SOCIETY FOR CHEMICAL EDUCATION
Golden Jubilee of Chemistry Dept. 2005
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SOCIETY FOR CHEMICAL EDUCATION Golden Jubilee of Chemistry Dept. 2005
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CHEMICAL EDUCATION IN ASSAM Teaching of chemistry should be an integral organic part of schooling. To improve mankind’s quality in culture, science, and technology, especially the quality of life of teenagers who will soon be working, a basic knowledge of chemistry is absolutely necessary. In fact, even citizens, not only who aspire to continue study in higher education, should learn chemistry. To achieve this goal, the school periods in chemistry in a week should be increased. To make teaching of chemistry purposeful and worthy of learning the mindset of the teachers should be changed. Language and mathematics are also important in school curriculum. But chemistry is also important in life. Hence emphasis should be laid on teaching chemistry at schools. Content of the of courses should be such as to make the students aware about chemistry and hazards of chemical substances in their uses and disposals. Air, water and soil pollution, use of polymeric materials, harmful effects of fertilizers and pesticides for plants and animals should form the content of curriculum intelligible to all. Survival of the human race is dependent on understanding the implications of harmful effects of misuse of chemical products. While improving standards of living of people, more awareness should be generated in these areas through knowledge and basics of chemistry. Number of experiments in school chemistry should be enough to have impact on understanding of chemistry, its usefulness and harmful effects of chemical substances. For example sulphuric acid, H2S, mercury in thermometer and lead should not be allowed in chemical laboratories of educational institutions The teachers should find out alternatives for these chemicals or avoid experiments using them.. We are still using DDT in India, which is abandoned as a harmful chemical in the developed world a few decades back. To become aware of disposals of chemicals and other wastes of industries, there are lots of rules and regulations even in India. But our concern is not significant. We bother little about handling of chemicals even in research laboratories. All organic chemicals like chloroform, acetone, benzene are no longer permissible for use in laboratories without precautions. Who bothers about safety in the chemical laboratory here in India? Put some sand buckets and unusable fire extinguishers nearby to fulfill the measures of safety. In order to make the citizens aware in all aspects of chemistry as referred to above, common knowledge in chemistry including the organic compounds and substances derived from them for domestic uses should be included in the courses in the different stages of school education also. The students should do as many practical experiments as possible. Experiments can be designed using chemicals from nature. National Science Foundation, U.S.A. recently has emphasized learning chemistry including organic substances through active learning methods. In an editorial in Journal of Chemical Education it is stated: 'Teachers of chemistry have a greater role to play to make chemistry attractive to the learners. The teachers should make them better students not just in the classrooms but to make them chemists outside the class rooms.
CHEMISTRY AND MATERIALS To make the people aware of proper use of chemicals and materials for sustainable development in 21st century, the following areas need emphasis on class rooms and in general:
Chemical Education in Assam A.
Department of Chemistry, Gauhati University
Established in 1955 for education and research.
1.
Dr. B.S.Rao 1955-1960 11. Dr.Bhabesh Chandra Goswami 2005- Research areas where active research are
pursued- 1.
Organic synthesis Board of Secondary Education, Assam Chemistry in General Chemistry Course Up to class X Science is taught as general science comprising physics,chemistry,botany, zoology etc. But there is no syllabus on general science subject wise. Only curriculum outline is presented for teacher and pupil activity. This makes writing a text book difficult. So from the curriculum the chemistry portion is summarized to show the topics. Class IX: Matter and its composition: Elements, Gas laws, Avogadro's hypothesis, concept of gram mole. Standard temperature and pressure, chemical equation, Reversible chemical reactions, oxidation and reduction, Electrolysis and electro deposition. environmental pollution, energy and alternative sources. Chemistry and industry- Polymers-types of plymers, natural and synthetic thermo setting and thermoplastic polymers. ,Chemical Fertilizers, Portland cement, Paper-chemical pulp and fillers. Class X(Revised 2004) Chemical bonding, Molecules and compounds -models. Electrovalent and covalent bonds,Metals and non metals-sources of metals, different forms, characteristics of metals, Metallurgy, Zinc- Sodium, Gold, Copper and Mercury. Alloys and composition, Alloys of Fe, Cu and Al (iron, copper and aluminum). Carbon and its unique properties. Organic compounds- Hydrocarbons-alkanes,alkenes and alkynes. Industrial chemicals- Sodium hydroxide, Sodium carbonate, Sulphuric acid, liquid air , ammonia and bleaching powder. Balanced diet- deficiency diseases, protein energy malnutrition,Anaemia cause of rickets, beri beri, pellagra and scurvy. Over in take of food, obesity, Sodium balance, flurosis, hypervitaminosis. Food processing and technology-edible oils, soft drinks, , snacks, canned food. Food preservation- bactericidal and bacteriostatic, dehydration, sun drying and cooking. pasteurization and fermentation. Chemical preservation. Food adulteration and prevention. Testing of common adulterants. Fossil fuels and coal. Liquid fuels and natural gas. LPG and petrochemicals. Assam Higher Secondary Education Council Higher Secondary Chemistry Syllabus 2004 First year course Marks 100, Time 3 hours, one paper Unit no contents marks period Unit no.1- units and measurements 2 3 Unit 2 Structure of matter (I) 6 8 Unit 3 States of matter (I) 6 12 Unit 4 Chemical thermodynamics (I) 4 7 Unit 5 Chemical equilibrium 5 8 Unit 6 Properties of dilute solutions 6 11 Unit 7 Surface Chemistry 2 5 Unit 8 Oxidation and reduction 3 5 Unit 9 Electrochemistry (I) 4 5 Unit 10 Structure of Matter (II) 8 12 Unit 11 Periodic classification of elements 4 7 Unit 12 Chemical bonding (I) 4 4 Unit 13 Nuclear chemistry 4 6 Unit 14 Hydrogen and its compounds 4 6 Unit 15 Boron, carbon and silicon 4 6 Unit 16 Oxygen and sulphur 4 6 Unit 17 Nitrogen and phosphorus 5 8 Unit 18 Metals and metallurgy 12 12 Unit 19 Organic compounds 5 8 Unit 20 Purification of organic compounds 2 3 Unit 21 Hydrocarbons 6 8 Course Contents: Unit 1: Units and Measurements SI and non-SI units of pressure, volume, density, temperature and other physical quantities. Scientific notations, significant figures, accuracy and precision of measurements. Unit 2: Structure of matter (I) Molecules, atoms, isotopes, relative atomic masses. Mole concept, formula masses, chemical equation. Calculations based on stoichiometry using mole ratio method for mol-mol, mol-vol, and vol-vol data. Unit 3: States of matter (I) Brief introduction to three states of matter. Gaseous state: Boyles' law, Charles' law and Avogadro's law, Ideal gas equations, Mol. gas constant, Graham's law of diffusion, and Dalton's law of partial pressure. Derivation from Avogadro's law-(i) Molar volume of ideal gas at NTP is 22.4 dm3 , (ii) relative mol. mass of gas is twice its vapour (relative) density, (iii) atomicity of elementary gases. Kinetic theory of gases-postulates. Kinetic equation ( no derivation) . Deduction of Boyles', Charles' and Avogadro's, Graham's and Dalton's laws from kinetic equation. Simple calculations related to kinetic equation. Deviation from ideal behaviour of gases- Van der Wall's equation (no derivation). Unit 4: Chemical thermodynamics (I) Thermodynamic systems (open, closed and isolated), properties 9extensive and intensive) processes (isothermal, adiabatic, isobaric and isochoric), functions (state and path). First law of thermodynamics (statements only) - internal energy and enthalpy. Heat of reaction and its measurements. Hess's law, types of enthalpy changes. Bond enthalpy. Simple problems and calculations. Unit 5: Chemical equilibrium Reversible and irreversible reactions. Law of mass action, definition and characteristics of chemical equilibrium (dynamic nature). Equilibrium Constants Kp and Kc . Application of law of mass action to the following gaseous equilibrium: (1) H2 + I2=2HI, (2PCL5 =) PCl3 + Cl2, N2 +3H2 = 2NH3 . Le Chatelier and Brown principle. Factors affecting the state of equilibrium- (a) concentration, (b) temperature, (c) pressure. Physicochemical principles involved in the industrial processes- (i) synthesis of NH3 by Haber-Bosch process (ii) production of HNO3 by Oswald's process, (iii) production of H2 SO4 by contact process. Unit 6: Properties of dilute solutions Types of solutions, Different units for expressing concentrations- mol-3 normality, mass%, volume%, mass-volume%, mol fraction, parts per million (ppm) etc.Temperature dependence of solubility, and utility of solubility curves of solid in liquid. Colligative properties, definition of dilute solution, vapour pressure of solution and Raoult's law. Lowering of vapour pressure, elevation of boiling point and depression of freezing point, osmosis, osmotic pressure and laws of osmotic pressure. Abnormal values of Colligative properties, Van't Hoff factor. Ideal and non-ideal solutions. (for dilute solutions of non-volatile solutes). Simple problems and calculations. Unit 7: Surface chemistry Adsorption-physical and chemical adsorption- factors affecting adsorption. Ideas of particle size and ass coarse suspension, colloids and crystalloids, classification, preparation and properties (mechanical, optical and electrical) of sols. Emulsions and gels, aerosols (general ideas only). Unit 8: Oxidation and reduction Electronic concept of oxidation and reduction. Oxidising agents and reducing agents and their equivalents. Ion electron method of balancing red ox reactions. Unit 9: Electrochemistry (I) Electronic and electrolytic conductors, electrolytes and non-electrolytes. Arrhenius theory of electrolytic dissociation-strong and weak electrolytes. Electrolysis, application of electrolysis. Unit 10: Structure of matter (II) Brief description of construction of atom-electron, proton and neutron. Rutherford's nuclear atom model. Atomic number, mass number, isotopes, isobars and isotones. Bohr's theory of hydrogen atom (qualititative treatment only). Limitations of Bohr's theory. Wave particle duality of matter and radiation ( qualitative treatments of photoelectric effect, Plank's interpretation on black body radiation), de Broglie hypothesis, electron diffraction, uncertainty principle and concept of probability. Wave mechanical model of hydrogen atom-wave function, probability of electronic position, shapes of s and p orbital. Quantum designation of atomic orbital and electrons energy in terms of principal, angular momentum and magnetic quantum numbers. Concept of electron spin and spin quantum numbers. Pauli exclusion principle, general idea of screening (constant) of outer electrons by inner electrons in atom, Aufbau principle, Hund's rules and electronic configuration of atoms. Unit 11: Periodic classification of elements Modern periodic law. Long form of periodic table (I PAC classification). Types of elements (definition and examples of the following types s- and p- block elements and inner transitional (f-block) elements. Periodic properties-effective nuclear charge, atomic (covalent radii, ionization energy, electron affinity (affinity energy) and electro-negativity. Variations along periods 1 to 4 and within all groups. Unit 12: Chemical Bonding Electronic theory of valence -ionic, covalent and coordinate bond( LLewis electronic dot structure only to be discussed. Factors favouring formation of ionic bonds. Co-valence in ionic compounds. Unit 13: Nuclear Chemistry Natural radioactivity-(properties of α,β and γ rays, rate of decay and half life of radioactive substances. Nuclear reactions-fission and fusion, nuclear energy, artificial transmutation and artificial radioactivity, synthetic elements and extension of the periodic table. Uses of radio isotopes-radiation therapy and radio carbon dating. Simple numerical problems relating to radioactive decay. Unit 14: Hydrogen and its compounds Posdition of hydrogen in the periodic table. Isotopes of hydrogen. Ortho and para hydrogen. Manufacture of hydrogen from natural gas and by electrolysis of water. Hydrides-their classification and properties. Water: production and uses, H2O2: preparation, properties and uses. Unit 15: Boron, Carbon and Silicon Boron: Occurence and isolation, preparation, properties and uses of boric acid and borax. Carbon: Allotropic forms-graphite, fullerine and diamond, their general characteristics,, Inorganic compounds of carbon. Silicon: Occurence and isolation. Preparation, properties and uses of glass, coloured glass. Unit 16: Oxygen and sulphur Allotropes of oxygen.Ozone-preparation, properties and uses, Classification of oxides. Allotropes of sulphur. Survey of hydrides, oxides and oxyaxids of sulphur. Preparation, properties uses of H2S and SO2. Reaction of H2SO4 . Unit 17: Nitrogen and Phosphorus Nitrogen cycle in nature. Natural and artificial fixation of nitrogen. Survey of hydrides, oxides and oxyacids of nitrogen, properties and uses of nitric acid and ammonia. Allotropes of phosphorus.- occurence and isolation,Survey of hydrides, oxides and oxyaxids of phosphorus. Preparation, properties and uses of of P phosphorus. Preparation, properties and uses of P4O6 , P4H10 and H3PO4. Preparation and uses of nitrogenous fertilizers and phosphorus fertilizers. Unit 18: Metals and metallurgy Metals versus non-metals, activity series of metals, occurence of metals on earth. Minerals and ores. Different processes involved in metallurgy- ore dressing, ore concentration, calcination,/roasting of ores, smelting, reduction by carbon, self reduction, flectrolytic reduction, aluminothermic reduction. Amalgamation method and chemical method like cyanide extraction of metals. Purification of metals including zone refining. Extraction of sodium and zinc. Principles of manufacture and uses of sodium carbonate by Solvay's process and sodium hydroxide by Caster Kellner's process. Unit 19: Organic compounds Definition, scope and development of organic chemistry. Classification of organic compounds, homologous series and functional groups. Common names and systematic names of organic compounds. Systematic nomenclature of aliphatic, alucyclic and aromatic compounds. Systematic nam,es of aliphatic, alicyclic and aromatic names by IUPAC, priority order of functional groups for manufacture of polyfunctional organic componds. Unit 20: Purification of organic compounds Chromatography-paper,column and TLC , distillation methods-fractional and under reduced pressure, crystallisation and fractional crystallisation. Unit 21: Hydropcarbons Origin and composition of coal and petroleum. Aliphatic hydrocarbons from petroleum. Cracking and refining. Quality of gasoline-octane number, antioknock compounds and flash point, unleaded petrol. Natural gas and LPG as fuel.General methods of prparation and properties of alkenes and alkynes. Alicyclic and aromatic hydrocarbons, isolation from natural source and general properties. Problems relating to determination of molecular formula from percentage elemental composition. Practical syllabus for H.S.First year class 1. Identification of laboratory apparatus and accessories Period 2 Marks 2 At least 20 items should be shown to students, by their nams and ne chief use of each. ( In examination a student will be asked to write the names and use of four items.) 2. Preparation and studies of propertiesof gases Period 2 Marks2 H2, CO2, C2H2, NH3 etc ( only demonstration) 3. Separation of mixtures (one) Period 1 Marks 2 a) sand and ammonim chloride b) Iodine and ammonium chloride 4. Preparation of inorganic compounds (one) Period 2 Marks 2 a) CUSO4.5H2O from CUCO3 b) FeSO4.7H2O from Kipp's waste 5. Determination of m.p. of organic compounds (one) Period 2 Marks 4 Use capillary method in a paraffin oil bath, m.p. shoul be preferably below 1000C There will be no practical examination in first year class. These lab courses will be tagged with those prescribed for second yesr class and examination will be held at the end of second year class for 30 Higher Secondary Second Year Course Unit no. Title Marks Periods _______________________________________________________________________ Unit 1: States of Matter (II) 4 7 Unit 2: Chemical thermodynamics (II) 3 6 Unit 3: Chemical kinetics 4 8 Unit 4: Electrochemistry (II) 4 7 Unit 5: Acids and bases 4 8 Unit 6: Ionic equilibrium 6 10 Unit 7: Chemical bonding (II) 8 14 Unit 8: Group study, Hydrogen and noble gas 5 12 Unit 9: Metals and their compounds 6 10 Unit 10: Transition metals and coordination compounds 4 8 Unit 11: Structure and reactivity of organic compounds 5 14 Unit 12: Reactions of organic compounds 10 16 Unit 13: Biomolecules 2 4 Unit 14:Chemistry in the service of mankind 4 8 Distribution of course contents Unit 1: States of matter (II): Properties of liquids-elementary ideas about vapour pressure, surface tension and viscosity- temperature dependence of them. The solid state-classification of solids, closed packed structure of metals. Crystal lattice of ionic compounds, unit cells, octahedral and tetrahedral holes, hcp, fcc, bcc systems, crystal structures of ionic compounds- NaCl and C aF2 Unit 2: Chemical thermodynamics (II): Reversible, irreseversible and cyclic thermodynamic processes. Statement of second law of thermodynamics-concepts of entropy and free energy. Spontaneity of chemical reactions in terms of entropy and free energy changes. Relation between free energy change and equilibrium constant. Unit 3: Chemical kinetics: Elementary and complex reactions (definition and examples). Rate of chemical reactions, factors affecting reaction rates. Order and molecularity of reactions. Differential rate laws and rate constants. Differential and integral forms of first order rates. Arrhenius theory-activation energy, collision theory of reaction rates 9no derivation ) . Catalysis-type and criteria. Effects of radiation on reaction rates-photochemical reactions (examples only). Simple problems. Unit 4:Electrochemistry (II) Conductance of eletrolytes-specific a, molar and eqivalent.Principle of determination f conductance. Variation of conductance with concentration. Electrochemical cells (DAniel cell), electromotive force and electrode potential, Nerst equation. Electrochemical series of Oxidising and reducing agents. Conventional representation of cells and emf's. Gibb's free energy and cell potentials. Red ox titrations, red ox indicators. Simple problems and calculations. Unit 5:Acids and bases Bronsted- Lowry and Lewis (electronic theories of acids and bases. Acid base neutralization reactions in aqueous solution. Acidimetry and alkalimetry. Equivalents of acids and bases, strengths of acids and bases in solutions., standard acid and alkali solutions. Titrimetric analyses, use of base indicators. Calculations involving acid base titrations. Unit 6: Ionic equilibrium Dissociation of photonic acids and bases in water. Ostwald's dilution law, pH,pOH and pK values, pH scale. Buffer solutions, Henderson equation, mechanism of buffer action. Salt hydrolysis exemplified by NaOCOCH3' Na2CO3, NH4Cl and NH4OCOCH3. Solubility product, common ion effect, application of solubility product principle to inorganic analysis. Simple problems on ionic equilibrium. Unit 7: Chemical bonding (II) Valence bond theory of chemical bonding-postulates of VBT. Bond parameters such as bond energies, average bond energies, bond lengths and bond angles. Overlap of atomic orbital and chemical bond. s and p orbital. Valence cell electron repulsion theory ( up to six electron pairs on the central atom) of the molecular shapes. Polarity of covalent bonds, bond diple moments and molecular dipole moments, polar and non-polar molecules, hydrogen bond, resonance (O3,CO32_, SO42_, -COO-, C6H6). Elementary idea about molecular orbital theory,∂- and π- bonds and MO's. Formation of homonuclear diatomic molecule and their energy level diagrams for elements of 1st and 2nd period of the periodic table. Bond order and magnetic properties of these molecules from MOT. Free electron model of metallic bond. Unit 8: Group study-halogen and noble gases General studies of following groups of elements with reference to- (a) electronic configuration, (b) characteristic properties and (c) oxidation states of (i) alkali metals (ii) alkaline earth metals, (iii) boron family (iv) carbon family, (v) nitrogen family, (vi) oxygen family, (vii) halogen family and (viii) noble gases. Halogens-preparation of fluorine, general methods of preparation of other halogens. Preparation, properties and uses of HF and HCl. Noble gases: Isolation of He from natural gas. Isolation of other noble gases from air. Uses of noble gases. Preparation and properties of Xenon fluorides. Unit 9: Metals and their compounds Extraction process of Al,Cu,Ag and Fe (steel) Preparation and uses of alum, blue vitriol, Mohr's salt, plaster of Paris, Bleaching powder, Goober's salt. Chemistry of cement and photography. Corrosion and protection of metals. General ideas about alloys- composition and uses of important alloys of Cu, Zn, Al and Fe. Unit 10: Transitional metals and coordination compounds Electronic configuration, general characteristics, oxidation states of transition elements of the 1st transition series. Preparation, properties and uses of KMnO4 and K2S2O7. Coordination compounds: Werner's coordination theory. Types of leg ands, IUPAC nomenclature of coordination compounds, isomerism ( ionization and stereoisomerism) in 4 and 6 coordination compounds. Valence bond theory and coordination compounds-magnetic properties. Application of coordination compounds-analytical and therapeutic. Unit 11: Structure and reactivity of organic compound sp3, sp2 and sp hybridized carbon, orbital depiction-CH4,C2H6 , C2H4, C2H2. Acidity of acetylenes. Structure of benzene, stability of C6H6 on the basis of delocalization of π electrons, C-C and C-H bond energies in alkane, alkyne, alkynes and arene (benzene). Aromaticity and Huckel's rule. Isomerism in aliphatic, alicyclic and benzene derivatives-constitutional, functional, stereo and conformational isomerism. Chirality and optical activity, Newman projection formula, conformation of ethane and cyclohexane. Reactivity of organic compounds-inductive effect and its application to acidity of monocarboxylic acids and basicity of amines, mesomeric effect and stability of phenoxide ion, variable (electromeric). Types of organic reagents- electrophiles and nucleophiles. Oxidising and reducing agents ( some common examples). Reaction intermediates-carboctions, carbanions and free radicals, their structure and stability. Mechanism of electrophilic and free radical substitution reactions. Friedal Craft alkylation and nitration of benzene, alkaline hydrolysis of bromoethane and chlorination of methane), addition and elimination reactions. Reaction of cyclohexane and benzene, aromatization, conversion of aliphatic to aromatic hydrocarbons and vice versa. Unit 12: Reactions of the following classes of organic compounds (a) Reactions of halogen derivatives of hydrocarbons-alkyl and aryl halides. (b) Reactions of hydroxy compounds- classification of alcohols into10, 20 and 30 , mono and polyhydric alcohols. Reactions of mono and trihydric alcohols.Reactions of phenols. Tests to distinguish between phenol and alcohol. and among primary, secondary and tertiary alcohols. (c) Reactions of ethers including cyclic ethers. (d)Reactions of aldehydes and ketones. Tests to distinguish between aldehydes and ketones, between methyl ketone and other ketones and between aliphatic and aromatic aldehydes. ( also formaldehyde) (e) Reactions of monocarboxylic acids, acid chlorides, acid anhydrides and amides. Reactions of nitrites and nitro compounds. (f) Classification of amines. Reactions of amines. Tests to distinguish among primary, secondary and tertiary amines. Tests to distinguish aliphatic primary amine from aromatic primary amine. Interconversion of functional groups illustrated by one or two important general methods of preparation of each of the above classes of compounds. Synthetic applications of Grignard reagent. Interconversion of isomeric compounds. Determination of empirical/molecular formulae of organic compounds from percentage elemental compositions and identification of organic compounds through class reactions. Unit 13: Biomolecules Carbohydrates, lipids, amino acids and proteins-classification and functions. Enzymes-fermentation of starch. Nucleic acids biological functions of RNA and DNA. Hemoglobin and respiration, chlorophylls and photosynthesis. Vitamins and hormones-source, functions and deficiency disease. Chemistry in the service of mankind (a) Medicines: general idea, function and uses of medicinal compounds-antiseptic and analgesic, antipyretic, antimalarial;, anesthetic, antibiotic , disinfectant, tranquilizer, sulpha drugs. (b) Pesticides: definition, classification and application specificity of insecticides, fungicides etc. (c) Polymers: Natural and synthetic. Preparation and uses of nylon 66, backelite. Buna-s rubber, polythene and polyvinyl chlorode. Teflon and silicone polymers./ (d) Soaps and detergents: General ideas only. (e) Dyes. pigments and paints: General ideas only. (f) Food chemistry: General ideas, classification and examples of food additives, preservation and adulterations.
Three years degree course in Chemistry,2003-2004, Gauhati University The chemistry syllabi both at general and major levels are being revised and upgraded regularly by the department of chemistry, Gauhati University. The syllabi adopted in2003- 2004 is presented below_ B.Sc. (Part I, Part II, and Part III. The examination pattern is as follows- General Course Part I Examination Paper I General chemistry 100 marks Part II Examinations Paper II General chemistry 100 marks Paper III Practical 50 marks Paper IV Practical 50 marks Part III Examinations Paper V General chemistry 75 marks Paper VI Industrial, Environmental and Biological Chemistry 75 marks Paper VII Practical 50 marks Total 500 marks Syllabus for TDC General Course in Chemistry Part I Examination Paper I (General Chemistry) Total Marks 100 Group A Inorganic 35 marks Unit 1.1 Structure of matter 15 marks Quantization of energy (Planck energy), particle nature of photon (photoelectric effect, Compton effect). Calculations based on Bohr's theory, Energy levels of hydrogen atom, Atomic spectrum of hydrogen. Qualitative treatment of the following-Dual nature of matter (De Broglie equation). Heisenberg's uncertainty principle, electron in an atom (Schrödinger's wave equation) and the energy levels. Quantum numbers (n,m and l). Graphical representation of hydrogen atom orbital, the meaning of wave function, spin quantum number and meaning of electronic spin. Many electron atoms, electron repulsion. Pauli exclusion principle and Hund's rule. Energy levels of hydrogen like atoms, electronic configuration of atoms, effective nuclear charge of atoms. Aufbau principle. Unit 1.2: Covalent bonding 15 marks Covalent bond and properties of covalent compounds. The molecular orbital approach and energy level diagram of simple diatomic molecules( H2, B2, C2, N2, O2, CO and NO) The valence bond approach: Lewis electron pair bonds ( H2, HF, N2, CO, NO, NH3, H2O, H2O2), Hybridization ( in BeH2, C2H2, CH4, BF3, CO32-, PCL5, SF6 and benzene). Resonance ( in benzene,O3, CO32-, NO3- ). Resonance energy, Resonance versus delocalization. Polar molecules, the concept of eletronegativity ( Pauling and Miuliken scale). Bond moment and dipole moment (CO, NH3, NF3 ), Percentage ionic character of bonds ( in HF, HCl, HBr ). Principles and applications of Valence Shell Electron Repulsion (VESPER) theory, Examples ( BF3, CH4, NH3, H2O, PCl5, SF6, XeF4, IF7 ). Unit 1.3: Ionic bonding and Intermolecular forces Ion pairs and ionic bond, properties of ionic compounds, Lattice energy of ionic compounds ( example NaCl), Calculation of lattice energy and heats of formation of ionic compounds using Born Haber cycle, ionic radii and factors affecting radius of ions, radius ration and structure of ionic crystals. Covalency in ionic compounds, Fajan's rule, results of polarization on melting and boiling points. The hydrogen bond, structure of liquid and ice. Group B Organic Chemistry 35 marks Unit 1.4: Hydrocarbons I 20 marks a) Introduction to classification and nomenclature opf organic compounds on the basis of their functional groups. b) Alkanes: Preparation of alkanes ( Wurtz, Kolbe, Corey-House reactions) and their properties and reactions. Homolytic bond fission. Free radical generation and reactivity. Photochlorination of alkanes. c) Cycloalkanes: Preparation of cyclopropane, cyclobutane, cyclopentane, cyclohexane. Reactions of cyclopropane. Conformastions of cyclohexane, Disubstituted cyclohexane. Free rotation of ∂ bonds, rotamers of n-butane, their nomenclature and stability. d) Alkenes: Preparation of alkenes ( elimination of alkyl halides, alcohols,Wittig reaction, pyrolysis of esters). Reactions of alkenes. π d-diastereomerism, stability and Interconversion. Markownikov and Zaitzeff rules. Mechanism of electrophilic addition reactions. e) Alkynes and alkadienes: Preparation, properties and reactions of alkynes ( ethyne, propyne and butyne as examples) Addition of alkynes with polar reagents, ozonolysis, catalytic hydrogenation ( Lindlers catalyst). Preparation of 1,3-butadiene and isoprene, 1,2- and 1,4-addition of conjugated dienes. Unit 1.5: Hydrocarbons II 10 marks a) Reactive intermediates and stereo chemistry: Carbocations and carbanions- their shape, generation, stability and reactions. Stereochemistry: Basic concepts erythro and threo isomers, asymmetry, enatiomerism, diastereomerism, dissymmetry and meso structures. Chirality and prochirality. Racemisation, racemic mixtures, resolution of racemic mixtures. Nomenclature-R.S, asnd D,L notation. b) Alkyl halides and 1,2-dihalides: Preparation, properties and reactions of alkyl halides. Mechanism of SN! and SN2 reactions, E1 and E2 reactions. Effect of solvent, substrate and other factors in mechanism of SN1 and SN2 reactions. Substitution versus elimination. Conversion of alkyl halides to alcohols, ethers, amines, thioethers and thiols. Preparation and synthetic uses of Grignard reagens. Unit 1.6: Hydrocarbons III 5 marks a) Preparation and synthetic uses of diazomethane, ketene. b) Aromatic hydrocarbons: IUPAC nomenclature. Aromaticity. Preparation and reactions of benzene. Mechanism of electrophilic aromatic substitution. Activation, deactivation and directive influence of groups. Conversion of benzene to its derivatives and vice versa. Preparation and properties of naphthalene, anthracene. Group C Physical Chemistry 35 marks Unit 1.7: States of matter Postulates of kinetic theory of gases, derivatives of expression for pressure and temperature from from kinetic theory. Calculation of root mean square speed and average kinetic energy. Maxwell distribution molecular speeds ( derivation not required). Deviation from ideal behaviour, van der Wals' equation of state, calculation of critical constants from van der Wals' equation. Heat capacities of gases, degrees of freedom and the law of equipartition of energy ( derivation not required) Structure of liquids, kinetic and molecular model and properties of liquids. Definition and experimental measurement of vapour pressure ( dynamic method). Surface tension ( drop number method) and viscosity ( Ostwald method), variation of these properties with temperature. Crystal lattices, unit cell of seven crystal systemS , density of a cubic unit cell. The fcc, bcc and simple cubic systems. Closed packed structures. Imperfection of solids ( introduction to Schotsky and Frenkel defects). Unit 1.8: Chemical thermodynamics 10 marks Basic definitions and concepts. The zeroth law, nature of work and heat. The first law of thermodynamics-enthalpy and internal energy. Relation between Cp and Cv. Relation between P, V and T in adiabatic process. Thermochemistry: enthalpy of reaction, relation between H and U. Standard enthalpy changes. Hess's law and Kirchoff's law. Calculation of bond energy from thermo chemical data. The second law of thermodynamics. Carnot cycle. Entropy and spontaneity, calculation of entropy changes during vaporization and fusion, Troton's rule. Free energy, standard free enerfy and its significance, dependence of free energy on temperature and pressure. Free energy change and equilibrium constant. Thermdynamic criteria for chemical equilibrium. Unit 1.9: Phase rule 5 marks Definition of phase, component and degree of freedom. Phase rule. Phase diagram of water and sulphur systems. Ideal and non-ideal solutions. Principle of fractional distillation of liquid-liquid mixtures, Azotrope. PART II Examinations Paper II ( General chemistry) Marks 100 Group A: Inorganic Chemistry 35 marks Unit 2.1: Chemistry of non-transition elements I 15 marks Groupwise study of physical properties, chemical reactivity of elements and their important compounds- oxides and hydroxides, oxyacids, halides, hydrides. Groups (!, 15, 16, 17) Periodicity: General trends in size, ionization energy, electron affinity and electro negativity, first and second row anomalies., diagonal relationships, the use of orbital by third period elements, catenation and inert pair effect ( in Pb and Tl). Inorganic chains, rings and cages: Synthesis, structure and reactions of silicones, borazine and diborane. Unit 2.2: Chemistry of non-transition elements 5 marks Carbides and nitrides. Interhalogen compounds, polyhalides, pseudohalogens-synthesis and structure. Noble gas elements-sybthesis, structure and bonding. Unit 2.3: Transition elements 15 marks Comparative study of elements of first transition series with emphasis on electronic configuration, relative stability of oxidationnstates, ionization potentials,. red ox potentials, reactivity. Occurence, principles of extraction of Cr, Mn and Ni and their important compounds ( example KMnO4, K2Cr2O7). Werner theory, types of ligands, isomerism and IUPAC nomenclature of coordination compounds. Chelates eSSENTIAL AND TRACE ELEMENTS USEFUL TO LIFE AND AN INTRODUCTION TO THEIR BIOLOGICAL CYCLE. tOXICITY due to METALS AND NON-METALS. uSE OF METAL COMPOUNDS IN MEDICINE. Group B: Organic Chemistry 30 marks Unit 2.4: Aliphatic and aromatic hydroxy compounds and ethers 10 marks Classification of alcohols, 10, 20 and 30 alcohols and their distinguishing reactions. General methods of preparation, properties and general reactions of primary alcohols, glycols and glycerol. Basic concept of hydrogen bonding and their influence on properties of organic compounds. Williamson's ether synthesis and hydrolysis of ethers. Benzyl alcohol-preparation and reactions. Synthesis and reactions of phenols. Acidity of phenols and substituted phenols. Electrophilic aromatic substitution of phenols. Synthesis of bakelite. Unit 2.5: Aliphatic amine and aniline 5 marks 10, 20 and 30 amines. Basicity of amines. Preparation, properties and reactions of 10 amines. Basicity of amines and substituted aniline. Electrophilic aromatic substitution. Diazonium ions and their synthetic utility. Unit 2.6: Aliphatic and aromatic carbonyl compounds 5 marks General methods of preparation and reactions of carbonyl compounds ( formaldehyde, acetaldehyde, acetone and 2-butanone as examples.) Difference and reactivity of aldehydes and ketones. Polarization of carbonyl group. Nucleophilic addition of aldehydes and ketones. Mechanism with examples. Preparation and reactions of aniline. Electrophilic aromatic substitution. Diazonium ions and their synthetic utility. Unit 2.7: Aromatic and aliphatic carboxylic acids 5 marks Acidity of carboxylic acids, and substituted carboxylic acids. General methods of preparation, properties and reactions of aliphatic carboxylic acids( methanoic, ethanoic and propanoic acid as examples). Synthesis, properties and reactions of benzoic acid. Acidity of substituted benzoic acids. Conversion of carboxylic acids to their derivatives. Synthetic uses of ethylacetoacetate and diethyl malonate. Unit 2.8: Amino acids, carbohydrates, fats and oils 5 marks Elementary ideas of amino acids, essential amino acids, optical activity, D,L-nomenclature. Synthesis reactions of glycine. Simple methods of preparation of dipeptides. Monosaccharides: Open chain and ring chain structure of glucose and fructose. Concept of mutarotation, anomers, epimers. Reactions of glucose and fructose. Structure, physical properties and difference of fats, oils and soaps. Analysis of fats and oils. Group C: Physical Chemistry 35 marks Unit 2.9: Electrochemistry 15 marks Galvanic cells-description and working process. Standard electrode potentials and electromotive force (emf). The Nerst equation and calculation of cell potential. Concentration cells. Relation between cell emf and equilibrium constant. Standard and reference electrodes. Measurement of pH. Commercial applications of galvanic cell- dry cell, lead storage battery, fuel cells. Conductance of electrolytes- specific and molar conductance. Variation of molar conductivity with concentration. Kohlrausch's law of independent migration of ions. Transport number of ions and their determination. Unit 2.10: Chemical kinetics and surface chemistry 15 marks Reaction rates and rate laws. Order and molecularity of a reaction. Differential and integral rate equations of first and second order reactions. Experimental determination of reaction rates and order of reaction. Consecutive reactions. Chain reactions. Steady state approximations. Effect of temperature on reaction rate, Arrhenius equation. Collision theory of reaction rate (qualitative treatment only). Homogenous catalysis, acid base catalysis. Physisorption and chemisorption. Freuundlich and Langmuir adsorption isotherms. Their validity and significance. Heterogeneous catalysis-adsorption theory (qualitative treatment only). Colloids- Classification, preparation and purification, structure and stability. Surfactants-definition, micelle formation and critical micelle concentration. Unit 2.11 Ionic equilibrium 5 marks Dissociation equilibrium of weak electrolytes, Ostwald dilution law. Strengths of acids and bases. Solubility products and application in analytical chemistry. pH and pH scale. Handerson and Hasselbach equation and calculation of pK values. Buffer solutions and buffer action, uses of buffer solutions in chemistry and biology. Paper III ( Practical ); Time 5 hours Total marks 50 Unit 2.12 : Qualitative organic analysis 25 marks a) Detection of N,S and halogens in organic compounds b) Detection of functional groups ( one among the following ) -OH (alocoholic), -OH ( phenolic), -CHO, --COOH, -NO2, NH2, Hydroccarbon. ( Students will have to perform analysis of at least 5 liquid and/or solid organic compounds and record the results systematically in practical book). nit 2.13 : General experiments 10 marks a) Paper chromatographic separation of cations of group I b) Determination of solubility of a salt at a given temperature. ( In the examination, amny one of the above experiments will be allotted by lot.) Unit 2.14: Sessional examination 10 marks Marks to be awarded by holding an examination at the end of a session.) Unit 2.15 Viva voce 5 marks Paper IV ( Practical) Time 5 hours Total Marks 50 Unit 2.16: Qualitative inorganic analysis 15 marks Identification of not more than 3 radicals in a mixture of of the following: Cations: Hg2+, Pb2+. Cu2+, Bi2+, Cd2+, As3+, Sb3+, Sn2+, Sn4+, Fe2+/Fe3+, Cr3+, Al3+, Co2+, Ni2+, Mn2+, Zn2+, Ba2+, Ca2+< Sr2+, Mg2+ Anions: Cl-, Br-, NO3-, NO3-, S2-, F-, BO3-, , SO4-, F-, PO43-, AsO43- ( Presence of Na+, K+, NH4+ and CO32- radicals are to be neglected ) At least 4 salt mixtures have to be done by each student in practical class keeping records carefully. Distribution of marks: Result 5x3=15 marks ). Unit 2.17: Quantitative Inorganic analysis 10 marks Unit 2.18: Session examination 10 marks ( Marks to be awarded by holding an examination at the end of a session). Unit 2.19: Viva voce 5 marks Part III Examination Paper IV (General chemistry) Total marks 75 Unit 3.1 ; Chemistry of materials 15 marks Electrical properties of solids: Band theory ( From MO theory), conductors, insulators and semiconductors, intrinsic and extrinsic semiconductors ( examples from chemical compounds and explanation of electrical property from bonding theory). Superconductivity and examples of superconducting materials, Ferroelectric and Piezoelectric materials. Preparation of electronic grade pure silicon. Magnetic properties of solids: Ferro and antifero magnetism ( examples from chemical compounds). Application of clays, zeolites, ceramics, glass and liquid crystals. Unit 3.2: Principles of chemical analysis 15 marks Separation and identification of a mixture of cat ions and anions ( qualitative analysis). Application of solubility product and common ion effect in chemical analysis. Principle of estimation of metals quantitatively by complexometric method, Principle of acid base titration, Theory of indicators. Principle and application of solvent extraction. Basic principles of chromatography, nature of absorbent, solvent system, Rf values . Different types of chromatographic methods and their applications. Unit 3.3: Principles and application of spectroscopy I 15 marks The nature of electromagnetic radiation, the region of electromagnetic spectrum, the energy levels of hydrogen atom ( from Bohr' theory, the line spectrum of hydrogen. Electronic spectroscopy: The Beer-Lambert law, Molar absorption coefficient and absorbance, the selection rule for electronic transition, the influence of vibration on electronic spectra, re-emission of energy by excited molecules, ( fluorescence and phosphorescence). Structural elucidation by UV-Visible spectroscopy, Colour and electronic transitions, quantitative estimation by colorimetric method. Vibration spectroscopy: Introduction to vibration energy levels in diatomic molecules, Fundamental vibration modes of water molecule. Conditions of infrared and Raman activity in molecules, simple examples of structure elucidation by Infrared and Raman spectroscopy. Unit 3.4: Principle and application of spectroscopy II 10 marks Basic principles of mass spectroscopy. Applications of mass spectroscopy in structure elucidation of simple organic compounds. Basic principles Nuclear Magnetic Resonance ( NMR) spectroscopy,Represantation of NMR spectra. Approximate chemical shifts of simple organic molecules and functional groups. Unit 3.5: Nuclear chemistry 10 marks Nuclear charge, isotopes and isobars, nuclear composition, structure and properties ( size. mass, binding energy and shape), Artificial radioactivity, rates of radioactive decay, artificial radioactivity, nuclear fission and fusion, nuclear reactors. Applications of radioactivity, radio isotopes: Radio isotopes and their uses, radiocarbon dating, nuclear medicines. Environmental hazards due to nuclear radiation. Unit 3.6: Lanthanides and actinides 15 marks Chemistry of the lanthanide and actinide elements, electronic configuration, Oxidation states, properties, reactions and uses. Paper VI Industrial,environmental and biological chemistry Total marks 75 Unit 3.7: Industrial chemistry- inorganic 15 marks Water: modern methods of water treatment and purification. Fertilizers: Different types of N and P fertilizers, manufacture of ammonia, ammonium nitrate, urea, phosphates and superphosphates. Nitrogen fixation by plants. Glass: Various types of glass, composition and properties of glass, coloured glass, glazing, vitrification, glass ceramics. Cement: Various types of cement, their composition, manufacture, Portland cement. Paints: Constituents of different paints, role of binder and solvent. Lead and zinc containing paints, Paints of common use. Metals and alloys: General procedures of extraction of metals, manufacture, properties, composition and uses of important alloys. Manufacture of steel and stainless steel, Galvanization, rusting, corrosion. Unit 3.8: Industrial chemistry-organic 15 marks Polymers: Types of polymers and the polymerization. Manufacture, structure, properties and applications of a) Synthetic rubber ( including of cross linking and vulcanization). b) Synthetic fibers c) plastics d) foaming agents e) resins and f) silicones Coal: Fischer Trops process. Chemicals from coal. Petroleum: Manufacture and industrial reactions of ethane, propene, butadiene, acetylene and xylene. Synthesis of methanol from natural gas. Cracking of petroleum. Knocking and octane number. LPG and CNG, biodiene.Oils, fats and detergents: Catalytic hydrogenation of vegetable oil and fat for production of soap, synthesis of detergents. Principle of cleaning action. Enzymes in Industry: Production of alcohol by fermentation of starch and sugar ( reaction conditions, nature of polymers used, structural transformation during reaction), preparation and use of cellulose. Unit 3.9: Environmental chemistry: 15 marks Composition of the atmosphere, photochemical reactions in the atmosphere, vehicle exhausts in the atmosphere, vehicle exhausts and photochemical smog, acid rain, carbon monoxide and its effect,Suspended particles of matter-size and effect on health, Dual role of ozone in the atmosphere-topospheric ozone, ozone hole, Carbon dioxide and other gases responsible for global warming. Measurement to control air pollution. Quality of water for drinking and other purposes, permissible limits, Common water pollutants-organic and inorganic. Heavy metals and their toxic effects. Pollution of water through use of chemical fertilizers. Fluoride contamination and flurosis. Pollution due to mining. Measures taken to control water pollution. Unit 3.10: Biological chemistry 20 marks The cell and its components, the structure cell membrane, transport of ions and molecules across the membrane. Molecular structure and functions of amino acids, peptides, polypeptides, conformation of proteins, primary, secondary, tertiary and quarternary structures of proteins. Structure of purines and pyrimidines, the double helical structure of DNA, structure of RNA, Basic ideas of gene and heredity. Genetic code and genetic mutation. Biosynthesis of DNA (replication ), RNA (transcription) and protein (transmission). Enzymes and their role ( with a few examples), Catalysis by enzymes,Lock-key hypothesis. Specificity of enzyme reaction. Inhibition and denaturation. Vitamins and their importance. Coenzymes, examples of variousvitamins and coenzymes, basic idea of nutrition. Transformation of energy by cells. Elementary idea of chemical reactions involved in glycolysis and Kreb's cycle. Photosynthesis and respiration. Oxidative phosphorylation. 3.11: Natural products and medicines 10 marks Terpenes-classification, structures and isolation. Alkaloids: classification, structure and isolation. Physiological action of alkaloids. Steroids and hormones: elementary introduction, structure and functions of hormones, neurotransmitters. Medicines: Structure amnd uses of aspirin, quinine, penicillin, teracycline. Sulpha drugs and mechanmism of their actin. Cancer and anticancer drugs. Paper VII ( Practical ) Time 6 hours Total marks 75 Unit 3.11: Experiments of physical chemistry 15 marks a) To study the distribution of iodine between two immiscible solvents at room temperature. b) To determine water of crystallization in ferrous sulphate crystals by titration with 0.1 Normal KMnO4 solution. c) To determine the water of crystallization of hydrated salts by igniting and weighing. d) To determine the coefficient of viscosity with Ostwald's viscometer. Unit 3.12: Preparation of organic compounds 10 marks a) Tribromoaniline from aniline b) Tribromophenol from phenol c) m-dinitrobenzene from nitrobenzene d) Benzil from benzoin e) Phthalic anhydride from phthalic acid f) Iodoform from acetone g) Osazone from glucose. Unit 3.14: Sessional examinations 10 marks Marks to be awarded by holding an examinationb at the end of the session. Viva voce examination 5 marks TDC MAJOR COURSE IN CHEMISTRY Part I examination Paper I (Physical chemistry) Total marks 75 Unit 1.1 Gaseous state 15 marks Unit 1.2 Chemical thermodynamics I 10 marks Unit 1.3 Chemical thermodynamics II 15 marks Unit 1.4 Colligative properties and liquid state 10 marks Unit 1.5 Chemical kinetics 15 marks Unit 1.6 Electrochemistry and ion transport 15 marks Paper II ( Organic chemistry) Total marks 75 Unit 1.7 Introductin to organic compounds 5 marks Unit 1.8 Stereochemistry 10 marks Unit 1.9 Organic compounds 20 marks Unit 1.10 Organic reaction mechanism 25 marks Unit 1.11 Organic reaction mechanism II 15 marks Paper III ( Practical) Time 6 hours Total marks 50 Unit 1.12 Qualitative organic analysis 25 marks A0 Detection of N<S and halogens b) Tests for functional groups by analytical methods c) Solubility, melting point/ boiling point and d0 Preparation of a derivative and determination of its melting points Unit 1.13 General Chemistry Experiments 10 marks a) To determine the rate of iodination by water by Clock reaction b) To determine the solubility of a given substance at different temperatures and to plot the solubility curve c) To determine the water of crystallization of hydrated salt by ignition and weighing Unit 1.14 Sessional examination 10 marks Unit 1.15 Viva voce 5 marks Part II Examination Paper ( IV) Structure and bonding Total marks 75 Unit 2.1 Atomic structure 25 marks Unit 2.2 Chemical bonding I 25 marks Unit 2.3 Chemical bonding 15 marks Unit 2.4 Ionic and solids 10 marks Paper V ( Inorganic chemistry) Total marks 100 Unit 2.5 Properties of Inorganic compounds 15 marks Unit 2.6 Chemistry of nontransition elements I 15 marks]Unit uNIT 2.7 CHEMISTRY OF NONTRANSITION ELEMENTS ii 15 MARKS uNIT 2.8 chemistry OF METALS 15 MARKS Unit2.9 Transition metals 15 marks Paper VI ( Practical) Total marks 50, Time 6 hours Unit 2.10 Quantitative inorganic analysis 25 marks Analysis of a mixture inorganic salts containing total of four cations and anions including interfering anions and insoluble salts Unit 2.11 General chemistry experiments 10 marks a) To identify the constituents of a given mixture by paper chromatography b) To determine the water of crystallisation of green vitriol by titration with 0.1 N KMnO4 by EDTA titration. Unit 2.12 Sessional examination 10 marks ( Marks to be awarded by holding an examination at the end of a session). Unit 2.13 Viva voce 5 marks Part III Examinations Paper VII ( Quantum Chemistry and Spectroscopy) Total marks 100 Unit 3.1 Quantum theory 25 marks Unit 3.2 Atomic structure and atomic spectra 20 marks Unit 3.3 The nature of the chemical bond 10 marks Unit 3.4 Principles of spectroscopy 20 marks Unit 3.5 Infrared and electronic spectroscop[y 15 marks UNit 3.6 Spin resonance and mass spectra 10 marks Paper VIII ( Physical chemistry) Total marks 100 Unit 3.7 Phase equilibria 20 marks Unit 3.8 Molecular reaction dynamics 20 marks Unit 3.9 Surface chemistry and colloids 20 marks Unit 3.10 Macromolecules and properties of solids 20 marks Unit 3.11 Statistical thermodynamics 12 marks Unit 3.12 Data analysis 8 marks Paper IX ( Organic chemistry) Total marks 100 Unit 3.13 Organic reaction mechanisms 20 marks Unit 3.14Polynuclear aromatic compounds and N,S,P Compounds 20 marks Unit 3.15 Unit 3.15 Organic photochemistry, Polymers and fibres 20 marks Unit 3.16 Biochemistry 20 marks Unit 3.17 Natural products and medicinal chemistry 20 marks Paper X ( Inorganic chemistry) Total masrks 100 Unit 3.18 Bonding in coordination compounds 20 marks Unit 3.19 Spectra of cordination compounds 20 marks Unit 3.20 Organometallic compounds 20 marks Unit 3.21 Bioinorganic chemistry 20 marks Unit 3.23 Nuclear chemistry, lanthanides and actinides 20 marks Paper XI ( Practical) Time 6 hours Total marks 100 Unit 3.23 Inorganic quantitative analysis 50 marks Estimation of inorganic ions by volumetric, complexometric, gravinetric, redox and precipitation methods. The following one component systems should be estimated first- Cu, Fe, Mg, Ni, Cl, and SO42-. This should be followed by separation and estimation of individual ions in two component systems of a) Cu and Fe b) Fe and Ca c) Cu and Ni and Cl- and SO4- ions. Unit 3.24 Organic quantitative analysis 30 marks Unit 3.25 Sessional examination 10 marks Unit 3.26 Viva voce 10 marks Paper XII ( Practical ) Total marks 100, Time 6 hours Unit 3.27 Physical chemistry experiments 50 marks At least 10 experiments are to be performed from the list of experiments given below- a) To determine the solubility of a substance (KCN, KNO3, NaNO3) at different temperatures and to obtain the solubility curve. b) To determine the coefficient of viscosity of the given liquid by Ostwald's viscometer. c) To determine the composition of a givenmixture by viscosity method. d)To determine the surface tension of a given liquid by stalagmometer. e) To determine the composition of a given mixture by surface tension method. f) To determine the mutual solubility of phenol and water. g) To determine the molecular mass of a volatile liquidby Victor Meyer's method. h) To determine the specific rotation of an optically active substance by polarimeter.To determine the concentration of a optically active substance by polarimetric method. i) To determine the concentration of an optically active substance polarimetric method. j) To determine the specific reaction rate of hydrolysis of methyl acetate catalyzed by hydrogen ion at room temperature. k) To find the rate of decomposition of H2O2 catalyzed by Fe3+ ion. l) To study the rate of acid catalyzed iodination of acetone. m) To obtain Freundlich's isotherm for absorption of oxalic acid on activated charcoal. n) To study the distributionof iodine between CCl4 and water. o) To verify Debye Huckel and Onsager equation for sodium chloride. q) Conductometric titration: HCl vs. NaOH, Oxalic acid vs. NaOH and Acetic acid vs. NaOH. Unit 3.28 Inorganic preparation 30 marks a) Preparation of the following 1 Chrome alum and crystallization 2. Tetramine Cu(II) sulphate 3. Cu ( glycinate) 4. Hexamine Ni (II) chloride 5. Potassium trioxalato ferrate (III) 6. Potassium trioxalatoferrate (III) 7. Copper thiurea complex 8. Mohr's salt. b) Characterization of the compound prepared Students should recrystallise the product and verify presence of anions and cations by qualitative analysis. Unit 3.29 Organic preparation 30 marks The following preparations are to be done by each student in the class to be given one of them for final examination. a) Acetylation: Preparation of acetanlide from aniline b) Benzoylation: Preparation of benzanilide from aniline c) Nitration: Preparation of m-dinitrobenzene from nitrobenzene. d) halogenation: Preparation of p-bromoacetanilide from acetanilide, Preparation of 2,4,6-tribromophenol from phenol. e) Diazocoupling: Preparation of methyl orange f) Oxidation: Preparation of benzil from benzoin. g) Reduction: Preparation from m-nitroaniline from m-dinitrobenzene. Unit 3.30 Sessional examination ( by holding examination) 10 marks Unit 3.31 Viva voce 10 marks
Students having major in Chemistry and with Physics and Mathematics as elective subjects will only be considered for admission to M.Sc. Course in Chemistry.
Notes: (1) In Semester IV, students will have the option to offer special papers and advanced practical/project work with literature review in any one of the three branches, Physical, Organic and Inorganic Chemistry as follows:
Physical Chemistry
1. Special Paper I: Chemical Kinetics and Electrochemistry 2. Special Paper II: Polymer Chemistry 3. Special Paper III: Heterogeneous Catalysis 4. Special paper IV: Advanced Practical or Project Work 5. Special Paper V: Literature review on an assigned topic
Organic Chemistry
1. Special Paper I: Natural Products chemistry 2. Special Paper II: Organic Synthesis 3. Special Paper III: Bioorganic and Medicinal chemistry 4. Special paper IV: Advanced Practical or Project Work 5. Special Paper V: Literature review on an assigned topic
Inorganic Chemistry
1. Special Paper I: Transition Metals and Inorganic Materials 2. Special Paper II: Organometallics and Photoinorganic Chemistry 3. Special Paper III: Bioinorganic Chemistry 4. Special paper IV: Advanced Practical or Project Work 5. Special Paper V: Literature review on an assigned topic
(2) The distribution of marks for the Special Paper IV (Semester IV) will be as follows:
i) For Advanced Practical: Internal 30 + External 120 = Total 150 ii) For Project Work, a) Examination of dissertation: Internal 50 + External 50 = 100 b) Oral Presentation: Board of examiners 25 + External 25 = 50
(3) The distribution of marks for the Special Paper V (Semester IV) will be as follows: i) For Literature Review: Internal 25 + External 25 = Total 50
The Board of Examiners will be constituted with all the faculty members belonging to the relevant special group.
(3) Duration of Theory Examination will be 4 hours for full paper (80 Marks) and 2 ˝ hours for half paper (40 Marks).
(4) Duration of Practical Examination will be 18 hours spread over 3 days.
Semester I · Paper I PHYSICAL CHEMISTRY Total Marks: 100
Unit 1 Equilibrium and non-equilibrium thermodynamics 10 Marks
(a) Non-ideal systems. Thermodynamics of real gases and gas mixtures, fugacity and its determination. Non-ideal solutions, activity and activity coefficient - different scales of activity coefficients, electrolytic activity coefficients. (b) Phase equilibrium. Thermodynamic criteria of phase equilibrium, Gibbs phase rule and its application to three-component systems - triangular plots - water-acetic acid-chloroform and ammonium chloride-ammonium sulphate-water system.
(c) Non-equilibrium thermodynamics. Forced flows and entropy of production, coupled flows and phenomenological relations; Onsager reciprocal relations. Thermoelectric effects - Seebeck and Peltier and Thompson effects.
Unit 2 Statistical mechanics 20 Marks
Statistical mechanics of systems independent particles - Maxwell Boltzmann distribution, entropy and probability. Calculation of thermodynamic properties for independent particles - molecular partition functions - evaluation of translational, rotational, vibrational, electronic and nuclear partition functions.
Thermodynamic properties of ideal monoatomic and diatomic gases (Suckur Tetrode equation) - calculation of partition functions, thermodynamic functions, principles of equipartition, heat capacities (Einstein model and Debye modification), residual entropy, equilibrium constant. Unit 3 Dynamic electrochemistry 10 Marks
Ion-solvent interactions - the Born model. Thermodynamic parameters of ion-solvent interactions - structural treatment; the ion-dipole model - its modifications, ion-quadrupole and ion-induced dipole interactions. Primary solution - determination of hydration number, compressibility method and viscosity-mobility method. Debye-Hückel theory of ion-ion interactions - derivation, validity and limitations; extended Debye-Hückel equation - ion association and effect of conductance - Debye-Hückel-Onsager equation. The random walk model of ionic diffusion - Einstein-Smoluchowski relation.
Unit 4 Basic principles of quantum mechanics 20 Marks
(a) Wave functions of one-particle and many-particle systems: Born interpretation. Well-behaved functions and normalized functions. Schwartz inequality (without derivation). (b) Dynamical variables and quantum mechanical operators - Hermitian operators and their properties. (c) Eigenvalues and eigenfunctions of quantum mechanical operators, their physical significance. Schrödinger’s wave equation. Orthogonal functions - Schmidt’s orthogonalisation technique.
(d) Expectation values of observable properties. Compatible observables and compatibility theorem. Incompatible observables and the (generalized) uncertainty principle from Schwartz inequality.
(e) Basic ideas about the theory of angular momenta - spin and orbital angular momenta, conservation of angular momenta. General angular momentum operators Jx, Jy, Jz, step-up and step-down operators. Eigenvalues of J2 and Jz operators. Coupling of orbital and spin angular momenta - theoretical basis of the L-S and j-j coupling schemes.
Unit 5 Exactly solvable problems in quantum mechanics 20 Marks
Solutions of the energy eigenvalue equations for: (a) Problem of two interacting particles - separation of center of mass and relative motion. (b) Linear harmonic oscillator, vibrational energy levels of diatomic molecules. (c) Particle in a ring. Free electron MO theory of benzene. (d) Rectangular potential barrier problems. Quantum mechanical tunneling. (e) The two-particle rigid rotor problem, rotational energy levels of a diatomic molecule. (f) The hydrogen atom. Radial solution- radial probability distribution function. Angular solutions, representation of orbitals. Internal Assessment 20 Marks
Semester I · Paper II ORGANIC CHEMISTRY Total Marks: 100
Unit 1 Stereoelectronic effect and reactivity 15 Marks
The electronic basis of stereoelectronic effects – orbital-orbital interactions (from AO to MO), interaction between molecules (HOMO & LUMO); aromaticity and antiaromaticity – nonclassical concepts should be emphasized; HSAB concepts and their applications; symbiosis
Stereoelectronic effects on reactivity – effects through bonds, through space; conformation and reactivity.
Unit 2 Stereochemistry 25 Marks
Brief overview of the following: designation of configuration; Fischer-Sawhorse-Newman interconversion.
Molecular symmetry, asymmetry & dissymmetry; classification of organic molecules into different Point Groups; Concept of stereogenic center – chirotopic and achirotopic center; Homotopic and heterotopic ligands and faces (prostereoisomerism and prochirality etc.); optical purity and enantiomeric excess; meaning of absolute and relative configuration; chirality in molecules devoid of chiral centers – allenes, spiranes and biphenyls.
Unit 3 Organic Reaction Mechanism 25 Marks
Reaction intermediate vs. transition state, thermodynamic product vs. kinetic product; factors affecting mechanism and reactivity in nucleophilic substitution reactions; factors affecting mechanism and reactivity in elimination reactions, and competition with substitution reactions; reactivity–selectivity principle – chemoselectivity, regioselectivity, stereoselectivity & stereospecificity in substitution, elimination and addition reactions; steric acceleration and steric retardation.
Unit 4 Investigation of organic reaction mechanism 15 Marks
Kinetic & nonkinetic methods; kinetic isotope effects and isotope labeling studies; significance of rate limiting step in multi-step reactions; from rate law to mechanism and from mechanism to rate law. Hammett & Taft equation ; partial rate factor.
Internal Assessment 20 Marks
Semester I · Paper III INORGANIC CHEMISTRY Total Marks: 100
Unit 1 Chemical bonding and intermolecular interactions 20 Marks
Chemical bonding of simple inorganic covalent compounds - molecular orbital treatments, hybridization; understanding molecular properties from bonding. Molcular orbital theory of homo- and heteronuclear diatomics, molecular orbitals of polyatomic molecules, molecular shape in terms of molecular orbitals - Walsh diagrams.
Atomic and ionic radii - bond length and bond strength, van der Waals forces. Hydrogen bonding interactions, effects of hydrogen bonding and other chemical forces on melting and boiling points and solubility.
Unit 2 Structure of simple solids 20 Marks
Packing of spheres - hexagonal and cubic close-packing, tetrahedral and octahedral holes in close-packed structures - metals and alloys, solid solutions. The ionic model for the description of bonding in ionic solids. Characteristic structures of ionic solids - the NaCl and CsCl types, the sphalerite and wurtzite types of ZnS, the NiAs structure type, the perovskite and spinel structure types of mixed-metal oxides - importance of ionic radii and the radius ratios in determining structure type among ionic solids. Lattice energy considerations, thermal stability and solubility of inorganic solids.
Unit 3 Descriptive inorganic chemistry 20 Marks
Synthesis, structure, bonding and reactivity of boron hydrides including polyhedral boranes, carboranes and mettalocarboranes. Allotropes of carbon (including fullerenes), phosphorous and sulpher. Chemistry of silicates, aluminosilicates, zeolites and clays. Unit 4 Acid-base and redox chemistry 20 marks
Hard and soft acid-base (HSAB) concept and its applications. Strength of oxo acids and halo acids, strength of inorganic bases - periodic trends in acidity and basicity of hydrides, oxides, oxyacids of non-transition elements. Relevance of acidity and basicity in catalysis.
Standard electrode potentials, pH dependence of elctrode potentials. Redox stability of metal ions in water, oxidation by atmospheric oxygen. Applications of Latimer and Frost diagrams, redox behaviour of non-transition elements based on electrode potential data. Internal Assessment 20 Marks
Semester I · Paper IV BIOCHEMISTRY Total Marks: 50
Unit 1 Biology for chemists 10 Marks
(i) Structure of prokaryotic and eukaryotic cells, intracellular organelles and their functions, comparison of plant and animal cells. Overview of metabolic processes - catabolism and anabolism.
(ii) Constituents of the cell nucleus and cytoplasm, structure of chromosomes, mitosis and meiosis. Biological membranes – lipids and lipoproteins, composition and function. Lipid aggregates – micelles, bilayers, liposomes and their biological functions.
(iii) Origin of life - unique properties of carbon, chemical evolution and rise of living systems. Carbohydrate metabolism – Kreb’s cycle, glycolysis.
Unit 2 Biophysical chemistry 10 Marks
(i) Bioenergetics – standard free energy change in biochemical reactions, hydrolysis of ATP, synthesis of ATP from ADP. Biological oxidation & reduction reactions – electron transfer in and redox potentials of biologically important half reactions, chemistry involved in oxidative phosphorylation.
(ii) Chain configuration of biological macromolecules, polypeptide and protein structure - protein folding.
(iii) Thermodynamics of biopolymer solutions, osmotic pressure. Cell membrane, active transport of ions through cell membranes, membrane equilibrium, muscular contraction, energy generation in living systems. Transmission of nerve impulses.
Unit 3 Bioorganic chemistry 10 Marks
(i) Nucleic acids, structure and functions of DNA and RNA – the double helix structure. Chemical and enzymatic hydrolysis of nucleic acids. Genetic code – replication, transcription, translation of genetic information – chemical basis of heredity.
(ii) Enzymes – classification and catalytic behaviour; enzyme specificity, conformation, kinetics, mechanism of action; factors affecting enzyme activity; enzyme regulators and inhibitors, enzyme models – host-guest chemistry. Biotechnological applications of enzymes.
(iii) Co-enzymes – Co-enzymes involved in biological oxidation-reduction reactions.
Unit 4 Bioinorganic chemistry 10 Marks
Distribution of metal ions in nature and their biological significance. Iron storage and transport – siderophores, ferritin and tranferrin, Na+/K+ pump. Dioxygen storage and transport – structure and functions of myglobin, haemoglobin. Electron transfer proteins – structure and function of iron-sulphur proteins, cytochromes and plastocyanine. Metal enzymes – nitrogenases and dioxygen fixation, vitamin B12, Inorganic drugs (gold compounds and cisplatin), chelate therapy.
Internal Assessment 10 Marks
Semester I · Paper V Laboratory Course (Organic Chemistry) Total Marks: 150 A. Qualitative Organic Analysis 30 Marks
Binary mixtures of organic compounds, covering compounds with major functional groups, should be given with an objective to train students in
I. Qualitative separation by physico-chemical methods and II. Identifying the compounds by chemical analysis
B. Organic Estimation 20 Marks
I Glycine by sodium hydroxide in the presence of formaldehydeII Number of hydroxy groups in a disaccharide by acetylation III Percentage purity of carbonyl compounds by 2,4-dinitrophenylhydrazine IV Carboxylic acid by Ag-salt method V Glucose & sucrose in a mixture
C. Chromatographic Application 15 Marks
I. Separation and identification of aromatic nitro compounds present in a binary mixture by TLC II. Separation and identification of aminoacids present in a ternary mixture by paper chromatography
D. Organic Preparation 20 Marks One-step preparation I m-Dinitrobenzene from nitrobenzene II Benzhydrol from benzophenone by reduction in alkaline medium III Anthraquinone from anthracene by oxidation with chromium trioxide Two-step preparation I Benzanilide from benzophenone II Benzilic acid from benzoin III Dibenzyl from benzoin IV Anthranilic acid from phthalic anhydride
E. Isolation of Natural Products 15 marks
I Soxhlet extraction of carotenoids/chlorophyll from carrot/ tomato/ papaya/spinach and determination of Rf values by TLC II Isolation of nicotine from tobacco III Extraction of milk proteinsIV Extraction of essential oils from orange peels/rose petals/clove/ginger
F. Viva-voce 20 Marks
G. Internal Assessment 30 Marks Semester II · Paper I PHYSICAL CHEMISTRY Total Marks: 100 Unit 1 Chemical kinetics 16 MarksSteady-state approximation and its applications. Oscillating reactions, chemical chaos. Belousov-Zhabotinski reaction. Straight-chain reaction - hydrogen-halogen reactions, alkane pyrolysis. Branching-chain reactions - the hydrogen oxygen reaction, explosion limits. Enzyme catalysed reactions, Michaelis-Menten mechanism - Lineweaver-Burk and Eadie plots, enzyme inhibition.
Unit 2 Molecular reaction dynamics 16 MarksCollisions of real molecules - trajectory calculations. Laser techniques, reactions in a molecular beam - reaction dynamics. Estimation of activation energy and the calculation of potential energy surfaces - the transition state theory (TST) of bimolecular gaseous reactions, statistical and thermodynamic formulations. Comparison between TST and hard-sphere collision theory. Theory of unimolecular reactions - Lindemann theory and its limitations; Kinetics of reactions in solution -diffusion controlled and chemically controlled reactions. TST of reactions in solution - Bronsted and Bjerrum equation, effect of ionic strength, kinetic salt effect
Unit 3 Homogeneous catalysis 16 MarksAtom transfer and electron transfer processes. Role of transition metal ions with special reference to Cu, Pd, Pt, Co, Ru and Rh, catalysis in non-aqueous media. Rates of homogeneously catalysed reactions, turnover number and frequency. Catalysis of isomerisation, hydrogenation, oxidation and polymerization reactions. Asymmetric catalysis, biocatalysis, photoactivated catalysis and metal clusters in catalysis. Phase-transfer catalysis.
Unit 4 Adsorption on solid surfaces 16 MarksAdsorption of gases on solid surfaces - Langmuir’s theory and its limitations. Derivation of BET equation - determination of surface area of an adsorbent, thermodynamics of adsorption processes. Capillary condensation - adsorption in micropores, hysteresis loop. Kinetics of heterogeneous catalysis - Langmuir-Hinselwood model and Riedel-Eley model, electrokinetic phenomena at the interface - electrical double layer. Colloidal stability, micelles and reverse micelles - microemulsions.
Unit 5 Polymer science 16 MarksPolymers and polymerization - natural and synthetic polymers - molecular weights, control of molecular mass. Technological applications of polymers. Frictional properties of macromolecules (polymers) in solution, the concept of free draining, equivalent sphere model. Chain configuration of macromolecules - root mean square end to end distance and radius of gyration; random flight model and chain stiffness, average dimension of polymer chains. Kinetics of step polymerization and copolymerization - ring-scission polymerization.
Internal Assessment 20 Marks Semester II · Paper II ORGANIC CHEMISTRY Total Marks: 100
Unit 1 Stereoselective synthesis 10 Marks
Classification of stereoselective synthesis – diastereoselective, enantioselective & double stereodifferentiating reactions; nucleophilic addition to aldehyde and acyclic ketones – Cram, Felkin and Felkin-Anh model; nucleophilic addition to cyclic ketones.
Enantioselective synthesis – use of chiral reagent, chiral catalyst and chiral auxiliary.
Unit 2 Oxidation reactions of synthetic importance 20 Marks
Allylic oxidation of alkenes – use of chromium trioxide-pyridine complex (Collin’s reagent) and selenium dioxide.
Oxidation of alcohols – use of PCC, PDC, Swern oxidation, Mn(IV) oxide, silver carbonate, tetrapropylammonium perruthenate(VII). Oxidation of 1,2-diols – use of periodic acid and Pb-tetraacetate.
Oxidation of carbon-carbon double bonds – perhydroxylation by KMnO4, OsO4 (including Sharpless dihydroxylation & epoxidation), oxidation with iodine, silver carbonate and peroxy acids; introduction to electrooxidation – oxidation of tertiary amines, alkenes and carboxylates.
Unit 3 Reduction reactions of synthetic importance 20 Marks
Use of H2/Pd-C, LAH, NaBH4, NaCNBH3, 9-BBN, Lindlar catalyst, DIBAL, diimide, alkali metals in liquid ammonia, super hydride and selectrides; chiral reducing agents; introduction to electroreduction – reduction of carbonyl compounds, alkyl halides and nitro compounds. Unit 4 Pericyclic reactions 15 Marks
Introduction pericyclic reactions, MO symmetry; FMO of conjugated polyenes. Woodward-Hoffmann principle of conservation of orbital symmetry, allowed and forbidden reactions, stereochemistry of pericyclic reactions. Cycloaddition reactions – [2+2], [4+2], [6+2] cycloadditions, stereoselectivity of the reactions. Sigmatropic rearrangement – fluxional molecules, stereoselectivity in Cope and Claisen rearrangement. Unit 5 Organic Photochemistry 15 Marks
General principles of photochemistry; excited state and photosensitization, photochemical processes – chemiluminescence, chemical and photochemical method of producing singlet oxygen, photostereomutation of cis-trans isomers.
Internal Assessment 20 Marks Semester II · Paper III INORGANIC CHEMISTRY Total Marks: 100
Unit 1 Coordination Chemistry I 10 Marks
General properties of transition elements, coordination compounds – types of ligands and complexes. Mononuclear complexes – commonly observed coordination geometries and their symmetry properties. Tetragonal, rhombic and trigonal distortions in octahedral complexes. Unit 2 Coordination Chemistry II 20 Marks
Crystal field theory of bonding in octahedral, tetrahedral and square planar transition metal complexes. Factors affecting crystal field splitting, crystal field stabilization energy, spectrochemical series. Ligand field theory of metal complexes - electronic spectra - d-d spectra interpretation of spectral behaviour of octahedral and tetrahedral complexes. Charge transfer spectra.
Unit 3 Complexes of π-acceptor ligands and organometallic compounds 20 Marks
Synthesis, structure, bonding, and reactivity of transition metal complexes of π-accepting ligands such as CO, NO, PPh3. Metal carbonyl hydrides and metal carbonyl clusters. Metal – metal bonding in Re2Cl82-. Complexes containing alkenes and alkynes as ligands. Ferrocene – synthesis, structure, bonding and reactivity.
Unit 4 Reactivity of complexes 20 Marks
Stability constants, the chelate effect, labile and inert complexes, mechanism of substitution reactions in octahedral complexes and associated stereochemical changes, isomerisation and racemisation of tris-chelate complexes. The trans effect. Electron transfer reactions – outer and inner sphere mechanism.
Unit 5 Chemistry of lanthanides and actinides 10 Marks
Important aspects of the chemistry of the lanthanides - oxidation states, lanthanide contraction, separation of lanthanide elements, lanthanide shift reagents. Chemistry of actinides - electronic configurations, oxidation states, sources of the actinide elements, their extraction and applications. Radioactivity of actinides.
Internal Assessment 20 Marks
Semester II · Paper IV MOLECULAR SPECTROSCOPY Total Marks: 50 Unit 1 Introduction to molecular spectroscopy 5 MarksElectromagnetic spectrum, interaction of electromagnetic radiation with molecular systems. Spectroscopic transitions - absorption, emission, reflection, polarization and scattering processes. Natural line width and broadening - intensity of spectral transitions, selection rules. Sampling techniques in different branches of spectroscopy.
Unit 2 Rotational (microwave) spectroscopy 5 Marks(a) Classification of molecules according to their moments of inertia, rotational energy levels of HCl. Determination of molecular geometry by isotopic substitution effects on pure rotational spectrum. Stark effect, estimation of molecular dipole moments. Spectra of symmetric top and asymmetric top type molecules. (b) Rotational Raman spectra - anisotropic polarisability. Specific selection rule in Raman spectroscopy, Stokes and anti-Stokes lines.
Unit 3 Vibrational-rotational spectroscopy 8 Marks(a) Diatomic molecules - force constants. Fundamental vibration frequencies. The anharmonicity of molecular vibrations and its effect on vibrational frequencies, second and higher harmonics. (b) Vibration-rotation spectrum of HCl - P, Q and R branches. Vibrational Raman spectra of diatomic molecules. (c) Polyatomic molecules (e.g., CO2, NH3) - normal modes vibrations, symmetry of vibrations - group theoretical treatment. Elements of normal coordinate analysis for the CO2 molecule.
Unit 4 Electronic spectroscopy 8 MarksElectronic transitions, the Frank-Condon principle, ground and first excites states of diatomic molecules, selection rules on the basis of the symmetry properties of the electronic states. Vibronic transitions. Fluorescence and phosphorescence, laser action. Electronic spectra of conjugated, aromatic and coordination compounds - d-d and charge-transfer spectra. Change of molecular shape upon electronic excitation.
Unit 5 Magnetic resonance spectroscopy 7 + 7 = 14 marks (a) Nuclear spin, Larmor frequency, population of nuclear spin levels. Spin-spin and spin-lattice relaxation. Spin-spin coupling, chemical shifts, ring currents and aromaticity, Proton and 13C NMR spectroscopy of simple organic molecules, living systems - MRI. Introduction to the NMR of solids - MAS-NMR.
(b) Characteristic features of ESR spectra - line shapes and line widths. The g value and the hyperfine coupling parameter (A) - origin of hyperfine interaction, contact and dipolar mechanisms. Spin Hamiltonian, anisotropy of g and A. ESR spectra of simple organic radicals, spectral behaviour transition metal complexes of octahedral and distorted octahedral geometry.
Internal Assessment 10 Marks
Semester II · Paper V Laboratory Course (INORGANIC CHEMISTRY) Total Marks: 150
A. Qualitative and Quantitative Analysis 40 Marks
(a) Separation and determination of two metal ions Cu-Ni, Ni-Zn, Cu-Fe, etc. involving volumetric and gravimetric methods (b) Analysis of ores/alloys, cement and steel, etc.
Ores: Haematite, Limestone, Dolomite, Cement, Pyrolussite, and other ores
Alloys: Brass, Gunmetal, Cupronickel, Solder, Bronze, Phosphor Bronze, Steel, Copper concentrate, other alloys
(c) Determination of hardness of water
B. Preparation and characterization (30 + 30) Marks
Preparation of selected inorganic compounds and their physico-chemical characterization by elemental analysis, IR and electronic spectrophotometry, magnetic susceptibility measurements, magnetic resonance spectroscopy, solution conductivity measurements, wherever appropriate and possible.
(i) Complexes with O-donor ligands
(a) A3M(C2O4)3 - M = Al, Cr, Fe; A = alkali metal (b) VO(acac)2 (c) Cu2Ac4(H2O)2 (d) Cu(acac)2
(ii) Complexes with N donor ligands
(a) [Co(NH3)5Cl]Cl2, [Co(NH3)5(ONO)]Cl2, [Co(NH3)5(NO2)]Cl2 (b) Hg[Co(NCS)4] (c) Ni(dmg)2 (d) N4[Cr(NH3)2(SCN)4]
C. Viva 20 Marks
D. Internal Assessment 30 Marks
Semester III · Paper I :: QUANTUM CHEMISTRY
Total Marks: 100 Unit 1 Approximate methods of quantum mechanics 20 Marks(a) Time-independent first-order perturbation theory for (i) non-degenerate and (ii) degenerate systems - applications to the ground and first-excited states of the helium atom. (b) The variation theorem, linear variation function - secular equation.
Unit 2 Electronic structure of Many-electron atoms 10 MarksProduct wave functions - complete many-electron wave functions including electron spin. Pauli’s anti-symmetry and exclusion principles. Spin states of a two-electron system - singlet and triplet states.Independent particle central field model of many-electron atoms - the helium atom. Atomic orbital theory - Slater type orbitals (STO), electron repulsion parameters (Racah and Condon-Shortley types). Spectroscopic term symbols for the s1p1, p2 and d2 configurations - splitting of term energies due to electron repulsion and magnetic effects - spin-orbit coupling and Zeeman splitting.
Unit 3 General Theorems in molecular quantum mechanics 10 Marks(a) Born-Oppenheimer approximation, separation of electronic and nuclear motion. (b) Hellmann-Feynmann theorem and its chemical applications. The electrostatic theorem and the force field concept in chemistry. (c) Introduction to the molecular electronic virial theorem. (d) Elementary ideas about density functional theory.
Unit 4 Chemical bonding 25 Marks(a) The hydrogen molecule ion: linear combination of atomic orbital (LCAO)-molecular orbital (MO) theory - ground and excited electronic states. (b) The hydrogen molecule: LCAO-MO and valence bond (VB) treatments. Equivalence of the MO and VB methods. (c) Extension of the LCAO-MO method to homo- and heteronuclear diatomics -inclusion of hybridization. (d) Term symbols for molecular electronic states, their symmetry classification - ligand field terms. Correlation diagrams and the non-crossing rule. (e) LCAO-MO theory of simple polyatomic molecules (e.g., the H2O molecule) (f) -electron theory - Hückel molecular orbital (HMO) method for unsaturated carbon compounds showing chain and ring structures, introduction to extended Hückel theory. HMO treatment of infinite linear polyenes, elements of band theory. Unit 5 Ab initio and semi-empirical SCF theories 15 marks(a) The self consistent field method, Hartree-Fock theory of closed shell electronic configurations of atoms and molecules. Coulmb and exchange integrals, canonical Hartree-Fock equations, Koopman’s theorem without derivation. (b) SCF LCAO-MO theory of molecules - Roothan equation. (c) Semi-empirical SCF theory: Parriser-Parr-Pople approximation.
Internal Assessment 20 Marks
Semester III· Paper II PHYSICAL METHODS IN CHEMISTRY Total Marks: 100 [Students are required to write answers to questions from Part A and Part B in two separate books]
Part A: Applications in Organic Chemistry (35 Marks)
Unit 1 Mass and IR spectroscopy 4 + 4 = 8 Marks
Mass spectroscopy: Ion fragmentation mechanism, base peak and molecular ion peak, nominal mass and exact mass, isotopic distribution - problems.
IR spectroscopy: Characteristic bands for different functional groups, change in band frequency due to FGI. Effects of hydrogen bonding on band frequency. Problems.
Unit 2 NMR spectroscopy 12 marks
Chemical shifts and splitting patterns of signals, coupling constant and its distinction from chemical shift - use of coupling constant in structural elucidation. Simplification of spectra by use of shift reagents and high magnetic fields, integration and its use in proton count and molecular ratios - determination of enantiomeric excess. Deuterium exchange technique in the determination of labile hydrogen, spin-decoupling and NOE, 2D NMR (1H - 1H and 1H - 13C COSY), DEPT. Complexity of 13C NMR spectra and use of spin decoupling in its simplification, CINDP and its applications. Simple worked out examples using application of NMR.
Unit 3 Optical spectroscopy and chiroptical properties 5 Marks
UV-visible spectroscopy - max and molar absorptivity, factors affecting them. Calculation of max - Woodward Fieser’s rules.
Chiroptical properties - introduction to CD (Circular Dichroism), ORD (Optical Rotatory Dispersion) and CPE. Applications of CD and ORD - octant rule.
Unit 4 Chromatography 10 Marks
Introduction to different chromatographic techniques - principles involved and the effect of solvent polarity on retention factor. Sensitivity and quantitative limitations of thin-layer chromatography (TLC) and column chromatography. Reagents commonly used in the detection of TLC spots, reverse phase chromatography and its applications. General treatment of gas chromatography (GC) and high performance liquid chromatography - basic ideas of instrumentation, advantages.
Part B: Applications in Inorganic Chemistry (45 Marks)
Unit 5 Vibrational and electronic spectroscopy 7 + 4 + 4 = 15 Marks
(a) Symmetry criteria for intensity of spectroscopic transitions (qualitative treatment), symmetry and spectral changes upon coordination.
Infrared and Raman Spectroscopy: Symmetry and IR/Raman activity of normal modes of vibrations, Mutual exclusive principle, interpretation of IR and Ramsn spectra of simple inorganic and coordination compounds.
(b) Study of metal-ligand equilibria and Job’s method, CD, ORD and MCD of inorganic compounds.
(c) Photoelectron spectroscopy: Basic principles and applications of PES (O2, N2 and N3-) only, chemical information from ESCA. Unit 6 ESR, NMR and Mossbauer spectroscopy 5 + 5 + 5 = 15 Marks
(a) ESR Spectroscopy: Basic principles, factors effecting g-tensors, hyperfine splitting in inorganic free radicals and metal complexes, zero field splitting. Application of ESR to d1 and d9 complexes of various symmetry.
(b) NMR Spectroscopy: Simple application to diamagnetic inorganic compounds, NMR paramagnetic shifts, simple application to paramagnetic compounds, NMR of 31P and 19F in inorganic compounds.
(c) Mossbauer: Basic principles, isomer shift, quadruple splitting, and effect of magnetic field. Application to the study of high-spin and low-spin iron compounds, and of Sn compounds in various oxidation states and coordination geometries.
Unit 7 Electrochemical, Thermal and X-ray diffraction methods 4 + 4 + 7 = 15 Marks
(a) Electrochemical methods: principles, instrumentation and applications of cyclic voltammetry.
(b) Thermal methods: Principles and applications of thermogravimetry, DTA, TGA and DSC of inorganic compounds.
(c) X-ray diffraction: Crystal symmetry, Space groups, Bragg condition, Miller indices, Laue and Bragg methods, Debye and Scherrer method of X-ray structural analysis of crystals, index reflections, identification of unit cells from systematic absence in diffraction pattern, Structure of simple lattices and X-ray intensities, structure factor and its relation to intensity and electron density, phase problem, Description of the procedure for an X-ray structure analysis of small molecules.
Internal Assessment 20 Marks
Semester III · Paper III ENVIRONMENTAL AND ANALYTICAL CHEMISTRY Total Marks: 100
Unit 1: Environmental Chemistry: Global Perspective 5 Marks
Introduction to Environmental Chemistry, Chemical processes in the environment, Water cycle and its implications, Water resource flux, Case histories of environmental disasters and accidents. Green chemistry concepts.
Unit 2: Atmospheric Chemistry 25 Marks
Temperature and pressure variations in the atmosphere, Chemical composition of the atmosphere and the influence of solar radiations, Thermodynamic, kinetic and photochemical considerations, Role of free radicals in atmospheric chemistry.
Chemistry of the stratosphere, Role of UV-radiations in production and destruction of ozone, Catalytic decomposition processes with special reference to the role of NO., .OH and ClO. Radicals, Anthropogenic sources of Cl, Formation of Antarctic and Arctic ozone holes.
Smog formation, Chemical species in smog, VOCs and their oxidation, Emissions from two-stroke and four-stroke gasoline engines, Emissions from diesel engines, CNG and alternative fuels, Production of ozone in the lower atmosphere and its impact.
Nitrogen and Sulphur species present in the atmosphere and their sources, Production of nitric and sulphuric acids in the atmosphere, Acidifying agents in rain, fog and snow, Control of anthropogenic nitrogen and sulphur emissions – fluidised bed combustion, desulphurisation, SONOX process, Conversion of coal to liquid and gaseous fuels. Aerosol chemistry, Polyaromatic hydrocarbons (PAHs) and heavy metals in aerosols, Condensation aerosols, the Arctic haze, Lifetime and transport of aerosol particles.
Pollutants in the urban atmosphere, Indoor air pollution, Radioactivity and radon pollution.
Energy balance of the earth in terms of black body radiation, Greenhouse gases and their generation from various sources, the global warming potential.
Unit 3: Hydrosphere Chemistry 20 Marks
Distribution of chemical species in water, The Phosphorous and Sulphur systems, Gases in water, Alkalinity.
Organic matter in water, Humic matter in water – origin, formation and environmental role.
Environmental classification of metals in water, Behaviour of Calcium, Copper and Mercury in the hydrosphere, Formation of complexes between metals and anthropogenic pollutants in water.
Partitioning of small organic molecules between water and soil or sediment, sorption of organic species by soil, octanol-water partition coefficient, Role of clay minerals in the environment.
Wastewater treatment processes, Use of chemical coagulants, Treatment of water containing excessive iron, phosphate, nitrate and fluoride.
Unit 4: Soil Chemistry 10 Marks
Composition of soil, Chemical weathering, Physical properties of soil – particle size, texture, bulk density, permeability, Chemical properties – Cation Exchange Capacity, pH, macro and micro nutrients, Leachate formation.
Wastes from mining and metal production, Acid Mine Drainage, Sewage sludge, Biogas synthesis, Hazardous wastes and their disposal, Incineration.
Pesticides and their role in the environment, DDT and its fate in the environment.
Unit 5: Analytical Techniques 20 Marks
Analysis of Common Ions – Ultraviolet and Visible Spectrometry, Emission Spectrometry, Ion Chromatography.
Preparation of sample for trace metal analysis in water, air, soil and plants, Extraction and dissolution techniques, Microwave digestion. Chemical speciation technique.
Analysis of metal ions – Atomic Absorption Spectrometry, Anodic Stripping Voltammetry, Inductively Coupled Plasma Mass Emission Spectrometry, Neutron Activation Analysis.
Analysis of trace organics with particular reference to phenolic compounds, PCBs and PAHs – Extraction techniques for Chromatographic Analysis, Gas Chromatography, HPLC, GC-MS, Immunoassay technique.
Sampling and analysis of PM10 and gases in air.
Internal Assessment 20 Marks
Semester III · Paper IV COMPUTERS IN CHEMISTRY Total Marks: 50
Unit 1 Introduction to computers 10 Marks
The components of a computer, Central Processing Unit, Secondary Storage Devices (magnetic disks, FD, HD, CD), Input and Output Devices, Hardware and Software. Types of Computers, The Personal Computer.
Programming Languages - Algorithms, flow charts aand Computer Programs. An Example: Program to reverse a four-digit number 1234 to 4321. Windows Operating System, Software Packages in Windows and their use.
Unit 2 Principles of FORTRAN and BASIC programming 10 Marks
Elements of FORTRAN and BASIC languages, constants and variables, expressions, operations and symbols, common mathematical functions, arithmatic expressions and assignment statements, input and output statements, Format statement, Termination statement, GO TO, Arithmetic IF and Logical IF statements, Complex and Logical Variables, Subscripted Variables and DIMENSION and DO statements. Subprograms, Functions and Subroutines, Arraying and Dimensioning, EQUIVALENCE, COMMON and DATA statements.
Unit 3 Applications in Chemistry I 10 Marks
Solution of simultaneous equations with examples from chemistry, solution of quadratic equations with examples from chemistry, Least squares method of fitting data to a straight line, applications of programming for Hückel Molecular Orbital calculations, calculation of delocalisation energy of an aromatic system.
Unit 4 Applications in chemistry II 10 marks
Computer program for calculation of rate constants of reactions from concentration vs. time data. Calculation of concentration of a (Fe(II)‑phenanthroline) complex from absorbance data for calculation of wavelength maxima of conjugated dienes. Plotting of data of an experiment (e.g., first order kinetics, spectra at different concentrations), data-fitting and evaluation of the parameters (e.g., rate constants, extinction coefficient). Learning to use MOPAC and CHEMDRAW for chemical applications. Molecular graphics - use of ORTEP and PLUTON to generate molecular structure, practical work. Practical work - using the Internet for chemical information retrieval.
Internal Assessment 10 Marks
Semester III · Paper V Laboratory Course (PHYSICAL CHEMISTRY) Total Marks: 150
[The students will complete a minimum of 20 experiments with at least 6 experiments from Unit 1 and 3 experiments each from subsequent units. In the examination, 3 experiments - one from unit 1, one from Units 2 and 3 and 1 from Units 4 and 5 will be required to be done.]
Unit 1 Chemical Kinetics
1. Determine the temperature coefficient and energy of activation of acid hydrolysis of methyl acetate, using least-squares calculation. 2. Study the kinetics of the reaction between iodine and acetone in acidic medium by half-life period method and determine the order with respect to iodine and acetone. 3. Determine the inversion of sucrose in presence of two acids polarimetrically using Guggenheim plots and hence determine the relative strengths of the acids. 4. Study the saponification of ethyl acetate by sodium hydroxide and determine the order of the reaction and energy of activation. 5. Study the autocatalytic reaction between oxalic acid and KMnO4 and determine the order of the reaction. 6. Study the mutarotation of glucose in presence of acid and base by polarimetric method. Investigate the influence of acid and base strength on the rate of the reaction. 7. Study the decomposition kinetics of the formation of complex between sodium sulphide and sodium nitroprusside spectrophotometrically. Determine rate constant and order of reaction. 8. Study the kinetics of the reaction between peroxydisulphate and potassium iodide and find the influence of ionic strength on the rate constant. 9. Study the kinetics of the oxidation of ethanol by chromium(VI) and find the rate constant of the reaction . Also find the order of the reaction by half-life period method. 10. Establish the order of reaction
by the method of ratio variation.
Unit 2 Conductometry
1. Determine the equivalent conductivity of acetic acid at infinite dilution by Kohlrausch’s method and hence find the degree of dissociation constant of the acid. 2. Compare the relative strength of acetic acid and monochloroacetic acid by conductance measurement. 3. Determine the solubility and the solubility product of a sparingly soluble salt like PbSO4 or PbI2 at room temperature by conductance measurement. 4. Determine the degree of hydrolysis and the hydrolysis constant of aniline hydrochloride / sodium acetate. 5. Determine the strength of the components of the following mixtures by conductometric titration. (a) Hydrochloric acid and acetic acid. (b) Sulphuric acid and copper sulphate. (c) Hydrochloric acid and potassium chloride.
Unit 3 pH-metry and potentiometry
1. Determine the dissociation constant of acetic acid / oxalic acid by Albert-Serheart method / using Hendersen’s equation. 2. Find the amount of the components of the following mixtures using PH-metric titration. (a) Hydrochloric acid + acetic acid (b) Hydrochloric acid + oxalic acid (c) Potassium chloride + potassium bromide + potassium Iodide. 3. Determine the apparent ionisation constant of acetic acid by potentiometric titration of the acid against sodium hydroxide using quinhydrone electrode. 4. Potentiometrically estimate strengths of solutions of hydrochloric acid and acetic acid individually and a mixture of the two using standard sodium hydroxide solution. 5. Titrate potentiometrically ferrous ammonium sulphate against potassium dichromate and determine the standard electrode potential of the ferrous/ferric system.
Unit 4 Spectrophotometry, refractometry and others
1. Verify Beer’s law and determine the concentration of solutions like KMnO4 /K2Cr2O7 /CuSO4 2. Determine the concentration of chromium and manganese in a mixture of dichromate and permanganate by spectrophotometric method 3. Determine the composition of iron-salicylic acid complex spectrophotometrically by Job’s method of continuous variation 4. Determine the refractive index of a liquid like carbon tetrachloride and hence find the radius of its molecule 5. Verify the mixture law of refraction and draw the calibration curve for mixtures like glycerol/water, n-heptane/n-hexane. Hence determine the composition of an unknown mixture of two components.
Unit 5 Miscellaneous experiments
1. Determine the molar mass of a polymer by viscometric method.2. Study the variation of surface tension of a solution of n-propyl alcohol/ethanol with concentration and determine the limiting cross-sectional area of the alcohol molecule.3. Determine the partial molar volume of methanol/ethanol/formic acid by graphical method by determining the densities of solutions at different concentrations. 4. Determine the influence of NaCl, naphthalene and succinic acid on the critical solution temperature of phenol-water system using 0.5, 1 and 1.5% concentrations. 5. Study the complex formation between Cu2+ ion and ammonia by distribution method and find the composition of the complex. 6. Perform theoretical calculations using a computer on
(i) Least squares fitting and plotting linear and exponential graphs. (ii) Charge density distribution and shapes of s and p orbitals. (iii) Potential energy diagram of hydrogen molecule ion.
Marks distribution in the Examination:
i) Experiment 1 from Unit 1: 40 Marks ii) Experiment 2 from Units 2 & 3: 30 Marks iii) Experiment 3 from Units 4 & 5: 30 Marks iv) Viva voce: 20 Marks v) Internal Assessment: 30 Marks
Semester IV · Physical Chemistry Special Group
Physical Special Paper I :: CHEMICAL KINETICS AND ELECTROCHEMISTRY Total Marks: 100
Part A: Chemical Kinetics (50 Marks) Unit 1 Study of fast reactions 10 Marks Stopped flow technique, temperature and pressure jump methods, NMR studies in fast reactions, shock tube kinetics, relaxation kinetics. Linearised rate equation, relaxation time in single step fast reactions, determination of relaxation time.
Unit 2 Theories of unimolecular reactions 10 marks Drawbacks of Lindemann theory - Hinselwood modification, RRK theory, Slater’s treatment, RRKM theory.
Unit 3 Reactions in solution 10 Marks Effect of dielectric constant on reaction rate in solution, effect of pressure on rate, cage reactions, cluster reactions, electron transfer reactions in solution, linear free energy relationship, Hammett equation, Taft equation - their applications.
Unit 4 Photochemical reactions 10 Marks Photophysical properties of electronically excited molecules - radiationless transitions - IC and ISC, fluorescence and phosphorescence. Photophysical kinetics - state energy diagrams. Delayed fluorescence - the mechanism and kinetics of fluorescence quenching - Stern-Volmer equation, concentration dependence of quenching & excimer formation, quenching by added substances. Photodissociation, stratospheric chemistry, ozone layer depletion, photochemical smog. Unit 5 Chemical kinetics in the elucidation of reaction mechanism 10 Marks Organic reactions: ammonium cyanate - urea conversion - hydrolysis of lactones, aldol condensation and the cleavage of diacetone alcohol, nitration of aromatic hydrocarbons. Inorganic reactions: Thermal decomposition of nitrogen pentoxide - ligand replacement reactions of octahedral complexes, electron transfer reactions.
Part B: Electrochemistry (30 Marks) Unit 6 Theories of electrical interface 10 Marks Electrocapillary phenomena - Lippmann equation. Electron transfer at interfaces - polarisable and nonpolarisable interfaces, Butler-Volmer equation, Tafel Plots.
Unit 7 Electrochemical methods used in electrode kinetics 10 Marks Polarography - rotating disc electrode (RDE) - chronopotentiometric method, elucidation of mechanism of multistep electrode reactions. Electrodeposition on metals, convective diffusion - applications in electrode processes.
Unit 8 Electrocatalysis and redox reactions 10 Marks Electrochemical energy storage - primary and secondary fuel cells. Corrosion - kinetics, mechanism and prevention.
Internal Assessment 20 Marks
Physical Special Paper II POLYMER CHEMISTRY Total Marks: 100
Unit 1 Classification, molecular weights and size of polymers 16 Marks
Natural and synthetic polymers, plastics, fibres and elastomers. Step-reaction polymerization: Chemistry and kinetics. Carother’s equation, control of molecular weight, reactivity of larger molecules. Interchange reactions. Typical condensation polymerization processes, ring-scission polymerization. Determinations based on colligative properties measurements, ultracentrifugation, light scattering, solution viscometry and end group analysis. Molecular weight distribution, fractionation of polymers, size exclusion chromatography.
Unit 2 Thermodynamics of polymer solutions 16 Marks
Basic principles, entropy-heat and free energy of mixing - solubility parameter. Liquid lattice theory - Flory-Huggins model. Configuration of polymer chains in solution, statistical distribution for average dimensions. Expansion factor, excluded volume effect and theta-temperature. Hydrodynamic volume and solution viscosity. Viscoeleasticity - Newton, Maxwell and Voigt-Kelvin models of viscoeleastic behaviour. Stress-strain relations, Boltzmann principle. Stress relaxation, time temperature, superposition principle.
Unit 3 Free radical polymerization 16 Marks
Chemistry and steady-state kinetics. Chain transfer - Mayo equation, chain transfer constants. Inhibition and retardation - kinetics and mechanism, allylic inhibition. Mean lifetime of active center, absolute values for individual rate constants.
Unit 4 Copolymerisation 16 Marks
Types of copolymers, copolymer equation. Monomer reactivity rates - determination of structural effects. Alfrey Price Q-e scheme. Kinetics of binary polymerization. Non-radical chain polymerization: cationic and anionic polymerization - chemistry, kinetics and degree of polymerization. Coordination polymerization - Ziegler-Natta catalysts and stereospecific polymerization. Unit 5 Commercial polymers 16 Marks
Linear and branched polyethene, polypropylene, polystyrene, polyvinyl chloride, polyacrylonitrile. Natural polymers: Native and regenerated cellulose, starch. Inorganic polymers: Phosphorous polymers - polyphosphazenes. Silicones - polysiloxanes, polysilanes.
Internal Assessment 20 Marks
Physical Special Paper III HETEROGENEOUS CATALYSIS Total Marks: 100
Unit 1 Heterogeneous catalysis and kinetics of heterogeneous catalysis 16 Marks
Adsorption of molecules on solid surfaces, adsorption isotherms, surface area determination from adsorption isotherms and point B methods, porosity determination by volumetric and gravimetric methods, porosity determination by mercury porosimeter method. Chemisorption on metals, semiconducting oxides and insulator oxides. Adsorbed states molecules on metals, potential energy curves.
Kinetics of heterogeneous catalysis, effect of temperature on rates of catalysed reactions, Langmuir Hinselwood and Eley Redial models. Mass transport limitation of catalysed reactions. Surface dependence of reaction rates, volcano principle.
Unit 2 Preparation and characterization of industrial catalysts 16 Marks
What makes a good catalyst? Catalyst design methods, catalyst support and preparation of industrial catalyst, supported and unsupported metal catalysts, bimetallic catalysts.
Electron microscopy, XPS and PES, ESCA, IR and magnetic resonance spectroscopy, temperature programmed desorption (TPD), and DTA and TGA.
Unit 3 Zeolites and Clays 16 Marks
Zeolites (natural and synthetic) - shape selectivity properties - solid acids, acidity of zeolites and clays. Mesoporous materials, poorly crystalline silicates and aluminosilicates - MCM-41 type materials.
Applications of zeolites and clays as heterogeneous catalysts in cracking, reforming and olefin reaction. Zeolites as catalyst supports.
Unit 4 Catalysis in energy conversion, hydrocarbon and petroleum industry 16 Marks
Hydrodesulphurization, synthetic gas and production of chemicals from it. Bifunctional catalysts.
Nonselective and selective oxidation of hydrocarbon compounds. Manufacture and transformation of hydrocarbons - hydrogenation and isomerization. Production of margarine, edible oils and fine chemicals.
Unit 5 Catalytic Reactors, Environmental Catalysts 16 Marks
Catalytic reactors, catalytic deactivation and reactivation, control of pollution from automobile exhaust, catalytic converters. Abatement of nitrogen oxides and odours, cleaning of industrial effluents.
Internal Assessment 20 Marks Physical Special Paper IV Lab Course (Advanced Physical Chemistry Practical) Total Marks: 150
[The students will perform at least 15 experiments. The examination will be of 18 hrs duration with one experiment from each unit.]
Unit 1 Conductometry, Potentiometry and Polarography
1. Study the variation of solubility of potassium hydrogen tartrate (or any such sparingly soluble salt)/Ca(IO3)2 with ionic strength using solution of KCl at room temperature conductometrically. Hence determine the ionic activity coefficient. 2. Determine the amount of each component of the following ternary mixture by conductometric titration. (i) Hydrochloric acid, acetic acid and copper sulphate (ii) Hydrochloric acid, sodium chloride and ammonium chloride 3. Determine the basicity of a polybasic acid by potentiometric titration using NaOH solution and find out the dissociation constant. 4. Study the thermodynamics of a Galvanic cell and determine G, S and H of a suitable reaction. 5. Determine the transport number of Ag+ and NO3- ions (or H+ in HCl) by measuring emf of concentration cells with or without transference. 6. Determine the instability constant of silver-ammonia complex and the stoichiometry of the complex potentiometrically. 7. Determine the half-wave potential of cadmium(II) ion in 1M potassium chloride solution and estimate the amount of cadmium ion in an unknown solution containing 1M KCl. 8. Determine the composition and stability constant of a metal complex like copper glycine/lead oxalate. Unit 2 Spectrophotometry, Computational Analysis
1. Determine the composition of iron-thiocyanate complex spectrophotometrically and hence find the stability constant of the complex at ionic strength of 1M. 2. Study the kinetics of the reduction of methyl orange with stannous chloride catalyzed by Cl- ion spectrophotometrically under the following conditions: (i) reaction pseudo first order with respect to methyl orange, (ii) dependence of rate on Sn2+ ion concentration, (iii) dependence of rate on Cl- concentration. 3. Determine spectrophotometrically the indicator constant of an indicator, (e.g. methyl red). 4. Determine the composition of Cu(II) and Fe(III) in a mixed solution by spectrophotometric titration using EDTA. 5. Rotational probability distribution for HCl at two different temperatures, comparison of its rotational partition function by direct calculations and by the simple formula q = T/θrot. 6. (a) Drawing a moderately complex molecule (e.g. aniline/pyridine/furan/ethylene diamine using PC Model, and obtaining its nuclear framework Z‑matrix in usual MOPAC form. (b) Conversion of this Z-matrix to Cartesian coordinate form using MOPAC. 7. Plots for Maxwell’s speed distribution formula in speed and translational energy form, and calculation of the fraction of molecules in a given speed range by numerical integration. 8. Justification of Job’s method of continuous variation for determination of the formula of a complex using the ferric-thiocyanate complex example. 9. Iterative evaluation of the Wein’s displacement law constant b for a Black Body.
Unit 3 Miscellaneous Experiments 1. Study the ternary system of acetic acid-chloroform-water at room temperature and construct the phase diagram. 2. Determine the apparent molar mass of a non-volatile solute like benzoic acid in benzene and find its degree of association by cryoscopic method. 3. Study the following equilibrium : I2 + I– = I3–, and determine the value of the equilibrium constant of the reaction by distribution method. 4. Compare the cleansing power of different samples (at least four) of soaps and detergents by surface tension measurement. 5. Determine the transport number of Ag+ and NO3–, or Cu2+ and SO42– ions by Hittorf’s method. Or determine the transport numbers of H+ and Cl– ions in HCl by the moving boundary method. 6. Study the kinetics of decomposition of benzene diazonium chloride, determine the rate constant of the reaction at different temperatures and hence determine the activation energy of the reaction. 7. Study the salt effect and the solvent effect on the rate law of alkaline hydrolysis of crystal violet. 8. Determine the percentage of polymerization of MMA or styrene initiated by AIBN at 60oC by dilatometric method. 9. Study the decomposition kinetics of oxalic acid in solution photosensitized by uranyl sulphate.
Marks distribution in the Examination:
(i) Three Experiments: 100 Marks (ii) Viva voce: 20 Marks (iii) Internal Assessment: 30 Marks
Students can opt for Project work in lieu of Advanced Physical Chemistry Practical on an assigned topic under the supervision of a faculty member. The student will be required to submit 3 copies of a dissertation giving the results of the Project work and make an oral presentation.
Physical Special Paper V Literature Review Total Marks: 50
All the students are required to prepare a Literature Review on an assigned topic under the supervision of a faculty member (50 Marks).
Semester IV · Organic Chemistry Special Group
Organic Special Paper I NATURAL PRODUCTS CHEMISTRY Total Marks: 100
Unit 1: Chemistry of Carbohydrates 16 Marks Classification of carbohydrates. Monosaccharides – D- & L- series, acyclic and ring structure of ketoses and aldoses and their configurational representation; anomerization, epimerization and mutarotation, anomeric effect; reactions with periodic acid, lead tetraacetate, and phenylhydrazine; methods of ascending and descending the sugar series; conversion of aldose to ketose and vice versa.
Dissaccharides – Ring structure of sucrose, maltose, lactose and their hydrolysis. Polysaccharides – Representative structure of starch, glycogen and cellulose. Introduction to deoxysugars, glycosides, glycals, glycosamines and glycosans.
Unit 2: Chemistry of Terpenoids 16 Marks Occurrence and classification; isoprene rule, general methods of structure determination; chemistry including syntheses of the following compounds – caryophyllene, a-santonin, abietic acid, giberellic acid, longifolene; biogenetic pathway of mono- and sesquiterpenes.
Introduction and general reactions; introduction to cholesterol, ergosterol, vitamin D1 and D2; introduction to sex hormones.
Unit 3: Chemistry of alkaloids 16 marks General methods of extraction and structure determination; chemistry including total chiral syntheses of reserpine and morphine.
Unit 4: Chemistry of vitamins 16 Marks Carotenoids – classification, chemistry of b–carotene, lycopene and canthaxanthin. Synthesis of b–carotene, provitamin A, singlet oxygen quenching and food coloring properties of carotenes.
Classification and functional role in biological systems; chemistry of thiamine, riboflavin, retinol, tocopherols, vitamin C and pyridoxine.
Unit 7: Chemistry of porphyrins 16 marks
Porphyrin ring and chemistry of heme; oxygen transport by haemoglobin; chemistry of chlorophyll and its role in photosynthesis.
Internal Assessment 20 Marks
Organic Special Paper II ORGANIC SYNTHESIS Total Marks: 100 Unit 1 Organic Photochemistry 16 Marks
Photochemistry of carbonyl compounds – representation of the excited states of ketones, photolysis of saturated and b, g-unsaturated ketones. Photoreduction of saturated, arylalkyl and a,b-unsaturated ketones and p-benzoquinone; Patterno-Buchi reaction, [2+2]-cycloaddition, reactions of singlet oxygen- photooxidation, ene reaction, synthetic applications of singlet oxygen.
Olefinic photochemistry – photostereomutation of cis-trans isomers, optical pumping, [2+2]cycloadition. Photochemistry of conjugated polyenes – cycloaddition and dimerization of 1,2-butadiene, photochemistry of vision. Photorearrangements – di-p-methane rearrangement, Photo-Fries rearrangement and photorearrangement of cyclohexadienones, Barton rearrangement.
Unit 2 Formation of carbon-carbon single bonds 16 Marks
Alkylation – importance of enolate anions, alkylation of activated methylene groups, dianion in synthesis, alkylation of ketones, enamine and related reactions; alkylation of thio- and seleno-carbanions; allylic alkylation of alkenes, Michael addition(conjugate addition).
Aldol reaction – use of boron and silyl enolates; directed aldol reaction. Synthetic applications of carbene and carbenoids; formation of carbon-carbon bond by adition of free radicals to alkenes; photocyclization reactions.
Unit 3 Formation of carbon-carbon double bond 16 marks
Elimination reactions - acid catalysed dehydration of alcoholls, solvolytic and base-induced elimination from alkyl halides & sulphones, Hofmann elimination from quaternary ammonium salts.
Pyrolytic syn elimination – pyrolyses of carboxylic esters and xanthates (Chugaev reaction) and amine oxides (Cope reaction).
Wittig and related reactions – use of stabilized and unstabilized phosphorus ylides, Peterson reaction.
Alkenes from sulphones, decarboxylation of lactones, stereoselective synthesis of tri- and tetra-substituted alkenes.
Unit 4 Pericyclic reactions 16 Marks
Classification of pericyclic reactions, theories of pericyclic reactions – FMO, orbital symmetry correlation method, orbital coefficients, PMO method. Cycloaddition reactions – [2+2], [4+2], [6+2] cycloadditions; [3+2] & [4+3] dipolar cycloaditions; stereoselectivity of the reactions.
Sigmatropic rearrangement – [m+n] sigmatropic rearrangements of hydrogen and chiral alkyl group; divinylcyclopropane rearrangements; fluxional molecules; stereoselectivity in Cope and Claisen rearrangement.
Electrocyclic reactions and cyclo reversions – stereoselectivity of the reactions. Cheletropic reactions – linear and nonlinear cheletropic rearrangement; theories of cheletropic reactions, stereoselectivity of the reactions.
The ene reactions – ene reactions of 1,7-dienes, carbonyl enophiles; simple problems.
Unit 5 8 + 8 Marks
a) Synthetic application of Organometallics and activation of C–H bonds
Preparation, stability. reactivity and synthetic applications of organo-lithium, tin, copper, zinc and palladium reagents.
Hofmann-Loeffler-Freytag reactions, cyclisation reactions of nitrenes, Barton reaction and related processes, photolysis of hypohalides, reactions of monohydric alcohols with lead tetraacetate.
b) Designing Organic Synthesis
Retrosynthesis – disconnection approach, synthons and synthetic equivalents; retrons and transform; umpolung; Functional Group Interconversions (FGI); Functional Group Protections – protection and deprotection of hydroxy, dihydroxy, carbonyl, carboxyl and amino groups; retrosynthesis of some simple compounds.
Internal Assessment 20 Marks
Organic Special Paper III BIOORGANIC AND MEDICINAL CHEMISTRY Total Marks: 100
Part A: Bioorganic Chemistry 4 x 10 = 40 Marks
Unit 1: Metabolism of Carbohydrates
Glycolysis and gluconeogenesis; fate of pyruvic acid and Krebs cycle; biosynthesis of fatty acids, triacylglycerols, phospholipids, chloresterol and related steroids; nucleic acids – DNA replication and RNA transcription; introduction to cloning.
Unit 2: Lipids
Biosynthesis of fatty acids, triacylglycerols, phospholipids, cholesterol and related steroids; prostaglandins.
Unit 3: Proteins
Aminoacids; primary, secondary, tertiary, and quaternary structure of proteins; biosynthesis of aminoacids, activation of aminoacids, tRNA, ribosomes, mRNA, mechanism of transcription and translation; sequencing of amino-acids in polypeptides.
Unit 4: Nucleic acids
Classification; nucleotides, their structures and functions; biosynthesis of nucleotides, DNA-replication and RNA-transcription.
Part B: Medicinal Chemistry 5 x 8 = 40 Marks
Unit 5: Introduction
Definition of drugs and factors affecting their bioactivity; definition chemotherapeutic index and therapeutic index; theoretical aspects of drug-receptor interaction, the two-state Model of Receptor Theory; QSAR, drug agonist and antagonist; pharmaco-kinetics and pharmacodynamics; mechanism of drug action.
Lead compound, molecular modification; elementary idea of molecular modelling of drug; introduction to combinatorial library of drugs.
Unit 6: Sulphadrugs
Historical significance of sulpha drugs as antibacterial agents; introduction to suphanilamide and other important sulpha drugs and their mode of action.
Unit 7: Antibiotics
Introduction and classification. b-Lactam antibiotics – Natural and semisynthetic penicillins, their structure-action relationship and chemical modification, penicillins sensitive and resitant to penicillinase; mode of action of b–lactam antibiotics.
Unit 8: Aminoglycoside antibiotics Streptomycin, gentamycin, kanamycin, neomycin and their mode of action.
Unit 9: Tetracyclines Structure-action relationship and therapeutic uses.
Unit 10: Chloramphenicol Synthesis and characterization, mode of action. Introduction to macrolide and peptide antibiotics.
Unit 11: Antimalarials Classification of humane malaria and plasmodia responsible for them, life cycle of plasmodia; quinine, chloroquine, trimethoprim, mefloquin-their structure and activity as antimalarial; artemisinin and its derivatives, structure-action relationship;
Unit 12: Drugs for the treatment of cancer, tuberculosis and AIDS Drugs used for treatment of cancer, tuberculosis and AIDS, and recent developments; anti-viral agents; introduction to gene therapy.
Internal Assessment 20 Marks
Organic Special Paper IV Lab Course (Advanced Organic Chemistry Practical) Total Marks: 150 Examination Time: 18 hrs
A. Three-step preparation: spectroscopic identification of intermediates and final products should be emphasized 45 Marks 1. 1,3,5-Tribromobenzene from nitrobenzene via aniline and 2,4,6-tribromoaniline. 2. m-Nitrophenol from nitrobenzene via m-dinitrobenzene and m-nitroaniline. 3. Benzidine from nitrobenzene via azobenzene and hydrazobenzene. 4. Acridone from anthranilic acid via o-chlorobenzoic acid and N-phenylbenzoic acid. 5. Benzanilide from benzene via benzophenone and benzophenone oxime. 6. Pivalic acid from acetone via pinacol and pinacone. 7. Tritylchloride from bromobenzene via phenylmagnesiumbromide and triphenyl carbinol. 8. Anthranilic acid from phthalic acid via phthalic anhydride and phthalimide. 9. 2,4-Dinitrophenylhydrazine from aniline via chlorobenzene and 2,4- dinitrochlorobenzene 10. Phenyl-p-totylthiourea from aniline via thiocarbanilide and phenylisothiocyanate.
B. Estimation 30 Marks 1. Number of hydroxy groups in an organic compound by acetylation method. 2. Estimation of formaldehyde by iodometry. 3. Equivalent weight of carboxylic acids by (a) volumetric and (b) gravimetric (Ag-salt) method. 4. Percentage purity of carbonyl compounds by gravimetric method (with DNP). 5. Nitro group by reduction with titanous salts. 6. Unsaturated compounds by bromination method. 7. Iodine value, saponification value, and RM value of fats. 8. Molecular weight determination of organic compounds by Rast’s camphor method. 9. Estimation of azobenzene by UV-Visible spectroscopy.
C. Separation and identification (by comparison of Rf value) of organic compounds in a ternary mixture by (a) Paper chromatography, (b) Thin layer chromatography and (c) Column chromatography. 25 Marks D Viva-voce 20 Marks E. Internal Assessment 30 Marks Students can opt for Project work in lieu of Advanced Organic Chemistry Practical on an assigned topic under the supervision of a faculty member. The student will be required to submit 3 copies of a dissertation giving the results of the Project work and make an oral presentation.
Organic Special Paper V Literature Review Total Marks: 50
All the students are required to prepare a Literature Review on an assigned topic under the supervision of a faculty member (50 Marks).
Semester IV · Inorganic Chemistry Special Group
Inorganic Special Paper I :: Transition Metals and Inorganic Materials Total Marks: 100 Unit 1 Applications of group theory 16 MarksRepresentation of symmetry operators by matrices, representation of groups - reducible and irreducible representations, the Great orthogonality theorem and properties of irreducible representations, Character tables Mulliken notations.Transformation properties of atomic orbitals, the Direct Product, construction of Hybrid orbitals for ABn molecules, construction of symmetry adapted linear combinations (SALCs) and MOs of simple ABn molecules. Selection rules for electronic and vibrational spectroscopy.
Unit 2 Ligand Field Theory 16 MarksThe d wave functions (orbitals), Crystal field potential, Symmetry aspects of d orbital splitting by ligands. Electron repulsion in many electron atoms, Free ion terms for dn configurations, Electron repulsion parameters, spin –orbit coupling, Effect of weak crystal field on Oh symmetry on the S,P,D, and F terms, Free ions in strong crystal fields. Term energy level diagram for dn configurations in Oh and Td symmetries, Tanabe-Sugano diagrams.Influence of the d-configuration on the geometry and stability of complexes. MO theory of complex compounds, LGO and MOs of ML6 and tetrahedral complexes.Unit 3 Electronic spectra 16 Marks La Porte Selection Rules, Effect of vibronic coupling and spin-orbit coupling, band intensities and band widths, Jahn Teller effect. Spectra of aqueous solutions of M(H2O)6+, Spectra of high-spin and low-spin ML6n+ complexes, Calculation of 10Dq and values from spectra, distorted octahedral and tetrahedral complexes, M-L and L-M charge transfer complexes.
Unit 4 Magnetic properties of transition metal ion 16 MarksMagnetic properties of free ions, spin-only magnetic moments of dn ions in weak and strong crystal fields of Oh and Td symmetries, orbital contribution and the effect of spin-orbit coupling, quenching of orbital angular momenta by crystal fields, temperature independent paramagnetism, high-spin low-spin equilibria, Ferromagnetism and antiferromagnetism with examples from metal complexes, Magnetic properties of second and third transition series and the lanthanide elements. Measurement of magnetic susceptibility.
Unit 5 Inorganic Materials 16 Marks Magnetic exchange and exchange coupling phenomena, magnetic materials, molecular magnets, ferrofluids. Crystalline, liquid crystalline and amorphous materials, non-stoichiometric oxides, crystal defects, nano materials. Band theory of metals, semiconductors, p and n type semi conductor. Defect perovskites, high Tc superconductivity in cuprates, preparation and characterization of 1-2-3 materials, application of high Tc materials. Thermoelectric properties – dielectric, ferroelectric, piezo electric materials, solid electrolytes and Fuel cells.
Internal Assessment 20 Marks Inorganic Special Paper II ORGANOMETALLICS AND PHOTOINORGANIC CHEMISTRY Total Marks: 100
Unit 1 Nature of metal-carbon bonds in transition metal compounds 16 Marks
Classification of organometallic compounds, C–H s bond in metal alkyls, b-hydrogen elimination. Complexes with metal-carbon bonds – with olefins, acetylenes, allylic groups and dienes – electronic structure and bonding. Bonding in metal carbocyclic systems – cyclopentadienyl and other carbocyclic ligands, MO treatment of bonding in ferrocene based on symmetry properties of the ligand and metal orbitals. Bonding in carbene and carbyne complexes.
Unit 2 Synthesis, structure and properties of organometallic complexes 16 marks
Olefin complexes, acetylene complexes, complexes formed by polyenes and allylic compounds – synthesis and relevance. Cyclopentadiene and arene metal complexes – general reactions. Transition metal alkyls and ylides complexes, metal carbene and metal carbyne complexes – synthesis and reactivity.
Synthesis of metal carbonyls and metal carbonyl hydrides – reactions and synthetic utilities. High nuclearity carbonyl clusters, structures, electron counting schemes and bonding – Wade’s rules (isolobal analogy).
Unit 3 Fundamental reactions of organotransition metal complexes 16 marks
Ligand co-ordination and dissociation – displacement reaction in square planar complexes, steric and electronic influences of ligands. Oxidative addition and reductive elimination. Insertion reactions – insertion of CO, alkenes. Reactions of co-ordinated ligands – reactions of co-ordinated olefins, acetylenes and arenes.
Unit 4 Organometallics in catalysis 16 Marks
Homogeneous and heterogeneous catalysis. Polymerization and oligomerization of olefins and dienes. Hydrogenation, hydroformylation, isomerization, metathesis and carboxylation of olefins. Synthesis of acetic acid from methanol, reactions of synthesis gas. Oxidation of olefins by Wacker process, synthesis of acrylates, olefin epoxidation. C–H bond activation – hydroxylation and autoxidation – basic ideas. Allylic oxidations.
Unit 5 Photoinorganic chemistry 16 Marks
Ligand field and charge transfer states (Thexi and DOSENCO states), Energy dissipation by radiative and non radiative processes, Jablonski diagram. Photosubstitution on Cr(III) and Co(II) compounds, cis-trans isomerisation, metal carbonyls. Photoredox reactions of Co(III) complexes, Photo catalysis and solar energy conservation by Ru(bpy)32+.
Internal Assessment 20 Marks
Inorganic Special Paper III BIOINORGANIC CHEMISTRY Total Marks: 100
Unit 1 Supramolecular Chemistry and Ion Transport 16 Marks
Definition and examples of Supramolecules, Self assembly and membranes, Molecular receptors-Cryptands, Valinomycine, Spherands, Molecular recognition, Interaction of metal ions and metal complexes with DNA.
Supramolecular Transport : Active transport of ions across cell membranes, Selectivity of Na and K with crown ethers, cryptands and Ionophores, Na/K pump; Transport of Ca2+ , Bio-minerals containing Ca and Fe; Transport and Storage of Iron ; Transferrins, Sideraphores, and Ferritin.
Unit 2 Carrier, Transport, Storage and Activation of Dioxygen 16 Marks
Active site structure and function of oxygen carrying proteins: Metalothionins and Ceruloplasmin. Haemoglobin, Myoglobin, Haemerythrin, and Haemocyanine; O2 binding equilibria and mechanism of cooperativity in Hemoglobin, Design of Model O2 carriers, Reaction leading to toxicity due to dioxygen.
Oxidases and Oxygenase : Catalase, Peroxidase, Superoxide Dismutase, Cytochrome C Oxidase, Cytochrome P-450, and Pyrocatechol Dioxygenase – their biological functions, role of metal, and dioxygen reactivity.
Unit 3 Metalloenzymes 16 Marks
Structure and function of Carboxypeptidase A and carbonic anhydrase. Importance of Co(II) substitution in Zn proteins ; Structure and function of co-enzyme B12. Role of Ni, Cr and V in enzymes; Molybdenum enzymes, structure and function of Nitrogenase, chemistry of dinitrogen fixation, Xanthine oxidases. Unit 4 Electron transfer proteins 16 Marks
Metalloproteins in the electron transfer chains in membrane, The Cytochromes (a, b, c types), Mechanism of electron transfer reactions in proteins; Iron Sulfur proteins – Rubredoxin, Ferredoxin, and HiPIP
Unit 5 Metals in medicine 16 Marks
Metal deficiency and disease, toxic effect of metals – Fe and Cu overload, Thalassemia, toxicity due to Hg, As, Cd, and Pd; Chelation therapy (EDTA, BAL, Penicillamine); Gold compounds in Rh. Arthritis, Cisplatin and related Anticancer Drugs. Internal Assessment 20 Marks
Inorganic Special Paper IV Lab Course (Advanced Inorganic Chemistry Practical) Total Marks: 150 Examination Time: 18 hrsA. Chromatography 20 MarksSeparation of cations and anions by(a) Paper chromatography (b) Column chromatography - ion exchange
B. Preparation and characterization 40 MarksPreparation of selected inorganic compounds and their physico-chemical characterization by elemental analysis, IR and electronic spectrophotometry, magnetic susceptibility measurements, magnetic resonance spectroscopy, solution conductivity measurements as well as cyclic voltammetric measurements, powder XRD measurements wherever appropriate and possible. Handling of air and moisture sensitive compounds.
1. M(acac)3, M = Mn, Co 2. Prussian Blue, Turnbull’s Blue 3. Co(en)2Cl2, Co(en)2(NO2)2 and study of their isomerization by electronic spectroscopy 4. [Fe(phen)3](ClO4)2
C. Other Experiments 40 Marks(a) Preparation of an optically active Co(III) complex and its optical activity measurement. [Ref.: H.R. Hunt, Jr., J. Chem. Educ., 54 (1977) 711.] (b) Preparation of the fac and mer isomers of Co(NH3)3(NO2)3. [Ref.: M. Laing, J. Chem. Educ., 62 (1985) 707] (c) Determination of composition of and Fe-SCN complex by Job’s method of continuous variation. [Ref.: W.R. Carmody, J. Chem. Educ., 41 (1964) 615.] (d) A preparation in a nonaqueous medium (e) A preparation of solid state compounds at high temperature
D Viva-voce 20 Marks
E. Internal Assessment 30 Marks
Students can opt for Project work in lieu of Advanced Organic Chemistry Practical on an assigned topic under the supervision of a faculty member. The student will be required to submit 3 copies of a dissertation giving the results of the Project work and make an oral presentation.
Inorganic Special Paper V Literature Review Total Marks: 50
All the students are required to prepare a Literature Review on an assigned topic under the supervision of a faculty member (50 Marks).
Recommended Books and References
A. Physical Chemistry
1. Physical Chemistry, PW Atkins (OUP-ELBS) 2. Physical Chemistry, IN Levine (McGraw Hill) 3. Physical Chemistry, GW Castellan (Narosa) 4. Textbook of Physical Chemistry A W Adams 5. Quantum Chemistry, I N Levine 6. Elementary Quantum Chemistry, F I Pilar 7. Introductory Quantum Chemistry, A K Chandra 8. Coulson’s valence, R McWeeny 9. Valiancy Theory, Murrel, Kettle and Teddler 10. Molecular Quantum Mechanics, Atkins 11. Quantum Chemistry, Mcquarrie 12. Heat and Thermodynamics, Zemansky 13. Statistical Thermodynamics, MC Gupta (New Age International) 14. Modern Electrochemistry, Bokris and Reddy, Vols. 1 & 2 (Butterworth) 15. Chemical Kinetics, KJ Laidler 16. Reaction Kinetics, Pilling and Seakins (OUP) 17. Text Book of Polymer Science, FW Billmeyer 18. Polymer Science, Gowarikar, Viswanathan and Sreedhar 19. Principles of the Solid State, HV Keer 20. Physical Chemistry through Problems, Dogra and Dogra 21. Thermodynamics, Randall, Pitzer and Brewer 22. Chemical Thermodynamics, EN Yeremin 23. Non-Equilibrium Thermodynamics, DD Fitts 24. Homogeneous Catalysis, Parshall and Ittel (Wiley) 25. Heterogeneous Catalysis, Principles & Applications , G C Bond 26. Introduction to the principles of Heterogeneous catalysis, Thomas and Thomas 27. Catalysis by metals, G C Bond 28. New methods of catalyst preparation and characterization, G C Bond and P A Germer 29. Catalysis, J C Kuriakose 30. Heterogeneous catalysis, D K Chakrabarty 31. Catalysis: Science and Technology, J R Anderson and M Boudart 32. Principles of Biochemistry, A Lehninger 33. Outlines of Biochemistry, Cohn and Stumpf 34. Rates and Mechanism of Chemical Reactions, Gardiner WG (WA Benjamin Inc.) 35. Kinetics and Mechanism, Frost AA and Pearson RG (Wiley Eastern) 36. Kinetics and Mechanism of Chemical Transformations, Kuriacose R (McMillan, India) 37. Fundamentals of Photochemistry, Rohatgi-Mukherji (Wiley Eastern) 38. Photochemistry, Lalverts and Pitts. 39. Principles of Electrochemistry, Koryto J and Dvorak. 40. Principles of Polymer Chemistry, Flory PJ. 41. Textbook of Polymer Science, Billimeyer FW. 42. Physical Chemistry of Macromolecules, Tanford C. 43. Inorganic Polymers, Stone and Graham. 44. Introduction to Polymers, Young RJ. 45. Physical Chemistry of Polymers, Tagger A.
B. Organic Chemistry
1. Organic Synthesis by Michael B. Smith, Mc Graw-Hill International Edition 2. Advanced Organic Chemistry by Jerry March, Wiley Eastern Ltd 3. Organic Reactions and their Mechanisms by P. S. Kalsi, New Age International 4. Reaction Mechanism by Peter Syke 5. Chemical Hardness by R. G. Pearson, Wiley-VCH 6. Stereochemistry of Organic Compounds by Eliel & Wilen, John Wiley & Sons 7. Stereochemistry of Organic Compounds: Principles and Applications by Nasipuri, John Wiley & Sons 8. Organic Chemistry by Pine, McGraw Hill International Edition 9. Lehniger Principles of Biochemistry by David L. Nelson & Michael M. Cox, Macmillan Worth Publishers 10. Biological Chemistry by Mahler & Cordes, Harper International 11. Fundamentals of Biochemistry by A.C. Dev, New Central Book Agency(P) Ltd 12. Enzymatic Reaction Mechanisms by C. Walsh, W. H. Freeman & Company 13. Some Modern Methods of Organic Synthesis by Carruthers, Cambridge Univ. Press 14. Molecular Orbitals by Lehr & Merchand 15. Importance of Antibonding Molecular Orbitals by Jaffe & Orchin 16. Organic Spectroscopy by William Kemp by ELBS 17. Spectroscopic methods in org. chemistry by Williams & Fleming, McGraw-Hill Book 18. Spectroscopic Identification of org. Compounds by Silverstein, Bassler & Morril, John Wiley & Sons 19. Mass Spectrometry by Reg Davis & martin Frearson, John Wiley & Sons 20. Organic Chemistry by I. L. Finar, Longman Group Ltd. 21. Introduction to Medicinal Chemistry by Alex Gringauz, Wiley-VCH 22. Medicinal Chemistry-An Introduction by Gareth Thomas, John Wiley & Sons 23. Organometallic Chemistry by Mehrotra & Singh, Wiley Eastern Ltd. 24. Principles of Organometallic Chemistry by P. Powel, Chapman & Hall 25. Designing organic Synthesis: A Programmed Introduction to Synthon Approach by Stuard Warren, John Wiley & Sons 26. The Logic of Chemical Synthesis by Corey & Cheng, John & Wiley & Sons 27. Classics in Total Synthesis: Targets, Strategies and methods by Nicolaou & Sorensen 28. New Horizons of Organic Synthesis by Nair & Kumar, New Age International 29. Organic Chemistry by Gilman (four volumes) 30. Natural Products by Nakanishi 31. Terpenoids – series of three volumes by Simonsen, Mayo & Pindar respectively 32. Alkaloids – two volumes by Dalton & Boutley respectively 33. Heterocyclic Chemistry: Synthesis, Reactions & Mechanisms by R. K. Bansal, Wiley Eastern Ltd. 34. Organic Chemistry by P. Y. Bruice, Prentice-Hall International 35. Organic Chemistry by R. V. Hoffman, Oxford University Press 36. Organic Chemistry by Sundberg 37. Organic Chemistry by Norman
C. Inorganic Chemistry
1. Advanced Inorganic Chemistry by Cotton, Wilkinson, Murillo and Bochmann 2. Inorganic Chemistry by DF Shriver, PW Atkins and CH Langford 3. Inorganic Chemistry: Principles of Structure and Reactivity by Huheey, Keiter and Keiter 4. Theoretical Inorganic Chemistry by MC Day and J Selbin 5. Chemical Applications of Group Theory by FA Cotton 6. Structural Inorganic Chemistry, A.F. Wells, Oxford Science Publishers 7. Chemistry of the Elements, Greenwood and Earnshaw 8. Modern Inorganic Chemistry, W.L. Jolly, McGraw Hill 9. A New Concise Inorganic Chemistry, J.D. Lee, Van Nostrand 10. Introduction to Ligand Fields by BN Figgis 11. Multiple Bonds Between Metal Atoms by FA Cotton and RA Walton 12. Comprehensive Coordination Chemistry, Vol. I 13. Magnetochemistry by RL Carlin 14. Physical Inorganic Chemistry, S.F.A. Kettle 15. C.N.R. Rao and J. Gopalakrishnan, New Directions in Solid State Chemistry, CUP 16. A.R. West, Solid State Chemistry and Its Applications, John Wiley & Sons 17. L.V. Interrante and M.J. Hamden-Smith, Chemistry of Advanced Materials: An Overview. 18. D.K. Chakrabarty, Introduction to Solid State Chemistry, Wiley Eastern Limited 19. R. Hoffmann, Solids and Surfaces: A Chemist’s View of Bonding in Extended Structures 20. D.W. Bruce and D. O’Hare, Inorganic Materials, John Wiley & Sons 21. Bertini, Gray, Lippard and Valentine (Eds.), Bioinorganic Chemistry 22. S.J. Lippard and J.M. Berg, Principles of Bioinorganic Chemistry 23. Progress in Inorganic Chemistry, Lippard (Ed.), Volumes 18 & 38, John Wiley & Sons 24. J.M. Lehn, Supramolecular Chemistry, VCH 25. J.L. Atwood, Textbook of Supramolecular Chemistry 26. Special Issue on Inorganic Photochemistry, J. Chem. Educ., Vol. 60, No. 10, 1983. 27. Adamson and Fleischauer, Concepts of Inorganic Photochemistry, John Wiley & Sons 28. Progress in Inorganic Chemistry, Vol. 30 29. Comprehensive Coordination Chemistry, Vol. 1 30. V. Balzan and V. Carassiti, Photochemistry of Coordination Compounds, Academic Press 31. G.J. Ferraudi, Elements of Inorganic Photochemistry, John Wiley & Sons.
D. Computers in Chemistry
1. K.V. Raman, Computers in Chemistry, Tata McGraw Hill 2. T.R. Dickson, The Computers and Chemistry, W.H. Freeman 3. P. Lykos, Personal Computers in Chemistry, John Wiley and Sons
E. Biochemistry
1. A.L. Lehninger, Principles of Biochemistry 2. L. Freeman, Biochemistry, W.H. Freeman 3. E.E. Conn and P.K. Stumpf, Outlines of Biochemistry 4. D.E. Metzler, Biochemistry: The Chemical Reactions of Living Cells, Academic Press 5. H. Dugas and C. Penny, Bioorganic Chemistry: A Chemical Approach to Enzyme Action 6. F.A. Cotton and G. Wilkinson, Advanced Inorganic Chemistry, John Wiley & Sons 7. J.E. Huheey, Inorganic Chemistry: Structure and Reactivity, Harper-Row 8. I. Bertini, H.B. Gray, S.J. Lippard and J.S. Valentine (Eds.), Bioinorganic Chemistry. 9. S.J. Lippard and J.M. Berg, Principles of Bioinorganic Chemistry 10. Progress in Inorganic Chemistry, S.J. Lippard (Ed.), Volumes 18 & 38 F. Environmental and Analytical chemistry
1. Environmental Chemistry, G W vanLoon and S J Duffy (OUP) 2. Environmental Chemistry, S.E. Manahan, Lewis Publishers 3. Environmental Chemistry, A.K. De 4. Environmental Chemistry, C. Baird, W.H. Freeman 5. Introduction to Environmental Analysis, Roger Reeve (Wiley) 6. Environmental Pollution Analysis, S.M. Khopkar 7. Standard Method of Chemical Analysis, F.J. Welcher, Volumes I and II 8. Environmental Toxicology, J. Rose (Ed.), Gordon and Breach Science Publishers 9. Elemental Analysis of Airborne Particles, Landsberger and Creatchman (Eds.), Gordon and Breach Science Publishers 10. Analytical Chemistry, G.D. Christian, John Wiley & Sons 11. Basic Concepts of Analytical Chemistry, S.M. Khopkar, New Age International 12. Principles of Instrumental Analysis, D.A. Skoog and J.L. Loary, W.B. Saunders 13. Quantitative Analysis, R.A. Day, Jr. and A.L. Underwood, Prentice Hall 14. Analytical Chemistry: Principles and Techniques, L.G. Hargis, Prentice Hall 15. Fundamentals of Analytical Chemistry, D.A. Skoog, D.M. West and F.J. Holler, W.B. Saunders Chemical Analysis, K.A. Rubinson, Harper Collins Pub
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