JEE Main 2022 Syllabus Chemistry

Classification of solids: molecular, ionic, covalent
and metallic solids, amorphous and crystalline
solids (elementary idea); Bragg's Law and its
applications: Unit cell and lattices, packing in solids
(fcc, bcc and hcp lattices), voids, calculations
involving unit cell parameters, an imperfection in
solids; Electrical and magnetic properties.

UNIT 3: ATOMIC STRUCTURE

Thomson and Rutherford atomic models and their
limitations; 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, its important features. Concept of
atomic orbitals as one-electron wave functions:
CHEMISTRY Variation of  and 2 with r for 1s and 2s orbitals;
various

quantum numbers (principal, angular momentum,
PHYSICAL CHEMISTRY and magnetic quantum numbers) and their
significance; shapes of s, p, and d - orbitals, electron
UNIT I: SOME BASIC CONCEPTS IN CHEMISTRY
spin and spin quantum number: Rules for filling
Matter and its nature, Dalton's atomic theory: electrons in orbitals – Aufbau principle. Pauli's
Concept of atom, molecule, element, and exclusion principle and Hund's rule, electronic
compound: Physical quantities and their configuration of elements, extra stability of half-
measurements in Chemistry, precision, and filled and completely filled orbitals.
accuracy, significant figures. S.I.Units, dimensional
analysis: Laws of chemical combination; Atomic UNIT 4: CHEMICAL BONDING AND MOLECULAR
and molecular masses, mole concept, molar mass, STRUCTURE
percentage composition, empirical and molecular Kossel - Lewis approach to chemical bond
formulae: Chemical equations and stoichiometry. formation, the concept of ionic and covalent bonds.
UNIT 2: STATES OF MATTER Ionic Bonding: Formation of ionic bonds, factors
Classification of matter into solid, liquid, and affecting the formation of ionic bonds; calculation
gaseous states. of lattice enthalpy.

Covalent Bonding: Concept of electronegativity.
Gaseous State:
Fajan’s rule, dipole moment: Valence Shell Electron
Measurable properties of gases: Gas laws - Boyle's Pair Repulsion (VSEPR ) theory and shapes of
law, Charle’s law. Graham's law of diffusion. simple molecules.
Avogadro's law, Dalton's law of partial pressure;
Quantum mechanical approach to covalent bonding:
Concept of Absolute scale of temperature; Ideal gas
Valence bond theory - its important features, the
equation; Kinetic theory of gases (only postulates); concept of hybridization involving s, p, and d
Concept of average, root mean square and most orbitals; Resonance.
probable velocities; Real gases, deviation from Ideal
behaviour, compressibility factor, and van der Molecular Orbital Theory - Its important features.
Waals equation. LCAOs, types of molecular orbitals (bonding,
antibonding), sigma and pi-bonds, molecular orbital
Liquid State: electronic configurations of homonuclear diatomic
Properties of liquids - vapour pressure, viscosity and molecules, the concept of bond order, bond length,
surface tension, and effect of temperature on them and bond energy.
(qualitative treatment only). Elementary idea of metallic bonding. Hydrogen
Solid State: bonding and its applications.

UNIT 5: CHEMICAL THERMODYNAMICS

Fundamentals of thermodynamics: System and assigning oxidation number, balancing of redox
surroundings, extensive and intensive properties, reactions.
state functions, types of processes.
Electrolytic and metallic conduction, conductance in
The first law of thermodynamics - Concept of electrolytic solutions, molar conductivities and their
work, heat internal energy and enthalpy, heat variation with concentration: Kohlrausch’s law and
capacity, molar heat capacity; Hess’s law of its applications.
constant heat summation; Enthalpies of bond
dissociation, combustion, formation, atomization, Electrochemical cells - Electrolytic and Galvanic
sublimation, phase transition, hydration, ionization, cells, different types of electrodes, electrode
and solution. potentials including standard electrode potential,
half - cell and cell reactions, emf of a Galvanic cell
The second law of thermodynamics - Spontaneity and its measurement: Nernst equation and its
of processes; S of the universe and G of the applications; Relationship between cell potential
system as criteria for spontaneity. G (Standard and Gibbs' energy change: Dry cell and lead
Gibbs energy change) and equilibrium constant. accumulator; Fuel cells.

UNIT 6: SOLUTIONS UNIT 9: CHEMICAL KINETICS

Different methods for expressing the concentration Rate of a chemical reaction, factors affecting the
of solution - molality, molarity, mole fraction, rate of reactions: concentration, temperature,
percentage (by volume and mass both), the vapour pressure, and catalyst; elementary and complex
pressure of solutions and Raoult's Law - Ideal and reactions, order and molecularity of reactions, rate
non-ideal solutions, vapour pressure - composition, law, rate constant and its units, differential and
plots for ideal and non-ideal solutions; Colligative integral forms of zero and first-order reactions, their
properties of dilute solutions - a relative lowering of characteristics and half-lives, the effect of
vapour pressure, depression of freezing point, the temperature on the rate of reactions, Arrhenius
elevation of boiling point and osmotic pressure; theory, activation energy and its calculation,
Determination of molecular mass using colligative collision theory of bimolecular gaseous reactions
properties; Abnormal value of molar mass, van’t (no derivation).
Hoff factor and its significance.
UNIT 10: SURFACE CHEMISTRY
UNIT 7: EQUILIBRIUM
Adsorption- Physisorption and chemisorption and
Meaning of equilibrium, the concept of dynamic their characteristics, factors affecting adsorption of
equilibrium. gases on solids - Freundlich and Langmuir
adsorption isotherms, adsorption from solutions.
Equilibria involving physical processes: Solid-
liquid, liquid - gas and solid-gas equilibria, Henry's Catalysis - Homogeneous and heterogeneous,
law. General characteristics of equilibrium activity and selectivity of solid catalysts, enzyme
involving physical processes. catalysis, and its mechanism.

Equilibrium involving chemical processes: Law Colloidal state- distinction among true solutions,
colloids, and suspensions, classification of colloids -
of chemical equilibrium, equilibrium constants (Kp lyophilic. lyophobic; multi-molecular.
and Kc) and their significance, the significance of macromolecular and associated colloids (micelles),
G and G in chemical equilibrium, factors preparation and properties of colloids - Tyndall
affecting equilibrium concentration, pressure, effect. Brownian movement, electrophoresis,
temperature, the effect of catalyst; Le Chatelier’s dialysis, coagulation, and flocculation: Emulsions
principle. and their characteristics.

Ionic equilibrium: Weak and strong electrolytes, INORGANIC CHEMISTRY
ionization of electrolytes, various concepts of acids
and bases (Arrhenius. Bronsted - Lowry and Lewis) UNIT 11: CLASSIFICATION OF ELEMENTS AND
and their ionization, acid-base equilibria (including PERIODICITY IN PROPERTIES
multistage ionization) and ionization constants,
ionization of water. pH scale, common ion effect, Modem periodic law and present form of the
hydrolysis of salts and pH of their solutions, the periodic table, s, p. d and f block elements, periodic
solubility of sparingly soluble salts and solubility trends in properties of elements atomic and ionic
products, buffer solutions. radii, ionization enthalpy, electron gain enthalpy,
valence, oxidation states, and chemical reactivity.
UNIT 8: REDOX REACTIONS AND
ELECTROCHEMISTRY UNIT 12: GENERAL PRINCIPLES AND PROCESSES
Electronic concepts of oxidation and reduction, OF ISOLATION OF METALS
redox reactions, oxidation number, rules for

Modes of occurrence of elements in nature, Group -16
minerals, ores; Steps involved in the extraction of
metals - concentration, reduction (chemical and Preparation, properties, structures, and uses of
electrolytic methods), and refining with special ozone: Allotropic forms of sulphur; Preparation,
reference to the extraction of Al. Cu, Zn, and Fe; properties, structures, and uses of sulphuric acid
Thermodynamic and electrochemical principles (including its industrial preparation); Structures of
involved in the extraction of metals. oxoacids of sulphur.

UNIT 13: HYDROGEN Group-17

Position of hydrogen in periodic table, isotopes, Preparation, properties, and uses of hydrochloric
preparation, properties and uses of hydrogen; acid; Trends in the acidic nature of hydrogen
Physical and chemical properties of water and heavy halides; Structures of Interhalogen compounds and
water; Structure, preparation, reactions, and uses of oxides and oxoacids of halogens.
hydrogen peroxide; Classification of hydrides -
Group-18
ionic, covalent, and interstitial; Hydrogen as a fuel.
Occurrence and uses of noble gases; Structures of
UNIT 14: S -BLOCK ELEMENTS (ALKALI AND fluorides and oxides of xenon.
ALKALINE EARTH METALS)
UNIT 16: d - and f- BLOCK ELEMENTS
Group -1 and 2 Elements
Transition Elements
General introduction, electronic configuration, and
general trends in physical and chemical properties General introduction, electronic configuration,
of elements, anomalous properties of the first occurrence and characteristics, general trends in
element of each group, diagonal relationships. properties of the first-row transition elements -
physical properties, ionization enthalpy, oxidation
Preparation and properties of some important
states, atomic radii, colour, catalytic behaviour,
compounds - sodium carbonate and sodium
magnetic properties, complex formation, interstitial
hydroxide and sodium hydrogen carbonate;
compounds, alloy formation; Preparation,
Industrial uses of lime, limestone. Plaster of Paris
properties, and uses of K2Cr2O7, and KMnO4.
and cement: Biological significance of Na, K. Mg,
and Ca. Inner Transition Elements
UNIT 15: P- BLOCK ELEMENTS Lanthanoids - Electronic configuration, oxidation
states, and lanthanoid contraction.
Group -13 to Group 18 Elements
Actinoids - Electronic configuration and oxidation
General Introduction: Electronic configuration
states.
and general trends in physical and chemical
properties of elements across the periods and down UNIT 17: CO-ORDINATION COMPOUNDS
the groups; unique behaviour of the first element in
each group. Introduction to coordination compounds. Werner's
theory; ligands, coordination number, denticity.
Groupwise study of the p - block elements Group chelation; IUPAC nomenclature of mononuclear co-
-13 ordination compounds, isomerism; Bonding-
Valence bond approach and basic ideas of Crystal
Preparation, properties, and uses of boron and
field theory, colour and magnetic properties;
aluminum; Structure, properties, and uses of borax,
Importance of co-ordination compounds (in
boric acid, diborane, boron trifluoride, aluminum
qualitative analysis, extraction of metals and in
chloride, and alums.
biological systems).
Group -14
UNIT 18: ENVIRONMENTAL CHEMISTRY
The tendency for catenation; Structure, properties,
and uses of Allotropes and oxides of carbon, silicon Environmental pollution - Atmospheric, water,
tetrachloride, silicates, zeolites, and silicones. and soil.

Group -15 Atmospheric pollution - Tropospheric and
Stratospheric
Properties and uses of nitrogen and phosphorus;
Allotrophic forms of phosphorus; Preparation, Tropospheric pollutants - Gaseous pollutants:
properties, structure, and uses of ammonia, nitric Oxides of carbon, nitrogen, and sulphur,
acid, phosphine, and phosphorus halides, (PCl3. hydrocarbons; their sources, harmful effects, and
PCl5); Structures of oxides and oxoacids of nitrogen prevention; Greenhouse effect and Global warming:
and phosphorus. Acid rain;

Particulate pollutants: Smoke, dust, smog, fumes, Classification, isomerism, IUPAC nomenclature,
mist; their sources, harmful effects, and prevention. general methods of preparation, properties, and
reactions.
Stratospheric pollution- Formation and breakdown
of ozone, depletion of the ozone layer - its Alkanes - Conformations: Sawhorse and Newman
mechanism and effects. projections (of ethane): Mechanism of halogenation
of alkanes.
Water Pollution - Major pollutants such as.
pathogens, organic wastes, and chemical pollutants; Alkenes - Geometrical isomerism: Mechanism of
their harmful effects and prevention. electrophilic addition: addition of hydrogen,
halogens, water, hydrogen halides (Markownikoffs
Soil pollution - Major pollutants such as; Pesticides and peroxide effect): Ozonolysis and
(insecticides. herbicides and fungicides), their polymerization.
harmful effects, and prevention. Strategies to control
environmental pollution. Alkynes - Acidic character: Addition of hydrogen,
halogens, water, and hydrogen halides:
Polymerization.
ORGANIC CHEMISTRY
Aromatic hydrocarbons - Nomenclature, benzene -
UNIT 19: PURIFICATION AND structure and aromaticity: Mechanism of
CHARACTERISATION OF ORGANIC electrophilic substitution: halogenation, nitration.
COMPOUNDS
Friedel - Craft's alkylation and acylation, directive
Purification - Crystallization, sublimation, influence of the functional group in mono-
distillation, differential extraction, and substituted benzene.
chromatography - principles and their applications.
UNIT 22: ORGANIC COMPOUNDS CONTAINING
Qualitative analysis - Detection of nitrogen, HALOGENS
sulphur, phosphorus, and halogens.
General methods of preparation, properties, and
Quantitative analysis (basic principles only) - reactions; Nature of C-X bond; Mechanisms of
Estimation of carbon, hydrogen, nitrogen, halogens, substitution reactions.
sulphur, phosphorus.
Uses; Environmental effects of chloroform,
Calculations of empirical formulae and molecular iodoform freons, and DDT.
formulae: Numerical problems in organic
quantitative analysis, UNIT 23: ORGANIC COMPOUNDS CONTAINING
OXYGEN
UNIT 20:SOME BASIC PRINCIPLES OF ORGANIC
CHEMISTRY General methods of preparation, properties,
reactions, and uses.
Tetravalency of carbon: Shapes of simple molecules
- hybridization (s and p): Classification of organic ALCOHOLS, PHENOLS, AND ETHERS
compounds based on functional groups: and those
containing halogens, oxygen, nitrogen, and sulphur; Alcohols: Identification of primary, secondary, and
tertiary alcohols: mechanism of dehydration.
Homologous series: Isomerism - structural and
stereoisomerism. Phenols: Acidic nature, electrophilic substitution
reactions: halogenation. nitration and sulphonation.
Nomenclature (Trivial and IUPAC)
Reimer - Tiemann reaction.
Covalent bond fission - Homolytic and heterolytic:
Ethers: Structure.
free radicals, carbocations, and carbanions; stability
of carbocations and free radicals, electrophiles, and Aldehyde and Ketones: Nature of carbonyl group;
nucleophiles. Nucleophilic addition to >C=O group, relative
Electronic displacement in a covalent bond reactivities of aldehydes and ketones; Important
reactions such as - Nucleophilic addition reactions
- Inductive effect, electromeric effect, resonance, (addition of HCN. NH3, and its derivatives),
and hyperconjugation. Grignard reagent; oxidation: reduction (Wolf
Common types of organic reactions- Substitution, Kishner and Clemmensen); the acidity of -
addition, elimination, and rearrangement. hydrogen. aldol condensation, Cannizzaro reaction.
Haloform reaction, Chemical tests to distinguish
UNITS 21: HYDROCARBONS between aldehydes and Ketones.

Carboxylic Acids

Acidic strength and factors affecting it, Chemicals in Medicines - Analgesics,
tranquilizers, antiseptics, disinfectants,
UNIT 24: ORGANIC COMPOUNDS CONTAINING
NITROGEN
antimicrobials, anti-fertility drugs,
antibiotics, antacids. Anti-histamines -their
General methods of preparation. Properties, meaning and common examples.
reactions, and uses.
Chemicals in food - Preservatives,
Amines: Nomenclature, classification
artificial sweetening agents - common
structure, basic character, and
examples.
identification of primary, secondary,
and tertiary amines and their basic Cleansing Agents - Soaps and detergents,
character. cleansing action
Diazonium Salts: Importance in synthetic UNIT 28: PRINCIPLES RELATED TO
organic chemistry. PRACTICAL CHEMISTRY
UNIT 25: POLYMERS Detection of extra elements (Nitrogen,
General introduction and classification of polymers,
Sulphur, halogens) in organic compounds;
general methods of polymerization, - Addition and Detection of the following functional groups;
condensation, copolymerization. hydroxyl (alcoholic and phenolic), carbonyl
(aldehyde and ketones) carboxyl, and amino groups
Natural and synthetic, rubber and vulcanization, in organic compounds.
some important polymers with emphasis on their
monomers and uses – polythene, nylon, polyester,  The chemistry involved in the preparation of the
and bakelite. following:

UNIT 26: BIOMOLECULES Inorganic compounds; Mohr’s salt, potash alum.

General introduction and importance of Organic compounds: Acetanilide, p-nitro
acetanilide, aniline yellow, iodoform.
biomolecules.
 The chemistry involved in the titrimetric exercises –
CARBOHYDRATES - Classification; aldoses Acids, bases and the use of indicators, oxalic-acid vs
and ketoses: monosaccharides (glucose KMnO4, Mohr’s salt vs KMnO4
and fructose) and constituent  Chemical principles involved in the qualitative salt
monosaccharides of oligosaccharides analysis:
(sucrose, lactose, and maltose).
Cations – Pb2+, Cu2+, Al3+, Fe3+, Zn2+, Ni2+,
PROTEINS - Elementary Idea of -amino Ca2+, Ba2+, Mg2+, NH4+
acids, peptide bond, polypeptides.
Proteins: primary, secondary, tertiary, and Anions- CO2− 2-
3 , S ,SO4 ,
2− NO3-
, NO2-, Cl-,
quaternary structure (qualitative idea Br-, I- ( Insoluble salts excluded).
only), denaturation of proteins, enzymes. Chemical principles involved in the following
experiments:
VITAMINS – Classification and
functions. 1. Enthalpy of solution of CuSO4

NUCLEIC ACIDS – Chemical 2. Enthalpy of neutralization of strong acid
constitution of DNA and RNA. and strong base.

Biological functions of nucleic acids. 3. Preparation of lyophilic and lyophobic
sols.
UNIT 27: CHEMISTRY IN EVERYDAY LIFE
4. Kinetic study of the reaction of iodide ions with
hydrogen peroxide at room temperature.