IIT JEE Main Chemistry Study Materials Chapter Wise

 Section A: Physical 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

• 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

• 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

• 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, concept of atomic orbitals as one electron wave functions
• 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.

• 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.

• 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

• 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

• 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.

• 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.

• 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 ofzero 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).

• 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

• 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

Group – 13 to Group 18 Elements

General Introduction: Electronic configuration and general trends in physical and chemical properties of elements across the periods and down the groups; unique behaviour of the first element in each group.

Groupwise study of the p – block elements

• Group – 13: Preparation, properties and uses of boron and aluminium; properties of boric acid, diborane, boron trifluoride, aluminium chloride and alums.
• Group – 14: Allotropes of carbon, tendency for catenation; Structure & properties of silicates, and zeolites.
• Group – 15: Properties and uses of nitrogen and phosphorus; Allotrophic forms of phosphorus; Preparation, properties, structure and uses of ammonia, nitric acid, phosphine and phosphorus halides, (PCl3, PCl5); Structures of oxides and oxoacids of phosphorus.
• Group – 16: Preparation, properties, structures and uses of ozone; Allotropic forms of sulphur; Preparation, properties, structures and uses of sulphuric acid (including its industrial preparation); Structures of oxoacids of sulphur.
• Group – 17: Preparation, properties and uses of hydrochloric acid; Trends in the acidic nature of hydrogen halides; Structures of Interhalogen compounds and oxides and oxoacids of halogens.
• Group –18: Occurrence and uses of noble gases; Structures of fluorides and oxides of xenon.

• Introduction to co-ordination compounds, Werner’s theory
• ligands, co-ordination number, denticity, chelation; IUPAC nomenclature of mononuclear co-ordination compounds, isomerism
• Bonding-Valence bond approach and basic ideas of Crystal field theory, colour and magnetic properties; Importance of co-ordination compounds (in qualitative analysis, extraction of metals and in biological systems).

• Environmental pollution – Atmospheric, water and soil.
• Atmospheric pollution – Tropospheric and Stratospheric
• Tropospheric pollutants – Gaseous pollutants: Oxides of carbon, nitrogen and sulphur, hydrocarbons; their sources, harmful effects and prevention; Greenhouse effect and Global warming; Acid rain;
• Particulate pollutants: Smoke, dust, smog, fumes, mist; their sources, harmful effects and prevention.
• Stratospheric pollution- Formation and breakdown of ozone, depletion of ozone layer – its mechanism and effects.
• Water Pollution – Major pollutants such as, pathogens, organic wastes and chemical pollutants; their harmful effects and prevention.
• Soil pollution – Major pollutants such as: Pesticides (insecticides,. herbicides and fungicides), their harmful effects and prevention. Strategies to control environmental pollution.

Section C: Organic Chemistry

• Alcohols: Identification of primary, secondary and tertiary alcohols; mechanism of dehydration.
• Phenols: Acidic nature, electrophilic substitution reactions: halogenation, nitration and sulphonation, Reimer – Tiemann reaction.
• Ethers: Structure.
• Aldehyde and Ketones: Nature of carbonyl group
• Nucleophilic addition to >C=O group, relative reactivities of aldehydes and ketones
• Important reactions such as – Nucleophilic addition reactions (addition of HCN, NH3 and its derivatives), Grignard reagent; oxidation; reduction (Wolff Kishner and Clemmensen); acidity of r – hydrogen, aldol condensation, Cannizzaro reaction, Haloform reaction; Chemical tests to distinguish between aldehydes and Ketones.

• General methods of preparation, properties, reactions and uses.
• Amines: Nomenclature, classification, structure, basic character and identification of primary, secondary and tertiary amines and their basic character.
• Diazonium Salts: Importance in synthetic organic chemistry.

• General introduction and classification of polymers, general methods of polymerization-addition and condensation, copolymerization
• Natural and synthetic rubber and vulcanization
• some important polymers with emphasis on their monomers and uses – polythene, nylon, polyester and bakelite.

• General introduction and importance of biomolecules.
• Carbohydrates – Classification: aldoses and ketoses; monosaccharides (glucose and fructose) and constituent monosaccharides of oligosacchorides (sucrose, lactose and maltose).
• Proteins – Elementary Idea of r – amino acids, peptide bond, polypeptides; Proteins: primary, secondary, tertiary and quaternary structure (qualitative idea only), denaturation of proteins, enzymes.
• Vitamins – Classification and functions.
• Nucleic Acids – Chemical constitution of DNA and RNA. Biological functions of nucleic acids.

• Chemistry involved in the preparation of the following: Inorganic compounds: Mohr’s salt, potash alum.
• Organic compounds: Acetanilide, pnitroacetanilide, aniline yellow, iodoform.