CBSE: All India Engineering
Entrance Examinations (AIEEE)
Syllabus: Chemistry - 2012
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
and van der Waals equation.
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:
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.
Unit 7: Equilibrium:
Meaning of equilibrium, concept of dynamic equilibrium.
Equilibria involving physical processes: Solid -liquid, liquid - gas and solid –
gas
equilibria, Henry’s law, general characterics of equilibrium involving physical
processes.
Equilibria involving chemical processes: Law of chemical equilibrium,
equilibrium
constants (Kp and Kc) and their significance, significance of DG and DGo in
chemical equilibria, factors affecting equilibrium concentration, pressure,
temperature, effect of catalyst; Le Chatelier’s principle.
Ionic equilibrium: Weak and strong electrolytes, ionization of electrolytes,
various
concepts of acids and bases (Arrhenius, Br??nsted - Lowry and Lewis) and their
ionization, acid - base equilibria (including multistage ionization) and
ionization
constants, ionization of water, pH scale, common ion effect, hydrolysis of salts
and pH of their solutions, solubility of sparingly soluble salts and solubility
products, buffer solutions.
Unit 8: Redox Reactions and Electrochemistry
Electronic concepts of oxidation and reduction, redox reactions, oxidation
number, rules for assigning oxidation number, balancing of redox reactions.
Eectrolytic and metallic conduction, conductance in electrolytic solutions,
specific and molar conductivities and their variation with concentration:
Kohlrausch’s law and its applications.
Electrochemical cells - Electrolytic and Galvanic cells, different types of
electrodes, electrode potentials including standard electrode potential, half -
cell
and cell reactions, emf of a Galvanic cell and its measurement; Nernst equation
and its applications; Relationship between cell potential and Gibbs’ energy
change; Dry cell and lead accumulator; Fuel cells.
Unit 9 : Chemical Kinetics:
Rate of a chemical reaction, factors affecting the rate of reactions:
concentration, temperature, pressure and catalyst; elementary and complex
reactions, order and molecularity of reactions, rate law, rate constant and its
units, differential and integral forms of zero and first order reactions, their
characteristics and half - lives, effect of temperature on rate of reactions –
Arrhenius theory, activation energy and its calculation, collision theory of
bimolecular gaseous reactions (no derivation).
Unit-10 : Surface Chemistry:
Adsorption- Physisorption and chemisorption and their characteristics, factors
affecting adsorption of gases on solids - Freundlich and Langmuir adsorption
isotherms, adsorption from solutions.
Colloidal state - distinction among true solutions, colloids and suspensions,
classification of colloids - lyophilic, lyophobic; multi molecular,
macromolecular
and associated colloids (micelles), preparation and properties of colloids -
Tyndall effect, Brownian movement, electrophoresis, dialysis, coagulation and
flocculation; Emulsions and their characteristics.
SECTION – B
INORGANIC CHEMISTRY
Unit 11: Classification of Elements and Periodicity in Properties
Modem periodic law and present form of the periodic table, s, p, d and f block
elements, periodic trends in properties of elements atomic and ionic radii,
ionization enthalpy, electron gain enthalpy, valence, oxidation states and
chemical reactivity.
Unit 12: General Principles and Processes of Isolation of Metals
Modes of occurrence of elements in nature, minerals, ores; Steps involved in the
extraction of metals - concentration, reduction (chemical and electrolytic
methods) and refining with special reference to the extraction of Al, Cu, Zn and
Fe; Thermodynamic and electrochemical principles involved in the extraction of
metals.
Unit 13: Hydrogen:
Position of hydrogen in periodic table, isotopes, preparation, properties and
uses of hydrogen; Physical and chemical properties of water and heavy water;
Structure, preparation, reactions and uses of hydrogen peroxide; Hydrogen as a
fuel.
