NEET Chemistry Syllabus 2026 (Out): Download PDF, Topics-Wise Syllabus

Parameter

Details

Exam Name

NET UG 2026

Exam Level

National level

Conducting Body

National Testing Agency (NTA)

Mode of Exam

Offline

Type of Questions

Multiple-Choice Questions (MCQs)

NEET exam pattern for Chemistry

45 questions carrying 4 marks each

Subject

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NEET 2026 Chemistry

NEET Chemistry Syllabus PDF link

Unit Name

Topics

Unit 1- Some Basic Concepts of 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

Unit 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, the quantum mechanical model of the atom, it's important feature

Concept of atomic orbitals as one-electron wave functions

Variation of 4 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

Hund's rule, electronic configuration of elements, extra stability of half-filled and completely filled orbitals

Unit 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.

Unit 4- Chemical Thermodynamics

Fundamentals of thermodynamics: System and surroundings, extensive and intensive properties, state functions, types of processes.

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 - Spontaneity of processes; AS of the universe and AG of the system as criteria for spontaneity. AG (Standard Gibbs energy change) and equilibrium constant

Unit 5- Solutions

Different methods for expressing the concentration of solution-molality, molarity, mole fraction, percentage (by volume and mass both), the vapour pressure of solutions.

Raoult's Law - Ideal and non-ideal solutions, vapour pressure - composition, plots for ideal and non-ideal solutions;

Colligative properties of dilute solutions - a relative lowering of vapour pressure, depression of 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

Unit 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 (K, and Ke) and their significance, the significance of AG and AG 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 multi stage 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

Unit 7- Redox Reaction 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, 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

Unit 8- 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 law

Rate constant and its units

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

Arrhenius theory

Activation energy and its calculation

Collision theory of bimolecular gaseous reactions (no derivation)

Unit 9: Classification of Elements and Periodicity in Properties

Modem periodic law and present form of the periodic table

s, p, d and f block elements

periodic trends in properties of elements atomic and ionic radii

ionization enthalpy, electron gain enthalpy, valence, oxidation states, and chemical reactivity

Unit 10: p-block Elements

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

Unit 11: d and f-block Elements

Transition Elements General introduction

Electronic configuration, occurrence and characteristics

General trends in properties of the first-row transition elements - physical properties, ionization enthalpy, oxidation states, atomic radii, colour, catalytic behaviour, magnetic properties, complex formation, interstitial compounds, alloy formation

Preparation, properties, and uses of K2Cr2O7, and KMnO4.

Inner Transition Elements

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

Actinoids - Electronic configuration and oxidation states

Unit 12: Co-ordination Compounds

Introduction to coordination compounds.

Werner's theory; ligands, coordination 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)

Unit 13: Purification and Characterization of Organic Compounds

Purification - Crystallization, sublimation, distillation, differential extraction

Chromatography - principles and their applications.

Qualitative analysis - Detection of nitrogen, sulphur, phosphorus, and halogens

Quantitative analysis (basic principles only) - Estimation of carbon, hydrogen, nitrogen, halogens, sulphur, and phosphorus.

Calculations of empirical formulae and molecular formulae

Numerical problems in organic quantitative analysis

Unit 14: Some Basic Principles of Organic Chemistry

Tetravalency of carbon

Shapes of simple molecules - hybridization (s and p)

Classification of organic compounds based on functional groups: and those containing halogens, oxygen, nitrogen, and sulphur

Homologous series

Isomerism - structural and stereoisomerism.

Nomenclature (Trivial and IUPAC)

Covalent bond fission - Homolytic and heterolytic

Free radicals, carbocations, and carbanion

Stability of carbocations and free radicals, electrophiles, and nucleophiles.

Electronic displacement in a covalent bond - Inductive effect, electromeric effect, resonance, and hyperconjugation.

Common types of organic reactions - substitution, addition, elimination, and rearrangement

Unit 15: Hydrocarbons

Classification, isomerism,

IUPAC nomenclature

General methods of preparation, properties, and reactions.

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 halide

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 monosubstituted benzene

Unit 16: Organic Compounds Containing Halogens

General methods of preparation, properties, and reactions

Nature of C-X bond

Mechanisms of substitution reactions. Uses

Environmental effects of chloroform, iodoform freons, and DDT

Unit 17: Organic Compounds Containing Oxygen

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 (Wolf Kishner and Clemmensen)

The acidity of hydrogen. aldol condensation, Cannizzaro reaction. Haloform reaction

Chemical tests to distinguish between aldehydes and Ketones. Carboxylic Acids Acidic strength and factors affecting it

Unit 18: Organic Compounds Containing Nitrogen

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

Unit 19: Biomolecules

General introduction and importance of biomolecules

CARBOHYDRATES - Classification; aldoses and ketoses: monosaccharides (glucose and fructose) and constituent monosaccharides of oligosaccharides (sucrose, lactose, and maltose).

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 – Chemical constitution of DNA and RNA. Biological functions of nucleic acids. Hormones (General introduction)

Unit 20: Principles Related to General Chemistry

Detection of extra elements (Nitrogen, Sulphur, halogens) in organic compounds

Detection of the following functional groups; hydroxyl (alcoholic and phenolic), carbonyl (aldehyde and ketones) carboxyl, and amino groups in organic compounds.

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 analysis: Cations – Pb2+, Cu2+, Al3+, Fe3+ , Zn2+ , Ni2+ , Ca2+ , Ba2+ , Mg2+ , NH+ Anions- CO2−, S 2- ,SO2−, 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 ions with hydrogen peroxide at room temperature.