This page gives the details of AIEEE Chemistry Syllabus 2012. This page details the 10 units of AIEEE Chemistry Syllabus which covers various aspects of Chemistry like States of Matter, Atomic Structure, Chemical Bonding and Solutions
AIEEE Chemistry Syllabus 2012 Units 1-10
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
dielectricproperties
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
colligativeproperties; 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; Corrosion and its prevention.
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.Catalysis -
Homogeneous and heterogeneous, activity and selectivity of solid
catalysts, enzyme catalysis and its mechanism.Colloidal state -
distinction among true solutions, colloids and suspensions,
classification of colloids - lyophilic, lyophobic; multi molecular,
macromolecular and associated colloids (micelles), preparation
andproperties of colloids - Tyndall effect, Brownian movement,
electrophoresis, dialysis, coagulation and flocculation; Emulsions and
their characteristics.
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