WBJEE Exam 2026: Application, Syllabus, Result & Counselling

hemistry: Unit 01 – Atoms, molecules, and chemical arithmetic

• Dalton’s atomic theory; Gay Lussac’s law of gaseous volume; Avogadro’s hypothesis and its applications
• Atomic mass; molecular mass; equivalent weight; valency; gram atomic weight; gram molecular weight; gram equivalent weight and mole concept; chemical formulae; balanced chemical equations
• Calculations (based on mole concept) involving common oxidation-reduction, neutralization, and displacement reactions; concentration in terms of mole fraction, molarity, molality, and normality
• Percentage composition, empirical formula, and molecular formula; numerical problems

Chemistry: Unit 02 – Atomic structure

• Concept of nuclear atom-electron, proton, and neutron (charge and mass), atomic number
• Rutherford’s model and its limitations; extra nuclear structure; line spectra of hydrogen atom
• Quantization of energy (Planck’s equation E = hν); Bohr’s model of hydrogen atom and its limitations, Sommerfeld’s modifications (elementary idea); the four quantum numbers
• Ground state electronic configurations of many electron atoms and monatomic ions; the Aufbau principle; Pauli’s exclusion principle and Hund’s rule
• Dual nature of matter and light, De Broglie’s relationship, uncertainty principle; the concept of atomic orbitals, shapes of s, p, and d orbitals (pictorial approach)

Chemistry: Unit 03 – Radioactivity and nuclear chemistry

• Radioactivity α-, β-, γ rays, and their properties; artificial transmutation; rate of radioactive decay, decay constant, half-life and average age life period of radio-elements; units of radioactivity; numerical problems
• Stability of the atomic nucleus-effect of neutron-proton (n / p) ratio on the modes of decay; group displacement law, radioisotopes and their uses (C, P, Co, and I as examples) isobars and isotones (definition and examples)
• Elementary idea of nuclear fission and fusion reactions

Chemistry: Unit 04 – The periodic table and chemical families

• Modern periodic law (based on atomic number); modern periodic table based on electronic configurations, groups (Gr. 1-18) and periods
• Types of elements-representative (s-block and p-block), transition (d-block) elements and inner transition (f-block/ lanthanides and actinides), and their general characteristics
• Periodic trends in physical and chemical properties-atomic radii, valency, ionization energy, electron affinity, electronegativity, metallic character, acidic, and basic characters of oxides and hydrides of the representative elements (up to Z = 36)
• Position of hydrogen and the noble gases in the periodic table; diagonal relationships

Chemistry: Unit 05 – Chemical bonding and molecular structure

• Valence electrons, the octet rule, electrovalent, covalent, and coordinate covalent bonds with examples; properties of electrovalent and covalent compounds
• Limitations of octet rule (examples); Fajans rule
• Directionality of covalent bonds, shapes of polyatomic molecules (examples); concept of hybridization of atomic orbitals (qualitative pictorial approach): sp, sp2, sp3, and dsp2
• Molecular orbital energy diagrams for homonuclear diatomic species-bond order and magnetic properties
• Valence shell electron pair repulsion (VSEPR) concept (elementary idea)-shapes of molecules
• Concept of resonance (elementary idea), resonance structures (examples)
• Elementary idea about electronegativity, bond polarity and dipole moment, inter-and intra-molecular hydrogen bonding, and its effects on physical properties (mp, bp, and solubility); hydrogen bridge bonds in diborane

Chemistry: Unit – 06 Coordination compounds

• Introduction, double salts and complex salts, coordination compounds (examples only), Werner’s theory, coordination number (examples of coordination number 4 and 6 only), colour, magnetic properties, and shapes
• IUPAC Nomenclature of mononuclear coordination compounds

Chemistry: Unit 07 – Solid state

• Classification of solids based on different binding forces: Molecular, ionic, covalent, and metallic solids, amorphous, and crystalline solids (elementary idea)
• Unit cell in two dimensional and three dimensional lattices, calculation of density of unit cell, packing in solids, packing efficiency, voids, number of atoms per unit cell in a cubic unit cell, point defects, electrical, and magnetic properties
• Band theory of metals, conductors, semiconductors, and insulators and n and p type semiconductors

Chemistry: Unit 08 – Liquid state

• Vapour pressure, viscosity, and surface tension (qualitative idea only, no mathematical derivations)

Chemistry: Unit 09 – Gaseous state

• Measurable properties of gases
• Boyle’s law and Charles law, absolute scale of temperature, kinetic theory of gases, ideal gas equation-average, root mean square and most probable velocities, and their relationship with temperature
• Dalton’s law of partial pressure, Graham’s law of gaseous diffusion
• Deviations from ideal behaviour
• Liquefaction of gases, real gases, Van Der Waals equation; numerical problems

Chemistry: Unit 10 – Chemical energetics and chemical dynamics

• Chemical energetics-conservation of energy principle, energy changes in physical and chemical transformations
• First law of thermodynamics; internal energy, work, and heat, pressure-volume work; enthalpy
• Internal energy change (ΔE) and enthalpy change (ΔH) in a chemical reaction
• Hess’s law and its applications (numerical problems)
• Heat of reaction, fusion, and vaporization; second law of thermodynamics; entropy; free energy; criterion of spontaneity
• Third law of thermodynamics (brief introduction)
• Chemical equilibrium-the law of mass action, dynamic nature of chemical equilibrium
• Equilibrium constants, Le Chatelier’s principle
• Equilibrium constants of gaseous reactions (Kp and Kc) and relation between them (examples)
• Significance of ΔG and ΔG°
• Chemical dynamics-factors affecting the rate of chemical reactions (concentration, pressure, temperature, catalyst), concept of collision theory
• Arrhenius equation and concept of activation energy
• Order and molecularity (determination excluded); first order reactions, rate constant, half-life (numerical problems), examples of first order and second order reactions

Chemistry: Unit 11 – Physical chemistry of solutions

• Colloidal solutions: Differences from true solutions; hydrophobic and hydrophilic colloids (examples and uses); coagulation and peptization of colloids; dialysis and its applications; Brownian motion; Tyndall effect and its applications
• Colloidal solutions: Elementary idea of emulsion, surfactant, and micelle
• Electrolytic solutions: Specific conductance, equivalent conductance, ionic conductance, Kohlrausch’s law, Faraday’s laws of electrolysis, applications. Numerical problems
• Non-electrolytic solutions: Types of solution, vapour pressure of solutions; Raoult’s law; colligative properties-lowering of vapour pressure, elevation of boiling point, depression of freezing point
• Non-electrolytic solutions: Osmotic pressure and their relationships with molecular mass (without derivations); numerical problems

Chemistry: Unit 12 – Ionic and redox equilibrium

• Ionic equilibria: Ionization of weak electrolytes, Ostwald’s dilution law; ionization constants of weak acids and bases, ionic product of water, the pH-scale, pH of aqueous solutions of acids and bases; buffer solutions
• Ionic equilibria: Buffer action and Henderson equation
• Ionization constants of weak acids and bases, ionic product of water, the pH-scale, pH of aqueous solutions of acids and bases; buffer solutions, buffer action and Henderson equation
• Acid-base titrations, acid-base indicators (structures not required)
• Hydrolysis of salts (elementary idea), solubility product, common ion effect (no numerical problems)

Chemistry: Unit 13 – Redox equilibrium

• Oxidation-reduction reactions as electron transfer processes, oxidation numbers, balancing of redox reactions by oxidation number and ion-electron methods
• Standard electrode potentials (E°), electrochemical series, feasibility of a redox reaction
• Significance of Gibb’s equation: ΔG° = – nFΔE° (without derivation), no numerical problems
• Redox titrations with (examples); Nernst equations (numerical problems)

Chemistry: Unit 14 – Hydrogen

• Position of hydrogen in periodic table, occurrence, isotopes, preparation, properties, and uses of hydrogen, hydrides-ionic covalent and interstitial; physical and chemical properties of water, heavy water, hydrogen peroxide-preparation
• Reactions and structure and use; hydrogen as a fuel

Chemistry: Unit 15 – Chemistry of non-metallic elements and their compounds

• Carbon: Occurrence, isotopes, allotropes (graphite, diamond, fullerene); CO and CO₂ production, properties and uses
• Nitrogen and phosphorus: Occurrence, isotopes, allotropes, isolation from natural sources and purification, reactivity of the free elements. Preparation, properties, reactions of NH₃, PH₃, NO, NO₂, HNO₂, HNO₃, P₄O₁₀, H₃PO₃, and H₃PO₄
• Oxygen and sulphur: Occurrence, isotopes, allotropic forms, isolation from natural sources and purification, properties and reactions of the free elements. Water, unusual properties of water, heavy water (production and uses)
• Oxygen and sulphur: Hydrogen peroxide and ozone (production, purification, properties, and uses)
• Halogens: Comparative study, occurrence, physical states, and chemical reactivities of the free elements, peculiarities of fluorine and iodine; hydracids of halogens (preparation, properties, reactions, and uses), interhalogen compounds (examples)
• Halogens: Oxyacids of chlorine

Chemistry: Unit 16 – Chemistry of metals

• General principles of metallurgy-occurrence, concentration of ores, production and purification of metals, mineral wealth of India
• Typical metals (Na, Ca, Al, Fe, Cu, and Zn)-occurrence, extraction, purification (where applicable), properties and reactions with air, water, acids, and nonmetals
• Manufacture of steels and alloy steel (Bessemer, open-hearth, and LD process)
• Principles of chemistry involved in electroplating, anodizing, and galvanizing
• Preparation and Properties of K₂Cr₂O₇ and KMnO₄
• Lanthanoids-electronic configuration, oxidation states, chemical reactivity, and lanthanoid contraction and its consequences
• Actinoids-electronic configuration, oxidation states and comparison with lanthanides

Chemistry: Unit 17 – Chemistry in industry

• Large scale production (including physicochemical principles where applicable, omitting technical details) and uses of sulphuric acid (contact process), ammonia (Haber’s process), nitric acid (Ostwald’s process)
• Sodium bicarbonate, and sodium carbonate (Solvay process)

Chemistry: Unit 18 – Polymers

• Natural and synthetic polymers, methods of polymerization (addition and condensation), copolymerization, some important polymers-natural and synthetic like polythene, nylon polyesters, bakelite, rubber
• Biodegradable and non-Biodegradable polymers

Chemistry: Unit 19 – Surface chemistry

• Adsorption-physisorption and chemisorption, factors affecting adsorption of gases on solids, catalysis, homogenous and heterogenous activity, and selectivity; enzyme catalysis colloidal state distinction between true solutions, colloids and suspension
• Lyophilic, lyophobic multimolecular and macromolecular colloids; properties of colloids; Tyndall effect, Brownian movement, electrophoresis, coagulation, emulsion-types of emulsions

Chemistry: Unit 20 – Environmental chemistry

• Common modes of pollution of air, water, and soil
• Ozone layer, ozone hole-important chemical reactions in the atmosphere, smog; major atmospheric pollutants; greenhouse effect; global warming pollution due to industrial wastes, green chemistry as an alternative tool for reducing pollution
• Strategies for control of environment pollution

Chemistry: Unit 21 – Chemistry of carbon compounds

• Hybridization of carbon: σ- and π-bonds
• Isomerism-constitutional and stereoisomerism; geometrical and optical isomerism of compounds containing up to two asymmetric carbon atoms
• IUPAC nomenclature of simple organic compounds-hydrocarbons, mono and bifunctional molecules only (alicyclic and heterocyclic compounds excluded)
• Conformations of ethane and n-butane (Newman projection only)
• Electronic effects: Inductive, resonance, and hyper conjugation
• Stability of carbocation, carbanion, and free radicals; rearrangement of carbocation; electrophiles and nucleophiles, tautomerism in β-dicarbonyl compounds, acidity and basicity of simple organic compounds Chemistry: Unit 22- Compounds
• Alkanes: Preparation from alkyl halides and carboxylic acids; reactions-halogenation and combustion
• Alkenes and alkynes: Preparation from alcohols; formation of Grignard reagents and their synthetic applications for the preparation of alkanes, alcohols, aldehydes, ketones, and acids; SN1 and SN2 reactions (preliminary concept)
• Alkenes and alkynes: Markownikoff’s and anti-Markownikoff’s additions; hydroboration; oxymercuration-demercuration, reduction of alkenes and alkynes (H₂/ Lindlar catalyst and Na in liquid NH₃), metal acetylides

Chemistry: Unit 23 – Haloalkanes and Haloarenes

• Haloalkanes-preparation from alcohols; nomenclature, nature of C-X bond, physical and chemical properties, mechanism of substitution reactions, optical rotation
• Formation of Grignard reagents and their synthetic applications for the preparation of alkanes, alcohols, aldehydes, ketones, and acids; SN1 and SN2 reactions (preliminary concept)
• Uses and environmental effects of-dichloromethane, trichloromethane, tetrachloromethane, iodoform, freons, DDT

Chemistry: Unit 24 – Alcohols

• Preparation of alcohols from carbonyl compounds and esters
• Reaction-dehydration, oxidation, esterification, reaction with sodium, ZnCl₂/HCl, phosphorus halides
• Ethers: Preparation by Williamson’s synthesis; cleavage with HCl and HI
• Aldehydes and ketones: Preparation from esters, acid chlorides, gem-dihalides, Ca-salt of carboxylic acids
• Reaction: Nucleophilic addition with HCN, hydrazine, hydroxyl amines, semi carbazides, alcohols; aldol condensation, Clemmensen and Wolff-Kishner reduction, haloform, Cannizzaro, and Wittig reactions
• Carboxylic acids: Hydrolysis of esters (mechanism excluded) and cyanides; Hunsdiecker and HVZ reactions
• Aliphatic amines: Preparation from nitro, cyano, and amido compounds. Distinction of 1°, 2°, and 3° amines (Hinsberg method); reaction with HNO₂; carbylamine reaction

Chemistry: Unit 25 – Aromatic compounds

• Benzene-Kekule structure, aromaticity, and Hückel rule
• Electrophilic substitution-halogenation, sulfonation, nitration, Friedel Crafts reaction, ozonolysis
• Directive influence of substituents in monosubstituted benzenes
• Carcinogenicity and toxicity
• Amines-preparation from reduction of nitro compounds; formation of diazonium salts and their stability; replacement of diazonium group with H, OH, X (halogen), CN and NO₂, diazo coupling and reduction
• Haloarenes-nature of C-X bond, substitution reactions; nucleophilic substitution, cine substitution (excluding mechanism, directive influence of halogen in monosubstituted compounds only)
• Phenols-halogenation, sulfonation, nitration, Reimer-Tiemann, and Kolbe reactions
• Aromatic aldehydes-preparation by Gattermann, Gattermann-Koch, Rosenmund, and Stephen’s method
• Reactions-Perkin, benzoin, and Cannizzaro

Chemistry: Unit 26 – Application oriented chemistry

• Main ingredients, their chemical natures (structures excluded) and their side effects, if any, of common antiseptics, analgesics, antacids, vitamin-C

Chemistry: Unit 27 – Introduction to biomolecules

• Carbohydrates-pentoses and hexoses
• Distinctive chemical reactions of glucose
• Aminoacids-glycine, alanine, aspartic acid, cysteine (structures)
• Zwitterion structures of amino acids, peptide bond
• ADP and ATP-structures and role in bioenergetics; nucleic acids-DNA and RNA skeleton structures
• Names of essential elements in biological system

Chemistry: Unit 28 – Principles of qualitative analysis

• Detection of water soluble non-interfering acid and basic radicals by dry and wet tests from among: (i) Acid radicals: Cl⁻, S²⁻, SO₄²⁻, NO₃⁻, CO₃²⁻ (ii) Basic radicals: Cu²⁺, Al³⁺, Fe³⁺, Fe²⁺, Zn²⁺, Ca²⁺, Mg²⁺, Na⁺, NH₄⁺
• Detection of special elements (N, Cl, Br, I, and S) in organic compounds by chemical tests
• Identification of functional groups in: Phenols, aromatic amines, aldehydes, ketones, and carboxylic acids