IIT JEE Syllabus 2012:
IIT JEE Syllabus Chemistry Physical chemistry
of atoms and molecules; Dalton’s atomic theory; Mole concept; Chemical
formulae; Balanced chemical equations; Calculations (based on mole
concept) involving common oxidation-reduction, neutralisation, and
displacement reactions; Concentration in terms of mole fraction,
molarity, molality and normality.
Gaseous and liquid states:Absolute
scale of temperature, ideal gas equation; Deviation from ideality , van
der Waals equation; Kinetic theory of gases, average, root mean square
and most probable velocities and their relation with temperature; Law of
partial pressures; Vapour pressure; Diffusion of gases.
Atomic structure and chemical bonding:Bohr
model, spectrum of hydrogen atom, quantum numbers; Wave-particle
duality, de Broglie hypothesis; Uncertainty principle; Qualitative
quantum mechanical picture of hydrogen atom, shapes of s, p and d
orbitals; Electronic configurations of elements (up to atomic number
36); Aufbau principle; Pauli’s exclusion principle and Hund’s rule;
Orbital overlap and covalent bond; Hybridisation involving s, p and d
orbitals only; Orbital energy diagrams for homonuclear diatomic species;
Hydrogen bond; Polarity in molecules, dipole moment (qualitative aspects
only); VSEPR model and shapes of molecules (linear, angular, triangular,
square planar, pyramidal, square pyramidal, trigonal bipyramidal,
tetrahedral and octahedral).
of thermodynamics; Internal energy, work and heat, pressure-volume work;
Enthalpy, Hess’s law; Heat of reaction, fusion and vapourization; Second
law of thermodynamics; Entropy; Free energy; Criterion of spontaneity.
of mass action; Equilibrium constant, Le Chatelier’s principle (effect
of concentration, temperature and pressure); Significance of ΔG and ΔG°
in chemical equilibrium; Solubility product, common ion effect, pH and
buffer solutions; Acids and bases (Bronsted and Lewis concepts);
Hydrolysis of salts.
cells and cell reactions; Standard electrode potentials; Nernst equation
and its relation to ΔG; Electrochemical series, emf of galvanic cells;
Faraday’s laws of electrolysis; Electrolytic conductance, specific,
equivalent and molar conductivity, Kohlrausch’s la w; Concentration
of chemical reactions; Order of reactions; Rate constant; First order
reactions; Temperature dependence of rate constant (Arrhenius equation).
of solids, crystalline state, seven crystal systems (cell parameters a,
b, c, α, β, γ), close packed structure of solids (cubic), packing in
fcc, bcc and hcp lattices; Nearest neighbours, ionic radii, simple ionic
compounds, point defects.
law; Molecular weight determination from lowering of vapour pressure,
elevation of boiling point and depression of freezing point.
concepts of adsorption (excluding adsorption isotherms); Colloids:
types, methods of preparation and general properties; Elementary ideas
of emulsions, surfactants and micelles (only definitions and examples).
isotopes and isobars; Properties of α, β and γ rays; Kinetics of
radioactive decay (decay series excluded), carbon dating; Stability
of nuclei with respect to proton-neutron ratio; Brief discussion on
fission and fusion reactions.
Isolation/preparation and properties of the following non-metals:
Boron, silicon, nitrogen, phosphorus, oxygen, sulphur and halogens;
Properties of allotropes of carbon (only diamond and graphite),
phosphorus and sulphur.
Preparation and properties of the following compounds:Oxides,