Physical Chemistry

 Atomic and Molecular Structure:

• Planck’s black body radiation, Photoelectric effect, Bohr’s theory, de Broglie postulate, Heisenberg’s Uncertainty Principle.
• Schrödinger’s wave equation (including mathematical treatment), postulates of quantum mechanics, normalized and orthogonal wave functions, its complex conjugate (idea of complex numbers) and significance of Ψ².
• Operators, Particle in one-dimension box, radial and angular wave functions for hydrogen atom, radial probability distribution.
• Finding maxima of distribution functions (idea of maxima and minima), energy spectrum of hydrogen atom.
• Shapes of s, p, d, and f orbitals, Pauli’s Exclusion Principle, Hund’s rule of maximum multiplicity.

 Gaseous State:

• Kinetic molecular model of a gas: collision frequency, collision diameter, mean free path, and viscosity of gases.
• Maxwell-Boltzmann distribution: molecular velocities, law of equipartition of energy, molecular basis of heat capacities.
• Ideal gases, and deviations from ideal gas behaviour, van der Waals equation of state, critical state, law of corresponding states.

 Liquid State:

• Physical properties of liquid, vapour pressure, surface tension and co-efficient of viscosity and their applications.
• Effect of concentration of solutes on surface tension and viscosity, effect of temperature on viscosity of liquids.

 Solid State:

• Unit Cells, Miller indices, crystal systems and Bravais Lattices, elementary applications of vectors to crystal systems.
• X-ray diffraction, Bragg’s Law, Structure of NaCl, CsCl, and KCl, diamond, and graphite.
• Close packing in metals and metal compounds, semiconductors, insulators; Defects in crystals, lattice energy; isomorphism; heat capacity of solids.

 Chemical Thermodynamics:

• Mathematical treatment: Exact and in-exact differentials, partial derivatives, Euler’s reciprocity, cyclic rule.
• Reversible and irreversible processes; Laws of thermodynamics, thermochemistry, thermodynamic functions, such as enthalpy, entropy, and Gibbs free energy, their properties and applications.
• Partial molar quantities, dependence of thermodynamic parameters on composition, Gibbs Duhem equation, chemical potential and its applications.

 Chemical and Phase Equilibria:

• Law of mass action; Kp, Kc, Kx and Kn; Effect of temperature on K; Le-Chatelier principle.
• Ionic equilibria in solutions; pH and buffer solutions; Salt hydrolysis; Solubility and solubility product.
• Acid–base titration curves; Indicators; Dilute solutions; Raoult’s and Henry’s Laws and their applications; Colligative properties.
• Gibbs phase rule; Phase equilibria; single and two-component phase diagrams.

 Electrochemistry:

• Conductivity, equivalent and molar conductivity and their properties; Kohlrausch law; Debye-Hückel-Onsager equation.
• Ionic velocities, mobilities, transference numbers; Applications of conductance measurement; Quantitative aspects of Faraday’s laws of electrolysis.
• Applications of electrolysis in metallurgy and industry; Electromotive force of a cell, Nernst equation; Standard electrode potential, Electrochemical series.
• Concentration cells with and without transference; Applications of EMF measurements including potentiometric titrations.

 Chemical Kinetics:

• Order and molecularity of a reaction, differential and integrated form of rate expressions – basic ideas of integration and differentiation.
• Kinetics of opposing, parallel, and consecutive reactions; Steady state approximation in reaction mechanisms.
• Chain reactions; Uni-molecular reaction (Lindemann mechanism); Temperature dependence of reaction rates, Arrhenius equation.
• Activation energy; Collision theory of reaction rates; Types of catalysts, specificity and selectivity, mechanisms of catalyzed reactions at solid surfaces.
• Enzyme catalysis (Michaelis-Menten mechanism, Double reciprocal plot), Acid-base catalysis.

 Adsorption:

• Gibbs adsorption equation; adsorption isotherm; types of adsorption; surface area of adsorbents; surface films on liquids.

 Spectroscopy:

• Beer-Lambert’s law; fundamental concepts of rotational, vibrational, electronic and magnetic resonance spectroscopy.

  Organic Chemistry

 Basic Concepts in Organic Chemistry and Stereochemistry:

• Electronic effects (resonance, inductive, hyperconjugation) and steric effects and its applications (acid/base property).
• Optical isomerism in compounds with and without any stereocenters (allenes, biphenyls); conformation of acyclic systems (substituted ethane/n-propane/n-butane) and cyclic systems, substituted cyclohexanes, and polycyclic (cis and trans decalins) systems.
• Organic Reaction Mechanism and Synthetic Applications:
• Chemistry of reactive intermediates (carbocations, carbanions, free radicals, carbenes, nitrenes, benzynes); nucleophilic substitution, elimination reactions and mechanisms.
• Hofmann-Curtius-Lossen rearrangement, Wolff rearrangement, Simmons-Smith reaction, Reimer-Tiemann reaction, Michael reaction, Darzens reaction, Wittig reaction and McMurry reaction.
• Pinacol-pinacolone, Favorskii, benzilic acid rearrangement, Baeyer-Villeger reaction.
• Oxidation and reduction reactions in organic chemistry.
• Organometallic reagents in organic synthesis (Grignard, organolithium, organocopper, and organozinc (Reformatsky only)).
• Diels-Alder, electrocyclic and sigmatropic reactions; functional group inter-conversions and structural problems using chemical reactions.

 Qualitative Organic Analysis:

• Identification of functional groups by chemical tests; elementary UV, IR and ¹H NMR spectroscopic techniques as tools for structural elucidation of simple organic molecules.

 Natural Products Chemistry:

• Chemistry of alkaloids, steroids, terpenes, carbohydrates, amino acids, peptides and nucleic acids.

 Aromatic and Heterocyclic Chemistry:

• Monocyclic, bicyclic, and tricyclic aromatic hydrocarbons, and monocyclic compounds with one hetero atom: synthesis, reactivity, and properties, aromaticity.
• Electrophilic and nucleophilic aromatic substitution reactions.

  Inorganic Chemistry

 Periodic Table:

• Periodic classification of elements, Aufbau’s principle, periodicity.
• Variations of orbital energy, effective nuclear charge, atomic, covalent, and ionic radii, ionization enthalpy, electron gain enthalpy, and electronegativity with atomic number.
• Electronic configuration of diatomic molecules (first and second row elements).

 Extractions of Metals:

• General methods of isolation and purification of elements.
• Principles and applications of Ellingham diagram.

 Chemical Bonding and Shapes of Molecules:

• Ionic bond: Packing of ions in crystals, radius ratio rule, Born-Landé equation, Kapustinskii expression, Madelung constant, Born-Haber cycle, solvation energy, polarizing power, and polarizability.
• Fajan’s rules, covalent bond: Lewis structure, valence bond theory.
• Hybridization, molecular orbital theory, molecular orbital diagrams of diatomic and simple polyatomic molecules and ions.
• Multiple bonding (σ and π bond approach) and bond lengths.
• Van der Waals forces, ion-dipole forces, dipole-dipole interactions, induced dipole interactions, instantaneous dipole-induced dipole interactions, hydrogen bonding.
• Effect of intermolecular forces on melting and boiling points, solubility energetics of dissolution process.
• Bond dipole, dipole moment, and molecular polarizabilities, VSEPR theory, and shapes of molecules, ionic solids.

 Main Group Elements (s and p blocks):

• Reactions of alkali and alkaline earth metals with oxygen, hydrogen, and water.
• Alkali and alkaline earth metals in liquid ammonia.
• Gradation in properties of main group element in a group, inert pair effect.
• Synthesis, structure, and properties of diborane, ammonia, silane, phosphine, and hydrogen sulphide.
• Allotropes of carbon, oxides of nitrogen, phosphorus, and sulphur.
• Oxoacids of phosphorus, sulphur, and chlorine.
• Halides of silicon and phosphorus, synthesis and properties of borazine, silicone, and phosphazene.
• Synthesis and reactions of xenon fluorides.

 Transition Metals (d block):

• Characteristics of d-block elements, oxide, hydroxide, and salts of first row metals.
• Coordination complexes: structure, isomerism, reaction mechanism, and electronic spectra.
• VB, MO, and crystal field theoretical approaches for structure, color, and magnetic properties of metal complexes.
• Organometallic compounds with metal-ligand single and multiple bonds (such as metal carbonyls, metal nitrosyls, and metallocenes).
• Homogenous catalysis involving Wilkinson’s catalyst.

 Bioinorganic Chemistry:

• Essentials and trace elements of life, basic reactions in the biological systems and the role of metal ions, especially Fe²⁺ and Zn²⁺.
• Structure and function of myoglobin, hemoglobin, and carbonic anhydrase.

 Instrumental Methods of Analysis:

• Basic principles, instrumentations, and simple applications of conductometry, potentiometry, and UV-vis spectrophotometry.
• Analyses of water, air, and soil samples.

 Analytical Chemistry:

• Principles of qualitative and quantitative analysis.
• Acid-base, oxidation-reduction, and complexometric titrations using EDTA.
• Precipitation reactions, use and types of indicators.
• Use of organic reagents in inorganic analysis.
• -Use of organic reagents in inorganic analysis;
• Radioactivity, nuclear reactions, applications of isotopes;
• Mathematical treatment in error analysis, elementary statistics and probability theory.