JEE Main 2026 Chemistry Syllabus: Download Latest PDF (Free), Topic-Wise Weightate & More

Some Basic Concepts in Chemistry 

Matter and its Nature, Dalton’s Atomic Theory; Concept of Atom, Molecule, Element and Compound; Laws of Chemical Combination: Atomic and Molecular Masses, Mole Concept, Molar Mass, Percentage Composition, Empirical and Molecular Formulae; Chemical Equations and Stoichiometry. 

Atomic Structure 

Thomson and Rutherford's Atomic Models and their Limitations, Nature of Electromagnetic Radiation, Photoelectric Effect, Spectrum 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 and its important features.

Concept of atomic orbitals as one-electron wave functions, Variation of t|/ and \|/2 with r for Is 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 filled orbitals.  

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.

The second law of thermodynamics - Spontaneity of processes, AS of the universe and AG of the system as criteria for spontaneity, AG” ( Standard Gibbs energy change) and equilibrium constant.

Chemical Bonding and Molecular Structure 

Kossel-Lewis approach to chemical bond formation, the 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, 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.

Solutions 

Different methods for expressing the concentration of solution - molality, molarity, mole fraction, percentage, vapour pressure of solutions and Raoult’s Law - ideal and non-ideal solutions, vapour pressure - composition.

Colligative properties of dilute solutions - relative lowering of vapour pressure, depression of freezing point, the elevation of boiling point and osmotic pressure, and Determination of molecular mass using colligative properties. Abnormal value of molar mass, Van’t Hoff factor and its significance. 

Equilibrium 

Meaning of equilibrium, is the concept of dynamic equilibrium.

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

Equilibria involving chemical processes: Law of chemical equilibrium, equilibrium constants (Kp and Kc) and their significance, significance of AG and AG" 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, 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 Electro - Chemistry 

Electronic concepts of oxidation and reduction, redox reactions, oxidation number, rules for assigning oxidation number, and balancing of redox reactions. 

Electrolytic and metallic conduction, conductance in electrolytic solutions, 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. 

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 constant and its units, differential and integral forms of zero and first-order reactions, their characteristics and half-lives, effect of temperature on the rate of reactions - Arrhenius theory, activation energy and its calculation, collision theory of bimolecular gaseous reactions.

Transition Elements and Coordinate Geometry 

3 

12 

9.9%

Periodic Table and Representative Elements 

3

12

9.9%

Thermodynamics and Gaseous State 

2

8

6.6%

Atomic Structure 

2

8

6.6%

Chemical Bonding 

2

8

6.6%

Solid-State and Surface Chemistry 

2

8

6.6%

Nuclear Chemistry and Environment 

2

8

6.6%

Chemical and Ionic Equilibrium 

2

8

6.6%

Redox Reaction 

1

4

3.3%

Electrochemistry 

1

4

3.3%

Mole Concept 

1

4

3.3% 

Solution and Colligative Properties 

1

4

3.3% 

Chemical Kinetics 

1

4

3.3%

Stereochemistry 

1

4

3.3%

General Organic Chemistry 

1

4

3.3%

Alkyl Halides 

1

4

3.3%

Hydrocarbon 

1

4

3.3%

Aromatic Compounds 

1

4

3.3% 

Carbohydrates, Amino Acids and Polymers 

1

4

3.3%

Carboxylic Acid and its Derivatives 

1

4

3.3%

NCERT Textbooks (for Class XI & XII) 

Majority of the questions are asked directly from the NCERT Textbook

Modern Approach to Chemical Calculations by R.C. Mukherjee

For practicing the physical chemistry numericals 

Organic Chemistry by OP Tandon 

The topics are explained in detail

Concept of Physical Chemistry by P Bahadur 

Good quality of numericals 

Concise Inorganic Chemistry by JD Lee 

Excellent reference book on Inorganic Chemistry 

Physical Chemistry by P.W. Atkins 

For practising 

Organic Chemistry by Morrison & Boyd

For practising 

Atomic Structure

Thompson and Rutherford atomic models and their limitations

Chemical Thermodynamics

Third law of thermodynamics

p-Block Elements

Group-wise study, of which only the following topics are deleted:

• Trends in chemical & physical properties
• Anomalous behaviour 

Some Basic Concepts in Chemistry

Physical quantities and their measurements in Chemistry

• Precision and accuracy
• Significant Figures SI Units
• Dimensional Analysis

Chemistry in Everyday Life

Full Chapter Deleted

Environmental Chemistry

Full Chapter Deleted

Gaseous State

Full Chapter Deleted

Hydrogen

Full Chapter Deleted

Metallurgy

Full Chapter Deleted

Polymers

Full Chapter Deleted

s-Block Elements

Full Chapter Deleted

Solid State

Full Chapter Deleted

Surface Chemistry

Full Chapter Deleted