (Opt any one)

Course Course Title of Paper Credit Code Structure CHM T 801 Elective Advanced Analytical Chemistry 04 CHM P 801 Lab Advanced Analytical Chemistry Lab 02 CHM T 802 Elective Advanced Organometallic Chemistry 04 CHM P 802 Lab Advanced Organometallic Chemistry Lab 02 CHM T 803 Elective Advanced Materials Chemistry 04 CHM P 803 Lab Advanced Materials Chemistry Lab 02 CHM T 804 Elective Nanoscience & it’s Applications 04 CHM P 804 Lab Nanoscience & it’s Applications Lab 02 CHM T 805 Elective Polymers Chemistry 04 CHM P 805 Lab Polymers Chemistry Lab 02 CHM T 806 Elective Bioorganic and Drug Chemistry 04 CHM P 806 Lab Bioorganic and Drug Chemistry Lab 02 CHM T 807 Elective Advanced Heterocyclic Chemistry 04 CHM P 807 Lab Advanced Heterocyclic Chemistry Lab 02 CHM T 808 Elective Chemistry of Natural Products 04 CHM P 808 Lab Chemistry of Natural Products Lab 02 CHM T 809 Elective Advanced Synthetic Organic Chemistry 04 CHM P 809 Lab Advanced Synthetic Organic Chemistry Lab 02 CHM T 810 Elective Principles of X-ray Diffraction and Electron Microscope 04 CHM P 810 Lab Principles of X-ray Diffraction and Electron Microscope Lab 02

* Notes:

 Research scholars those who studied above mentioned courses in their PG Programme they must opt different course.

 All the elective papers will be offered as suggested by the concern DRC.

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CHM T 700: Research Methodologies Credits: 04 Theory: 60 Hours 1. An overview of research methodology: Research concept, steps involved, identification, selection and formulation of research problem, justification, hypothesis; literature collection- textual and digital resources (internet) 2. Research design, data collection and interpretation: Research design; sampling techniques, collection and documentation, presentation, analysis and interpretation of data 3. Scientific writing: Forms of scientific writing- Article, notes, reports, review article, monographs, dissertations, popular science articles, bibliographies, 4. Formulation of scientific communication - Outline preparation, drafting title, sub titles, tables, illustrations; Formatting tables- title, body footnotes; figures & graphs- structure, title and legends, Impact factor, citation indices, plagiarism 5. Computer application: MS office, excel, power point, graphics (Origin), statistical software (SPSS), CHEMDRAW, Full Prof etc. 6. Statistics: Standard deviation/error; Correlation coefficient, types of correlation, regression equation, Test of significance, chi-square test, analysis of variance