Bankim Sardar College A College with Potential for Excellence
Department of Chemistry
Programme Specific Outcome (PSO) - Course Outcome (CO)
Programme Specific Outcome (PSO) :
PSO 01. To understand basic facts and concepts in Chemistry while retaining the exciting aspects of Chemistry so as to develop interest in the study of chemistry as a discipline. PSO 02. To develop the ability to apply the principles of Chemistry. PSO 03. To appreciate the achievements in Chemistry and to know the role of Chemistry in nature and in society. PSO 04. To develop problem solving skills. PSO 05. To be familiarised with the emerging areas of Chemistry and their applications in various spheres of Chemical sciences and to apprise the students of its relevance in future studies. PSO 06. To develop skills in the proper handling of apparatus and chemicals. PSO 07. To be exposed to the different processes used in industries and their applications.
Core Content of CU Syllabus Course Outcome Courses
Semester 1
CCH01A INORGANIC CHEMISTRY-1 Students will be able to Extra nuclear Structure of atom CO 01. Develop an ability to use Quantum numbers and their significance, Schrödinger‟s wave conceptual and mathematical tools equation, significance of ψ and ψ2. Radial and angular wave functions to express and predict atomic and for hydrogen atom. Radial and angular distribution curves. Shapes of molecular behavior s, p, d and f orbitals. Pauli‟s Exclusion Principle, Hund‟s rules and CO 02. Discuss the Quantum mechanical multiplicity, Exchange energy, Aufbau principle and its limitations, concept of atom in the light of Ground state Term symbols of atoms and ions for atomic number upto modern chemistry 30. CO 03. Interpret and explain the theories Acid-Base reactions associated with various acid –base Acid-Base concept: Arrhenius concept, theory of solvent system (in reactions
H2O, NH3, SO2 and HF), Bronsted-Lowry‟s concept, relative strength CO 04. Perceive the electronic of acids, Pauling‟s rules. Lux-Flood concept, Lewis concept, group interpretations of Reduction and characteristics of Lewis acids, solvent leveling and differentiating Oxidation reactions effects.Thermodynamic acidity parameters, Drago-Wayland equation. CO 05. Make use of an analytical balance Superacids, Gas phase acidity and proton affinity; HSAB principle. for mass measurement Acid-baseequilibria in aqueous solution (Proton transfer equilibria in CO 06. Make use of graduated cylinders, water), pH, buffer.Acid-base neutralisation curves; indicator, choice graduated pipettes, and volumetric of indicators. pipettes for volumetric Redox Reactions measurement Ion-electron method of balancing equation of redox reaction. CO 07. Have hands on experience of Elementary idea on standard redox potentials with sign conventions, different common laboratory Nernst equation (without derivation). Influence of complex formation, techniques like acid/base titrations precipitation and change of pH on redox potentials; formal potential. and redox titrations Feasibility of a redox titration, redox potential at the equivalence CO 08. Undertake experiments in point, redox indicators. Redox potential diagram (Latimer and Frost laboratory condition for the diagrams) of common elements and their applications. estimation of metals in different Disproportionation and comproportionation reactions (typical mixtures examples). 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. Solubility and solubility effect – common ion effect and their applications to the precipitation and separation of common metallic ions as hydroxides, sulfides, phosphates, carbonates, sulfates and halides Practical: Acid and Base Titrations: (DEMO ONLY) 1. Estimation of carbonate and hydroxide present together in mixture 2. Estimation of carbonate and bicarbonate present together in a mixture. 3. Estimation of free alkali present in different soaps/detergents. Oxidation-Reduction Titrations:
1. Estimation of Fe(II) using standardized KMnO4 solution 2. Estimation of oxalic acid OR sodium oxalate in a given mixture
3. Estimation of Fe(II) and Fe(III) in a given mixture using K2Cr2O7 solution. 4. Estimation of Fe(III) and Mn(II) in a mixture using standardized
KMnO4 solution
5. Estimation of Fe(III) and Cu(II) in a mixture using K2Cr2O7.
6. Estimation of Fe(III) and Cr(III) in a mixture using K2Cr2O7. The students will develop a clear concept of CCH01B Basics of Organic Chemistry 1.Bonding and Physical Properties CO 09. The Valence(18Lectures) bond (i) Valence Bond Theory: concept of hybridisation, shapes of CO 10. Various Electronic displacements molecules, resonance (including hyperconjugation); calculation of effects formal charges and double bond equivalent (DBE); orbital pictures of CO 11. Molecular Orbital Theory for bonding (sp3, sp2, sp: C-C, C-N & C-O systems and s-cisand s-trans Highest Occupied Molecular geometry for suitable cases). Orbital (HOMO), Lowest (ii) Electronic displacements: inductive effect, field effect, Unoccupied Molecular orbital mesomeric effect, resonance energy; bond polarization and bond (LUM and Single occupied polarizability; electromeric effect; steric effect, steric inhibition of Molecular Orbital (SOMO) resonance. CO 12. Aromaticity, Antiaromaticity, MO theory: qualitative idea about molecular orbitals, bonding and Homoaromaticity and Non antibonding interactions, idea about σ, σ*, π, π *, n – MOs; concept of aromaticity HOMO, LUMO and SOMO; sketch and energy levels of π MOs of i) CO 13. Several Physical properties such as acyclic p orbital system (C=C, conjugated diene, triene, allyl and bond dissociation energy and bond pentadienyl systems) ii) cyclic p orbital system (neutral systems: [4], energy; bond distances, bond [6] annulenes; charged systems: 3-,4-,5-membered ring systems); angles, bond angle strain, polarity, Hückel‟s rules for aromaticity up to [8] annulene (including Heat of Hydrogenation and heat of mononuclear heterocyclic compounds up to 6- membered ring); combustion etc. concept of antiaromaticity and homoaromaticity; non-aromatic molecules; Frost diagram (qualitative drawing). Physical properties: influence of hybridization on bond properties: The students will be able to develop an bond dissociation energy (BDE) and bond energy; bond distances, understanding of bond angles; concept of bond angle strain; melting point/boiling point CO 14. Definition of Reaction mechanism and solubility of common organic compounds in terms of covalent & and Mechanistic classification e.g, non-covalent intermolecular forces; polarity of molecules and dipole ionic, radical and pericyclic moments; relative stabilities of isomeric hydrocarbons in terms of heat mechanism of hydrogenation and heat of combustion data. CO 15. Explanation of ionic mechanism 2. General Treatment of Reaction Mechanism with examples Mechanistic classification: ionic, radical and pericyclic (definition CO 16. Explanation of pericyclic and example); reaction type: addition, elimination and substitution mechanism with examples reactions (definition and example); nature of bond cleavage and bond CO 17. Examples and reason of homolytic formation: homolytic and heterolytic bond fission, homogenic and and heterolytic bond cleavage heterogenic bond formation; curly arrow rules in representation of CO 18. Examples and reason of mechanistic steps; reagent type: electrophiles and nucleophiles homogenic and heterogenic bond (elementary idea). formation
CO 19. Representation of mechanistic
steps using arrow formalism
CO 20. Basic idea of electrophilesand
nucleophiles
The students will be able to distinguish Practical different organic compounds from the given Separation based upon solubility, by using common laboratory mixture by reagents like water (cold,hot), dil. HCl, dil. NaOH, dil. NaHCO3, etc., of components of a binary solid mixture; purification of any one of CO 21. Separation based upon solubility the separated components by crystallization and determination of its CO 22. Purification based on melting point. The composition of the mixture should be of the crystallization using proper following types :p-Nitrobenzoic acid/p-Aminobenzoic acid; p- solvents Nitrotolune/p-Anisidine; benzoic acid/naphthalene; urea/phenyl CO 23. Determination of its melting point benzoate; p-toluidine/benzophenone; p-chlorobenzoic acid/ by using Conc. H2SO4 Bath, Metal benzophenone, Benzoic acid/Anthracene; Glucose/Biphenyl; Benzoic bath acid/Benzophenone; Urea/Benzophenone. Use of pH paper is recommended. CCH02A PHYSICAL CHEMISTRY-1 Students will be able CO 01. To understand kinetic theory of Kinetic Theory and Gaseous state gases Kinetic Theory of gases: Concept of pressure and temperature; CO 02. To get an introduction to the basic Collision of gas molecules; Collision diameter; Collision number and concepts of pressure, temperature mean free path; Frequency of binary collisions (similar and different and velocity of ideal gases. molecules); Wall collision and rate of effusion Maxwell‟s distribution CO 03. To get a picture about the of speed and energy: Nature of distribution of velocities, Maxwell's probability of finding a molecule distribution of speeds in one, two and three dimensions; Kinetic with a speed falling in a particular energy distribution in one, two and three dimensions, calculations of range average, root mean square and most probable values in each case; CO 04. To explain the key concepts of Calculation of number of molecules having energy≥ε, Principle of degree of freedom, equipartition of equipartitionof energy and its application to calculate the classical energy and specific heat limit of molar heat capacity of gases Real gas and virial equation: CO 05. To get a concept of collision among Deviation of gases from ideal behavior; compressibility factor; Boyle molecules and with the wall temperature; Andrew's and Amagat's plots; van der Waals equation CO 06. To understand deviation of real gas and its features; its derivation and application in explaining real gas from ideal behavior. behaviour, other equations of state (Berthelot, Dietrici); Existence of CO 07. To understand critical constant and critical state, Critical constants in terms of van der Waals constants; vanderwall‟s constant. Law of corresponding states; virial equation of state; van der Waals CO 08. To learn about the different equation expressed in virial form and significance of second virial intermolecular forces coefficient; CO 09. To be able to derive rate equations Intermolecular forces (Debye, Keesom and London interactions; from mechanistic data Lennard-Jones potential - elementary idea) CO 10. To make use of simple models for Transport processes predictive understanding of Diffusion : Fick‟s law, Flux, force, phenomenological coefficients & physical phenomena associated to their interrelationship (general form), different examples of transport kinetics properties CO 11. To study the dependence of the Viscosity: General features of fluid flow (streamline flow and rate of chemical reactions on turbulent flow); Newton‟s equation, viscosity coefficient; Poiseuille‟s properties like pressure, equation ( with derivation); principle of determination of viscosity temperature, presence of catalyst coefficient of liquids by falling sphere method and using Ostwald's CO 12. To understand transport properties viscometer. Temperature variation of viscosity of liquids and
comparison with that of gases. Relation between viscosity coefficient
of a gas and mean free path.
Chemical kinetics Rate law, order and molecularity: Introduction of
rate law, Extent of reaction; rate constants, order; Forms of rates of
First, second and nth order reactions; Pseudo first order reactions
(example using acid catalyzed hydrolysis of methyl acetate);
Determination of order of a reaction by half-life and differential
method; Rate determining step and steady-state approximation –
explanation with suitable examples;) Opposing reactions, consecutive
reactions and parallel reactions (with explanation of kinetic and
thermodynamic control of products; all steps first order). Role of
Temperature : Temperature dependence of rate constant; Arrhenius
equation, energy of activation; Homogeneous catalysis: Homogeneous catalysis with reference to acid-base catalysis; Enzyme catalysis; Michaelis-Menten equation, Lineweaver-Burk plot, turn-over number.
Practical: Experiment 1: Study of kinetics of decomposition of H2O2 CO 13. To have a hands on experience Experiment 2: Study of kinetics of acid-catalyzed hydrolysis of about the different concepts of methyl acetate kinetics theory, flow properties and solubility Experiment 3: Study of viscosity of unknown liquid (glycerol, sugar) with respect to water.
Experiment 4: Study of the variation of viscosity with the concentration of the solution
Experiment 5: Determination of solubility of sparingly soluble salt in water, in electrolyte with common ions and in neutral electrolyte (using common indicator)
CCH02B Organic Chemistry Students will gather knowledge about Stereochemistry I CO 14. the three dimensional structure of Bonding geometries of carbon compounds and representation of any Sp3hybridised chiral organic molecules:tetrahedral nature of carbon and concept of asymmetry; compound by understanding Fischer, sawhorse, flying wedge and Newman projection formulae CO 15. Bonding geometries of carbon
and their inter translations. compounds and representation of Concept of chirality and symmetry:symmetry elements, molecular molecules by Projection chirality and centre of chirality; asymmetric and dissymmetric Formulae,Interconversion of a three molecules; enantiomers and diastereomers; concept of stereogenicity, dimensional structure, Chirality and chirotopicity and pseudoasymmetry; chiral centres and number of asymmetry, Dextrorotatory and stereoisomerism: systems involving 1/2/3-chiral centre(s) (AA, AB, laevorotatory isomers ABA and ABC types). CO 16. Concept of chirality and symmetry Relative and absolute configuration:D/L and R/S descriptors; by Definition with examples of erythro/threoand mesonomenclature of compounds; syn/anti Symmetry elements and its nomenclatures for aldols; E/Z descriptors for C=C, conjugated diene, classification, optical isomers , triene, C=N and N=N systems; combination of R/S- and E/ Z- Concept of Stereogenicity and isomerisms. Chirotopicity , Difference between them Optical activity of chiral compounds:optical rotation, specific rotation CO 17. Definition and rules of writing and molar rotation; racemic compounds, racemisation (through Relative (D-L)and absolute (R-S cationic, anionic, radical intermediates and through reversible )Configuration and also their formation of stable achiral intermediates); resolution of acids, bases Assignments, Examples of and alcohols via diastereomeric salt formation; optical purity and threo/erythro nomenclatures for enantiomeric excess; invertomerism of chiral trialkylamines. aldols with definition, syn/anti, General Treatment of Reaction Mechanism II cis/trans , E/Z Reactive intermediates:carbocations (carbenium and carbonium CO 18. Optical activity of chiral ions), non-classical cabocations, carbanions, carbon radicals, compounds by optical rotation, carbenes: generation and stability, structure using orbital picture and specific rotation, optical purity or electrophilic/nucleophilic behavior of reactive intermediates enantiomeric excess, Definition (elementary idea). classification of racemic
modification, racemisation and resolution. invertomerism of trialkylamines CO 19. Students will have a clear concept of Structures, Types and Applications of Reactive intermediates and their stabilities. CO 20. Electrophilic behavior of Carbocations&Nucleophilic behavior of Carbanions CO 21. Electrophilic / Nucleophilic behavior of Carbon Radicals CO 22. Elementary idea of generation and fate of the all intermediates
ORGANIC CHEMISTRY: O(1B)LAB ORGANIC CHEMISTRY: O (1B) LAB Determination of boiling point of common organic liquid CO 23. The students will be able to compounds :n- butyl alcohol, cyclohexanol, ethyl methyl ketone, determine the boiling points of cyclohexanone, acetylacetone,isobutyl methyl ketone, isobutyl common organic liquid compounds alcohol, acetonitrile, benzaldehyde and acetophenone. [Boiling by using boiling point bath. points of the chosen organic compounds should preferably be within1800C].
Core Content of CU Syllabus Course Outcome Courses
Semester 2
CCH 03 Stereochemistry II The 2nd part of Stereochemistry will give the Chirality arising out of stereoaxis: stereoisomerism of substituted students a clear picture of cumulenes with even and odd number of double bonds; chiral axis in allenes, spiro compounds, alkylidenecycloalkanes and CO 01. Chirality arising out of stereoaxis in
biphenyls;relatedconfigurational descriptors (Ra/Sa);atropisomerism; allens and biphenyls racemisation of chiral biphenyls. Atropisomerism, Assignment of Concept of prostereoisomerism: prostereogeniccentre; concept of R/S descriptor in allenes and (pro)n-chirality: topicity of ligands and faces (elementary idea); biphenyls pro-R/pro-S, pro-E/pro-Z and Re/Si descriptors;pro-rand pro-s CO 02. Concept of prostereoisomerism, descriptors of ligands on propseudoasymmetriccentre prochirality, prostereogenicity, Conformation: conformational nomenclature: eclipsed, staggered, Topicity of ligands and faces, gauche, synandanti; dihedral angle, torsion angle;Klyne-Prelog Pseudoasymmetry, Pro-R and Pro-S terminology; P/M descriptors; energy barrier of rotation, concept of designation of enantiotopic groups, torsional and steric strains; relative stability of conformers on the Re /Si designation designation of basis of steric effect, dipole-dipole interaction and H-bonding; enantiotopicnddiastereotopic faces butane gauche interaction; conformational analysis of ethane, CO 03. Conformational nomenclature, propane, n-butane, 2-methylbutane and 2,3-dimethylbutane; Determination of conformational haloalkane, 1,2-dihaloalkanes and 1,2-diols (up to four carbons); analysis and Potential Energy 1,2-halohydrin; conformation of conjugated systems (s-cisands- diagram of various hydrocarbons, trans). halohydrocarbons glycols CO 04. Reaction thermodynamics i.e., basic General Treatment of Reaction Mechanism III idea about free energy, Equilibrium, Reaction thermodynamics: free energy and equilibrium, enthalpy enthalpy, entropy, by Explaining and entropy factor, calculation of enthalpy change via BDE, intermolecular &intramolecular intermolecular & intramolecular reactions. reactions with examples Concept of organic acids and bases: effect of structure, substituent CO 05. Concept of organic acids and and solvent on acidity and basicity; proton sponge; comparison bases,their structure, effect of between nucleophilicity and basicity; application of thermodynamic substituent, solvent on acidity and principles in acid-base equilibria. basicity Tautomerism:prototropy (keto-enol, nitro - aci-nitro, nitroso- CO 06. Definition and types of tautomerism oximino, diazo-amino and enamine-imine systems); valence with examples tautomerism and ring-chain tautomerism; composition of the CO 07. Concept of Reaction kinetics with equilibrium in different systems (simple carbonyl; 1,2- and 1,3- Free energy profiles for one and dicarbonyl systems, phenols and related systems), factors affecting multi step reactions with rate keto-enoltautomerism; application of thermodynamic principles in constant and free energy of tautomeric equilibria. activation , Free energy profiles for Reaction kinetics: rate constant and free energy of activation; free catalysed reactions (electrophilic energy profiles for one-step, two-step and three-step reactions; and nucleophiliccatalysed catalyzed reactions: electrophilic and nucleophilic catalysis; kinetic reactions), Kinetic control and control and thermodynamic control of reactions; isotope effect: thermodynamic control of reactions, primary and β-secondary kinetic isotopic effect (kH /kD); principle Primary kinetic isotopic effect of microscopic reversibility; Hammond‟s postulate. (kH/kD), CO 08. Hammond postulate
Substitution and Elimination Reactions After studying this topic students will gain Free-radical substitution reaction: halogentaion of alkanes, the knowledge of the followings mechanism (with evidence) and stereochemical features; reactivity- CO 09. Concept, Types& Role of leaving selectivity principle in the light of Hammond‟s postulate. group (SN1, SN2, SNi) and 3 Nucleophilic substitution reactions: substitution at sp Mechanisms of Sustitution Reaction centre[systems: alkyl halides, allyl halides, benzyl halides, alcohols, at sp3 centre ethers, epox -halocarbonyls]:mechanisms (with CO 10. Concept, Types and Mechanisms of evidence),relative rates& stereochemical features: SN1, SN2, SN2', elimination reactions.( E1, E2 and SN1' (allylic rearrangement) and SNi; effectsof solvent, substrate E1cB), Reactivity of different structure, leaving group and nucleophiles (including ambident substrates on elimination reactions, nucleophiles, cyanide & nitrite); substitutions involving NGP (with Orientation (Saytzeff/ Hofmann hetero atoms and aryl groups); role of crown ethers and phase rules) transfer catalysts. CO 11. Substitution vs elimination Elimination reactions: E1, E2, E1cB and Ei (pyrolytic syn eliminations); formation of alkenes and alkynes; mechanisms (with evidence), reactivity, regioselectivity (Saytzeff/Hofmann) and stereoselectivity; comparison between substitution and elimination.
Practical Organic Preparations The students will develop the skill of A. The following reactions are to be performed, noting the CO 12. Synthesis of some organic yield of the crude product: compounds given in the syllabus by 1. Nitration of aromaticcompounds,2.Condensationreactions, several methods 3.Hydrolysis of amides/imides/esters, 4. Acetylation of CO 13. Purification of the crude product phenols/aromaticamines, 5. Brine mediated benzoylation of based on crystallization amines/aminoacids, 6. Side chain oxidation of CO 14. Determination of melting point of aromaticcompounds, 7. Diazo coupling reactions of the Crystals by using Conc. H2SO4 aromaticamines, 8. Bromination of anilides using green Bath, Metal bath approach (Bromate-Bromidemethod),9. Redox reaction CO 15. Calculation of % of Yield. including solid-phasemethod, 10. Green „multi-component- coupling‟reaction, 11.Selective reduction of m-dinitrobenzene tom-nitroaniline Students must also calculate percentage yield, based upon isolated yield (crude) and theoretical yield. B. Purification of the crude product is to be made by crystallisation from water/alcohol, crystallization after charcoal treatment, or sublimation, whichever is applicable. Melting point of the purified product is to be noted.
CCH04 Chemical Bonding-I Students will be able to (i) Ionic bond: General characteristics, types of ions, size CO 01. Discuss various aspects of chemical effects, radius ratio rule and its application and limitations. Packing bonding in ionic compounds and of ions in crystals.Born-Landé equation with derivation and associated theories. importance of Kapustinskii expression for lattice energy. Madelung CO 02. Explain the reasons of structural constant, Born-Haber cycle and its application, Solvation defects of various ionic compounds. energy.Defects in solids (elementary idea). Solubility energetics of CO 03. Appreciate and explain the concept dissolution process of chemical bonding in covalent (ii) Covalent bond: Polarizing power and polarizability, ionic compounds and discuss associated potential,Fazan‟s rules. Lewis structures, formal charge. Valence theories thereof. Bond Theory. The hydrogen molecule (Heitler-London approach), CO 04. Explain shape of molecule in the directional character of covalent bonds, hybridizations, equivalent light of VSEPR theory. and non-equivalent hybrid orbitals, Bent‟s rule, Dipole moments, CO 05. Appreciate and explain the theory of VSEPR theory, shapes of molecules and ions containing lone pairs LCAO method for molecular orbital and bond pairs (examples from main groups chemistry) and multiple designing bonding (ζ and π bondapproach). CO 06. Discuss the concept of HOMO, Chemical Bonding-II LUMO and Orbital mixing (i) Molecular orbital concept of bonding (The approximations CO 07. Draw MO Diagram of Homo of the theory, Linear combination of atomic orbitals (LCAO)) nuclear and Hetero nuclear molecules. (elementary pictorial approach): sigma and pi- bonds and delta CO 08. Discuss the various aspects of interaction, multiple bonding. Orbital designations: gerade, radioactivity, including nuclear
ungerade, HOMO, LUMO. Orbital mixing,. MO diagrams of H2, stability, artificial radioactivity,
Li2, Be2, B2, C2, N2, O2, F2, and their ions wherever possible; power generation, determination of + - Heteronuclear molecular orbitals: CO, NO, NO , CN , HF, BeH2, age of rocks and minerals, safety
CO2and H2O. Bond properties: bond orders, bondlengths. measures for handling and storage (ii) Metallic Bond:Qualitative idea of valence bond and band of radioactive compounds. theories. Semiconductors and insulators, defects insolids. (iii) Weak Chemical Forces:Hydrogen bonding (theories of hydrogen bonding, valence bond treatment), receptor-guest interactions, Halogen bonds. Effects of chemical force, melting and boiling points.
Radioactivity Nuclear stability and nuclear binding energy. Nuclear forces: meson exchange theory. Nuclear models (elementary idea): Concept of nuclear quantum number, magic numbers. Nuclear Reactions: Artificial radioactivity, transmutation of elements, fission, fusion and spallation. Nuclear energy and power generation.Separation and uses of isotopes. Radio chemical methods: principles of determination of age of rocks and minerals, radio carbon dating,
hazards of radiation and safety measures. Practical: Iodo-/ Iodimetric Titrations CO 09. Undertake iodometric 1. Estimation of VitaminC /iodimetricestmation of different 2. Estimation of (i) arsenite and (ii) antimony important compounds in laboratory iodimetrically condition. 3. Estimation of available chlorine in bleachingpowder. CO 10. Estimate different constituents of Estimation of metal content in some selective samples various alloys in laboratory 1. Estimation of Cu in brass. conditions 2. Estimation of Cr and Mn inSteel. 3. Estimation of Fe incement.
Core Content of CU Syllabus Course Outcome Courses
Semester 3
CCH05 Chemical Thermodynamics I Students will be able 1st law of Thermodynamics: Intensive and extensive variables; state CO 01. To provide an insight into some of and path functions; isolated, closed and open systems; zeroth law of the fundamental concepts and thermodynamics;Concept of heat, work, internal energy and principles that are very essential in statement of first law; enthalpy, H; relation between heat capacities, the study of chemistry. calculations of q, w, ΔU and ΔH for reversible, irreversible and free CO 02. To understand the principle of expansion of gases (ideal and van der Waals) under isothermal and conservation of energy and how this adiabatic conditions; Joule‟s experiment and its consequence principle can be used to assess the Thermochemistry:Standard states; Heats of reaction; enthalpy of energy changes that accompany formation of molecules and ions and enthalpy of combustion and its physical and chemical processes. applications; Laws of thermochemistry; bond energy, bond CO 03. To examine the means by which a dissociation energy and resonance energy from thermochemical system can exchange energy with its data, Kirchhoff‟s equations ; Adiabatic flametemperature. surroundings in terms of the work it ChemicalThermodynamicsII may do or the heat it may produce. Second Law:Need for a Second law; statement of the second law of CO 04. To understand the thermodynamic thermodynamics; Concept of heat reservoirs and heat engines; description of mixtures state function, Carnot cycle; Carnot engine and refrigerator; Kelvin – Planck and exact, inexact differential Clausius statements and equivalence of the two statements with CO 05. To understand the statements of 1st entropic formulation; Carnot's theorem; Values of §dQ/T and and 2nd laws of thermodynamics. Clausiusinequality;Physical concept of Entropy; Entropy is a CO 06. To learn the thermodynamic aspects measure of the microscopic disorder of the system. Entropy change of various processes and reactions. of systems and surroundings for various processes and CO 07. To understand the concept of transformations; Entropy and unavailable work; Auxiliary state thermochemistry enthalpy change of functions (G and A) and their variation with T, P and V. Criteria for different processes spontaneity and equilibrium. Thermodynamic relations: Maxwell's CO 08. To get the concept of Entropy (S) relations; Gibbs- Helmholtz equation, Joule- Thomson experiment from Carnot cycle and the and its consequences; inversion temperature; Joule-Thomson significance of Helmholtz free coefficient for a van der Waals gas; General heat capacity relations energy(A) & Gibb‟s free energy (G). Systems of Variable Composition: CO 09. To explain the criteria of spontaneity Partial molar quantities, dependence of thermodynamic parameters in terms of S, A and G. on composition; Gibbs-Duhem equation, chemical potential of ideal CO 10. To be able to derive important mixtures, change in thermodynamic functions in mixing of ideal thermodynamic relations gases. Activities and activity coefficients. Fugacity and fugacity CO 11. To learn the basic concept of coefficient. equilibrium CO 12. To develop an understanding of Applications of Thermodynamics–I electrochemistry and the methods Chemical Equilibrium: used to study the response of an electrolyte through current of Thermodynamic conditions for equilibrium, degree of potential advancement; van't Hoff's reaction isotherm (deduction from CO 13. To understand the difference between chemical potential); Variation of free energy with degree of voltaic/galvanic and electrolytic advancement; Equilibrium constant and standard Gibbs free energy electrochemical cells. change; Van't Hoff's reaction isobar and isochore from different CO 14. To understand why standard standard states; Le Chatelier's principle and its derivation, variation reduction potentials are used and how of equilibrium constant under different conditions Nernst‟s they are determined. distribution law; Application- (eg. dimerization of benzene in CO 15. To know how the standard states used benzoic acid). Solvent Extraction. for E° and ΔG° are defined for gases ELECTROCHEMISTRY: solids liquids and solutes. (i) Conductance and transport number CO 16. To be able to write balanced half Ion conductance; Conductance and measurement of conductance, reactions determine overall cell cell constant, specific conductance and molar conductance; reactions, calculate the standard Variation of specific and equivalent conductance with dilution for reduction potential and predict the strong and weak electrolytes; Kohlrausch's law of independent direction of electron anion and cation migration of ions; Equivalent and molar conductance at infinite flow based on a sketch of an dilution and their determination for strong and weak electrolytes; electrochemical cell or the description Debye –Huckel theory of Ion atmosphere (qualitative)-asymmetric of an electrochemical cell given in effect, relaxation effect and electrophoretic effect; Debye-Huckel limiting law-brief qualitative description. Estimation of activity shorthand notation. coefficient for electrolytes using Debye-Huckel limiting law. CO 17. To understand the relationship Ostwald's dilution law; Ionic mobility; Application of conductance between chemical energy (Gibbs free measurement (determination of solubility product and ionic product energy change for a redox reaction) of water); Conductometrictitrations.Transport number, Principles of and electrical energy (electromotive Hittorf‟s and Moving-boundary method; Wien effect, Debye- force or cell potential) in an Falkenhagen effect, Walden‟s rule electrochemical cell. (ii) Ionic equilibrium: CO 18. To be prepared to use standard Strong, moderate and weak electrolytes, degree of reduction potentials to calculate the ionization, factors affecting degree of ionization, ionization constant standard cell potential E° for an and ionic product of water. Ionization of weak acids and bases, pH electrochemical cell. scale, common ion effect; dissociation constants of mono-, di-and CO 19. To explain the various terms such as triprotic acids (exacttreatment). specific conductance, equivalent Salt hydrolysis- calculation of hydrolysis constant, degree of conductance and molar conductance. hydrolysis and pH for different salts (exact CO 20. To Explain the method of Treatment).Determination of hydrolysis constant determination of equivalent conductometrically. Buffer solutions; derivation of Henderson conductance understand the factors equation and its applications; buffer capacity, buffer range, buffer affecting the conductance of action . Qualitative treatment of acid electrolytic solution – base titration curves (calculation of pH at various stages). Theory CO 21. To Explain the effect of dilution on of acid–base indicators; selection of indicators and their limitations. specific conductance, equivalent Multistage equilibrium in polyelectrolyte systems; hydrolysis and conductance and molar conductance hydrolysis constants CO 22. To understand the ionic mobility of different ions, Electromotive Force: Rules of oxidation/reduction of ions based methods of determination of ionic on half-cell potentials,; Chemical cells, reversible and irreversible mobility of ions cells with examples; Electromotive force of a cell and its CO 23. To understand Kohlrausch‟s law and measurement, Thermodynamic derivation of Nernst equation; its applications Standard electrode (reduction) potential and its application to CO 24. To understand the basic concepts different kinds of half-cells. Application of EMF measurements in of Arrhenius theory of electrolytic determining (i) free energy, enthalpy and entropy of a cell reaction, dissociation, evidences in support of (ii) equilibrium constants, and (iii) pH values, using hydrogen, Arrhenius theory of electrolytic quinone-hydroquinone and glasselectrodes Concentration cells with dissociation and its limitation, and without transference, liquid junction potential; determination of CO 25. To understand Ostwald‟s dilution activity coefficients and transference numbers; Potentiometric law and its application in titrations (acid-base, redox,precipitation) determination of Dissociation constant of weak electrolyte CO 26. To understand the need of another
theory for strong electrolyte CO 27. To understand the term- Electrophoretic and Asymmetric effect CO 28. To understand Debye-Huckel theory of strong electrolyte and its mathematical equation
CO 29. To define -Transport number or
transference number of ions
CO 30. To understand the various methods
of determination of transport number of ions Practical : CO 31. To appreciate the importance of conductometric measurement, Experiment 1: Conductometric titration of an acid (strong, weak/ CO 32. To differentiate between various monobasic, dibasic, and acid mixture ) against strong base. types of conductometric titrations, Experiment 2: Study of saponification reaction conductometrically CO 33. To explain the nature of various acid- Experiment 3: Verification of Ostwald‟s dilution law and base titration curves as well as acid determination of Ka of weak acid mixture versus base graph, Experiment 4:Potentiometric titration of Mohr‟s salt solution CO 34. To explain the precipitation titrations against standard K2Cr2O7andKMnO4solution and displacement titrations, Experiment 5: Determination of Ksp for AgCl by potentiometric CO 35. To explain and determine the titration of AgNO3 solution against standard KCl solution solubility product of any sparingly Experiment 6: Determination of heat of neutralization of a strong soluble using conductivity method acid by a strong base CO 36. To describe the method of determination of ionic product of water using conductometric measurement
CCH06 Chemical periodicity Students will be able to Modern IUPAC Periodic table, Effective nuclear charge, screening CO 01. Discuss the properties of different effects and penetration, Slater‟s rules, atomic radii, ionic radii elements in the periodic table . (Pauling‟s univalent), covalent radii, lanthanide contraction. CO 02. Discuss the methods of preparation,- Ionization potential, electron affinity and electronegativity properties and structure of different (Pauling‟s, Mulliken‟s and Allred-Rochow‟s scales) and factors useful chemical compounds . Effectively articulate various aspects influencing these properties, group electronegativities.Group trends CO 03. of the noble gases‟ chemistry. and periodic trends in these properties in respect of s-, p- and d- CO 04. Explain the chemistry of Inorganic block elements.Secondary periodicity, Relativistic Effect, Inert Polymers paireffect. CO 05. Discuss about the Co ordination Chemistry of s and p BlockElements Compounds with respect to their Relative stability of different oxidation states, diagonal relationship nomenclature, classification and and anomalous behaviour of first member of each group. Allotropy geometries and catenation.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.Beryllium hydrides and halides.Boric acid and borates, boron nitrides, borohydrides (diborane) and graphitic compounds, silanes, Oxides and oxoacids
of nitrogen, phosphorus, sulphur and chlorine.Peroxo acids of sulphur, sulphur-nitrogen compounds, interhalogen compounds, polyhalide ions, pseudohalogens, fluorocarbons and basic properties of halogens. Noble Gases: Occurrence and uses, rationalization of inertness of noble gases, Clathrates; preparation and properties of XeF , XeF and XeF ; 2 4 6 Nature of bonding in noble gas compounds (Valence bond
treatment and MO treatment for XeF2 and XeF4). Xenon-oxygen compounds. Molecular shapes of noble gas compounds (VSEPR theory). Inorganic Polymers: Types of inorganic polymers, comparison with organic polymers,
synthesis, structural aspects and applications of silicones and siloxanes.Borazines, silicates and phosphazenes. CoordinationChemistry-I Coordinate bonding: double and complex salts. Werner‟s theory of coordination complexes, Classification of ligands, Ambidentate ligands, chelates, Coordination numbers, IUPAC nomenclature of coordination complexes (up to two metal centers), Isomerism in
coordination compounds, constitutional and stereo isomerism, Geometrical and optical isomerism in square planar and octahedralcomplexes. Practical: Complexometric titration 1. Zn(II) CO 06. Estimate quantitatively metals present in different mixtures Zn(II) in a Zn(II) and Cu(II)mixture. 2. complexometrically in laboratory 3. Ca(II) and Mg(II) in amixture. condition 4. Hardness ofwater. CO 07. Estimate quantitatively particular 5. Al(III) in Fe(III) and Al(III) in amixture metal ions from a mixture following Chromatography of metal ions paper chromatography technique CO 08. Estimate quantitatively different Principles involvedin chromatographicseparations. metals following Gravimetric Paper chromatographic separation of following metalions: Method 1. Ni (II) and Co(II) 2. Fe (III) and Al(III) Gravimetry 1. Estimation of Ni(II) using Dimethylglyoxime(DMG). 2. Estimation of copper asCuSCN. 3. Estimation of Al(III) by precipitating with oxine and weighing
as Al(oxine)3(aluminiumoxinate). 4. Estimation ofchloride The students will develop the knowledge of CCH07 Chemistry of alkenes and alkynes Addition reaction by learning Addition to C=C:mechanism (with evidence wherever applicable), CO 01. The Mechanism, Reactivity of reactivity, regioselectivity (Markownikoff and anti-Markownikoff Electrophilic Addition to C=C bond additions) and stereoselectivity; reactions: hydrogenation, with different electrophiles, halogenation, hydrohalogenation, hydration, oxymercuration- Difference between regioselectivity, demercuration, hydroboration-oxidation, epoxidation, syn and anti- stereoselectivity, Ozonolysis hydroxylation, ozonolysis, addition of singlet and triplet carbenes; reactions with mechanism, allylic and benzylicbromination, use of NBS, Simmons-Smith cyclopropanation reaction; electrophilic addition to Birch reduction of benzenoid diene (conjugated dienes and allene); radical addition: HBr addition; aromatics, interconversion of E- and mechanism of allylic and benzylic bromination in competition with Z- alkenes, electrophiilic addition to brominations across C=C; use of NBS; Birch reduction of benzenoid conjugated diene, allenes aromatics; interconversion of E- and Z- alkenes; contra- CO 02. Mechanism and Reactivity of thermodynamic isomerization of internal alkenes. Electrophilic Addition to C≡C Addition to C≡C (in comparison to C=C):mechanism, reactivity, CO 03. The acidities of the terminal alkynes regioselectivity(Markownikoff and anti-Markownikoff addition) and CO 04. Interconversion of terminal and non- stereoselectivity; reactions:hydrogenation, halogenations, terminal alkynes hydrohalogenation, hydration, oxymercuration- demercuration, The students will understand the hydroboration-oxidation, dissolving metal reduction of alkynes CO 05. General Mechanism, Orientation, (Birch); reactions of terminal alkynes by exploring its acidity; Reactivity of different Electrophilic aromatic substitution interconversion of terminal and non-terminal alkynes. CO 06. Mechanism of Nucleophilic aromatic Aromatic Substitution substitution Electrophilic aromatic substitution:mechanisms and evidences in favour of it; orientation and reactivity; reactions: nitration, nitrosation, sulfonation, halogenation, Friedel-Crafts reaction; one- carbonelectrophiles (reactions:chloromethylation, Gatterman-Koch, Gatterman, Houben-Hoesch,Vilsmeier-Haack, Reimer-Tiemann, Students will achieve the knowledge on Kolbe-Schmitt); Ipso substitituion. CO 07. Mechanism and Reactivity of Nucleophilic aromatic substitution:addition-elimination Nucleophilic addition to Carbonyl mechanism and evidences in favour of it; SN1 mechanism; cine and Related Compounds with substitution (benzyne mechanism), structure of benzyne. different nucleophiles Carbonyl and Related Compounds CO 08. Mechanism of some condensation, Addition to C=O: structure, reactivity and preparation of carbonyl reduction and oxidation reaction of carbonyls compounds; mechanism (with evidence), reactivity, equilibrium and CO 09. Exploitation of acidity of α-H of C=O kinetic control; formation of hydrates, cyanohydrins and bisulphite by alkylation, halogenations, adduct; nucleophilic addition-elimination reactions with alcohols, aldolcondensationetcrection thiolsand nitrogen- based nucleophiles;reactions: benzoin CO 10. Some named rearrangements with condensation, Cannizzaro and Tischenko reactions, reactions with mechamism ylides: Wittig and Corey-Chaykovsky reaction; Rupe rearrangement, CO 11. Alkylation of active methylene oxidations and reductions: Clemmensen, Wolff-Kishner, LiAlH4, compounds (diethyl malonate and
NaBH4, MPV, Oppenauer, Bouveault-Blanc, acyloin condensation; ethyl acetoacetate )with mechamism oxidation of alcohols with PDC and PCC; periodic acid and lead CO 12. Mechanism of Nucleophilic addition tetraacetate oxidation of 1,2-diols. to α,β-unsaturated carbonyl system Exploitation of acidity of α-H of C=O: formation of enols and CO 13. Substitution at sp2 carbon (C=O system) by esterification and enolates; kinetic and thermodynamic enolates; reactions (mechanism Hydrolysis (BAC2, AAC2, AAC1, with evidence):halogenation of carbonyl compounds under acidic and AAL1), amide, Anhydrides, Acyl basic conditions, Hell-Volhard-Zelinsky (H. V. Z.) reaction, halides formation and their nitrosation, SeO2 (Riley) oxidation; condensations (mechanism with corresponding hydrolysed products. evidence): Aldol,Tollens‟, Knoevenagel, Claisen-Schmidt, Claisen ester including Dieckmann, Stobbe; Mannich reaction,Perkin Students be knowledgable about reaction, Favorskii rearrangement; alkylation of active methylene compounds; preparation and synthetic applications of diethyl CO 14. The General Idea, Structure and malonate and ethyl acetoacetate; specific enol equivalents (lithium Types of Organometallic compounds. enolates, enamines and silyl enol ethers) in connection with Few examples. Preparation of Grignard reagent and alkylation, acylation and aldol type reaction. CO 15. organo lithium with mechanism .Nucleophilic addition to α,β-unsaturated carbonyl CO 16. Mechanism of the addition reactions system:general principle and mechanism (with evidence); direct and of Grignard reagents, organo lithium conjugate addition, addition of enolates (Michael reaction), Stetter and Gilman cuprates to different reaction, Robinson annulation. electrophilic sites 2 Substitution at sp carbon (C=O system): mechanism (with CO 17. Mechanism of Reformatsky reaction, evidence): BAC2, AAC2, AAC1, AAL1 (inconnection to acid and ester); Blaise reaction by using organozinc acid derivatives: amides, anhydrides & acyl halides (formation and compound hydrolysis including comparison). CO 18. Some abnormal behaviours of Grignard reagents Organometallics CO 19. comparison of reactivity among Grignard reagent; Organolithiums; Gilman cuprates: preparation Grignard, organolithiums and and reactions (mechanism with evidence); addition of Grignard and organocopper reagents organolithium to carbonyl compounds; substitution on -COX; CO 20. Reversal of polarity. i.e., Umpolung directed ortho metalation of arenes using organolithiums, conjugate The students will be able to identify a single compound addition by Gilman cuprates; Corey-House synthesis; abnormal CO 21. Single organic compounds can be behaviour of identified by checking its Physical Grignard reagents; comparison of reactivity among Grignard, state (Solid and Liquid) organolithiums and organocopper reagents; Reformatsky reaction; CO 22. Then Identification of some solid and Blaise reaction; concept of umpolung liquid compounds are done primarily by using Practical: CO 23. litmus paper, Solubility test, Action A. Identification of a Pure OrganicCompound of heat,FeCl3 test, Silver mirror test, Solid compounds: oxalic acid, tartaric acid, citric acid, succinic acid, Fluorescence test, Fehling‟s test etc. resorcinol, urea, glucose, cane sugar, benzoic acid and salicylic acid CO 24. After having the idea about the probable name and nature of the Liquid Compounds: formic acid, acetic acid, methyl alcohol, ethyl compound it is identified correctly by alcohol, acetone, aniline, dimethylaniline, benzaldehyde, chloroform doing a single test for each solid and and nitrobenzene liquid compounds. B. Quantitative Estimations: CO 25. Developing the skill for estimating Each student is required to perform all the experiments different organic compound solutions 1. Estimation of glycine by Sörensen‟sformolmethod quantitatively 2. Estimation of glucose by titration using Fehling‟ssolution
3. Estimation of sucrose by titration using Fehling‟ssolution 4. Estimation of aromatic amine (aniline) by bromination (Bromate- Bromide)method 5. Estimation of acetic acid in commercialvinegar 6. Estimation of urea (hypobromitemethod) 7. Estimation of saponification value ofoil/fat/ester Students will be able to SECA Analytical Clinical Biochemistry CO 01. Explain the structure carbohydrates Carbohydrates: Biological importance of carbohydrates, and amino acids, their physical and Metabolism, Cellular currency of energy (ATP), Glycolysis, chemical properties and their Alcoholic and Lactic acid fermentations, Krebs cycle. function in living organisms. CO 02. Describe the function of enzyme as a Isolation and characterization of polysachharides. catalyst in maximum biological Proteins:Classification, biological importance; Primary and reaction and learn about the function secondary and tertiary structures of proteins: α-helix and β- pleated of enzyme, and also see how they are sheets, Isolation, characterization, denaturation of proteins. related to things they come across in daily life. Enzymes:Nomenclature, Characteristics (mention of Ribozymes), CO 03. Understand the effect of cholesterol and Classification; Active site, Mechanism of enzyme action, and triglycerides in human body Stereospecificity of enzymes, Coenzymes and cofactors, Enzyme CO 04. Knowabout steroid hormone which inhibitors, Introduction to Biocatalysis: Importance in “Green regulates carbohydrate metabolism Chemistry” and ChemicalIndustry. and has an anti-inflammatory effect Lipids:Classification. Biological importance of triglycerides and on the body. It helps maintain blood phosphoglycerides and cholesterol; Lipid membrane, Liposomes and pressure and regulate the salt and their biological functions and underlying applications. water balance in our body. Lipoproteins:Properties, functions and biochemical functions of CO 05. understand some of the types of steroid hormones. Biochemistry of peptide hormones. disease that might be treatable by Structure of DNA (Watson-Crick model) and RNA, Genetic Code, gene therapy Biological roles of DNA and RNA: Replication, Transcription and CO 06. understand how genetics may be used Translation, Introduction to Gene therapy. in the design of drugs. Biochemistry of disease: A diagnostic approach by blood/ urine CO 07. know various biochemical tests to analysis. determine glucose, lipids, creatinine and albumin in blood. Correlate Blood:Composition and functions of blood, blood coagulation. Blood laboratory test results with common collection and preservation of samples.Anaemia, Regulation, diseases or conditions estimation and interpretation of data for blood sugar, urea, creatinine, CO 08. know the pathophysiological bases of cholesterol and bilirubin. the most relevant and prevalent Urine: Collection and preservation of samples. Formation of diseases in our population; the main urine.Composition and estimation of constituents of normal and biological properties that are altered pathological urine. in these diseases and are examined in Hands On Practical a clinical biochemistry laboratory; Identification and estimation of the following: 1. Carbohydrates – qualitative andquantitative. 2. Lipids –qualitative. 3. Determination of the iodine number ofoil. 4. Determination of the saponification number ofoil. 5. Determination of cholesterol using Liebermann- Burchardreaction. 6. Proteins –qualitative. 7. Isolation ofprotein. 8. Determination of protein by the Biuretreaction. 9. Determination of nucleicacids
Core Content of CU Syllabus Course Outcome Courses
Semester 4 The students will have a preliminary idea CCH08 Nitrogen compounds about Amines: Aliphatic & Aromatic:preparation, separation (Hinsberg‟s method) and identification of primary, secondary and CO 01. The structural differences of Amines: tertiary amines; reaction (with mechanism): Eschweiler–Clarke Aliphatic & Aromatic, Preparation, methylation,diazo coupling reaction, formation and reactions of Separation and Basicity of aliphatic phenylenediamines, diazomethane and diazoacetic ester. and aromatic amines, Identification Nitro compounds (aliphatic and aromatic): preparation and of primary, secondary and tertiary reaction (with mechanism): reduction under different conditions; Nef amines several reactions of amines carbonyl synthesis, Henry reaction and conjugate addition of with mechanism nitroalkane anion. CO 02. The preparation of Nitro compounds Alkylnitrile and isonitrile: preparation and reaction (with (aliphatic and aromatic), reduced mechanism): Thorpe nitrile condensation, von Richter reaction. products of nitro compounds on Diazonium salts and their related compounds: reactions (with acidic, neutral and alkaline condition mechanism) involving replacement of diazo group; reactions: CO 03. The various methods for preparing Gomberg, Meerwein, Japp-Klingermann. Alkylnitrile and isonitrile Rearrangements(1) CO 04. Preparation of aromatic Diazonium Mechanism with evidence and stereochemical features for the salts and their related compounds, to following: Rearrangement to electron-deficient carbon: Wagner- replace the N≡N group by different Meerwein rearrangement, pinacol rearrangement, dienone-phenol; groups, couplingproducts Wolff rearrangement in Arndt-Eistert synthesis, benzil- benzilicacid rearrangement, Demjanovrearrangement,Tiffeneau–Demjanov rearrangement The students will learn different types of Rearrangements(2) rearrangements including Mechanism with evidence and stereochemical features for the following: Rearrangement to electron-deficient oxygen: Baeyer- CO 05. Rearrangement to electron deficient Villiger oxidation, cumene hydroperoxide-phenol rearrangement and carbon, Dakin reaction. CO 06. Rearrangement to electron deficient Rearrangements(3) oxygen, Mechanism with evidence and stereochemical features for the CO 07. Rearrangement to electron deficient following: Aromatic Rearrangement to electron-deficient nitrogen: nitrogen rearrangements: Hofmann, Curtius, Lossen, Schmidt and Beckmann CO 08. Migrating the group from oxygen to Rearrangements(4) ring carbon Mechanism with evidence and stereochemical features for the CO 09. Migrating the group from nitrogen to following: rearrangements: Migration from oxygen to ring carbon: ring carbon Fries rearrangement and Claisen rearrangement Rearrangements(5) Mechanism with evidence and stereochemical features for the following: Migration from nitrogen to ring carbon: Hofmann-
Martius rearrangement, Sommelet Hauser rearrangement, Fischer- Hepp rearrangement, N-azo to C-azo rearrangement, Bamberger rearrangement, Orton rearrangement and benzidine rearrangement. The Logic of Organic Synthesis (1) Retrosynthetic analysis: Disconnections; synthons, donor and acceptor synthons; natural reactivity and umpolung; latent polarity in bifunctional compounds: illogical electrophiles and nucleophiles; synthetic equivalents; Students will have a clear idea about the functional group interconversion and addition (FGI and FGA) logic of organic synthesis by retrosynthetic The Logic of Organic Synthesis (2) Retrosynthetic analysis: approach after studying the following C-C disconnections and synthesis: one-group and two- group (1,2- to
1,5-dioxygenated compounds), reconnection (1,6-dicarbonyl); CO 10. Some Definitions related to retro protection- deprotection strategy (alcohol, amine, carbonyl, acid). synthesis Strategy of ring synthesis: Thermodynamic and kinetic factors; CO 11. How to do One-Group, Two-Group synthesis of large rings, application of high dilution technique. C-C disconnections and then Asymmetric synthesis: stereoselective and stereospecific synthesize, Concept of Reconnection reactions; diastereoselectivity and enantioselectivity (only and Protection-deprotection strategy definition); diastereoselectivity: addition of nucleophiles to C=O CO 12. Strategy of ring synthesis:Medium adjacent to a stereogenic centre: Felkin-Anh model. and large rings may be synthesized by high dilution principle. Organic Spectroscopy(1) CO 13. Asymmetric synthesis: Streoselective UV Spectroscopy Reactions, Stereospecific Reactions, : introduction; types of electronic transitions, end Diastereoselectivity, Enantiosectivity, absorption; transition dipole moment and CO 14. Diastereoselective synthesis may be allowed/forbidden transitions; chromophores and carried out by applying Cram‟s rule auxochromes; Bathochromic andHypsochromic shifts; using Felkin-Anh model for addition intensity of absorptions (Hyper-/Hypochromic effects); of nucleophiles to C=O adjacent to a
application of Woodward‟s Rules for calculation of λmax stereogeniccentre. for the following systems: conjugated diene, α,β- unsaturated aldehydes and ketones(alicyclic, homoannular and heteroannular); extended conjugated systems (dienes,
aldehydes and ketones); relative positions of λmax considering conjugative effect, steric effect, solvent effect, The student will have a clear concept of effect of pH; effective chromophore concentration: keto- CO 15. Emission Spectroscopy enol systems; benzenoid transitions. CO 16. Absorption Spectroscopy. Organic Spectroscopy(2) CO 17. It is again divided into the following IR Spectroscopy introduction; modes of molecular heads vibrations(fundamental and non- fundamental);IR active CO 18. UV Spectroscopy : molecules; application of Hooke‟s law, force constant; CO 19. IR Spectroscopy fingerprint region and its significance; effect of deuteration; NMR Spectroscopy overtone bands; vibrational coupling in IR; characteristic and CO 20.
diagnostic stretching frequencies of C-H, N-H, O-H, C-O, C- N, C-X, C=C (including skeletal vibrations of aromatic compounds), C=O, C=N, N=O, C≡C, C≡N;
characteristic/diagnostic bending vibrations are included; factors affecting stretching frequencies: effect of conjugation, electronic effects, mass effect, bond multiplicity, ring-size, solvent effect, H-bonding on IR absorptions; application in functional group analysis. Organic Spectroscopy(3) NMR Spectroscopy introduction;nuclear spin; NMR active molecules;basic principles of Proton Magnetic Resonance; choice of solvent and internal standard; equivalent and non- equivalent protons; chemical shift and factors influencing it; ring current effect;significance of the terms: up-/downfield, shielded and deshielded protons; spin coupling and coupling constant (1st order spectra); relative intensities of first-order multiplets: Pascal‟s triangle; chemical and magnetic equivalence in NMR ; anisotropic effects in alkene, alkyne, aldehydes and aromatics; NMR peak area, integration; relative peak positions with coupling patterns of common organic compounds (both aliphatic and benzenoid-aromatic); rapid proton exchange; interpretation of NMR spectra of simple compounds. Students will know about the Organic Spectroscopy(4) Applications of IR, UV and NMR spectroscopy for identification of CO 21. The basic fundamental knowledge simple organic molecules which are acquired in the previous Experiment: Qualitative Analysis of Single Solid Organic modules (MXIII, MXIV and MXV) for identification of simple organic Compounds molecules 1. Detection of special elements (N, S, Cl, Br) by Lassaigne‟s After completing this module students will test be able to analyse the given single solid 2. Solubility and classification (solvents: H2O, 5% HCl, 5% organic compound by NaOH and 5% NaHCO3) CO 22. Detection of special element by 3. Detection of the following functional groups by Lassaigne‟s test systematic chemical tests: aromatic amino (-NH2), CO 23. Solubility and classification aromatic nitro (-NO2), amido (-CONH2, including imide), Identification of nitrogeneous and phenolic –OH, carboxylic acid (-COOH), carbonyl CO 24. non-nitrogeneous functional groups. (distinguish between -CHO and >C=O); only one test for The structure of the given compound each functional group is to be reported. CO 25. may be achieved by corresponding 4. Melting point of the given compound suitable derivative preparation and 5. Preparation, purification and melting point CO 26. Melting point determination of both determination of a crystalline derivative of the given the given sample and the derivative compound. prepared. 6. Identification of the compound through literature survey.
Each student, during laboratory session, is required to carry out qualitative chemical tests for all the special elements and the functional groups with relevant derivatisation in known and unknown (at least six) organic compounds.
CCH09 Application of Thermodynamics–II Students will be able CO 01. To understand Raoult‟s law Colligative properties: Vapour pressure of solution; Ideal CO 02. To compare Henry‟s law and solutions, ideally diluted solutions and colligative properties; Raoult‟s law to explain ideal Raoult's law; Thermodynamic derivation using chemical potential solutions to derive relations between the four colligative properties [(i) CO 03. To describe ideal liquid mixtures. relative lowering of vapour pressure, (ii) elevation of boiling point, CO 04. To discuss P-C and T-C diagrams and (iii) Depression of freezing point, (iv) Osmotic pressure] and the usefulness amount of solute. Applications in calculating molar masses of CO 05. To explain non-ideal liquid-vapour normal, dissociated and associated solutes in solution; Abnormal systems. colligative properties. CO 06. To state and explain azeotropic Phase Equilibrium: Definitions of phase, component and degrees mixtures. of freedom; Phase rule and its derivations; Definition of phase CO 07. To explain partially miscible and diagram; Phase diagram for water, CO2, Sulphur. immiscible liquid systems by taking First order phase transition and Clapeyron equation; Clausius- appropriate examples. Clapeyron equation - derivation and use; Ehrenfest Classification of CO 08. To describe how a solute distribute phase transition. itself in two immiscible liquids, Binary solutions: Liquid vapour equilibrium for two component CO 09. To state and explain Nernst‟s systems Ideal solution at fixed temperature and pressure; Principle distribution law, of fractional distillation; Duhem-Margules equation; Henry's law; CO 10. To apply and derive an expression for Konowaloff's rule; Positive and negative deviations from ideal modified Nernst distribution law for a behaviour; Azeotropic solution; Liquid-liquid phase diagram using special case in which solute associate phenol- water system; Solid-liquid phase diagram; Eutectic mixture or dissociate in one of the solvent , Three component systems, water-chloroform-acetic acid system, CO 11. To classify systems as heterogeneous triangular plots and homogeneous systems CO 12. To define equilibrium and metastable Foundation of QuantumMechanics equilibrium Beginning of Quantum Mechanics: Black body radiation (Concept CO 13. To appreciate the importance of only) Wave-particle duality, light as particles: photoelectric and phase rule equation in dealing with Compton effects; electrons as waves and the de Broglie hypothesis; heterogeneous equilibrium of Uncertainty relations (without proof) different types. Wave function: Postulates of Quantum Mechanics, Schrodinger CO 14. To define Phase rule and understand time-independent equation; nature of the equation, acceptability the concepts number of components, conditions for the wave functions and probability interpretations of degrees of freedom wave function Vector representation of wave function. CO 15. To know conditions of equilibrium Orthonormality of wave function. between two and three phases Concept of Operators: Elementary concepts of operators, CO 16. To explain the changes expected in eigenfunctions and eigenvalues; Linear operators; Commutation of the system if we vary temperature or operators, commutator and uncertainty relation; Expectation value; pressure keeping the other variable Properties of Hermitian operator; Complete set of constant Eigenfunctions.Expansion of Eigenfunctions. CO 17. To understand why normal boiling Particle in a box: Setting up of Schrodinger equation for one- point and of water normal melting dimensional box and its solution; Comparison with free particle point of ice are 100°C and 0°C eigenfunctions and eigenvalues. Properties of PB wave functions respectively (normalisation, orthogonality, probability distribution); Expectation To get an idea how to use the phase 2 2 CO 18. values of x, x , px and px and their significance in relation to the diagram in developing practical uncertainty principle; Extension of the problem to two and three applications dimensions and the concept of degenerate energy levels. CO 19. To understand Clausius-Clapeyron
CO 20. Crystal Structure
Bravais Lattice and Laws of Crystallography: Types of solid, Bragg‟s law of diffraction; Laws of crystallography (Haϋy‟s law and Steno‟s law); Permissible symmetry axes in crystals; Lattice, space lattice, unit cell, crystal planes, Bravais lattice. Packing of uniform hard sphere, close packed arrangements (fcc and hcp);
Tetrahedral and octahedral voids. Void space in p-type, F-type and I-type cubic systems Crystal planes: Distance between consecutive planes [cubic, tetragonal and orthorhombic lattices]; Indexing of planes, Miller indices; calculation of d ; Relation between molar mass and unit hkl cell dimension for cubic system; Bragg‟s law (derivation).Determination of crystal structure: Powder method; Structure of NaCl and KCl crystals. equation and its applications Specific heat of solid: Coefficient of thermal expansion, thermal CO 21. To understand and explain miscibility compressibility of solids; Dulong –Petit‟s law; Perfect Crystal in the solid-state model, Einstein‟s theory – derivation from partition function, CO 22. To gain an understanding of the 3 limitations; Debye‟s T law – analysis at the two extremes limitations of classical mechanics at molecular length scales the Practical: differences between classical and Experiment 1: Kinetic study of inversion of cane sugar quantum mechanics the connection of using a Polarimeter ( PreferablyDigital) quantum mechanical operators to Experiment 2: Study of Phase diagram of Phenol-Water system. observables Experiment 3: Determination of partition coefficient for the CO 23. To see how operator algebra can be distribution of I2 between water and CCl4 used to solve simple eigenvalue Experiment 4: Determination of pH of unknown solution (buffer), problems by colour matching method CO 24. To understand the concepts of Experiment 5: pH-metric titration of acid (mono- and di-basic) probabilities, amplitudes, averages, against strong base expectation values, and observables Experiment 6 : pH-metric titration of a tribasic acid against strong CO 25. To get an overview about the base. structure and properties of solid crystals CO 26. To know the characterisation of crystals using X-Ray diffraction CO 27. To get hands-on experience of phase diagram, partition coefficient, buffer, pH etc CCH10 Coordination Chemistry-II VB description and its limitations. Elementary Crystal Field Theory: Students will be able to splitting of dn configurations in octahedral, square planar and CO 01. Explain the basics of Crystal field tetrahedral fields, crystal field stabilization energy (CFSE) in weak theory in the light of modern and strong fields; pairing energy. Spectrochemicalseries.Jahn- Teller chemistry. distortion.Octahedral site stabilization energy (OSSE).Metal-ligand CO 02. Perceive and narrate the nature of bonding (MO concept, elementary idea), sigma- and pi-bonding in different types of bonding in various octahedral complexes (qualitative pictorial approach) and their inorganic complexes effects on the oxidation states of transitional metals (examples). CO 03. Interpret and discuss magnetic Magnetism and Colour: Orbital and spin magnetic properties and colour of different moments,spinonlymomentsofdnionsandtheircorrelationwitheffective complexes in the light of magnetic electromagnetochemistry moments, including orbital contribution; quenching of magnetic CO 04. Perceive and narrate implications of moment: super exchange and antiferromagnetic interactions Orgel diagram in understanding the (elementary idea with examples only); d-d transitions; L-S coupling; behavior of transition metal qualitative Orgel diagrams for 3d1 to 3d9 ions. Racah parameter. complexes. Selection rules for electronic spectral transitions; spectrochemical CO 05. Explain the properties, electronic series of ligands; charge transfer spectra (elementary idea). configurations and different oxidation Chemistry of d- and f- block elements states of d and f block elements. Transition Elements: CO 06. Compare electronic configuration, General comparison of 3d, 4d and 5d elements in term of electronic different oxidation states , spectral configuration, oxidation states, redox properties, coordination and magnetic properties of different chemistry. Actinoids and Lanthanoids Lanthanoids and Actinoids: CO 07. Prepare different inorganic General Comparison on Electronic configuration, oxidation states, complexes under laboratory colour, spectral and magnetic properties; lanthanide contraction, conditions separation of lanthanides (ion-exchange method only). CO 08. Use spectrophotometer for studying Reaction Kinetics and Mechanism inorganic complexations and Introduction to inorganic reaction mechanisms. Substitution reactions associated. parameters in square planar complexes, Trans- effect and its application in complex synthesis, 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. Practical: Inorganic preparations
[Cu(CH3CN)4]PF6/ClO4
Cisand trans K[Cr(C2O4)2(H2O)2] Potassiumdiaquadioxalatochromate(III) Tetraamminecarbonatocobalt (III)ion Potassiumtris(oxalato)ferrate(III) Tris-(ethylenediamine) nickel(II)chloride.
[Mn(acac)3] and Fe(acac)3] (acac=acetylacetonate) Instrumental Techniques • Measurement of 10Dq by spectrophotometricmethod.
• Determination ofλmax of [Mn(acac)3] and
[Fe(acac)3]complexes.
SEC B PHARMACEUTICALS CHEMISTRY The students will develop knowledge about Drugs & Pharmaceuticals CO 01. Drug designing Drug discovery, design and development; Basic Retrosynthetic CO 02. The synthesis of several drugs e.g., approach. Synthesis of the representative drugs of the following Analgesics Agents, Antipyretic classes: analgesics agents, antipyretic agents, anti- inflammatory Agents, Anti-inflammatory Agents, agents (Aspirin, paracetamol, lbuprofen); antibiotics Antibiotics Agents, Antifungal (Chloramphenicol); antibacterial and antifungal agents Agents, Antiviral Agents, and HIV- (Sulphonamides; Sulphanethoxazol, Sulphacetamide, Trimethoprim); AIDS related drugs by adopting the antiviral agents (Acyclovir), Central Nervous System agents general established method. (Phenobarbital, Diazepam),Cardiovascular (Glyceryltrinitrate), CO 03. Aerobic and anaerobic fermentation antilaprosy (Dapsone), HIV-AIDS related drugs (AZT-Zidovudine). CO 04. Production of (i) Ethyl alcohol and Fermentation citric acid, (ii) Antibiotics; Penicillin, Aerobic and anaerobic fermentation. Production of (i) Ethyl alcohol Cephalosporin, Chloromycetin and and citric acid, (ii) Antibiotics; Penicillin, Cephalosporin, Streptomycin, (iii) Lysine, Glutamic Chloromycetin and Streptomycin, (iii) Lysine, Glutamic acid, acid, Vitamin B2, Vitamin B12 and Vitamin B2, Vitamin B12 and Vitamin C. Vitamin C. Hands On Practical The students will develop hands on 1. Preparation of Aspirin and itsanalysis. experience of 2. Preparation of magnesium bisilicate(Antacid). CO 05. Preparation of Aspirin and its analysis. CO 06. Preparation of magnesium bisilicate (Antacid).
Core Content of CU Syllabus Course Outcome Courses
Semester 5
CCH11 Quantum Chemistry II Students will learn Simple Harmonic Oscillator: Setting up of One dimensional CO 01. To use high-level mathematics as a Schrödinger equation and discussion of solution and wave tool to understand atomic and 2 functions. Classical turning points, Expectation values of x, x , px molecular structure and properties 2 and px . CO 02. To understand what is meant by the Angular momentum: Commutation rules, quantization of square of total angular momentum and z-component; Rigid rotator model orbital concept of rotation of diatomic molecule; Schrödinger equation, CO 03. To understand the role of rotational transformation to spherical polar coordinates; Separation of and spin angular momenta in variables. Spherical harmonics; Discussion of solution chemistry Hydrogen atom and hydrogen-like ions: Setting up of CO 04. To Be able to use approximate Schrödinger equation in spherical polar coordinates, Separation of methods in solving molecular variables, Solution of angular Part (φ part only), quantization of problems energy (only final energy expression); Real wave functions. CO 05. To master molecular orbital theory Average and most probable distances of electron from nucleus; in diatomic and polyatomic Setting up of Schrödinger equation for many-electron atoms (He, molecules Li)Need for approximation methods. Statement of variation CO 06. To understand the connection theorem and application to simple systems(particle-in- a-box, between common approximation harmonic oscillator, hydrogen atom). methods and standard chemical LCAO :Born-Oppenheimer approximation. Covalent bonding, frameworks (Born-Oppenheimer valence bond and molecular orbital approaches, LCAO-MO approximation, molecular orbitals, + treatment of H2 ; Bonding and antibonding orbitals; Qualitative for example) extension to H2; Comparison of LCAO-MO and VB treatments of CO 07. To understand the relationship H2 and their limitations.( only wavefunctions, detailed solutionnot between microscopic properties of required) and their limitations. molecules with macroscopic Statistical Thermodynamics thermodynamic observables Configuration:Macrostates, microstates and configuration; CO 08. To understand the statistical calculation with harmonic oscillator; variation of W with E; thermodynamics and various equilibrium configuration partition functions. Boltzmann distribution: Thermodynamic probability, entropy and CO 09. To understand the different aspects probability, Boltzmann distribution formula (with derivation); of statistical thermodynamics and Applications to barometric distribution; Partition function, concept its applications. of ensemble - canonical ensemble and grand canonical ensembles Partition function: molecular partition function and thermodynamic properties, 3rd law: Absolute entropy, Plank‟s law, Calculation of entropy, Nernst heat theorem Adiabatic demagnetization: Approach to zero Kelvin, adiabatic cooling, demagnetization, adiabatic demagnetization – involvedcurves Numerical Analysis Roots of Equation: Numerical methods for finding the roots of CO 10. To solve algebraic or transcendental equations: Quadratic Formula, Iterative Methods (e.g., Newton equations using appropriate Raphson Method). numerical methods Least-Squares Fitting.NumericalDifferentiation.Numerical CO 11. To approximate a function using an Integration( Trapezoidal and Simpson'sRule) appropriate numerical method CO 12. To solve a linear system of Practical: equations using an appropriate Computer programs(Using FORTRAN or C or C ++) based on numerical method numerical methods : CO 13. To prove results for numerical root Programming 1: Roots of equations: (e.g. volume of van der finding methods Waals gas and comparison with ideal gas, pH of a weakacid) CO 14. To calculate a definite integral Programming 2: Numerical differentiation (e.g., change in using an appropriate numerical pressure for small change in volume of a van der Waals gas, method Potentiometrictitrations) CO 15. To code numerical methods in Programming 3: Numerical integration (e.g. entropy/ enthalpy Fortran change from heat capacity data), probability distributions (gas kinetic theory) and mean values
CCH12 Carbocyles and Heterocycles The students will learn about the Polynuclear hydrocarbonsand their derivatives:synthetic methods CO 01. Chemistry of Polynuclear include Haworth, Bardhan-Sengupta, Bogert-Cook and other useful hydrocarbons, Their Types, syntheses (with mechanistic details);fixation of double bonds and Structures and several synthetic Fries rule;reactions (with mechanism) of naphthalene, methods for naphthalene, anthraceneand phenanthrene and their derivatives. anthracene and phenanthrene Heterocyclic compounds:Biological importance of heterocycles CO 02. Reactions with mechanism referred in the syllabus; 5- and 6-membered rings with one ofnaphthalene, anthracene and heteroatom; reactivity, orientation and important reactions (with phenanthrene e.g., sulphonation and mechanism) of furan, pyrrole,thiophene and pyridine; synthesis bromination with mechanism (including retrosynthetic approach and mechanistic details): Students will learn pyrrole: Knorr synthesis, Paal-Knorr synthesis, Hantzsch; furan: CO 03. Types, Structures, Reactivity, Paal-Knorr synthesis, Feist-Benary synthesis and its variation; Orientation and General properties thiophenes: Paal-Knorr synthesis, Hinsberg synthesis; pyridine: of Heterocyclic compounds Hantzsch synthesis;benzo-fused 5-and 6-membered rings with one CO 04. Important synthesis and reactions of heteroatom: reactivity, orientation and important reactions (with furan, pyrrole, Pyridine, indole, mechanistic details) of indole, quinoline and isoquinoline; synthesis quinolinendisoquinolinee.g (including retrosynthetic approachand mechanistic details): indole: nitration, Diels alder reaction, Fischer,quinoline: Skraup, isoquinoline: Bischler- Napieralski polymerisation synthesis. Students will learn about the Cyclic Stereochemistry CO 05. Cyclic Stereochemistry: Baeyer Alicyclic compounds:concept of I-strain (Baeyer‟s strain theory); strain theory, Brief idea about conformational analysis: cyclohexane, mono and disubstituted Conformation, Conformational cyclohexane; symmetry properties and optical activity; analysis of mono and di-substituted topomerisation; ring size and ease of cyclisation; conformation & cyclohexane, Optical activity, reactivity in cyclohexane system: consideration of steric and Nucleophilic substitution (SN1, stereoelectronic requirements; elimination (E2, E1), nucleophilic SN2, NGP) in cyclohexane system substitution (SN1, SN2, SNi, NGP), merged substitution-elimination; etc rearrangements; oxidation of cyclohexanol, esterification, CO 06. FMO approach involving 4π- and saponification, lactonisation, epoxidation, pyrolytic syn elimination 6π-electrons reactions in thermal and fragmentation reactions. and photochemical condition Pericyclic reactions CO 07. FMO approach involving Mechanism, stereochemistry, regioselectivity in case of Electrocyclic cycloreversion reactions of 4π- and reactions 6π-electrons in thermal and Mechanism, stereochemistry, regioselectivity in case of photochemicalcondition Cycloaddition reactions CO 08. Diels-Alder reaction Mechanism, stereochemistry, regioselectivity in case of Sigmatropic CO 09. Photochemical [2+2] cycloadditions reactions CO 10. Sigmatropic shifts and their order; Carbohydrates [1,3],[1,5], [3,3] shifts with Monosaccharides: Aldoses up to 6 carbons; structure of D-glucose & reference to Claisen and cope D-fructose (configuration & conformation); ring structure of rearrangements. monosaccharides (furanose and pyranose forms): Haworth The students will develop a concept of representations and non-planar conformations; anomeric effect CO 11. Types of Carbohydrates (including stereoelectronic explanation); mutarotation; epimerization; CO 12. Differences between Sugar and reactions (mechanisms in relevant cases): Fischer glycosidation, polysaccharides with Examples
osazone formation, bromine- water oxidation, HNO3 oxidation, CO 13. Classifications &Physical and
selective oxidation of terminal –CH2OH of aldoses, reduction to Chemical features of Sugars- alditols, Lobry de Bruyn-van Ekenstein rearrangement; stepping–up Monosaccharides and (Kiliani-Fischer method) and stepping–down (Ruff‟s &Wohl‟s Oligosaccharides with Examples methods) of aldoses; end-group-interchange of aldoses; acetonide CO 14. Ring structure of monosaccharides (isopropylidene and benzylidene protections; ring size determination; (furanose&pyranose forms) Fischer‟s proof of configuration of (+)-glucose. CO 15. Structure of D-glucose and D- Disaccharides: Glycosidic linkages, concept of glycosidic bond fructose (configuration & formation by glycosyl donor-acceptor, structure of sucrose, inversion conformation) of cane sugar. CO 16. Definition of anomeric effect, Biomolecules Aminoacids mutarotation, with explanation synthesis with mechanistic details: Strecker, Gabriel; acetamido CO 17. Reactions:of aldoses including malonic ester, azlactone, Bücherer hydantoin synthesis, synthesis osazone formation, oxidation, involving diketopiperizine, isoelectric point, zwitterions; reduction, Stepping–up and electrophoresis, reaction (with mechanism): ninhydrin reaction, Stepping–down of aldoses, Dakin-West reaction; resolution of racemic amino acids. Epimerisation BiomoleculesPeptides:peptide linkage and its geometry; syntheses CO 18. Ring size determination of (+)- (with mechanistic details) of peptides using N-protection & C- glucose by HIO4 protection, solid-phase (Merrifield) synthesis; peptide sequence: C- CO 19. Structure of Disaccharides terminal and N-terminal unit determination (Edman, Sanger and &Glycosidic linkages, Concept of „dansyl‟methods); partial hydrolysis; specific cleavage of peptides; glycosidic bond use of CNBr. CO 20. Structure of sucrose & Inversion of Biomolecules cane sugar. Nucleic acids:pyrimidine and purine bases (only structure & CO 21. Biomolecules: Synthesis and nomenclature); nucleosides and nucleotides corresponding to DNA reactions of Aminoacids, isoelctric and RNA;mechanism for acid catalysed hydrolysis of nucleosides point of several different amino (both pyrimidine and purine types); comparison of alkaline acid,electrophoresis hydrolysis of DNA and RNA; elementary idea of double helical CO 22. Ninhydrin reaction of amino acids structure of DNA (Watson-Crick model); complimentary base– with mechanism, Ninhydrin pairing in DNA. reaction of proline with mechanism CO 23. Definition of Peptides, Peptide Practical: linkage formation, Syntheses of A. Chromatographic Separations peptides using N-protection and 1. TLC separation of a mixture containing 2/3 amino acids using C-protection 2.TLC separation of a mixture of dyes (fluorescein and CO 24. Solid phase synthesis Merrifield methylene blue) resin 3.Column chromatographic separation of mixture of dyes CO 25. Peptide sequence: C–terminal and 4. Paper chromatographic separation of a mixture containing 2/3 N–terminal unit determination by amino acids various methods 5.Paper chromatographic separation of a mixture containing 2/3 CO 26. Nucleic acids : structures, sugars Structures of pyrimidine and purine B. Spectroscopic Analysis of Organic Compounds bases 1. Assignment of labelled peaks in the 1H NMR spectra of the known CO 27. Definition of nucleosides and organic nucleotides corresponding to DNA compounds explaining the relative δ-values and splitting pattern. and RNA with example 2. Assignment of labelled peaks in the IR spectrum of the same CO 28. The students will be skilled in compound explaining the relative frequencies of the absorptions (C- various chromatographic H, O-H, N-H, C-O, C-N, C-X, C=C, C=O, N=O, C≡C, C≡N separatation technique stretching frequencies; characteristic bending vibrations are CO 29. TLC separation of a mixture included). containing 2/3 amino acids e.g.,L- 3. The students must record full spectral analysis of at least 15 lysine, L-leucine,D/L- alanine and a (fifteen) compounds from the following list: mixture of dyes (fluorescein and -Bromoacetanilide (ii) 2-Bromo-4'-methylacetophenone (iii) methylene blue) - Methoxyacetophenone (v) 4-Aminobenzoic acid CO 30. Column chromatographic separation (vi) Salicylamide (vii) 2- Hydroxyacetophenone (viii) 1,3- of mixture of dyes e.g.,leaf Dinitrobenzene (ix) trans-Cinnamic acid (x) Diethyl fumarate (xi) 4- pigments from Spinach Leaves Nitrobenzaldehyde (xii) 4-Methylacetanilide (xiii) Mesityl oxide CO 31. Paper chromatographic separation (xiv) 2-Hydroxybenzaldehyde (xv) 4-Nitroaniline (xvi) 2,3- of a mixture containing 2/3 amino Dimethylbenzonitrile (xvii) Pent-1-yn-3-ol (xviii) 3- acids acidse.g.,L- lysine, L- Nitrobenzaldehyde (xix) 3-Aminobenzoic acid (xx) Ethyl 3- leucine,D/L- alanine and a mixture aminobenzoate (xxi) Ethyl 4-aminobenzoate (xxii) 3-nitroanisole. containing 2/3 sugars e.g., D-(-) Fructose, D-(+) Fructose, Sucrose CO 32. Assignment of labelled peaks in the 1H NMR spectra of the known organic compounds explaining the relative δ-values and splitting pattern. CO 33. Assignment of labelled peaks in the IR spectrum of the same compound explaining the relative frequencies of the absorptions (C-H, O-H, N-H, C-O, C-N, C-X, C=C, C=O, N=O, C≡C, C≡N stretching frequencies; characteristic bending vibrations are included). CO 34. The students must record full spectral analysis of compounds from th list given in the syllabus
Students will be able DSEA APPLICATIONS OF COMPUTERS IN CHEMISTRY CO 01. To get an exposure to the emerging world of computational chemistry Computer Programming Basics (FORTRAN): CO 02. To have a basic idea about computational chemistry Elements of FORTRAN Language. FORTRAN Keywords and calculations commands, Logical and Relational Operators, iteration, Array CO 03. To learn computer based variables, Matrix addition and multiplication.Function and presentation and statistical analysis Subroutine. of data using spreadsheet software Introduction to Spread sheet Software(MSExcel): applied in the computer labs to Creating a Spreadsheet, entering and formatting information, basic solve typical chemical problems, functions and formulae, creating charts, tables and graphs. which are taken from the actual Incorporating tables and graphs into word processing documents, research in the theoretical chemistry simple calculations. group. Solution of simultaneous equations (for eg: in chemical Equilibrium CO 04. To use computational tools in problems) using Excel SOLVER Functions. Use of Excel Goal his/her studies or later career in Seek function. academia or private industry. Numerical Modelling: Simulation of pH metric titration curves, CO 05. To perform an error analysis for a Excel functions LINEST and Least Squares. Numerical Curve given numerical method and their Fitting, Regression, Numerical Differentiation and Integration minimization during analysis Statistical Analysis: CO 06. To explain Accuracy and precision Gaussian Distribution and Errors in Measurement and their effect and their use in practical data or on data sets. Descriptive Statistics using Excel, Statistical results analysis and errors Significance Testing, the T test and the F test. CO 07. To learn to carry out some simple Practicals computational chemistry calculations APPLICATIONS OF COMPUTERS IN CHEMISTRY ( At least 10 experiments are to be performed.) 1. Plotting of Graphs using a spreadsheet. ( Planck's Distribution Law, Maxwell Boltzmann Distribution Curves as a function of temperature and molecularweight) 2. Determination of vapour pressure from Van der Waals Equation of State. 3. Determination of rate constant from Concentration-time data using LINEST function. 4. Determination of Molar Extinction Coefficient from Absorbent's data using LINEST function. 5. Determination of concentration simultaneously using Excel SOLVER Function.(For eg: Determination of [OH-], [Mg2+] and [H3O+] from Ksp and Kw data of Mg(OH)2.) 6. Simultaneous Solution of Chemical Equilibrium Problems to determine the equilibrium compositions from the Equilibrium Constant data at a given Pressure and Temperature. 7. Determination of Molar Enthalpy of Vaporization using Linear and Non Linear Least squares fit. 8. Calculation and Plotting of a Precipitation Titration Curve with MS Excel. 9. Acid-Base Titration Curve using Excel Goal Seek Function. 10. Plotting of First and Second Derivative Curve for pH metric and Potentiometric titrations 11. Use of spreadsheet to solve the 1D Schrodinger Equation(Numerov Method). 12. Michaelis-Menten Kinetics for Enzyme Catalysis using Linear and Non - Linear Regression
DSEB INORGANIC MATERIALS OF INDUSTRIALIMPORTANCE Students will be able to Silicate Industries: CO 01. Examine methodically the physico - Glass: Glassy state and its properties, classification (silicate and chemical properties of different non-silicate glasses).Manufacture and processing of glass. industrial raw materials and asses Composition and properties of the following types of glasses: Soda their suitability in the lime glass, lead glass, armoured glass, safety glass, borosilicate manufacturing processes , keeping glass, fluorosilicate, coloured glass, photosensitive glass. in mind the fields of application of Ceramics: Important clays and feldspar, ceramic, their types and those products and byproducts like manufacture. Hightechnology ceramics and their applications, glasses, ceramics, cements. superconducting and semiconducting oxides, fullerenes carbon CO 02. Examine methodically the physico nanotubes and carbon fibre. chemical properties and Cements: Classification of cement, ingredients and their role, manufacturing processes for Manufacture of cement and the setting process, quick setting different chemicals used as cements. fertilizers to find out their suitability Fertilizers: for use in the production of different Different types of fertilizers. Manufacture of the following agricultural produce. fertilizers: Urea, ammonium nitrate, calcium ammonium nitrate, CO 03. Suggest appropriate methods of use ammonium phosphates; polyphosphate, superphosphate, compound of different types of surface coating and mixed fertilizers, potassium chloride, potassium sulphate. materials from the angle of their Surface Coatings: varied physico -chemical properties Objectives of coatings surfaces, preliminary treatment of surface, vis a vis areas of application in the classification of surface coatings.Paints and pigments-formulation, domestic and industrial fields. composition and related properties. Oil paint, Vehicle, modified CO 04. Classify different types of batteries oils, Pigments, toners and lakes pigments, Fillers, Thinners, used in industries according to their Enamels, emulsifying agents. Special paints (Heat retardant, Fire components, functions, applications retardant, Eco-friendly paint, Plastic paint), Dyes, Wax polishing, and suitability. Water and Oil paints, additives, Metallic coatings (electrolytic and CO 05. Classify different types of alloys on electroless), metal spraying and anodizing. the basis of their compositions, Batteries: properties and scope of use. Narrate Primary and secondary batteries, battery components and their role, the methodology for manufacture of Characteristics of Battery.Working of following batteries: Pb acid, different types of steels in the Li-Battery, Solid state electrolyte battery.Fuel cells, Solar cell and industry. polymer cell. CO 06. Classify different types of catalysts Alloys: on the basis of their physico- Classification of alloys, ferrous and non-ferrous alloys, Specific chemical properties. Discuss properties of elements in alloys. Manufacture of Steel (removal of industrial use of catalyst like silicon decarbonization, demanganization, desulphurization zeolite. dephosphorisation) and surface treatment (Arand heat treatment, CO 07. Discuss the chemistry of some nitriding, carburizing). Composition and properties of different selected items of explosives and the types of steels. reasons behind such property of the Catalysis: chemicals. General principles and properties of catalysts, homogenous CO 08. Analyze systematically the catalysis (catalytic steps and examples) and heterogenous catalysis components present in selected (catalytic steps and examples) and their industrial applications, chemical compounds and estimate Deactivation or regeneration of catalysts. their relative proportions. Phase transfer catalysts, application of zeolites as catalysts. CO 09. Undertake preparation of pigment in Chemical explosives: the laboratory. Origin of explosive properties in organic compounds, preparation and explosive properties of lead azide, PETN, cyclonite (RDX).Introduction to rocket propellants. PRACTICALS 1. Determination of free acidity in ammonium sulphatefertilizer. 2. Estimation of Calcium in Calcium ammonium nitratefertilizer. 3. Estimation of phosphoric acid in superphosphatefertilizer. 4. Electroless metallic coatings on ceramic and plasticmaterial. 5. Determination of composition of dolomite (by complexometric titration). 6. Analysis of (Cu, Ni); (Cu, Zn ) in alloy or syntheticsamples. 7. Analysis ofCement. 8. Preparation of pigment (zincoxide).
Core Content of CU Syllabus Course Outcome Courses
Semester 6
CCH13 Theoretical Principles in Qualitative Analysis Students will be able to Basic principles involved in analysis of cations and anions and solubility products, commonion effect. Principles involved in CO 01. Explain the basic principle of separation of cations into groups and choice of group reagents. identification of cations and anions Interfering anions (fluoride, borate, oxalate and phosphate) and in the mixtures and also the theory need to remove them after GroupII. involved in the the separation of BioinorganicChemistry cations with the removal of Elements of life: essential and beneficial elements, major, trace and interfering anions. ultratrace elements. Basic chemical reactions in the biological CO 02. Narrate the basic biochemical systems and the role of metal ions (specially Na+, K+, Mg2+, Ca2+, reactions in the biological system Fe3+/2+, Cu2+/+, and Zn2+). Metal ion transport across biological of some selected metal ions. membrane Na+/ K+-ion pump. Dioxygen molecule in life. Dioxygen CO 03. Discuss the chemistry of different management proteins: Haemoglobin, Myoglobin, Hemocyanine and dioxygen management protein Hemerythrin. Hydrolytic enzymes: carbonate bicarbonate buffering CO 04. Narrate the toxic effects of some system and carbonic anhydrase and carboxyanhydrase A. Toxic metal ions. Cite examples of metal ions and their effects, chelation therapy (examples only), Pt chelation therapy, use of Au and Pt and Au complexes as drugs (examples only), metal dependent complexes in drug. diseases (examples only) CO 05. Discuss various organometallic Organometallic Chemistry compounds with particular Definition and classification of organometallic compounds on the reference to their electron basis of bond type. Concept of hapticity of organic ligands.18- arrangements and preparation electron and 16-electron rules (pictorial MO approach).Applications method and reactions of some of 18-electron rule to metal carbonyls, nitrosyls, cyanides. General important organometallic methods of preparation of mono and binuclear carbonyls of 3d compounds. series. Structures of mononuclear and binuclear carbonyls.pi- CO 06. Discuss some important reactions acceptor behaviour of CO, synergic effect and use of IR data to which arecatalysed by some explain extent of back bonding. Zeise‟s salt: Preparation, structure, organometallic compounds and evidences of synergic effect. Ferrocene: Preparation and reactions their industrial applications. . (acetylation, alkylation, metallation, Mannich Condensation). CO 07. Explain the concept of semimicro Reactions of organometallic complexes: substitution, oxidative analysis of different cations and addition, reductive elimination and insertionreactions. anions and undertake laboratory Catalysis by Organometallic Compounds analysis of mixtures containing Study of the following industrial processes various ions 1. Alkene hydrogenation (Wilkinson‟sCatalyst) 2. Hydroformylation 3. WackerProcess 4. Synthetic gasoline (Fischer Tropschreaction)
5. Ziegler-Natta catalysis for olefinpolymerization. Practical : Qualitative semimicro analysis of mixtures containing not more than three radicals. Emphasis should be given to the understanding of the chemistry of different reactions. + + 2+ 2+ 2+ 3+ 3+ 2+ 4+ Cation Radicals: Na ,K , Ca , Sr , Ba , Al , Cr , Mn /Mn , Fe3+, Co2+/Co3+, Ni2+, Cu2+, Zn2+, Pb2+, Cd2+ (Demo), Bi3+ (Demo), 2+ 4+ 3+ 5+ 3+/5+ + 2+ Sn /Sn , As /As , Sb (Demo), NH4 , Mg (Demo). ------2- 2- - Anion Radicals: F , Cl , Br , BrO3 , I , IO3 , SCN , S , SO4 , NO3 , - 3- NO2 ,PO4 , 3-- 3- 2- 2- 4- 3- AsO4 , BO3 , CrO4 / Cr2O7 , Fe(CN)6 , Fe(CN)6 .
Insoluble Materials: Al2O3(ig), Fe2O3(ig), Cr2O3(ig), SnO2, SrSO4,
BaSO4, CaF2, PbSO4.
CCH14 Molecular Spectroscopy Students will be able Interaction of electromagnetic radiation with molecules and various CO 01. To develop an elementary idea of types of spectra; Rotation spectroscopy: Selection rules, intensities spectroscopy and photochemistry of spectral lines, determination of bond lengths of diatomic and CO 02. To have a thorough knowledge of linear triatomic molecules, isotopic substitution Vibrational the fundamentals of microwave, spectroscopy: Classical equation of vibration, computation of force infra red, Raman and electronic constant, amplitude of diatomic molecular vibrations, CO 03. To discuss the principle and anharmonicity, Morse potential, dissociation energies, fundamental working of spectrophotometer. frequencies, overtones, hot bands, degrees of freedom for CO 04. To understand the laws of polyatomic molecules, modes of vibration, Diatomic vibrating photochemistry rotator, P, Q, Rbranches CO 05. To study the chemistry of surfaces Electronic Spectroscopy: Potential energy curves (diatomic and different types of surface molecules), Frank-Condon principle and vibrational structure of phenomena electronic spectra; Frank Condon factor. Bond dissociation and CO 06. To get an idea about the various principle of determination of dissociation energy (ground state); techniques employed for the Decay of excited states by radiative and non-radiative paths; Pre- characterisation of surfaces dissociation; Fluorescence and phosphorescence, Jablonskii CO 07. To have a clear concept of the diagram; theories of chemical kinetics Raman spectroscopy: Classical Treatment. Rotational Raman CO 08. To know the general properties of effect; Vibrational Raman spectra, Stokes and anti-Stokes lines; colloids and macromolecules their intensity difference, rule of mutual exclusion CO 09. To gave hands on experience of Photochemistry and Theory ofreactionrate: surface properties, and Lambert-Beer‟s law: Characteristics of electromagnetic radiation, spectrophotometry Lambert-Beer‟s law and its limitations, physical significance of absorption coefficients; Laws of photochemistry, Stark-Einstein law of photochemical equivalence quantum yield, actinometry, examples of low and high quantum yields Rate of Photochemical processes: Photochemical equilibrium and the differential rate of photochemical reactions, Photostationary
state; HI decomposition, H2-Br2reaction, dimerisation of anthracene; photosensitised reactions, quenching; Role of photochemical reactions in biochemical processes,chemiluminescence Collision theory of reaction rate ( detailed treatment). Lindemann theory of unimolecular reaction; Outline of Transition State theory (classical treatment) Primary Kinetic Salt Effect. Surface phenomenon Surface tension and energy: Surface tension, surface energy, excess pressure, capillary rise and surface tension; Work of cohesion and adhesion, spreading of liquid over other surface; Vapour pressure over curved surface; Temperature dependence of surface tension Adsorption: Physical and chemical adsorption; Freundlich and Langmuir adsorption isotherms; multilayer adsorption and BET isotherm (no derivation required); Gibbs adsorption isotherm and surface excess; Heterogenous catalysis (single reactant); Colloids: Lyophobic and lyophilic sols, Origin of charge and stability of lyophobic colloids, Coagulation and Schultz-Hardy rule, Zeta potential and Stern double layer (qualitative idea), Tyndall effect; Electrokinetic phenomena (qualitative idea only); Stability of colloids and zeta potential; Micelle formation Dipole momentandpolarizability: Polarizability of atoms and molecules, dielectric constant and polarisation, molar polarisation for polar and non-polar molecules; Clausius-Mosotti equation and Debye equation (both without derivation) and their application; Determination of dipole moments Practical: Experiment 1: Determination of surface tension of a liquid using Stalagmometer Experiment 2: Determination of the indicator constant of an acid base indicator spectrophotometrically
Experiment 3: Verification of Beer and Lambert‟s Law for KMnO4
and K2Cr2O7 solution
Experiment 4: Study of kinetics of K2S2O8+KI reaction spectrophotometrically Experiment 5: Determination of pH of unknown buffer spectrophotometrically Experiment 6: Determination of CMC of a micelle from Surface Tension Measurement.
DSEA Analytical Methods In Chemistry Analytical Methods In Chemistry Optical methods of analysis: The students will be develop a clear Origin of spectra, interaction of radiation with matter, fundamental concept of laws of spectroscopy and selection rules, validity of Beer- CO 01. Optical methods of analysis: Lambert‟slaw. CO 02. UV-Visible Spectrometry UV-Visible Spectrometry: Basic principles of instrumentation CO 03. Basic principles of quantitative (choice of source,monochromator and detector) for single and analysis double beam instrument; CO 04. Infrared Spectrometry Basic principles of quantitative analysis: estimation of metal ions CO 05. Flame Atomic Absorption and from aqueous solution,geometrical isomers, keto-enoltautomers. Emission Spectrometry Determination of composition of metal complexes using Job‟s CO 06. Thermal methods of analysis method of continuous variation and mole ratio method. CO 07. Electroanalytical methods Infrared Spectrometry: Basic principles of instrumentation (choice CO 08. Separation techniques: of source, monochromator& detector) for single and double beam CO 09. Solvent extraction: Classification, instrument; sampling techniques. principle and efficiency of the Structural illustration through interpretation of data, Effect and technique. importance of isotope substitution. CO 10. Mechanism of extraction: extraction Flame Atomic Absorption and Emission Spectrometry: Basic by solvation and chelation principles of instrumentation(choice of source, monochromator, CO 11. . Technique of extraction: batch, detector, choice of flame and Burner designs. Techniques of continuous and counter current atomization and sample introduction; Method of background extractions. correction, sources of chemical interferences and their method of CO 12. Qualitative aspects of solvent removal. Techniques for the quantitative estimation of trace level of extraction: extraction of metal ions metal ions from water samples. from aqueous solution, extraction of Thermal methodsofanalysis organic species from the aqueous Theory of thermogravimetry (TG), basic principle of and nonaqueous media. instrumentation. Techniques for quantitative estimation of Ca and CO 13. Quantitative aspects of solvent Mg from their mixture. extraction: extraction of metal ions Electroanalyticalmethods: from aqueous solution, extraction of Classification of electroanalytical methods, basic principle of pH organic species from the aqueous metric, potentiometric and conductometric titrations. Techniques and nonaqueous media used for the determination of equivalence points. Techniques used CO 14. Chromatography: Classification, for the determination of pKa values. principle and efficiency of the Separation techniques: technique. Solvent extraction: Classification, principle and efficiency of the CO 15. Mechanism of separation: technique. Mechanism of extraction: extraction by solvation and adsorption, partition & ion chelation. exchange. Technique of extraction: batch, continuous and counter current CO 16. Development of chromatograms: extractions. frontal, elution and displacement Qualitative and quantitative aspects of solvent extraction: extraction methods. of metal ions from aqueous solution, extraction of organic species CO 17. Qualitative and quantitative aspects from the aqueous and nonaqueous media. of chromatographic methods of Chromatography: Classification, principle and efficiency of the analysis: IC, GLC, GPC, TLC and technique. Mechanism of separation: adsorption, partition & ion HPLC. exchange. CO 18. Stereoisomeric separation and Development of chromatograms: frontal, elution and displacement analysis: Measurement of optical methods. rotation, calculation of Qualitative and quantitative aspects of chromatographic methods of Enantiomeric excess (ee)/ analysis: IC, GLC, GPC, TLC and HPLC. diastereomeric excess (de) ratios Stereoisomeric separation and analysis: Measurement of optical and determination of enantiomeric rotation, calculation of Enantiomeric excess (ee)/ diastereomeric composition using NMR, Chiral excess (de) ratios and determination of enantiomeric composition solvents and chiral shift reagents. using NMR, Chiral solvents and chiral shift reagents. Chiral Chiral chromatographic techniques chromatographic techniques using chiral columns (GC and HPLC). using chiral columns (GC and Role of computers in instrumental methods of analysis. HPLC). PRACTICALS CO 19. Role of computers in instrumental Separation Techniques by: methods of analysis. Chromatography: CO 20. The students will be technically (a) Separation and identification of the monosaccharides guided by the following ways present in the given mixture (glucose & fructose) by paper CO 21. Separation Techniques by
chromatography. Reporting the Rfvalues. Chromatography (b) Separate a mixture of Sudan yellow and Sudan Red by CO 22. Separation and identification of the TLC technique and identify them on the basis of their monosaccharides present in the Rfvalues. given mixture (glucose & fructose) (c) Chromatographic separation of the active ingredients of by paper chromatography. plants, flowers and juices by TLC Reporting the Rf values. Solvent Extractions: CO 23. Separate a mixture of Sudan yellow To separate a mixture of Ni2+& Fe2+ by complexation with and Sudan Red by TLC technique DMG and extracting the Ni2+-DMG complex in chloroform, and identify them on the basis of and determine its concentration by spectrophotometry. their Rf values. I. Analysis of soil: CO 24. Chromatographic separation of the (i) Determination of pH ofsoil. active ingredients of plants, flowers (ii) Estimation of calcium, magnesium,phosphate and juices by TLC CO 25. Separation Techniques by Solvent II. Ionexchange: Extractions Determination of exchange capacity of cation exchange resins CO 26. To separate a mixture of Ni2+& and anion exchange resins. Fe2+ by complexation with DMG III. Spectrophotometry and extracting the Ni2+-DMG 1. Determination of pKa values of indicator using complex in chloroform, and spectrophotometry. determine its concentration by 2. Determination of chemical oxygen demand (COD). spectrophotometry. 3. Determination of Biological oxygen demand (BOD). CO 27. Analysis of soil and determination of pH Estimation of calcium, magnesium, phosphate CO 28. Ion exchange: CO 29. Determination of exchange capacity of cation exchange resins and anion exchange resins. CO 30. Spectrophotometry CO 31. Determination of pKa values of indicator using spectrophotometry. CO 32. Determination of COD and BOD DSEB DSE B-4 : DISSERTATION CO 01. To know the role of research as In a total of 105 lecture hours, a student has to carry out means to more effective decision – research /review on a topic as assigned by the respective making college. A project report and digital presentation will be CO 02. To familiarize the student with the required for the assessment of the student at the end of the fundamental concepts and various semester. techniques of research that can be used in Chemistry CO 03. To assist students to develop an understanding of the research process and to conduct research leading to successful completion of their dissertation CO 04. To assist student to prepare and present their work.