JEE Main Chemistry Syllabus 2025 – Know Important Topic, Weightage and Preparation Tips

Heisenberg uncertainty principle. Elementary ideas of quantum mechanics, quantum mechanics, the quantum mechanical model of the atom, and its important features. 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 – 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, and extra stability of half-filled and filled orbitals.

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, the 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, the concept of bond order, bond length, and bond energy. Elementary idea of metallic bonding. Hydrogen bonding and its applications.

The 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.

The second law of thermodynamics is the spontaneity of processes; S of the universe and G of the system are criteria for spontaneity: G (Standard Gibbs energy change) and equilibrium constant.

Equilibria involving physical processes: Solid-liquid, liquid – gas and solid-gas equilibria, Henry’s law. General characteristics of equilibrium involving physical processes.

Equilibrium involving chemical processes: Law of chemical equilibrium, equilibrium constants (Kp and Kc) and their significance, the significance of G and G in chemical equilibrium, factors affecting equilibrium concentration, pressure, temperature, the effect of catalyst; Le Chatelier’s 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 multistage ionization) and ionization constants, ionization of water. pH scale, common ion effect, hydrolysis of salts and pH of their solutions, the solubility of sparingly soluble salts and solubility products, buffer solutions

Inner Transition Elements

Lanthanoids – Electronic configuration, oxidation states, and lanthanoid contraction.

Actinoids: Electronic configuration and oxidation states.

Qualitative analysis-Detection of nitrogen, sulfur, phosphorus, and halogens.

Quantitative analysis (basic principles only) – Estimation of carbon, hydrogen, nitrogen, halogens, sulfur, and phosphorus. Calculations of empirical formulae and molecular formulae: Numerical problems in organic quantitative analysis,

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 (Markownikoffs 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, directive influence of the functional group in mono-substituted benzene.

PROTEINS: Elementary Idea of -amino acids, peptide bonds, polypeptides. Proteins: primary, secondary, tertiary, and quaternary structure (qualitative idea only), denaturation of proteins, enzymes.

VITAMINS: Classification and functions.

Nucleic Acids: The chemical constitution of DNA and RNA. Biological functions of nucleic acids.

The chemistry involved in the preparation of the following: Inorganic compounds;

Mohr’s salt, potash alum.

Organic compounds: Acetanilide, p-nitro acetanilide, aniline yellow, iodoform.

The chemistry involved in the titrimetric exercises – Acids, bases, and the use of indicators, oxalic-acid vs KMnO4, Mohr’s salt vs KMnO4

Chemical principles involved in the qualitative salt analysts: Cations – Pb2+, Cu2+, Al3+, Fe3+, Zn2+, Ni2+, Ca2+, Ba2+, Mg2+, NH4 + Anions- CO3 2−, S 2-, SO4 2−, NO3-, NO2-, Cl-, Br-, I- ( Insoluble salts excluded). Chemical principles involved in the following experiments: 1. Enthalpy of solution of CuSO4 2. Enthalpy of neutralization of strong acid and strong base. 3. Preparation of lyophilic and lyophobic sols. 4. Kinetic study of the reaction of iodide ion with hydrogen