1.1 Atomic structure : Schrodinger wave equation, significance of γ and γ2 quantum numbers and their significance, radial and angular probability, shapes of orbitals, relative energies of atomic orbitals as a function of atomic number. Electronic configurations of elements; Aufbau principle, Hund’s multiplicity rule, Pauli exclusion principle.
1.2 Chemical periodicity : Periodic classification of elements, salient characteristics of s,p,d and f block elements. Periodic trends of atomic radii, ionic radii, ionisation potential, electron affinity and electronegativity in the periodic table.
1.3 Chemical bonding : Types of bonding, overlap of atomic orbitals, sigma and pi bonds, hydrogen and metallic bonds. Shapes of molecules, bond order, bond length, V.S.E.P.R. theory and bond angles. The concept of hybridization and shapes of molecules and ions.
1.4 Oxidation states and oxidation number : Oxidation and reduction, oxidation numbers, common redox reactions, ionic equations. Balancing of equations for oxidation and reduction reactions.
1.5 Acids and bases : Bronsted and Lewis theories of acids and bases. Hard and soft acids and bases. HSAB principle, relative strengths of acids and bases and the effect of substituents and solvents on their strength.
1.6 Chemistry of elements :
1.7 Extraction of metals : Principles of extraction of metals as illustrated by sodium, magnesium, aluminium, iron, nickel, copper, silver and gold.
1.8 Nuclear Chemistry : Nuclear reactions; mass defect and binding energy, nuclear fission and fusion. Nuclear reactors; radioisotopes and their applications.
1.9 Coordination compounds : Nomenclature, isomerism and theories of coordination compounds and their role in nature and medicine.
1.10 Pollution and its control : Air pollution, types of air pollutants; control of air and water pollution; radioactive pollution.
2.1 Bonding and shapes of organic molecules : Electronegativity, electron displacements-inductive, mesomeric and hyperconjugative effects; bond polarity and bond polarizability, dipole moments of organic molecules; hydrogen bond; effects of solvent and structure on dissociation constants of acids and bases; bond formation, fission of covalent bonds : homolysis and heterolysis; reaction intermediates-carbocations, carbanions, free radicals and carbenes; generation, geometry and stability; nucleophiles and electrophiles.
2.2 Chemistry of aliphatic compounds: Nomenclature; alkenes-synthesis, reactions (free radical halogenation) — reactivity and selectivity, sulphonation-detergents; cycloalkanes-Baeyer’s strain theory; alkenes and alkynes-synthesis, electrohilic addition reactions, Markownikov’s rule, peroxide effects, 1- 3-dipolar addtion; nucleophilic addition to electron-deficient alkenes; polymerisation; relative acidity; synthesis and reactions of alkyl halides, alkanols, alkanals, alkanones, alkanoic acids, esters, amides, nitriles, amines, acid anhydrides, a, ß-unsaturated ketones, ethers and nitro compounds.
2.3 Stereochemistry of carbon compounds : Elements of symmetry, chiral and achiral compounds. Fischer projection formulae; optical isomerism of lactic and tartaric acids, enantiomerism and diastereoisomerism; configuration (relative and absolute); conformations of alkanes upto four carbons, cyclohexane and dimethylcyclo-hexanes-their potential energy. D, L-and R, S-notations of compounds containing chiral centres; projection formulae-Fischer, Newman and sawhorse-of compounds containing two adjacent chiral centres; meso and dl-isomers, erythro and threo isomers; racemization and resolution; examples of homotopic, enantiotopic and diasteretopic atoms and groups in organic compounds, geometrical isomers; E and Z notations. Stereochemistry of SN1, SN2, E1 and E2 reactions.
2.4 Organometallic compounds : Preparation and synthetic uses of Grignard reagents, alkyl lithium compounds.
2.5 Active methylene compounds : Diethyl malonate, ethyl acetoacetate, ethyl cyanoacetate-applications in organic synthesis; tautomerism (keto-enol).
2.6 Chemistry of aromatic compounds : Aromaticity; Huckel’s rule; electrophilic aromatic substitution-nitration, sulphonation, halogenation (nuclear and side chain), Friedel-Crafts alkylation and acylation, substituents effect; chemistry and reactivity of aromatic halides, phenols, nitro-, diazo, diazonium and sulphonic acid derivatives, benzyne reactions.
2.7 Chemistry of biomolecules :
2.8 Basic principles and applications of UV, visible, IR and NMR spectroscopy of simple organic molecules.
3.1 Gaseous state : Deviation of real gases from the equation of state for an ideal gas, van der Waals and Virial equation of state, critical phenomena, principle of corresponding states, equation for reduced state. Liquification of gases, distribution of molecular speed, collisions between molecules in a gas; mean free path, speicific heat of gases
3.2 Thermodynamics :
3.3 Phase rule and its applications : Equilibrium bewteen liquid, solid and vapours of a pure substance, Clausius-Clapeyron equation and its applications. Number of components, phases and degrees of freedom; phase rule and its applications; simple systems with one (water and sulphur) and two components (lead-silver, salt hydrates). Distribution law, its modifications, limitations and applications.
3.4 Solutions : Solubility and its temperature dependence, partially miscible liquids, upper and lower critical solution temperatres, vapour pressures of liquids over their mixtures, Raoult’s and Henry’s laws, fractional and steam distillations.
3.5 Colligative Properties : Dilute solutions and colligative properties, determination of molecular weights using colligative properties.
3.6 Electrochemistry : Ions in solutions, ionic equilibria, dissociation constants of acids and bases, hydrolysis, pH and buffers, theory of indicators and acid-base titrations. Conductivity of ionic solutions, its variation with concentration, Ostwald’s dilution law, Kohlrausch law and its application. Transport number and its determination. Faraday’s laws of electrolysis, galvanic cells and measurements of their e.m.f., cell reactions, standard cell, standard reduction potential, Nernst equation, relation between thermodynamic quantities and cell e.m.f., fuel cells, potentiometric titrations.
3.7 Chemical kinetics : Rate of chemical reaction and its dependence on concentrations of the reactants, rate constant and order of reaction and their experimental determination; differential and integral rate equations for first and second order reaction, half-life periods; temperature dependence of rate constant and Arrhenius parameters; elementary ideas regarding collision and transition state theory.
3.8 Photochemistry : Absorption of light, laws of photochemistry, quantum yield, the excited state and its decay by radiative, nonradiative and chemical pathways; simple photochemical reactions.
3.9 Catalysis : Homogeneous and heterogeneous catalysis and their characteristics, mechanism of heterogeneous catalysis; enzyme catalysed reactions (Michaelis-Menten mechanism).
3.10 Colloids : The colloidal state, preparation and purification of colloids and their characteristics properties; lyophilic and lyophobic colloids and coagulation; protection of colloids; gels, emulsions, surfactants and micelles.
1. Atomic Structure:
Heisenberg’s uncertainty principle, Schrodinger wave equation (time independent); Interpretation of wave function, particle in one-dimensional box, quantum numbers, hydrogen atom wave functions; Shapes of s, p and d orbitals.
2. Chemical Bonding:
Ionic bond, characteristics of ionic compounds, lattice energy, Born-Haber cycle; covalent bond and its general characteristics, polarities of bonds in molecules and their dipole moments; Valence bond theory, concept of resonance and resonance energy; Molecular orbital theory (LCAO method); bonding in H2+, H2, He2+ to Ne2, NO, CO, HF, and CN–; Comparison of valence bond and molecular orbital theories, bond order, bond strength and bond length.
3. Solid State:
Crystal systems; Designation of crystal faces, lattice structures and unit cell; Bragg’s law; X-ray diffraction by crystals; Close packing, radius ratio rules, calculation of some limiting radius ratio values; Structures of NaCl, ZnS, CsCl and CaF2; Stoichiometric and nonstoichiometric defects, impurity defects, semi-conductors.
4. The Gaseous State and Transport Phenomenon:
Equation of state for real gases, intermolecular interactions and critical phenomena and liquefaction of gases, Maxwell’s distribution of speeds, intermolecular collisions, collisions on the wall and effusion; Thermal conductivity and viscosity of ideal gases.
5. Liquid State:
Kelvin equation; Surface tension and surface energy, wetting and contact angle, interfacial tension and capillary action.
Work, heat and internal energy; first law of thermodynamics.
Second law of thermodynamics; entropy as a state function, entropy changes in various processes, entropy–reversibility and irreversibility, Free energy functions; Thermodynamic equation of state; Maxwell relations; Temperature, volume and pressure dependence of U, H, A, G, Cp and Cv, a and ß; J-T effect and inversion temperature; criteria for equilibrium, relation between equilibrium constant and thermodynamic quantities; Nernst heat theorem, introductory idea of third law of thermodynamics.
7. Phase Equilibria and Solutions:
Clausius-Clapeyron equation; phase diagram for a pure substance; phase equilibria in binary systems, partially miscible liquids–upper and lower critical solution temperatures; partial molar quantities, their significance and determination; excess thermodynamic functions and their determination.
Debye-Huckel theory of strong electrolytes and Debye-Huckel limiting Law for various equilibrium and transport properties.
Galvanic cells, concentration cells; electrochemical series, measurement of e.m.f. of cells and its applications fuel cells and batteries.
Processes at electrodes; double layer at the interface; rate of charge transfer, current density; overpotential; electroanalytical techniques: Polarography, amperometry, ion selective electrodes and their uses.
9. Chemical Kinetics:
Differential and integral rate equations for zeroth, first, second and fractional order reactions; Rate equations involving reverse, parallel, consecutive and chain reactions; branching chain and explosions; effect of temperature and pressure on rate constant; Study of fast reactions by stop-flow and relaxation methods; Collisions and transition state theories.
Absorption of light; decay of excited state by different routes; photochemical reactions between hydrogen and halogens and their quantum yields.
11. Surface Phenomena and Catalysis:
Absorption from gases and solutions on solid adsorbents, Langmuir and B.E.T. adsorption isotherms; determination of surface area, characteristics and mechanism of reaction on heterogeneous catalysts.
12. Bio-inorganic Chemistry:
Metal ions in biological systems and their role in ion transport across the membranes (molecular mechanism), oxygen-uptake proteins, cytochromes and ferredoxins.
13. Coordination Compounds:
14. Main Group Chemistry:
Boranes, borazines, phosphazenes and cyclic phosphazene, silicates and silicones, Interhalogen compounds; Sulphur – nitrogen compounds, noble gas compounds.
15. General Chemistry of ‘f’ Block Elements:
Lanthanides and actinides; separation, oxidation states, magnetic and spectral properties; lanthanide contraction.
1. Delocalised Covalent Bonding:
Aromaticity, anti-aromaticity; annulenes, azulenes, tropolones, fulvenes, sydnones.
3. Pericyclic Reactions:
Classification and examples; Woodward-Hoffmann rules – electrocyclic reactions, cycloaddition reactions [2+2 and 4+2] and sigmatropic shifts [1, 3; 3, 3 and 1, 5] FMO approach.
5. Synthetic Uses of Reagents:
OsO4, HIO4, CrO3, Pb(OAc)4, SeO2, NBS, B2H6, Na-Liquid NH3, LiAlH4, NaBH4, n-BuLi and MCPBA.
Photochemical reactions of simple organic compounds, excited and ground states, singlet and triplet states, Norrish-Type I and Type II reactions.
Principle and applications in structure elucidation:
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