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.
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); Real gases, deviation from Ideal
behaviour, compressibility factor and van der Waals equation.
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; 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(only up to Atomic Numbers 30),
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.
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.
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: Electrochemistry
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 8: 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 9: d and f Block Elements
General introduction, electronic configuration, occurrence and characteristics of transition
metals, general trends in properties of the first-row transition metals – metallic character,
ionization enthalpy, oxidation states, ionic radii, colour, catalytic property, magnetic
properties, interstitial compounds, alloy formation, preparation and properties of K2Cr2O7 and
KMnO4.
Lanthanoids - Electronic configuration, oxidation states, chemical reactivity and lanthanoid
contraction and its consequences.
Actinoids - Electronic configuration, oxidation states and comparison with lanthanoids.
Unit 10: Coordination Compounds
Introduction, ligands, coordination number, colour, magnetic properties and shapes, IUPAC
nomenclature of mononuclear coordination compounds. Bonding, Werner's theory, VBT, and CFT;
structure and stereoisomerism, importance of coordination compounds (in qualitative analysis,
extraction of metals and biological system).
Unit 11: Haloalkanes and Haloarenes.
Haloalkanes: Nomenclature, nature of C–X bond, physical and chemical properties, optical
rotation mechanism of substitution reactions. Haloarenes: Nature of C–X bond, substitution
reactions (Directive influence of halogen in monosubstituted compounds only). Uses and
environmental effects of - dichloromethane, trichloromethane, tetrachloromethane, iodoform,
freons, DDT.
Unit 12: Alcohols, Phenols and Ethers
Alcohols: Nomenclature, methods of preparation, physical and chemical properties (of primary
alcohols only), identification of primary, secondary and tertiary alcohols, mechanism of
dehydration, uses with special reference to methanol and ethanol. Phenols: Nomenclature, methods
of preparation, physical and chemical properties, acidic nature of phenol, electrophillic
substitution reactions, uses of phenols. Ethers: Nomenclature, methods of preparation, physical
and chemical properties, uses.
Unit 13: Aldehydes, Ketones and Carboxylic Acids
Aldehydes and Ketones: Nomenclature, nature of carbonyl group, methods of preparation, physical
and chemical properties, mechanism of nucleophilic addition, reactivity of alpha hydrogen in
aldehydes, uses. Carboxylic Acids: Nomenclature, acidic nature, methods of preparation, physical
and chemical properties; uses.
Unit 14: Amines
Amines: Nomenclature, classification, structure, methods of preparation, physical and chemical
properties, uses, identification of primary, secondary and tertiary amines. Diazonium salts:
Preparation, chemical reactions and importance in synthetic organic chemistry.
Unit 15: Biomolecules
Carbohydrates - Classification (aldoses and ketoses), monosaccahrides (glucose and fructose),
D-L configuration oligosaccharides (sucrose, lactose, maltose), polysaccharides (starch,
cellulose, glycogen); Importance of carbohydrates. Proteins -Elementary idea of - amino acids,
peptide bond, polypeptides, proteins, structure of proteins - primary, secondary, tertiary
structure and quaternary structures (qualitative idea only), denaturation of proteins; enzymes.
Hormones - Elementary idea excluding structure. Vitamins - Classification and functions. Nucleic
Acids: DNA and RNA.
Unit 16: Hydrocarbons
Classification, isomerism, IUPAC nomenclature, general methods of preparation, properties and
reactions. Alkanes - Conformations: Sawhorse and Newman projections (of ethane); Mechanism of
halogenation of alkanes. Alkenes - Geometrical isomerism; Mechanism of electrophilic addition:
addition of hydrogen, halogens, water, hydrogen halides (Markownikoff’s and peroxide effect);
Ozonolysis and polymerization.
Alkynes - Acidic character; Addition of hydrogen, halogens, water and hydrogen halides;
Polymerization. Aromatic hydrocarbons - Nomenclature, benzene - structure and aromaticity;
Mechanism of electrophilic substitution: halogenation, nitration, Friedel – Craft’s alkylation
and acylation.sis
Unit 17: Organic Compounds Containing Halogens
Classification, isomerism, IUPAC nomenclature, general methods of preparation, properties and
reactions. Alkanes - Conformations: Sawhorse and Newman projections (of ethane); Mechanism of
halogenation of alkanes. Alkenes - Geometrical isomerism; Mechanism of electrophilic addition:
addition of hydrogen, halogens, water, hydrogen halides (Markownikoff’s and peroxide effect);
Ozonolysis and polymerization.
Unit 18: Chemistry in Everyday Life
Chemicals in medicines - Analgesics, tranquilizers, antiseptics, disinfectants, antimicrobials,
antifertility drugs, antibiotics, antacids, antihistamins - their meaning and common examples.
Chemicals in food - Preservatives, artificial sweetening agents - common examples. Cleansing
agents - Soaps and detergents, cleansing action.
Unit 19: Equilibrium
Equilibrium in physical and chemical processes, dynamic nature of equilibrium, law of mass
action, equilibrium constant, factors affecting equilibrium – Le Chatelier's principle, ionic
equilibrium- ionization of acids and bases, strong and weak electrolytes, degree of ionization,
ionization of poly basic acids, acid strength, concept of pH, hydrolysis of salts (elementary
idea), buffer solution, Henderson Equation, solubility product, common ion effect (with
illustrative examples).
Unit 20: Redox Reactions
Concept of oxidation and reduction, redox reactions, oxidation number, balancing redox
reactions, in terms of loss and gain of electrons and change in oxidation number, applications
of redox reactions.
Unit 21: Organic Chemistry
Some Basic Principles and Techniques General introduction, methods of purification, qualitative
and quantitative analysis, classification and IUPAC nomenclature of organic compounds.
Electronic displacements in a covalent bond: inductive effect, electrometric effect, resonance
and hyper conjugation. Homolytic and heterolytic fission of a covalent bond: free radicals,
carbocations, carbanions, electrophiles and nucleophiles, types of organic reactions
