B.Sc Syllabus Chemistry PDF

DEPARTMENT OF CHEMISTRY UNIVERSITY OF ALLAHABAD ALLAHABAD B.Sc. Part - I, II, III Syllabus & Instruction Manual  Syllabus for B.Sc. I from 1999 & onwards There will be three theory papers of three hours duration each....

DEPARTMENT OF CHEMISTRY UNIVERSITY OF ALLAHABAD ALLAHABAD B.Sc. Part - I, II, III Syllabus & Instruction Manual  Syllabus for B.Sc. I from 1999 & onwards There will be three theory papers of three hours duration each. FIRST PAPER INORGANIC CHEMISTRY (M.M. 34) 1. ATOMIC AND NUCLEAR STRUCTURE (12) (a) Bohr’s and Sommefields’ Atomic Models, de Broglie equation, Heisenberg uncertainty principle. Schrodinger wave egucation, Radial and angular wave function, Physical significance and characteristics of a wave function, shapes of s, p, d and f-orbitals. Aufbau principle and electronic configuration of atoms. Periodic classification of elements (IUPAC recommendation), Long from the periodic table including translawrencium elements. (b) Structure of nucleus, fundamental particles, forces in the nucleus, nuclear stability-N/P ratio and binding energy, Packing fanction. 2. PROPERTIES OF THE ELEMENTS (12) Atomic, Covalent and Ionic radii, Ionization, potential, Electron affinity, Electronegativity including idea about group electronegativity and their variation in the Periodic table. Ionisation Potential, Lattic energy and hydration energy and their relation to solubility of ionic compounds. 3. CHEMICAL BONDIG (12) Ionic, covalent (polar and non-polar), coordinate bonds, sigma and pi-bonds, odd electron bonds, hydrogen bond, van der Waal’s forces and metallic bond. Covalent character in ionic bonds (Fajans’ rules), partial ionic character of a covalent bond. 4. CO-ORDINATION CHEMISTRY (10) Double salts and co-ordination compounds. Werner’s theory, Sidgwick’s concept of effective atomic number (EAN), IUPAC system of nomenclature of co-ordiantion compounds. Types and classification of ligands. 5. ELECTRODE POTENTIAL (10) Electrode potential and importance of electrochemical series. Electrode potential diagramme and its applications. 6. CHEMISTRY OF ZERO GROUP AND S-BLOCK ELEMENTS (12) (a) Isolation and separation of inert gases from air and compounds of inert gases. (b) Chemical reacitvity of alkali and alkaline earth metals and group trends. Uses of s-block elements and their compounds (Li, Na and K only), Organometallic compunds of Li, Na, K, Be and Mg. Polyether complexes (crown ether complexes) of alkali metals. 7. EXTRACTION OF ELEMENTS (14) General principles of extraction and purification of metals. Occurence and isolation of the elements, Extraction and isolation of Li, Be and Ra from their minerals. 8. PREPARATIONS, PROPERTIES AND USES OF : (8) (a) Heavy water, lithium tetrahydroaluminate, lithium stearate, basic beryllium acetate. (b) Structure and Bonding of : H2O2, Be (BH4)2, BeMe2, Anhydrous beryllium chloride, basic beryllium acetate, polymeric Ca (C5H5)2. 9. PRINCIPLES INVOLVED IN QUALITATIVE AND VOLUMETRIC ANALYSIS (10) (a) Chemical reactions in qualitative analysis of inorganic mixture and problems based on mixture analysis. (b) Applications of Co-ordination compounds in qualitative analysis. (c) General principles of volumetric analysis, Redox titrations, Equivalent weight, normality,, molarity and molality. Numericals based on volumetric analysis.  SECOND PAPER ORGANIC CHEMISTRY (M.M. 33) 1. STRUCTURE AND BONDING Hybridization bond lengths and bond angles, bond energy, localized and delocalized chemical bond, resonance, hyperconjugation, aromaticity, inductive and field effects, hydrogen bonding. 2. MECHANISM OF ORGANIC REACTIONS Curved arrow notation, drawing electron movements with arrows, half-headed and double- headed arrows, homolytic and heterolytic bond breaking. Types of reagents electrophiles and nucleophiles. Types of organic reactions, Energy consideration, Reactive intermediates : carbocations, carbanions, free radicals, carbenes, arynes and nitrenes (with examples). 3. STEREOCHEMISTRY OF ORGANIC COMPOUNDS Concept of isomerism. Types of isomerism. Optical isomerism : elements of symmetry, molecular chirality, enantionmers, stereogenic centre, optical activity, properties of enantiomers, chiral and achiral molecules with two stereogenic centers, diastereomers, threo and erythro diastereomers, meso compounds, resoletion of enantiomers, inversion, retention and racemization. Relative and absolute configuration, sequence rules, D & L and R & S system of nomenclature. ‘Geometrical Isomers’- Elementry idea of geometrical isomerism determination of configuation of geometrical isomers. E & Z system of nomenclature, geometical isomerism in oximes and alicyclic compounds. Conformational isomerism : Conformational analysis of ethane and n-butane, conformations of cyclohexane, axial and equatorial bonds, conformation of monosubstituted cyclohexane derivatives. Newman projection and Fischer formulae. Difference between configuration and conformation. 4. ALKANES AND CYCLOALKANES Methods of formation : (with special reference to Wurtz reaction, Kolbe reaction, Corey-House reaction and decarboxylation of carboxylic acids) and chemical reactions of alkanes. Mechanism of free radical halogenation of alkanes; orientation, reactivity and selectivity. Cycloalkanes: Methods of formation, chemical reactions, Baeyer’s strain theory and its limitations, Ring strain in small rings (Cyclopropane), theory of strainless rings. The case of cyclopropane ring: banana bonds. 5. ALKENES, DIENES AND ALKYNES Alkenes: Methods of formation, mechanisms and dehydration of alcohals and dehydrohalogentation of alkyl halides, regioselectivity in alcohol dehydration. The Saytzeff rule, Hofmann elimination and relative stabilities of alkenes. Chemical reactoons of alkenes-mechanisms involved in hydrogenation, electrophilic and free radical additions, Markownikoff’s rule, hydroboration-oxidation, oxymercurationreduction, Epoxsidations, ozonolysis, hydration, hydroxylation and oxidation with KMnO4. Substitution at the allylic and vinylic positions of alkenes. Structure of allenes and butadiene, methods of formation. Chemical reactions-1, 2 and 1, 4 additions, Diels-Alder reaction. Alkynes: Methods of formation. Chemical reactions of alkynes, acidity of alkyes. mechanism of electrophilic and nucleophilic addition reactions, hydroboration Oxidation, metalammonia reductions and oxidation. 6. ARENES AND AROMATICITY Structure of benzene; molecular formula and Kekule structure. Stability and carbon-carbon bond lengths of benezene, resonance structure, MO picture. Aromaticity : The Huckel rule, aromatic ions. Aromatic electrophilic substitution-general pattern of the mechanism, role of –and -complexes. Mechanism of nitration. halogenation, sulphonation, mercuration and Friedel-Crafts reaction and deactivating substituents, orientation and ortho/para ratio. Side chain reactions of benzene derivatives, Birch reduction. Methods of formation and chemical reactions of alkyl benzenes, alkynylbenzenes and biphenyl. 7. ALKYL AND ARYLHALIDES Alkyl haides: methods of formation, chemical reactions. Mechanisms of nucleophilic substitution reactious of alkyl halides, SN2 and SN1 recations with energy profile diagrams. Aryl halides: The addition elimination and the elimination addition mechanisms of nucleophilic aromatic substitution reactions. Relative reactivities of alkyl halides vs allyl, vinyl and aryl halides.  THIRD PAPER PHYSICAL CHEMISTRY (M.M. 33) 1. GASES: Kinetic theory of gases and gas laws, specific heat ratio Cp/Cv. Non-ideality of gas behaviour, Van der Waals equation of state, critical constants and their determination. Reference to some other equations of state e.g. Berthelot and Dieterici. Law of corresponding states. Maxwell Law of Distrubtions (Quantitative treatment). 2. THE FIRST LAW OF THERMODYNAMICS: Themodynamic terras and statement of the first law themodynamic reversibility and maximum work, enthalpy of a system, heat capacity at constant volume and at constant pressure. Extensive and intensive properties, state functions and exact differentials, cyclic rule, integration factor. Variation of interal energy with temperature and volume; enthalpy as a function of temperature and pressure. Relation between Cp and Cv. Joule-Thomson effect: Joule and Joule-Thomson effect, Joule-Thomson conefficient. Inversion temperature. Van der Waals equation and J – T effect. Important thermodynamic quantitites (W.Q, E and H) in an isothermal expansion of an ideal gas and adiabatic expansion of an ideal gas. Calculations of various thermodyamic quantititees for Van der Waals gasses undergoning various operations under different conditions. 3. THERMOCHEMISTRY: Heat of reaction, formation, combusion and neutralisation, solvation, dilution and hydration, hess’s law and its application, Bond energy and resonance energy. 4. CHEMICAL KINETICS: Reaction rate, order and molecularity of reaction, zero, first, second and third order reactions. Methods for determining the order of a reaction. Complex reactions opposing reactions, consecutive reactions and side reactions with reference to first order reactions. Effect of temperature on reaction velocity. Energy of activation and collisions theory of bi-molecular gaseous reactions. 5. ELECTROCHEMISTRY: Electrolytic conductance: equivalence conductance, moecular conductance, variation of conductance with concentration, Kohlrausch’s law of independent migration of ions, conductance ratio, effect of other factors on conductance. Qualitative treatment of the interionic attraction theory. Ionic mobilities, transport number, determination of transport number (Hittorf and moving boundary method), some application of conductance measurements. Hydrolysis of salts. Bronsted and Lewis acids and bases. pH and pKa, acid-base concept in non-aqueous media, Buffer solutions. Theory of acid-base indicators. 6. CHEMICAL EQUILIBRIUM : Law of mass action and its application to homogeneous and heterogeneous equilibria, Le- Chatelier principle and its application to chemical equilibriam. Degree of dissociation and abnormal molecular weights.  Syllabus for B.Sc. I CHEMISTRY PRACTICAL Time : 6 Hours (1day) (M.M. 50) 1. Analysis of inorganic mixture including insolubles and interfering redicals (four Radials only). 2. Volumetric Analysis : (i) Use of K2Cr2O7 (Determination of Iron), and (ii) Iodometry and iodimetry (Determination of Copper, dichromate, Permanganate and arsenious oxide.) 3. Detection of elements and functional groups in organic compounds – only two compounds (one element and one group). 4. Records and viva-voce. Students shall be given three experiments each of two hours duration inorganic mixture of 12 marks, volumetric of 12 marks and two organic compounds of 16 marks) in the annual practical examination.  B.Sc. Part-I (Applied Sciences) CHEMISTRY – I Total Lectures : 45 PERIODIC TABLE Periodicity and periodic classification of elements including trans Lawrencium elements, General characteristics of transition elements, variable oxidation states, complex formation, color, magnetic and catalytic properties. COORDINATION CHEMISTRY Double salts and coordination compounds, Werner’s theory, Sidgwick’s effective atomic number, IUPAC system of nomenclature, Isomerism, Stereochemistry of transition metal complexes involving coordination numbers 4, 5, 6 CHEMICAL BOINDING: Valence bond theory, Heitler-London and Pauling-Slater theory and resonance, molecular orbital, LCAO method, bonding, non-bonding and anti-bonding molecular orbital’s, molecular orbital energy level diagrams for homo and hetero nuclear diatomic molecules, electronic structure, bond order, bond length and bond strength. SHAPES OF INORGANIC MOLECULES: Hybridization of valance shell atomic orbitals and directional nature of the covalent bond, Sidgwick-Pawell theory, valence shell electron pair repulsion theory, shapes of inorganic molecules and anions. NON-IDEAL GAS BEHAVIOR: Van-der Waal’s equation of state, critical constants and their determination, Maxwell’s law of distribution of velocities. THERMOCHEMISTRY: Hess’s law of constant heat summation, Heat of reaction, formation, combustion, solvation, dilution and hydration, Kirchoff’s equation. CHEMICAL KINETICS: Reaction rate, order and molecularity of a reaction, study of first order reactions comprising opposing reactions, consecutive reactions and side reactions, Law of mass action and its application to homologous and heterogeneous equilibrium, Le Chateliar’s principle, its application to chemical equilibrium. ELECTROCHEMISTRY: Electrolytic conductance, variation of conductance with concentration, types of electrodes and their electrode potential, ionic mobilities, transport number, some application of e.m.f. measurements, determination of solubility products, pH dissociation constants of acids, hydrolysis constants, solubility of sparingly soluble salts.  B.Sc. I (Applied Sciences) CHEMISTRY – II Total Lectures : 45 Bonding in carbon compounds-hybridization and shapes of molecular orbitals. (a) Factors affecting covalent bonds-inductive, electromeric and mesmeric (resonance) effects and hydrogen bonding. (b) Modern concepts of acids and bases, factors affecting strength of acids and bases, pH and buffers. (c) Homolytic and heterolytic bond fission – formation and stability of reactive intermediates (carbo- cations, carbanions and free radicals) General concepts of types of reactions-substitution, addition and elimination. Mechanism and following reactions: Halogenation of alkanes, Nucleophilic substitution with reference to alkyl halides, hydration of alkynes, Nucleophilic addition of HCN to carbonyl compounds, electrophilic and free radical addition of HBr to alkenes, Markownikov’s rule, aromatic electrobhilic substitution reactions specially with reference to nitration and Friedel-Crafts reactions. Petroleum and petrochemicals petroleum refining, knocking, octane and octane numbers reforming, cracking petrochemicals, LPG, CNG. Aromatic hydrocarbons-benzene and its homologs, structure of benzene, aromaticity and Huckel rule. Orgenometallic compounds and some important synthetic application of Grignard reagents. Oxidation and reduction of carbonyl compounds, Aldol condensation, Claisen-Schmidt reaction, Canizzaro reaction, Perkin reaction, Benzoin condensation, Haloform reaction, Knoevenagel reaction and Michael addition (mechanism of above reaction not required) Stereo isomerism – concept of asymmetry (chirality), chemical resolution of racemic mistures, R & S nomenclature of optical isomers, E & Z nomenclature of geometrical isomers. Spectroscopy – UV / visible and IR : origin, elementary idea of instruments used, simple application in structure determination of organic molecules, Woodward-Fieser rule for calculatini max of conjugated dienes. Preparation and uses of aspirin, salol, saccharine and chloramine-T. DDT and Grammexane. Polymers-mechanism of polymerization free radical and ionic, Synthetic polymers, polythene, PVC, Polyurethanes, Nylon and Terylene.  Syllabus for B.Sc. II from 2000 & onwards FIRST PAPER INORGANIC CHEMISTRY 1. SHAPES OF MOLECULES (12) Hybridization of orbitals and directional nature of covalent bond. Sidgwick – Powell theory. Valence Shell Electron Pair Repulsion (VSEPR) theory, shapes of inorganic molecules and anions such as BeCl2, BF3, InCl2-5, SiF4, NH3, H2O, OF2, Cl2O, ClO2, PCl3, PCl5, SF4, CIF3, ICI3, PPh3, BrF5, IF7, XeF4, XeF6, CO2-3, NO-3, PO3-4, CIO-4, SbF-4, SbF2-5, TeF-5, XeF+5, l-3 and l+3 related species. 2. p-BLOCK ELEMENTS (10) Characteristic : Chemical reactivity of elements and group trends. Synthesis, properties and structure of their hydrides and halides. Application of redox potential diagrams with reference to N, P, S, Cl, Br and I. 3. p-BLOCK ELEMENTS (10) Compounds : Allotropy of boron, carbon, phosphorus and sulphur. Peroxocompounds of B, C and S oxyacids of N, P, S and halogens interhalogens, pseudohalogens and polyhalides. 4. d-BLOCK ELEMENTS (10) Transition elements: General characteristics, variable oxidation states, complex formation, colour, magnetic properties and catalytic properties. Comparative account of 3d, 4d and 5d, transition metals with respect to their atomic and ionic sizes, stability of oxidation states and magnetic properties. 5. COORDINATION CHEMISTRY (8) Isomerism in coordination compounds (definitions and some typical examples). Stereochemistry of metal complexes involving coordination number 3 to 7. 6. EXTRACTION OF ELEMENTS (6) Chemical principles involved in the extraction and isolation of the following elements B, F, Si, Ge, Cr, Ni. 7. INORGANIC COMPOUNDS – PREPARATION, PROPERTIES AND USES OF (12) Boric acid, Borides, Diborane, Fibrous Alumina and Zirconia, Silanes, Ultrapure Si and Ge. Hydrazine, Hydroxylamine. Hydrazoic acid. Hyponitrous acid. Trialkyl and Triarylphosphates. Phosphate esters. Potassium hexacyanoferrate (II) and (III). Sodium hexanitrifocobaltate (III). 8. INORGANIC COMPOUNDS – STRUCTURE AND BONDING OF (10) Diborne, Borazine, Phosphazene, Dimeric aluminum chloride, Al2Me6, Al(BH4)3, Hyponitrous acid Nickel carbonyl. 9. GRAVIMETRY (12) Principles of gravimetric analysis, coprecipitation, post-precipitation and supersaturation, Numericals based on gravimetric analysis.  B.Sc. II (Effective from 2005-2006 ONWARDS) PAPER – II (Organic Chemistry) 60 Hrs (2Hrs/Week) 1. ELECTROMAGNETIC SPECTRUM : ABSORPTION SPECTRA 10 Hrs Ultraviolet (UV) absorption spectroscopy – absorption laws (Beer-Lambert’s law), molar absorptivity, presentation and analysis of UV-spectra, types of electronic transitions, effect of conjugation Concept of chromophore and auxochrome. Bathochromic, hypsochromic, hyperchromic and hypochromic shifts. UV spectra of conjugated enes and enones. Infrared (IR) absorption spectroscopy – molecular vibrations, Hooke’s law, selection rules, intensity and position of IR bands, measurement of IR Spectrum fingerprint region; characteristic absorptions of various functional groups and interpretation of IR spectra of simple organic compounds. 2. ALCOHOLS 6 Hrs Monohydric alcohols – Methods of formation by reduction of aldehydes, ketones, carboxylic acids and esters. Hydrogen bonding, Acidic nature, Reactions of alcohols. Dihydric alcohols – Methods of formation, chemical reactions of vicinal glycols, oxidative cleavage [Pb(OAc)4 and HIO4] and pinacol-pinacolone rearrangement. Trihydric alcohols – Methods of formation, chemical reactions of glycerol. 3. PHENOLS 6 Hrs Preparation of phenols, acidic character, Comparative acidic strengths of alcohols and phenols, resonance stabilization of phenoxide ion. Reactions of phenols – electrophilic aromatic substitution, acylation and carboxylation, Mechanisms of Fries rearrangement, Claisen rearrangement, Gatterman synthesis, Hauben – Hoesch reaction, Lederer – Manasse reaction and Reimer – Tiemann reaction. 4. ETHERS AND EPOXIDES 3 Hrs Ethers – Williamson’s synthesis, Reaction with HX. Synthesis of epoxides, Acid and base-catalyzed ring opening of epoxides, orientation of epoxide ring opening, reaction of Grignard and organolithium reagents with epoxides. 5. ALDEHYDES AND KETONES 14 Hrs Synthesis of aldehydes and ketones with particular reference to the synthesis of aldehydes from acid chiorides, synthesis of aldehydes and ketones using 1, 3 dithianes, synthesis of ketones from nitriles and from carboxylic acids. Mechanism of nucleophilic additions to carbonyl group with particular emphasis on benzoin, aldol, Perkin and Knoevengel condensations. Condensation with ammonia and its derivatives. Witting reaction, Mannich reaction. Use of acetals as protecting group. Oxidation of aldehydes, Bayer – Villiger oxidation of ketones, Cannizzaro reaction, MPV, Clemmensen, Wolff – Kishner, LiAlH4 and NaBH4 reductions, Halogenation of enolizable ketones. 6. CARBOXYLIC ACIDS 6 Hrs Acidity of carboxylic acids. Effects of substituents on acid strength. Preparation of carboxylic acids. Reactions of carboxylic acids. Hell- Volhard-Zelinsky reaction. Synthesis of acid chlorides, esters and amides. Reduction of carboxylic acids. mechanism of decarboxylation. Methods of formation and chemical reactions of halo acids and hydroxyl acids. 7. CARBOXYLIC ACID DERIVATIVES Relative reactivities of acyl derivatives. Interconversion of acid derivatives nucleophilic acyl substitution. Preparation of carboxylic acid derivatives chemical reactions. Mechanisms of esterification and hydrolysis (acidic and basic). 8. ORGANIC COMPOUNDS OF NITROGEN 12 Hrs. Preparation of nitro alkanes and nitroarenes. Chemical reactions of nitroalkanes. Mechanisms of nucleophilic substitution in of nitroarenes. Mechanisms of nucleophilic substitution in nitroarenes and their reductions in acidic netural andalkaline media. Separation of a mixture of primary secondary and tertiary amines. Structural features affecting basicity of amines. Amine salts as phase-transfer catalysts. Preparation of alkyl and aryl amines (reduction of nitro compounds, nitriles), reductive amination of aldehydic and ketonic compounds. Gabriel-phthalimide reaction, Hofmann bromamide reaction. Reaction of amines, electrophilic aromatic substitution in aryl amines, reactions of amines with nitrous acid. Synthetic transformations of aryl diazonium salts, azo coupling.  THIRD PAPER PHYSICAL CHEMISTRY 1. THERODYNAMICS Spontaneous processes, Carnot cycle, statement of second law, concept of entropy, combined form of the first and second law of thermodynamics, enthalpy and entropy. Thermodynamic equation of state (energy as a function of V. and T, enthalpy as a function of T and F), entropy change in isolated system. Variation of entropy with temperature and volume, Variation entropy with temperature and pressure. Entropy change in chemical reaction. Helmholtz and Gibbs free energies, Properitis of Gibbs function, Gibbs-Helmholtz equation Thermodynamic criteria of equilibrium Clapeyron-Clausium equation and its application. 2. PHASE EQUILIBRIA : Explanation of phase, component and degree of freedom. Phase rule and its application to one component (water and sulphur) and two component (signle eutectics) systems. Nernst distribution law, thermodynamic derivation of the distribution law. Limitations and applications of the distribution law. 3. ELECTROCHEMICAL CELLS : Reversible and irreversible cell, EMF of a cell and free energy change Nernst equation. EMF and equilibrium constant. Types of single electrodes. Electrode potentials. Standard electrode potential concept of concentration cell without transference. Applications of EMF measurement (determination of solubility product. pH. dissociation constants of acids, hydrolysis constant, solubility of sparigly soluble salt). 4. SURFACE PHENOMENON : Physical and chemical adsorption, Freundlich adsorption isotherm, Gibbs adsorption equation, Langmuir monomolecular theory and B.E.T. theory. 5. PHYSICAL PROPERTIES AND CHEMICAL CONSTITUTION: Molar volume, Parachor Molar refraction and polarisation, Dipolemoment, Debye equation (derivation not required) and Clausius-Mosotti equation. 6. COLLOIDAL STATE : Stability of colloids, determination of size of colloidal particle, Electrokinetic Potential (Zeta potential). Donnan membrane theory and its applications. CHEMISTRY PRACTICAL Time : 6 Hrs (1day) M.M. 50 1. Gravimetric Analysis (i) Barium as BaSO4 (ii) Iron as Fe2O3 (iii) Zinc as ZnO (iv) Aluminum as Ai2O3 and (v) Copper as CuO 10 Mark 2. Organic preparation (one step) and crystallisation: (i) Acetylation, (ii) Nitration (iii) Bromination (iv) Osazone formation (v) Picrate formation, and (vi) Azo-dye formation 15 Mark 3. Physical Chemistry experiments (i) Experiments of surface tension (using Stalgometer)  (ii) Experiments on viscosity (using viscometer) (iii) Partition coefficient determination (iv) Determination of solubility (at different temperatures) (v) Molecular weight determination of a volatile substance (by Victor Meyer’s method) 15 Marks 4. Records and viva –voce. Students shall be given three experiments each of two hours duration (gravimetric of 10 marks, organic preparation of 15 marks, and physical experiment of 15 marks) in the annual practical examination comprising 10 marks of records and viva-voce. Total M.M. : 50  Syllabus for B.Sc. III from 2001 & onwards FIRST PAPER INORGANIC CHEMISTRY 1. THEORIES OF COVALENT BOND (12) Valence bond theory-Heitler-London and Pauling-Slater theories and resonance, Molecular orbital theory-LCAO method, bonding, non-bonding and antibonding molecular orbitals. Molecular orbital energy level diagrams for homonuclear and heteronuclear diatomic molecules-electronic structure, bond order, bond length and bond energy. 2. THEORIES OF COORDINATE BOND (12) Valence bond theory and its limitations. Crystal field theory-d-orbital splitting in octahedral and tetrahedral crystal fields. Ligand field splitting (10Dq) and factors affecting its magnitude, spectrochemical series. Crystal field stablization energies (CFSE) for d1to d10 systems in octahedral and tetrahedral fields. 3. METALS AND METALLURGY (14) Comparative study of the chemistry of d-block elements and their important compounds : Sc, Y, La, Ti, Zr, Hf, V, Nb, Ta, Cr, Mo, W, Mn, Tc, Re, Fe, Co, Ni and platinum metals (Application of reduction potential diagrams whereever necessary). Metallurgical extraction of Ti, V, Mo, W, and Re. 4. 4 f-BLOCK ELEMENTS (10) Characteristics: Electronic structure, lanthanide contraction and its consequences, oxidation states, complex formation, magnetic and spectral properties and their differences from transition metals, ion exchange and solvent extraction methods of separation of lanthanides. 5. INORGANIC CHAINS, RINGS AND CAGES (8) Silicates, Silicones, Borazines, Phosphazenes, S-N compounds and Boranes. 6. STRUCTURES AND CHARACTERISTICS OF SOLIDS (10) Metallic, lonic, Covalent and molecular crystals, Structures of lonic solids, radius ratio rules, Structures of metals, close packed structures, Characteristics of Unit Cells. 7. CHEMICAL INDUSTRIES (8) Glass, cement, artificial fertilizers, steel and Phosphorus sulphides. 8. ENVIRONMENTAL POLLUTION (8) Air pollutants, their sources and toxic effects. Particulates, their sources and toxic effects. Acid rain and green house effects. Water pollutants. 9. METAL IONS IN BIOLOGICAL SYSTEMS (8) Essential and trace elements. Chemistry of chlorophyll, haemoglobin, myoglobin, and cyanocobalamine.  SECOND PAPER ORGANIC CHEMISTRY 1. SPECTROSCOPY 15 Hrs. Nuclear magnetic resonance (NMR) spectroscopy, nuclear shielding and deshielding, chemical shift and molecular structure, spin – spin splitting and coupling constants, area of signals, interpretation of PMR spectra of simple organic molecules such as ethylbromide, ethanol, acetaldehyde, 1, 1, 2- tribromoethane, ethyl acetate, toluene and acetophenone. Problems pertaining to the structure elucidation of simple organic compounds using UV. IR and PMR spectroscopic techniques. 2. ORGANOMETALLIC COMPOUNDS 5 Hrs. Organomagnesium compounds : the Grignard reagents – formation, structure and chemical reactions. Organozinc compounds : formation and chemical reactions. Organolithium compounds : formation and chemical reactions. 3. ORGANOSULPHUR COMPOUNDS 4 Hrs. Methods of formation and chemical reactions of thiols, thioethers, sulphonic acids, sulphonamides and sulphaguanidine. 4. HETEROCYLIC COMPOUNDS 8 Hrs. Introduction : Molecular orbital picture and aromatic characteristics of pyrrole, furan, thiophene and pyridine, Methods of synthesis and chemical reactions with particular emphasis on the mechanism of electrophillic substitution. Mechanism of nucleophilic substitution reactions in pyridine derivatives. Comparison of basicity of pyridine, piperidine and pyrrole. Introduction to condensed five and six – membered heterocycles. Preparation and reactions of indole, quinoline and isoquinoline with special reference to Fisher indole synthesis, Skraup synthesis and Bishler-Napleralski synthesis. Mechanism of electrophilic substitution reactions of indole, quinoline and isoquioline. 5. ORGANIC SYNTHESIS VIA ENOLATES 6 Hrs. Acidity of a-hydrogens, alkylation of diethyl malonate and ethyl acetoacetate. Synthesis of ethyl acetoacetate : the Claisen condensation Keto – enol tautomerism of ethyl acetoacetate. Alkylation of 1, 3- dithianes, Alkylation and acylation of enamines. 6. CARBOHYDRATES 10 Hrs. Classification and nomenclature. Monosaccharides, mechanism of osazone formation, interconversion of glucose and fructose, chain lengthening and chain shortening of aldoses. Configuration of monosaccharides. Erythro and threo diastereomers. Conversion of glucose into mannose, Formation of glycosides, ethers and esters, Determination of ring size of monosaccharides. Cyclic structure of D (+) – glucose, Mechanism of mutarotation. Dissocharides - maltose, Surcrose and lactose, Structure determination. 7. AMINO ACIDS, PEPTIDES AND PROTEINS 6 Hrs. Amino acids: acids – base behaviour, isoelectric point and electrophoresis, Preparation and reactions of – amino acids. Peptide structure determination, and group analysis, selective hydrolysis of peptides. Solid – phase peptide synthesis. 8. SYNTHETIC POLYMERS 6 Hrs. Addition or chain – growth polymerization Free radical vinyl polymerization ionic vinyl polymerization, Ziegler – Natta polymerization and vinyl polymers. Condensation or step growth polymerization. Polyesters, Polyamides. Phenol formaldehyde resinds, urea – formaldehyde resins and polyurethanes. Natural and synthetic rubbers.  THIRD PAPER PHYSICAL CHEMISTRY I. THERMODYNAMICS : Thermodynamic derivation of the law of mass action. Reaction lsotherm and Van’t Hoff equation (influence of temperature on equilibrium constant K Themodynamic derivation of phase rule. Partial molar quantities. Chemical potential, Gibbs-Duhem equation, Chemical potential, Gibbs- Duhem equation, Chemical potential and other thermodynamic functions. Effect of temperature of chemical potential. Effect of pressure on chemical potential. Chemical potential of real gases and fugacity of real gases. Colligative properties (thermodynamic treatment) : Lowering of vapour pressure osmotic pressure of boiling point and depression of freezing point. II. CHEMICAL KINETICS AND CATALSIS : Steady state approximation Lindemann’s theory of unimolecular reaction. Qualitative treatment of transition state theory of reaction rates. Primary salt effect in ionic reactions. Kinetics of homogeneous, acid – base and enzyme catalysis, heterogeneous catalysis, negative catalysis and inhibition. Effect of pH and temperature on enzyme catalysis. Effect of temperature on surface reaction promoters and poisons. III. PHOTOCHEMISTRY : Absorption of light, chain reaction, free radical chains (Rice-Herzfoid mechanism for the decomposition of ethane) Lamberts and Beer’s law, Grotthug Draper law, Einstein’s law of photochemical equivalance quantum efficiency, reasons for low and high quantum yields. Kinetics of some typical photochemical reactions (Decompostion of acetaldehyde, dimerisation of anthracene) Photo electric cell. Photosensitization. IV. E.M.F. : Concentration cells, with and without transference, liquid junction potential, fuel cells, chemical cells without transference. V. ATOMIC STRUCTURE : Bohr’s theory, Sommerfeld’s model, dual nature of electron de-Broglie’s equation. Experimental verification of the wave nature of electron (Davison & Germer’s experiment) Heisenberg’s uncertainty principle. One dimensional Schrodinger’s wave equation and physical significance of the wave function. Particle in a box (one dimension only). VI. NUCLEAR CHEMISTRY Radioactive decay and equilibrium. Nuclear reactions Q value, cross sections, types of reactions, Chemical effects of nuclear transformations, Natural and artificial radioacivity. theory of nuclear disintegration; disintegration and displacement laws: radioactive series. nuclear binding energy; nuclear reaction; fission and fusion products and fission yields ; radioactive isotopes and their uses. Radioactive techniques; tracer technique, neutron activation analysis, counting techniques such as G.M. ionisation and proportional counter. CHEMISTRY PRACTICAL Time : 6 Hours (1day) M.M. : 75 1. Organic Chemistry experiments: (i) Identification of single organic solid compound. (ii) Estimation of reducing and non-reducing sugars. (iii) Paper chromatographic separation of amino acids ad sugars (only binary mixtures) (20 Marks) 2. Physical Chemistry experiments : (i) Hydrolysis of methyl acetate catalysed by an acid.  (ii) Hydrolysis of ethyl acetate. (iii) Adsorption of acetic acid on charcoal. (iv) Heat of solution of a substance (oxalic acid) by solubility method. (v) Transition temperature of Glauber’s salt by therimometric method. (vi) Heat of neutralization of NaOH and HCl. (vii) Molecular weight determination of a volatile substance by Duma’s method. (viii) Relative strength of HCl and H2SO4 by catalysing the hydrolysis of methyl acetate. (ix) Acetone – iodine reaction catalysed by H+. 3. Inorganic analysis and preparations: (i) Paper chromatographic separation of metal ions – Cu2+, Pb2+, Zn2+, Cu2+, Ni2+, Cd2+, ions (binary mixtures only). (ii) EDTA titrations of Ca2+, Mg2+, Zn2+ and Cu2+ (iii) Determination of hardness of water. (iv) Determination of CO2 content in polluted water (v) Colorimetric determination of metal ions – Fe3+, Co2+, Ni2+ and Mn2+ (vi) Preparation of simple inorganic complexes. (15 marks) 4. Records and viva-voce. Students shall be given three experiments each of two hours duration (organic experiment of 20 marks. physical experiment of 25 marks, and inorganic experiment of 15 marks) in the annual practical examination comprising 15 marks of records and viva-voce.