NEET 2026 Chemistry Syllabus PDF - Download NEET Chemistry Syllabus Topic wise

Name of Event

NEET Chemistry Syllabus 2026

Releasing Body

National Testing Agency

Exam Name

NEET UG Exam 2026

Release Format

PDF

Release Mode

Online

Total Number of Questions from Chemistry Subject

50 Questions (45 to be attempted)

Types of Questions

Multiple Choice Questions (MCQs)

Sections in NEET 2026 Question Paper per Subject

Section A and Section B

NEET Chemistry Section Number of Questions

35 Compulsory Questions

NEET Chemistry Section B Number of Questions

15 Questions (Only 10 to be attempted)

Total Marks

180 marks (4 marks per question)

NEET Chemistry Syllabus Weightage

25%

1

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

2

Atomic Structure

• Nature of electromagnetic radiation

• Photoelectric effect

• Spectrum of the hydrogen atom

• Bohr model of a hydrogen atom - its postulates,

• Derivation of the relations for the 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 mechanics

• Quantum mechanical model of the atom, its important features

• Concept of atomic orbitals as one-electron wave functions

• Variation of Y and Y2 with r for ls and 2s orbitals. 

• 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 orbits - Aufbau principle

• Pauli's exclusion principle and Hund's rule

• Electronic configuration of elements

• Extra stability of half-filled and filled orbitals.

3

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.

4

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 solutions

• Second Law of Thermodynamics: Spontaneity of processes: ΔS of the universe and ΔC of the system as criteria for spontaneity. ΔG° (Standard' Gibbs energy change) and equilibrium constant.

5

Solutions

• Different methods for expressing the concentration of solution - molality, molarity, mole fraction

• Percentage (by volume and mass both), the vapor pressure of solutions and Raoult’s law - Ideal and non-ideal solutions, vapor pressure - composition

• Plots for ideal and non-ideal solutions: colligative properties of dilute solutions - a relative lowering of vapor pressure, depression or mass freezing point, the 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.Meaning of equilibrium, the concept of dynamic equilibrium.

6

Equilibrium

• Meaning of equilibrium, 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. 

• Equilibrium Involving Chemical Processes: Law of chemical equilibrium, equilibrium constants (Kp and Kc) and their significance, the significance of ΔG and ΔG° in chemical equilibrium, 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 multistage ionization and ionization constants, ionization constants, ionization of water. pH scale, common ion effect, hydrolysis of salts and pH of their solutions, the solutions, the solubility of sparingly soluble salts and solubility products, and buffer solutions.

7

Redox Reaction and ElectroChemistry

• Electronic Concepts of Oxidation and Reduction, Redox Reaction, Oxidation Number, Rules for assigning oxidation number, balancing of redox reaction. 

• Electrolytic and metallic conduction, conductance in electrolytes 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.

8

Chemical Kinetics

• Rate of a chemical reaction

• Factors affecting the rate of reactions: concentration

• Pressure, temperature, and catalyst 

• Elementary and complex reactions, order and molecularity of reactions

• Rate law and rate constant and its units

• Differential and integral forms of zero and first-order reactions, their characteristics and half-lives, and the effect of temperature on the rate of reactions

• Arrhenius theory, activation energy and its calculation, collision theory of bimolecular gaseous reactions (no derivation).

Physical Chemistry

Atomic Structure

3%

1

Solutions

4%

2

Chemical Bonding and Molecular Structure

6%

2

Chemical Thermodynamics

3%

1

Some Basic Concepts in Chemistry

2%

1

Equilibrium

4%

2

Redox Reactions

6%

3

Chemical Kinetics

4%

2

Inorganic Chemistry

Classification of Elements and Periodicity

4%

2

P Block Elements

7%

3

D and F Block Elements

4%

2

Coordination Compounds

6%

4

Organic Chemistry

Purification and Characterisation of Organic Compounds

2%

1

Organic Compounds Containing Nitrogen

3%

1

Some Basic Principles of Organic Chemistry

5%

2

Organic Compounds Containing Oxygen

4%

2

Hydrocarbons

4%

2

Organic Compounds Containing Halogens

3%

1

Biomolecules

4%

2

Principles Related to Practical Chemistry

2%

1

Some Basic Concepts of Chemistry

Some p-Block Elements

Chemical Bonding and Molecular Structure

Redox Reactions

Equilibrium

Classification of Elements and Periodicity

in Properties

Thermodynamics

Hydrocarbons

Structure of Atom

Organic Chemistry- Some Basic Principles and Techniques

-

-

ElectroChemistry

Solutions

Biomolecules

Organic Compounds Containing Nitrogen

Aldehydes, Ketones and Carboxylic Acids

Alcohols, Phenols, and Ethers

Haloalkanes and Haloarenes

Coordination Compounds

d- and f-Block Elements

p-Block Elements

General Principles & Processes of

Isolation of Elements

Chemical Kinetics

Some Basic Concepts of Chemistry

Concentration Terms

Relation Between Molarity and Normality

Mole Concept

Determination of Formula of Compound

Stoichiometric Calculations

Thermodynamics

P-V Work

Second Law of Thermodynamics

Heat Capacity

Thermochemistry

Chemical Bonding and Molecular Structure

Covalent Character in Ionic Bonds

Geometry or Shapes of Molecules

General Introduction

Polarity of Bonds

Concept of Orbital Overlap in Covalent Bonds

Molecular Orbital Theory (MOT)

Equilibrium

Expressing Hydrogen Ion Concentration

Buffer Solution

Solubility of Sparingly Soluble Salts

Applications of Equilibrium Constant

Equilibrium Constant

Factors Affecting the State of Equilibrium

Hydrocarbons

Stability of Alkene

Chemical Reactions of Alkenes

Aromatic Hydrocarbons

Conformations of Hydrocarbons

Isomerism in Alkenes

Chemical Reactions of Aromatic Hydrocarbons

Principles Related To Practical Organic Chemistry

Volumetric Analysis

Qualitative Salt Analysis

Enthalpy

Analysis of Organic Compounds

Solutions

Colligative Properties

Abnormal Molar Masses

Solubility of Gases in Liquids

Vapour Pressure of Liquid Solutions

Amines

Aldehydes & Ketones: Reduction Reactions

Carboxylic Acids

Aldehydes & Ketones: Nucleophilic Addition Reactions

Aldehydes & Ketones: Oxidation Reactions

Biomolecules

Disaccharides

Proteins

Glucose and Fructose

Glucose: Reaction Due to Open Chain Structure

Nucleic Acids

Coordination Compounds

Coordination Compounds

Isomerism in Coordination Compounds

Ligands

Werner’s Theory

Bonding in Coordination Compounds

The p-Block Elements Part 2

Group-15 Elements

Group-16 Elements

Group-17 Elements

Group-18 Elements