Full detailed syllabus of JEE Main Chemistry-
JEE Main Chemistry Syllabus
Some Basic Concepts In Chemistry
Matter and its nature, Daltons 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
States Of Matter
Classification of matter into solid, liquid and gaseous states.
Gaseous State: Measurable properties of gases
Gas laws Boyles law, Charles law, Grahams law of diffusion, Avogadros law, Daltons 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)
Braggs 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 Bohrs model
Dual nature of matter, de-Broglies 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, Paulis exclusion principle and Hunds rule, electronic configuration of elements, extra stability of half-filled and completely filled orbitals.
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, Fajans 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
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.
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
Hesss 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 Raoults 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, vant Hoff factor and its significance
Meaning of equilibrium, concept of dynamic equilibrium.
Equilibria involving physical processes: Solid -liquid, liquid gas and solid gas equilibria, Henrys 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 Chateliers principle.
Ionic equilibrium: Weak and strong electrolytes, ionization of electrolytes, various concepts of acids and bases (Arrhenius, Bronsted Lowry and Lewis) and their ionization, acid-base equilibria (including multi stage 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.
Redox Reactions and Electrochemistry
Electronic concepts of oxidation and reduction, redox reactions, oxidation number, rules for assigning oxidation number, balancing of redox reactions.
Electrolytic and metallic conduction,
conductance in electrolytic solutions,
specific and molar conductivities and their variation with concentration
Kohlrauschs law and its applications.