Syllabus All India Engineering/Architecture Entrance
Examination 2010
CHEMISTRY
SECTION-A : PHYSICAL CHEMISTRY
UNIT 1: Some Basic conceptS IN CHEMISTRY
Matter and its nature, Dalton’s atomic theory; Concept of
atom, molecule, element and compound; Physical quantities and their measurements
in Chemistry, precision and accuracy, significant figures, S.I. Units,
dimensional analysis; Laws of chemical combination; Atomic and molecular masses,
mole concept, molar mass, percentage composition, empirical and molecular
formulae; Chemical equations and stoichiometry.
UNIT 2: States of Matter
Classification of matter into solid, liquid and gaseous states.
Gaseous State:
Measurable properties of gases; Gas laws - Boyle’s law, Charle’s law, Graham’s
law of diffusion, Avogadro’s law, Dalton’s law of partial pressure; Concept of
Absolute scale of temperature; Ideal gas equation, Kinetic theory of gases (only
postulates); Concept of average, root mean square and most probable velocities;
Real gases, deviation from Ideal behaviour, compressibility factor, van der
Waals equation, liquefaction of gases, critical constants.
Liquid State: Properties of liquids - vapour pressure,
viscosity and surface tension and effect of temperature on them (qualitative
treatment only).
Solid State: Classification of solids: molecular, ionic, covalent and
metallic solids, amorphous and crystalline solids (elementary idea); Bragg’s Law
and its applications; Unit cell and lattices, packing in solids (fcc, bcc and
hcp lattices), voids, calculations involving unit cell parameters, imperfection
in solids; Electrical, magnetic and dielectric properties.
UNIT 3: Atomic Structure
Discovery of sub-atomic particles (electron, proton and
neutron); Thomson and Rutherford atomic models and their limitations; Nature of
electromagnetic radiation, photoelectric effect; Spectrum of hydrogen atom, Bohr
model of hydrogen atom - its postulates, derivation of the relations for energy
of the electron and radii of the different orbits, limitations of Bohr’s model;
Dual nature of matter, de-Broglie’s relationship, Heisenberg uncertainty
principle. Elementary ideas of quantum mechanics, quantum mechanical model of
atom, its important features, * and *2, concept of atomic orbitals as one
electron wave functions; Variation of * and * 2 with r for 1s and 2s orbitals;
various quantum numbers (principal, angular momentum and magnetic quantum
numbers) and their significance; shapes of s, p and d - orbitals, electron spin
and spin quantum number; Rules for filling electrons in orbitals – aufbau
principle, Pauli’s exclusion principle and Hund’s rule, electronic configuration
of elements, extra stability of half-filled and completely filled orbitals.
UNIT 4: Chemical Bonding and Molecular Structure Kossel -
Lewis approach to chemical bond formation, concept of ionic and covalent
bonds.
Ionic Bonding: Formation of ionic bonds, factors affecting the formation of
ionic bonds; calculation of lattice enthalpy.
Covalent Bonding: Concept of electronegativity, Fajan’s rule, dipole moment;
Valence Shell Electron Pair Repulsion (VSEPR) theory and shapes of simple
molecules.
Quantum mechanical approach to covalent bonding:
Valence bond theory - Its important features, concept of hybridization involving
s, p and d orbitals; Resonance.
Molecular Orbital Theory - Its important features, LCAOs, types of molecular
orbitals (bonding, antibonding), sigma and pi-bonds, molecular orbital
electronic configurations of homonuclear diatomic molecules, concept of bond
order, bond length and bond energy.
Elementary idea of metallic bonding. Hydrogen bonding and its
applications.
UNIT 5: CHEMICAL THERMODYNAMICS Fundamentals of
thermodynamics: System and surroundings, extensive and intensive properties,
state functions, types of processes.
First law of thermodynamics - Concept of work, heat
internal energy and enthalpy, heat capacity, molar heat capacity; Hess’s law of
constant heat summation; Enthalpies of bond dissociation, combustion, formation,
atomization, sublimation, phase transition, hydration, ionization and solution.
Second law of thermodynamics- Spontaneity of
processes; DS of the universe and DG of the system as criteria for spontaneity,
DGo (Standard Gibbs energy change) and equilibrium constant. UNIT 6: SOLUTIONS
Different methods for expressing concentration of solution - molality, molarity,
mole fraction, percentage (by volume and mass both), vapour pressure of
solutions and Raoult’s Law - Ideal and non-ideal solutions, vapour pressure -
composition, plots for ideal and non-ideal solutions; Colligative properties of
dilute solutions - relative lowering of vapour pressure, depression of freezing
point, elevation of boiling point and osmotic pressure; Determination of
molecular mass using colligative properties; Abnormal value of molar mass, van’t
Hoff factor and its significance.
