GALGOTIAS COLLEGE OF ENGINEERING AND TECHNOLOGY Knowledge Park-II, Greater Noida, U.P. CHEMISTRY KAS- 102/202 STUDY MATERIAL Session: 2019-2020 Course Coordinator: Dr. Monika Malik Subject Teachers Dr. Smriti Dwivedi Dr. Bipin Kumar Srivastava Dr. Ansar Anjum Dr. Mohd. Kashif Dr. Savita Verma Dr. Anuradha Saha Syllabus: Chemistry (KAS-102/202) Syllabus (as prescribed by affiliating university, i.e. AKTU) KAS-102/202 : Chemistry (L T P 3 1 3) Module-1 (8) Atomic And Molecular Structure Molecular orbital’s of diatomic molecules. Band theory of solids. Liquid crystals and its applications. Point defects in solids. Structure and applications of Graphite and Fullerenes. Concepts of nano-materials and its applications. Module- 2 (8) Spectroscopic Techniques And Applications Elementary ideas and simple applications of Rotational, Vibrational, Ultraviolet & Visible, and Raman spectroscopy. Module- 3 (8) Electrochemistry Nernst Equation and application, relation of EMF with thermodynamic functions (∆H, ∆F and ∆S). Lead storage battery. Corrosion causes, effects and its prevention. Phase rule and its application to water system. Module-4 (8) Water Analysis Hardness of water, Techniques of water softening (Lime- soda , Zeolite, Ion exchange resin and Reverse osmosis method). Fuels Classification of fuels, Analysis of Coal, Determination of Calorific values (bomb calorimeter & Dulong’s method), Module- 5 (8) Polymers Basic concepts of polymer – blends and composites, Conducting and biodegradable polymers, Preparations and applications of some industrially important polymers (Buna-S, Buna-N, Neoprene, Nylon 6, Nylon 6, 6, and Terylene). General methods of synthesis of organometallic compound (Grignard Reagent) and their applications. Syllabus: Chemistry (KAS-102/202) Syllabus as per CO KAS-102/202 : Chemistry (L T P 3 1 3) CO-1: On completion of this course student will be able to apply fundamental concepts of chemistry in different fields of Engineering. Module-1 (11) Atomic And Molecular Structure Molecular orbital’s of diatomic molecules. Band theory of solids. Liquid crystals and its applications. Point defects in solids. Structure and applications of Graphite and Fullerenes. Concepts of nano-materials and its applications. CO-2: On completion of this course student will be able to identify compounds using different spectroscopic techniques. Module- 2 (10) Spectroscopic Techniques And Applications Elementary ideas and simple applications of Rotational, Vibrational, Ultraviolet & Visible, and Raman spectroscopy. CO-3: On completion of this course student will be able to understand the basic principles of electrochemistry for different engineering applications. Module- 3 (10) Electrochemistry Nernst Equation and application, relation of EMF with thermodynamic functions (∆H, ∆F and ∆S). Lead storage battery. Corrosion causes, effects and its prevention. Phase rule and its application to water system. CO-4 : On completion of this course student will be able to illustrate different types of impurities in water and its softening techniques. Module-4 (16) Water Analysis Hardness of water, Techniques of water softening (Lime- soda , Zeolite, Ion exchange resin and Reverse osmosis method). Fuels Classification of fuels, Analysis of Coal, Determination of Calorific values (bomb calorimeter & Dulong’s method), CO-5: On completion of this course student will be able to recall the basic knowledge of polymerization & and applications Module- 5 (8) Polymers Basic concepts of polymer – blends and composites, Conducting and biodegradable polymers, Preparations and applications of some industrially important polymers (Buna-S, Buna-N, Neoprene, Nylon 6, Nylon 6, 6, and Terylene). General methods of synthesis of organometallic compound (Grignard Reagent) and their applications. Reference Books: 1. University Chemistry By B.H.Mahan 2. University Chemistry By C.N.R.Rao 3. Organic Chemistry By I.L. Finar 4. Physical Chemistry By S. Glasstone 5. Engineering Chemistry By S.S. Dara 6. Polymer Chemistry By Fre W. Billmeyer 7. Engineering Chemistry By Satya Prakash Galgotias College of Engineering and Technology Department of AS (Chemistry) Lecture Plan (Theory Subject) : B. Tech. –2019-20 Subject Name with Code: Chemistry KAS 102/202 Unit: 05 S. Lectur Modul CO Topics Remarks, No e No. eNo. if any . 1 1 1 1 Molecular orbital theory- Introduction 2 2 1 1 Application of Molecular orbital theory to Homodiatomic molecules 3 3 1 1 Application of Molecular orbital theory to Heterodiatomic molecules 4 4 1 1 Application of Molecular orbital theory to Heterodiatomic molecules 5 5 1 1 Band theory of solids 6 6 1 1 Point defects in solids 7 7 1 1 Liquid crystals- Introduction and classification 8 8 1 1 Applications of Liquid crystals 9 9 1 1 Structure and applications of Graphite and Fullerenes 10 10 1 1 Concepts of nano-materials 11 11 1 1 Applications of nano-materials 12 12 2 2 Elementary Idea of spectroscopy 13 13 2 2 UV Spectroscopy- THEORY 14 14 2 2 UV Spectroscopy- Application 15 15 2 2 IR Spectroscopy- Theory 16 16 2 2 IR Spectroscopy- Application 17 17 2 2 Raman Spectroscopy- Theory 18 18 2 2 Raman Spectroscopy- Applications 19 19 2 2 Rotational Spectroscopy- Theory 20 20 2 2 Rotational Spectroscopy- Applications 21 21 2 2 Numerical problems of spectroscopy 22 22 3 3 Basic concepts of electrochemistry- Nernst Equation 23 23 3 3 Applications of Nernst Equation 24 24 3 3 Relation of EMF with thermodynamic functions and Numerical 25 25 3 3 Lead storage battery S. Lectur Modul CO Topics Remarks, No e No. eNo. if any . 26 26 3 3 Corrosion; causes and types 27 27 3 3 Corrosion - theory 28 28 3 3 Corrosion; prevention 29 29 3 3 Phase Rule- Introduction and terminology 30 30 3 3 Application of phase rule to one component system (water system) 31 31 4 4 Hardness of water, Type and units of hardness and Numerical 32 32 4 4 Disadvantage of hard water- Boiler troubles 33 33 4 4 Techniques for water softening- Zeolite process 34 34 4 4 Techniques for water softening- Ion exchange process 35 35 4 4 Techniques for water softening- Lime-Soda process & types 36 36 4 4 Reactions and Calculation steps for numerical of Lime-Soda process 37 37 4 4 Numerical based on Lime-Soda process 38 38 4 4 Reverse osmosis 39 39 4 4 Fuels- Classification of fuels 40 40 4 4 Determination of calorific values by Bomb calorimeter 41 41 4 4 Numerical based on Determination of Calorific values 42 42 4 4 Analysis of Coal- proximate analysis 43 43 4 4 Analysis of Coal- Ultimate analysis 44 44 4 4 Analysis of Coal- Combustion 45 45 4 4 Numerical based on Combustion 46 46 4 4 Basic concepts of polymer 47 47 5 5 Polymer- blends 48 48 5 5 Polymer -composites 49 49 5 5 Preparations and applications of some industrially important polymers 50 50 5 5 Conducting polymers 51 51 5 5 Biodegradable polymers 52 52 5 5 General methods of synthesis of organometallic compound (Grignard Reagent) 53 53 5 5 Applications of organometallic compound 54 54 Revision 55 55 Revision UNIT I LECTURE - 1 Molecular Orbital Theory (MOT) Molecular orbital theory was given by Hund and Mulliken in 1932. The main ideas of this theory are: When two atomic orbitals combine or overlap, they lose their identity and form new orbitals. The new orbitals thus formed are called molecular orbitals. Molecular orbitals are the energy states of a molecule in which the electrons of the molecule are filled just as atomic orbitals are the energy states of an atom in which the electrons of the atom are filled. In terms of probability distribution, a molecular orbital gives the electron probability distribution around a group of nuclei just as an atomic orbital gives the electron probability distribution around the single nucleus. Only those atomic orbital can combine to form molecular orbital which have comparable energies and proper orientation. The number of molecular orbitals formed is equal to the number of combining atomic orbitals. When two atomic orbitals combine, they form two new orbitals called bonding molecular orbital and antibonding molecular orbital. The bonding molecular orbital has lower energy and hence greater stability than the corresponding antibonding molecular orbital. The bonding molecular orbitals are represented by σ, π etc, whereas the corresponding antibonding molecular orbitals are represented by σ* π* etc. (Figure 1) The shapes of the molecular orbitals formed depend upon the type of combining atomic orbitals. The filling of molecular orbitals in a molecule takes place in accordance with Aufbau principle, Pauli's exclusion principle and Hund's rule. Electrons are filled in the increasing energy of the MO which is in order Bond order ∞ Stability of molecule ∞ Dissociation energy ∞ (1/Bond Length). If all the electrons in a molecule are paired then the substance is a diamagnetic on the other hand if there are unpaired electrons in the molecule, then the substance is paramagnetic. More the number of unpaired electrons in the molecule greater are the paramagnetism of the substance. [1] Figure 1 [2] LECTURE- 2 Bond Order In molecular orbital theory, we calculate bond orders by assuming that two electrons in a bonding molecular orbital contribute one net bond and that two electrons in an antibonding molecular orbital cancel the effect of one bond. The stability of the molecule can be determined from the parameter called Bond Order. Bond order may be defined as half the difference between number of electrons in bonding molecular orbitals and number of electrons in antibonding molecular orbitals. N b – N a BO = 2 Molecular orbital diagrams of Homodiatomic molecules MO Diagrams for O2 and N2 as shown in Figure 2. MO diagrams – Contains same number of MOs as the number of atomic orbitals. The more electronegative element is kept on the right - lower in energy. Homoatomic means “of the same atom”—such a molecule contains only one kind of atom.