NEET Chemistry Syllabus 2025 by NTA (Updated)

Physical Chemistry

Topic

Key Concepts

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 completely filled orbitals.

Ionic Bonding: Formation of ionic bonds, factors affecting the formation of ionic bonds; calculation of lattice enthalpy.

Covalent Bonding: Concept of electronegativity. Fagan’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, atomisation, sublimation, phase transition, hydration, ionisation, and solution.

The second law of thermodynamics – Spontaneity of processes; DS of the universe and DG of the system as criteria for spontaneity. DG° (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 DG and DG° in chemical equilibrium, factors affecting equilibrium concentration, pressure, temperature, the effect of catalyst; Le Chatelier’s principle.

Ionic equilibrium: Weak and strong electrolytes, ionisation of electrolytes, various concepts of acids and bases (Arrhenius. Bronsted – Lowry and Lewis) and their ionisation, acid-base equilibria (including multistage ionisation) and ionisation constants, ionisation of water. pH scale, common ion effect, hydrolysis of salts and pH of their solutions, the solubility of sparingly soluble salts and solubility products, and buffer solutions.

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.

Inorganic Chemistry

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.

Inner Transition Elements

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

Actinoids – Electronic configuration and oxidation states.

Organic Chemistry

Qualitative analysis – Detection of nitrogen, sulphur, phosphorus, and halogens.

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

Calculations of Empirical Formulae and Molecular Formulae: Numerical problems in organic quantitative analysis,

Nomenclature (Trivial and IUPAC)

Covalent bond fission – Homolytic and heterolytic: free radicals, carbocations, and carbanions; 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.

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 polymerisation.

Alkynes – Acidic character: Addition of hydrogen, halogens, water, and hydrogen halides: Polymerisation.

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.

Uses; Environmental effects of chloroform, iodoform freons, and DDT

ALCOHOLS, PHENOLS,AND ETHERS

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. , and its derivatives), Grignard reagent; oxidation: reduction (Wolf Kishner and Clemmensen); the acidity of a-hydrogen. aldol condensation, Cannizzaro reaction. Haloform reaction, Chemical tests to distinguish between aldehydes and Ketones.

Carboxylic Acids

Acidic strength and factors affecting it,

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

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

PROTEINS – Elementary Idea of a-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)

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, Mohr’s salt vs  

Chemical principles involved in the qualitative salt analysis:

Cations: Pb2+, Cu2+, Al3+, Fe3+, Zn2+, Ni2+, Ca2+, Ba2+, Mg2+, NH4+

Anions: CO32−, S2−, SO42−, NO3−, NO2−, Cl−, Br−, I− (Insoluble salts excluded).

Chemical principles involved in the following experiments:

1. Enthalpy of solution of  

2. Enthalpy of neutralisation 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.

Chapter Name

Physical Chemistry

Inorganic Chemistry

Organic Chemistry