NTA will officially release the JEE Main 2021 Chemistry Syllabus on its official website soon. Owing to COVID 19 pandemic and the reduction in Class XII syllabus by some boards, the authorities might devise a new exam pattern and therefore update the JEE Main syllabus 2021. The new JEE Main syllabus will be available in PDF format at jeemain.nta.nic.in.
However, until the release of the 2021 syllabus, candidates can have a look at the 2020 syllabus and start their preparation accordingly. As per JEE Min 2020 syllabus, the Chemistry section will hold 25 objective type questions carrying 100 Marks.
Note: To download the syllabus in PDF, just press Ctrl + P (Print) and choose the option to save as PDF. Also, one can add the JEE Main Chemistry Syllabus PDF page in your ‘To-do list’ if you are beginning your revision orJEE Main preparations.
*JEE Main exam is majorly based on 11th and 12th CBSE syllabus. The syllabus of JEE Main is mapped in accordance with NCERT texts for uniformity throughout the country*. Therefore, below section details on subsections in Chemistry namely – Physical Chemistry, Inorganic Chemistry and Organic Chemistry that forms a major part of JEE Main Chemistry syllabus and carry equal weightage.
Some Basic Concepts in Chemistry
State of Matter
Chemical Bonding and Molecular Structure
Redox, Reaction and Electrochemistry
Classification of elements and periodicity in properties
Block elements (alkali and alkaline earth metals)
P Block elements group 13 to group 18 elements
d- and f – block elements
General principles and processes of isolation of metals
Purification and characterization of organic compounds
Given below is a detailed JEE Main Chemistry Syllabus with chapters and sub-topics of each chapter. JEE Main Chemistry syllabus is divided the same way as given above – Physical, Inorganic and Organic chemistry.
Syllabus for JEE Main Chemistry – Physical Chemistry
The JEE Main syllabus for Physical Chemistry is as follows:
Chapter 1 – Some Basic Concepts of Chemistry
Matter and its nature, Dalton’s the atomic theory, the concept of the atom, molecule, element, and compound.
Physical quantities and their measurements in Chemistry, precision, and accuracy, significant figures, S.I. Units, dimensional analysis.
Laws of chemical combination.
Atomic and molecular masses, mole concept, molar mass, percentage composition, empirical and molecular formulae.
Chemical equations and stoichiometry.
Chapter 2 – States of Matter
Classification of matter into solid, liquid and gaseous states.
Gaseous State: Measurable properties of gases; Gas laws – Boyle’s law, Charles’s law, Graham’s law of diffusion, Avogadro’s law, Dalton’s law of partial pressure.
The concept of the Absolute scale of temperature; Ideal gas equation, Kinetic theory of gases (only postulates).
The concept of average, root mean square and most probable velocities.
Real gases, deviation from Ideal behaviour, compressibility factor, van der Waals equation, liquefaction of gases, critical constants.
Liquid State: Properties of liquids – vapour pressure, viscosity and surface tension and effect of temperature on them (qualitative treatment only).
Solid State: 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, imperfection in solids.
Electrical, magnetic and dielectric properties.
Chapter 3 – Atomic Structure
Discovery of subatomic particles (electron, proton, and neutron).
Thomson and Rutherford atomic models and their limitations.
Nature of electromagnetic radiation, photoelectric effect.
The spectrum of hydrogen atom, Bohr model of hydrogen atom – its postulates, derivation of the relations for energy of the electron and radii of the different orbits, limitations of Bohr’s model.
Dual nature of matter, de-Broglie relationship, Heisenberg uncertainty principle.
Elementary ideas of quantum mechanics, the quantum mechanical model of an atom, its important features, the concept of atomic orbitals as one electron wave functions.
Variation of Ψ1 and Ψ2 with r for 1s 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 exclusion principle and Hund’s rule, electronic configuration of elements, the extra stability of half-filled and completely filled orbitals.
Chapter 4 – 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.
Chapter 5 – Chemical Thermodynamics
Fundamentals of thermodynamics: System and surroundings, extensive and intensive properties, state functions, types of processes.
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; Delta S of the universe and Delta G of the system as criteria for spontaneity, Delta Go (Standard Gibbs energy change) and equilibrium constant.
Chapter 6 – Solutions
Different methods for expressing the concentration of a solution: molality, molarity, mole fraction, percentage (by volume and mass both), the vapour pressure of solutions and Raoult’s Law.
Ideal and non-ideal solutions, vapour pressure – composition, plots for ideal and non-ideal solutions.
Colligative properties of dilute solutions, relative lowering of vapour pressure, depression of freezing point, elevation of boiling point and osmotic pressure.
Determination of molecular mass using colligative properties.
Abnormal value of molar mass, Hoff factor, and its significance.
Chapter 7 – Equilibrium
Meaning of equilibrium, the concept of dynamic equilibrium.
Equilibria involving physical processes: Solid – liquid, liquid – gas and solid – gas equilibria, Henry’s law, a general characteristic of equilibrium involving physical processes.
Equilibria involving chemical processes: Law of chemical equilibrium, equilibrium constants (Kp and Kc) and their significance, the significance of Delta G and Delta Go in chemical equilibria, factors affecting equilibrium concentration, pressure, temperature, the effect of the 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, solubility of sparingly soluble salts and solubility products, buffer solutions.
Chapter 8 – Redox Reactions 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, specific and 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.
Corrosion and its prevention.
Chapter 9 – Chemical Kinetics
The 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).
Chapter 10 – Surface Chemistry
Adsorption: Physisorption and chemisorption and their characteristics, factors affecting the adsorption of gases on solids: Freundlich and Langmuir adsorption isotherms, adsorption from solutions.
Catalysis: Homogeneous and heterogeneous, activity and selectivity of solid catalysts, enzyme catalysis, and its mechanism.
Colloidal state: Distinction among true solutions, colloids, and suspensions, classification of colloids: lyophilic, lyophobic.
Multimolecular, macromolecular and associated colloids (micelles), preparation and properties of colloids: Tyndall effect, Brownian movement, electrophoresis, dialysis, coagulation, and flocculation.
Syllabus for JEE Main Chemistry – Inorganic Chemistry
The JEE Main Inorganic Chemistry syllabus is as follows:
Chapter 11 – Classification of Elements and Periodicity in Properties
Modern 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.
Electrons gain enthalpy, valence, oxidation states and chemical reactivity.
Chapter 12 – General Principles and Process of Isolation of Metals
Modes of occurrence of elements in nature, minerals, ores.
Steps involved in the extraction of metals: concentration, reduction (chemical and electrolytic methods) and refining with special reference to the extraction of Al, Cu, Zn, and Fe.
Thermodynamic and electrochemical principles involved in the extraction of metals.
Chapter 13 – Hydrogen
The position of hydrogen in periodic table, isotopes, preparation, properties, and uses of hydrogen.
Physical and chemical properties of water and heavy water.
Structure, preparation, reactions, and uses of hydrogen peroxide.
Classification of hydrides: ionic, covalent and interstitial.
Hydrogen as a fuel.
Chapter 14 – S Block Elements (Alkali and Alkaline Earth Metals)
Group 1 and Group 2 Elements: General introduction, electronic configuration and general trends in physical and chemical properties of elements, anomalous properties of the first element of each group, diagonal relationships.
Preparation and properties of some important compounds: sodium carbonate, sodium chloride, sodium hydroxide and sodium hydrogen carbonate.
Industrial uses of lime, limestone, Plaster of Paris and cement.
The biological significance of Na, K, Mg and Ca.
Chapter 15 – 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. Groupwise study of the p block elements.
Group 13: Preparation, properties, and uses of boron and aluminium; Structure, properties and uses of borax, boric acid, diborane, boron trifluoride, aluminium chloride, and alums.
Group 14: Tendency for catenation; Structure, properties, and uses of allotropes and oxides of carbon, silicon tetrachloride, silicates, zeolites, and silicones.
Group 15: Properties and uses of nitrogen and phosphorus; Allotropic forms of phosphorus; Preparation, properties, structure, and uses of ammonia, nitric acid, phosphine and phosphorus halides, (PCl3, PCl5); Structures of oxides and oxoacids of nitrogen and phosphorus.
Group 16: Preparation, properties, structures and uses of dioxygen and ozone; Allotropic forms of sulfur; Preparation, properties, structures, and uses of sulfur dioxide, sulphuric acid (including its industrial preparation); Structures of oxoacids of sulfur.
Group 17: Preparation, properties, and uses of chlorine and hydrochloric acid; Trends in the acidic nature of hydrogen halides; Structures of Interhalogen compounds and oxides and oxyacids of halogens.
Group 18: Occurrence and uses of noble gases; Structures of fluorides and oxides of xenon.
Chapter 16 – 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: Lanthanides, Electronic configuration, oxidation states, chemical reactivity and lanthanide contraction, and Actinoids: Electronic configuration and oxidation states.
Chapter 17 – Coordination Compounds
Introduction to coordination compounds, Werner’s theory.
Calculations of empirical formula and molecular formulae; Numerical problems in organic quantitative analysis.
Chapter 20 – 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: -C = C- and those containing halogens, oxygen, nitrogen, and sulfur; Homologous series.
Isomerism: structural and stereoisomerism.
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.
Chapter 21 – 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 (Markownikoff’s and peroxide effect); Ozonolysis, oxidation, and polymerization.
Alkynes: Acidic character; Addition of hydrogen, halogens, water and hydrogen halides; Polymerization.
Aromatic hydrocarbons: Nomenclature, benzene structure and aromaticity.
Mechanism of electrophilic substitution: halogenation, nitration, Friedel Crafts alkylation and acylation, directive influence of the functional group in monosubstituted benzene.
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 (Wolff 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.
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.
Chapter 25 – Polymers
General introduction and classification of polymers, general methods of polymerization addition and condensation, co-polymerization.
Natural and synthetic rubber and vulcanization.
Some important polymers with emphasis on their monomers and uses, polyethene, nylon, polyester, and bakelite.
Chapter 26 – Biomolecules
General introduction and importance of biomolecules.
Carbohydrates: Classification: aldoses and ketoses; monosaccharides (glucose and fructose), constituent monosaccharides or oligosaccharides (sucrose, lactose, maltose) and polysaccharides (starch, cellulose, glycogen).
Proteins: Elementary Idea of amino acids, peptide bond, polypeptides; Proteins: primary, secondary, tertiary and quaternary structure (qualitative idea only), denaturation of proteins, enzymes.
Vitamins: Classification and functions.
B Chemical constitution of DNA and RNA. Biological functions of nucleic acids.
Chapter 27 – Chemistry in Everyday Life
Chemicals in medicines: Analgesics, tranquilizers, antiseptics, disinfectants, antimicrobials, antifertility drugs, antibiotics, antacids, antihistamines, their meaning and common examples.
Chemicals in food: Preservatives, artificial sweetening agents common examples.
Cleansing agents: Soaps and detergents, cleansing action.
Chapter 28 – Principles Related to Practical Chemistry
Detection of extra elements (N, S, halogens) in organic compounds.
Detection of the following functional groups: hydroxyl (alcoholic and phenolic), carbonyl (aldehyde and ketone), carboxyl and amino groups in organic compounds.
The chemistry involved in the preparation of the following: Inorganic compounds: Mohr’s salt, potash alum, and 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+, AI3+, Fe3+, Zn2+, Ni2+, Ca2+, Ba2+, Mg2+, NH4+, and Anions: CO32-, S2-, SO42-, NO2-, NO3-, CI-, Br, I. (Insoluble salts excluded).
Chemical principles involved in the following experiments: Enthalpy of solution of CuSO4, Enthalpy of neutralization of strong acid and strong base, Preparation of lyophilic and lyophobic sols, and Kinetic study of the reaction of iodide ion with hydrogen peroxide at room temperature.
Analysing the past few years JEE Main question papers, students can note certain frequently asked questions. Such questions are a vital part of JEE Main Syllabus. Therefore, candidates must give more attention and practice such important topics thoroughly.
Also, certain topics of JEE Main Chemistry syllabus carry more weightage, hence they should be practised thoroughly as well.
Such relevant topics from the JEE Main Chemistry syllabus along with the weightage is given below:
Important topics from JEE Main Organic Chemistry
In JEE Main, the type of questions asked is not fixed for Organic Chemistry. Questions can be asked randomly that makes almost every topic in JEE Main Chemistry syllabus important for JEE Main 2021 exam.
Some important topics in JEE Main organic chemistry are:-
Reactions and their mechanism
Tips to score well in JEE Main chemistry section:
Start from basic and frequent questions.
Practise topics with high weightage first.
In JEE Main, questions based on mechanism and named reactions have been asked repeatedly, so focus on that properly.
Prepare steps of common chemical reactions.
Develop daily 2-3 questions on average, from a topic.
Questions on organic synthesis are repeatedly asked in the exam.
For JEE Main Chemistry, there are theory-based questions. These questions are less time consuming as compared to Physics and Mathematics questions. Although complex, questions on chemistry topics can boost your marks in JEE Main exam. Given below is a weightage table for various chapters. This weightage is provided as per the trends in the past.
No of Questions
Transition Elements and Coordination Chemistry
Solid State And Surface Chemistry
Nuclear Chemistry And Environment
Thermodynamics And Gaseous State
General Organic Chemistry
Chemical And Ionic Equilibrium
Carboxylic Acid and their Derivatives
Periodic table and Representative Elements
Carbohydrates, amino acid and Polymers
Level of Difficulty of Chemistry in JEE Main
The question paper analysis of JEE Main 2020 January and September session is described below:
April/September Session 2020
The Chemistry section was considered to be the easiest among all the sections.
Questions from Organic Chemistry were a little tricky but overall, Chemistry was the easiest section.
Physics was more difficult than Mathematics and Chemistry.
Questions in the Physics section ranged from Moderate to difficult questions.
Mathematics was considered to be moderate as questions were time-consuming.
January Session 2020
The table below shows the segregation of questions in JEE Main 2020 January Session on an average basis of all shifts combined.
As per the table:
Chemistry section comprised the most number of difficult questions.
In 2020, NTA uploaded several video lectures recorded by some reputed IIT Professors under the name of IIT-PAL on Youtube. Students can make use of these lectures to ease their preparation. These lectures are divided into sub topics for each chapter. There are more than 100 videos of approximately 50 to 60 minute runtime for each video. Steps to access these videos are given below:
Practically it may sound impractical for one book to cover the entire JEE Main Chemistry syllabus as for chemistry, the syllabus is exhaustive. Most of the top educational writers publish separate books for the three subsections.
Given below are somebest books that aspirants can refer to while preparing the JEE Main syllabus for Chemistry.
Textbooks for Class 12 Chemistry (NCERT)
Exemplar Problems for Class 12 Chemistry (NCERT)
Textbooks for Class 11 Chemistry (NCERT)
Exemplar Problems for Class 11 Chemistry (NCERT)
Advanced Problems in Organic Chemistry for JEE by M S Chauhan
A Guidebook to Mechanism in Organic Chemistry for the JEE by Peter Sykes
Concise Inorganic Chemistry by J.D. Lee
Problems in Inorganic Chemistry for JEE Main & Advanced by V. K. JAISWAL
Atkins’ Physical Chemistry
Problems in Physical Chemistry – Narendra Awasthi
Things To Remember While Preparing for JEE Main Chemistry
JEE Main Chemistry is considered as a scoring section by majority students as the questions vary from easy to moderate. Also most of the questions are based on fundamental concepts. The questions are less time consuming as they are not calculation based. A lot of direct questions are also asked from NCERT textbooks. Moreover, JEE Main Chemistry syllabus is more about a planned approach rather than direct conceptual applications.
JEE Main aspirants must be thorough with all theimportant formulas, named reactions, chemical equations, and periodic table trends.
These concepts constitute a major portion of JEE Main Chemistry syllabus.
JEE Main study material plays a very important role in the exam preparations.
There could be a large chunk of direct and indirect questions from the above-mentioned concepts.
Try not to just memorize the theory and formulas as it does not improvise problem-solving skills.
At the end, there must be the knowledge of what logic works behind a particular concept.
Ques. The hardness of a water sample (in terms of equivalents of CaCO3) containing 10–3M CaSO4 is : (molar mass of CaSO4 = 136g/mol).
Ans. 100 ppm
Ques. The standard electrode potential Eº and its temperature coefficient (dEº/dT)p for a cell are 2V and –5×10–4 VK–1 at 300K respectively. The cell reaction is Zn(s) + Cu2+(aq)→ Zn2+(aq) + Cu(s). The standard reaction enthalpy (ΔrHº) at 300K is _________________ kJ/mol (F= 96485 C mol-1)
Ques. The number of monochlorinated products obtained on chlorination of 2 methylbutane is_________.
Click here to download the official PDF of JEE Main Sample Numerical Based Questions on Chemistry. Do more practise and solve as many questions as possible. Also, such numerical type questions do not carry any negative marking.