CHEMISTRY (CY)
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 Ѱ2; 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; DebyeHückel-
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.
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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 Ѱ2; 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; DebyeHückel-
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.
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