WBJEE Exam 2025: Answer Key (Out), Result Date, Admit Card, Syllabus, Pattern, Question Papers, Cutoff

Physics: Unit 01

• Physical world, measurements, units, and dimensions of physical quantities, dimensional analysis and its applications, error in measurements, significant figures

Physics: Unit 02

• Scalars and vectors, representation of vectors in 3D, dot and cross product, and their applications, elementary differential and integral calculus, time-velocity and relevant graphs, equations of motion with uniform acceleration

Physics: Unit 03

• Newton’s laws of motion, using algebra and calculus, inertial and non inertial frames, conservation of linear momentum with applications, elastic and inelastic collisions, impulse centripetal force, banking of roads, relative velocity
• Projectile motion and uniform circular motion work, power, energy: Work, power, energy Work, work-energy theorem, power, energy, work done by constant and variable forces, PE and KE, conservation of mechanical energy
• Conservative and non conservative forces, PE of a spring, motion of centre of mass, connected systems, friction: Centre of mass of two-particle system, motion of connected system, torque, equilibrium of rigid bodies
• Moments of inertia of simple geometric bodies (2D) [without derivation] conservation of angular momentum, friction and laws of friction

Physics: Unit 04

• Kepler’s laws, (only statement) universal law of gravitation, acceleration due to gravity (g), variation of g, gravitational potential and PE, escape velocity, orbital velocity of satellites, geostationary orbits

Physics: Unit 05

• Elasticity, Hooke’s law, Young’s modulus, bulk modulus, shear, rigidity modulus, Poisson’s ratio elastic potential energy
• Fluid pressure: Pressure due to a fluid column, buoyancy, Pascal’s law, effect of gravity on fluid pressure
• Surface tension: Surface energy, phenomena involving surface tension, angle of contact, capillary rise

Physics: Unit 06

• Coefficient of viscosity, streamline and turbulent motion, Reynold’s number, Stoke’s law, terminal velocity, Bernoulli’s theorem
• Heat and thermal physics: Heat and temperature, thermal expansion of solids, liquids and gases, ideal gas laws, isothermal and adiabatic processes; anomalous expansion of water and its effects, sp
• Heat and thermal physics: Heat capacity, Cp, Cv, calorimetry
• Change of state, specific latent heat capacity
• Heat transfer; conduction, thermal and thermometric conductivity, convection and radiation, Newton's law of cooling, Stefan's law

Physics: Unit 07

• Thermal equilibrium (zeroth law of thermodynamics), heat, work, and internal energy
• 1st law of thermodynamics, isothermal and adiabatic processes, 2nd law of thermodynamics, reversible, and irreversible processes

Physics: Unit 08

• Equation of state of a perfect gas, kinetic theory of gases, assumptions in kinetic theory of gases, concept of pressure, and temperature; RMS speed of gas molecules; degrees of freedom
• Law of equipartition of energy (introductory ideas) and application to specific heats of gases; mean free path, Avogadro number

Physics: Unit 09

• Periodic motion-time period, frequency, time-displacement equation, simple harmonic motion (S.H.M.) and its equation; phase; S.H.M. in different systems, restoring force and force const, energy in S.H.M.-KE and PE, free
• Forced and damped oscillations (introductory ideas), resonance wave motion, equation for progressive wave, longitudinal and transverse waves, sound waves, Newton’s formula and Laplace’s correction, factors affecting the velocity of sound in air
• Principles of superposition of waves, reflection of waves, standing waves in strings and organ pipes, fundamental mode, harmonics and overtones, beats, Doppler effect

Physics: Unit 10

• Conservation of electric charges, Coulomb's law-force between two-point charges, forces between multiple charges; superposition principle and continuous charge distribution
• Electric field and potential due to a point charge and distribution of charges, electric field lines electric field due to a dipole; torque on a dipole in uniform electric field; electric flux, Gauss' theorem and its simple applications
• Conductors and insulators, free charges and bound charges inside a conductor; dielectrics and electric polarisation, capacitors and capacitance, combination of capacitors in series and in parallel
• Capacitance of a parallel plate capacitor with and without dielectric medium between the plates, energy stored in a capacitor

Physics: Unit 11

• Electric current and conductor, drift velocity mobility and their relation with electric current; Ohm's law, electrical resistance, Ohmic and non-Ohmic conductors, electrical energy and power, carbon resistors, colour codes, combination of resistances
• Temperature dependence of resistances, electric cell, EMF and internal resistance of an electric cell, pd, combination of cells, secondary cells, (introductory) Kirchhoff’s laws of electrical network, simple applications, principle of Wheatstone bridge
• Metre bridge and potentiometer and their uses, thermoelectricity; Seebeck effect; Peltier effect, thermo EMF

Physics: Unit 12

• Concept of magnetic field, Oersted's experiment, Biot-Savart law and its application to current carrying circular loop; Ampere's law and its applications to infinitely long straight wire, straight and toroidal solenoids
• Force on a moving charge in uniform magnetic and electric fields, cyclotron frequency; force on a current-carrying conductor in a uniform magnetic field, force between two parallel current-carrying conductors-definition of ampere
• Torque experienced by a current loop in a uniform magnetic field; moving coil galvanometer-its current sensitivity and conversion to ammeter, and voltmeter, Inter-conversion of voltmeter and ammeter, and change of their ranges

Physics: Unit 13

• Current loop as a magnetic dipole and its magnetic dipole moment, magnetic dipole moment of a revolving electron, magnetic field intensity due to a magnetic dipole bar magnet along its axis and perpendicular to its axis
• Torque on a magnetic dipole (bar magnet) in a uniform magnetic field; magnet as an equivalent solenoid, magnetic field lines; earth's magnetic field and its magnetic elements
• Para-, dia-, and ferro- magnetic substances, with examples
• Electromagnets and the factors affecting their strengths, permanent magnets

Physics: Unit 14

• Electromagnetic induction; Faraday's laws, induced EMF and current; Lenz's Law, eddy currents, self and mutual induction, alternating currents, peak and RMS value of alternating current and voltage; reactance and impedance; LR and CR circuits
• Phase lag and lead, LCR series circuit, resonance; power in AC circuits, wattless current

Physics: Unit 15

• Electromagnetic waves and their characteristics (qualitative ideas only), transverse nature of electromagnetic waves, electromagnetic spectrum, applications of the waves from the different parts of the spectrum

Physics: Unit 16

• Reflection of light, spherical mirrors, mirror formula
• Refraction of light, total internal reflection, and its applications, optical fibres, refraction at spherical surfaces, lenses, thin lens formula, lensmaker's formula
• Newton's relation: Displacement method to find position of images (conjugate points) magnification, power of a lens, combination of thin lenses in contact, combination of a lens and a mirror refraction, and dispersion of light through a prism
• Optical instruments, human eye, image formation and accommodation, correction of eye defects (myopia, hypermetropia) using lenses, microscopes and astronomical telescopes (reflecting and refracting), and their magnifying powers

Physics: Unit 17

• Scattering of light-blue colour of the sky, elementary idea of Raman effect; wave optics: Wave front and Huygens principle, reflection and refraction of plane wave at a plane surface using wave fronts
• Proof of laws of reflection and refraction using Huygens principle interference, Young's double slit experiment and expression for fringe width, coherent sources, Fraunhofer diffraction due to a single slit

Physics: Unit 18

• Photoelectric effect, Hertz and Lenard’s observations; Einstein’s photoelectric equation-particle nature of light, matter waves; wave nature of particles, De Broglie relation

Physics: Unit 19

• Alpha-particle scattering experiment Rutherford's nuclear atom model of atom; Bohr model of hydrogen atom, energy levels in a hydrogen atom, hydrogen spectrum, continuous, and characteristic X-rays

Physics: Unit 20

• Composition and size of nucleus, atomic masses, isotopes, isobars; isotones, radioactivity-alpha, beta, and gamma particles/ rays and their properties; radioactive decay law; mass energy relation, mass defect
• Binding energy per nucleon and its variation with mass number; nuclear fission, and fusion

Physics: Unit 21

• Energy bands in solids (qualitative ideas only), conductors, insulators, and semiconductors; semiconductor diode-I-V characteristics in forward and reverse bias, diode as a rectifier; I-V characteristics of LED, photodiode, solar cell, and zener diode
• Zener diode as a voltage regulator, junction transistor (BJT), transistor action, characteristics of a BJT, BJT as an amplifier (CE configuration) and oscillator; logic gates (OR, AND, NOT, NAND, and NOR)

Chemistry: Unit 01

• 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

• 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 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

• 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

• 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

• 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

• 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

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

Chemistry: Unit 09

• 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-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 ΔGº
• 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

• 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 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

• 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

• 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

• 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

• 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

• 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

• 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

• 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

• 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

• 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

• 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; SNl 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-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

• 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 1º, 2º, and 3º amines (Hinsberg method); reaction with HNO2; carbylamine reaction

Chemistry: Unit 25

• 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

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

Chemistry: Unit 27

• 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

• 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¯. (b) 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

Chemistry: Unit 01

• 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

• 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 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

• 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

• 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

• 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

• 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

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

Chemistry: Unit 09

• 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-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 ΔGº
• 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

• 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 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

• 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

• 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

• 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

• 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

• 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

• 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

• 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

• 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

• 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

• 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; SNl 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-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

• 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 1º, 2º, and 3º amines (Hinsberg method); reaction with HNO2; carbylamine reaction

Chemistry: Unit 25

• 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

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

Chemistry: Unit 27

• 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

• 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¯. (b) 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