UPSC Chemist Exam Pattern & Syllabus for paper 2 is given below

S. No. | Name of Subject | Duration | Maximum Marks | Syllabus |

1. | General English | 3 Hours | 100 | Syllabus |

2. | Chemistry Paper I | 3 Hours | 200 | Syllabus |

3. | Chemistry Paper II | 3 Hours | 300 | Syllabus |

4. | Chemistry Paper III | 3 Hours | 300 | Syllabus |

## Paper-II: Physical Chemistry

### Kinetic theory and the gaseous state:

Gaseous state: Gas laws, kinetic theory of gas, collision and gas pressure, derivation of gas laws from kinetic theory, the average kinetic energy of translation, Boltzmann constant and absolute scale of temperature. Maxwell’s distribution of speeds. Kinetic energy distribution, calculations of average, root mean square and most probable velocities. The principle of equipartition of energy and its application to calculate the classical limit of the molar heat capacity of gases.

### Collision of gas molecules, Real gases:

Collision diameter; collision number and mean free path; frequency of binary collisions; wall collision and rate of effusion. Real gases, Deviation of gases from ideal behavior; compressibility factor; Andrew’s and Amagot’s plots; van der Waals equation and its characteristic features. Existence of critical state. Critical constants in terms of van der Waals constants. Law of corresponding state and significance of second virial coefficient. Boyle temperature. Intermolecular forces.

### Liquid state:

Physical properties of liquids and their measurements: surface tension and viscosity.

### Solids:

Nature of solid state, the law of constancy of angles, the concept of a unit cell, different crystal system, Bravais lattices, law of rational indices, Miller indices, symmetry elements in crystals. X-ray diffraction, Bragg’s law, Laue’s method, powder method, radius ratio and packing in crystals.

### Thermodynamics:

Definition of thermodynamic terms. Thermodynamic functions and their differentials. Zeroth law, First law and Second law of thermodynamics. Cyclic, reversible and irreversible processes. Internal energy (U) and enthalpy (H); the relation between Cp and Cv, calculation of w, q, ΔU and ΔH for expansion of ideal gas under isothermal and adiabatic conditions for reversible and irreversible processes including free expansion. Joule-Thomson Coefficient and inversion temperature. Application of First law of thermodynamics.

**Application of Second law of thermodynamics.**

Carnot cycle and its efficiency, Gibbs function (G) and Helmholtz function (A), Gibbs-Helmholtz equation, criteria for thermodynamic equilibrium and spontaneity of a process. Chemical equilibrium: chemical equilibria of homogeneous and heterogeneous systems, derivation of expression of equilibrium constants, Le Chatelier’s principle of dynamic equilibrium.

### Thermodynamics and Equilibrium:

The chemical potential in terms of Gibb’s free energy and other thermodynamic state functions and its variation with temperature and pressure. Gibbs-Duhem equation; fugacity of gases and fugacity coefficient. Thermodynamic conditions for equilibrium, the degree of advancement. Can’t Hoff’s reaction isotherm. Equilibrium constant and standard Gibbs free energy change. Definitions of KP, KC, and Kx; can’t Hoff’s reaction isobar and isochore. Le Chatelier’s principle. Activity and activity coefficients of electrolyte/ion in solution. Debye-Huckel limiting law.

### Acids-bases and solvents:

Modern aspects of acids and bases: Arrhenius theory, a theory of solvent system, Bronsted and Lowry’s concept, Lewis concept with typical examples, applications, and limitations. Strengths of acids and bases. Ionization of weak acids and bases in aqueous solutions, application of Ostwald’s dilution law, ionization constants, ionic product of water, pH-scale, buffer solutions and their pH values, buffer actions & buffer capacity; hydrolysis of salts.

### Solutions of non-electrolytes:

Colligative properties of the solution, Raoult’s Law, relative lowering of vapor pressure, osmosis and osmotic pressure; elevation of boiling point and depression of freezing point of solvents.

### Chemical kinetics and catalysis:

Order and molecularity of reactions, rate laws and rate equations for the first order and second order reactions; zero order reactions. Parallel and consecutive reactions. Determination of order of reactions. Temperature dependence of reaction rate, an energy of activation. Enthalpy of activation, the entropy of activation, the effect of dielectric constant and ionic strength of reaction rate, kinetic isotope effect; collision theory & transition State Theory of reaction rate, Catalytic Reactions.

### Adsorption and Surface Chemistry:

Physisorption & Chemisorption, adsorption isotherms, Freundlich and Langmuir adsorption isotherm, BET equation, surface area determination, heterogeneous catalysis; colloids, electrical double layer, and colloid stability, electro-kinetic phenomenon; elementary ideas about soaps & detergents, micelles, emulsions.

### Electrochemistry:

Conductance: cell constant, specific conductance and molar conductance. Kohlrausch’s law of independent migration of ions, ion conductance, and ionic mobility. Equivalent and molar conductance at infinite dilution. Ostwald’s dilution law. Debye-Huckel theory. Application of conductance measurement. Conductometric titrations. Determination of transport number by moving boundary method. Types of electrochemical cells, cell reactions, emf and change in free energy, ΔH and ΔS of cell reactions. Nernst equation. Standard cells. Half-cells/electrodes, different types of electrodes. Standard electrode potential and principles of its determination. Types of concentration cells. Liquid junction potential. Glass electrode and determination of pH of a solution. Potentiometric titrations acid-base and redox, electrochemical power sources; primary, secondary and fuel Cells, corrosion and inhibition of corrosion.

### Photochemistry:

Frank-Condon principle and vibrational structure of electronic spectra. Bond dissociation and the principle of determination of dissociation energy. The decay of excited states by radiative and non-radiative paths. Fluorescence and phosphorescence, Jablonsky diagram. Laws of photochemistry: Grotthus-Draper law, Stark-Einstein law of photochemical equivalence and Lambert-Beer’s law; quantum yield and its measurement for a photochemical process, actinometry. Photostationary state. Photosensitized reactions. Kinetics of HI decomposition, H2-Br2 reaction, dimerization of anthracene.

### Quantum Chemistry:

Wave-particle duality, Photoelectric and Compton effects, de Broglie hypothesis. Eigenfunctions and eigenvalues. Uncertainty relation, Expectation value. Hermitian operator. Schrodinger time-independent equation: nature of the equation, acceptability conditions imposed on the wave functions and probability interpretations of the wave function. Schrodinger equation for the one-dimensional box and its solution. Comparison with free particle eigenfunctions and eigenvalues.

### Basic principles and application of spectroscopy:

Electromagnetic radiation, interaction with atoms and molecules and quantization of different forms of energies. The condition of resonance and energy absorption for various types of spectra; origin of atomic spectra, spectra of hydrogen atoms, many electron atoms, spin and angular momentum. Rotational spectroscopy of diatomic molecules: rigid rotor model, selection rules, spectrum, characteristic features of spectral lines. Determination of bond length, an effect of isotopic substitution. Vibrational spectroscopy of diatomic molecules: Simple Harmonic Oscillator model, selection rules, Raman Effect. Characteristic features and conditions of Raman activity with suitable illustrations. Rotational and vibrational Raman spectra.

### UV Spectra:

Electronic transition (σ−σ*, n-σ*, π-π* and n-π*), relative positions of λmax considering the conjugative effect, steric effect, solvent effect, redshift (bathochromic shift), blue shift (hypsochromic shift), hyperchromic effect, hypochromic effect (typical examples). IR Spectra: Modes of molecular vibrations, application of Hooke’s law, characteristic stretching frequencies of O-H, N-H, C-H, C-D, C=C, C=N, C=O functions; factors affecting stretching frequencies.

### PMR Spectra:

Nuclear spin, NMR active nuclei, the principle of proton magnetic resonance, equivalent and non-equivalent protons, chemical shift), shielding/deshielding of protons, up-field, and down-field shifts. NMR peak area, diamagnetic anisotropy, relative peak positions of different kinds of protons, substituted benzenes.