JEE Main Chemistry Syllabus

The IIT JEE Main Chemistry syllabus 2022 has been made available in PDF format online by the National Testing Agency (NTA) on its official website (jeemain.nta.nic.in), along with a brochure. On the official website, candidates should review the chemistry syllabus for the Joint Entrance Examination Main 2022 Exam.

The exam conducting authority will base their questions on the topics covered in the IIT JEE Main 2022 chemistry syllabus in the JEE Main Chemistry section. It should be noted that the JEE Main Chemistry 2022 syllabus will cover the same subjects that are covered in 11th and 12th grade. Physical, Inorganic, and Organic Chemistry make up the three sections of the JEE Main Chemistry curriculum. Before beginning the preparation process, candidates are advised to review the JEE Main Chemistry syllabus so that they can plan their study time accordingly.

We have attempted to cover a variety of JEE Main Chemistry Syllabus topics in this article, including the topical weighting, video lectures, mock exams, reference materials, analysis of difficulty level, tips for passing the chemistry section, and preparation methods.


Unit-wise Syllabus by NTA for JEE Main Chemistry

The NCERT books should be used by candidates to complete the IIT JEE chemistry syllabus. The topics of physical, inorganic, and organic chemistry are provided below. To effectively prepare, review the JEE Main syllabus and weightage.

Section A: Physical Chemistry
Unit Number Topic Sub-topics
1. Some Basic Concepts of Chemistry

Matter and its nature, Dalton’s 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.

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 behavior, compressibility factor, van der Waals equation, liquefaction of gases, critical constants;

Liquid State: Properties of liquids – vapor 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, an imperfection in solids;

Electrical, magnetic, and dielectric properties.

3. Atomic Structure

Discovery of subatomic particles (electron, proton, and neutron);

Thomson and Rutherford’s atomic models and their limitations;

Nature of electromagnetic radiation, photoelectric effect;

The 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 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.

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, Fagan’s rule, dipole moment; Valence Shell Electron Pair Repulsion (VSEPR) theory and shapes of simple molecules;

Quantum mechanical approach to covalent bonding: Valence bond theory, Its important features, the concept of hybridization involving s, p, and d orbitals; Resonance;

Molecular Orbital Theory: Its important features, LCAOs, types of molecular orbitals (bonding, antibonding), sigma and pi-bonds, molecular orbital electronic configurations of homonuclear diatomic molecules, the concept of bond order, bond length, and bond energy;

Elementary idea of metallic bonding, Hydrogen bonding, and its applications.

5. Chemical Thermodynamics

Fundamentals of thermodynamics: System and surroundings, extensive and intensive properties, state functions, types of processes;

The first law of thermodynamics: Concept of work, heat internal energy, and enthalpy, heat capacity, molar heat capacity;

Hess’s law of constant heat summation;

Enthalpies of bond dissociation, combustion, formation, 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.

6. Solutions

Different methods for expressing the concentration of a solution: molality, molarity, mole fraction, percentage (by volume and mass both), the vapor pressure of solutions, and Raoult’s Law;

Ideal and non-ideal solutions, vapor pressure – composition, plots for ideal and non-ideal solutions;

Colligative properties of dilute solutions, relative lowering of vapor pressure, depression of freezing point, the elevation of boiling point, and osmotic pressure;

Determination of molecular mass using colligative properties;

Abnormal value of molar mass, Hoff factor, and its significance.

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 multistage ionization) and ionization constants, ionization of water, pH scale, common ion effect, hydrolysis of salts and pH of their solutions, the solubility of sparingly soluble salts and solubility products, buffer solutions.

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.

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, and the effect of temperature on the rate of reactions.

Arrhenius theory, activation energy, and its calculation, collision theory of bimolecular gaseous reactions (no derivation).

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.

Emulsions and their characteristics.

Section B: Inorganic Chemistry
Unit Number Topic Sub-topics
11. Classification of Elements and Periodicity in Properties

Modern periodic law and the 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.

Electron gain enthalpy, valence, oxidation states, and chemical reactivity.

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 are involved in the extraction of metals.

13. Hydrogen

The position of hydrogen in the 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.

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.

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 behavior of the first element in each group. Groupwise study of the p block elements.

Group 13: Preparation, properties, and uses of boron and aluminum; Structure, properties, and uses of borax, boric acid, diborane, boron trifluoride, aluminum 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.

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, color, catalytic behavior, 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 lanthanoid contraction, and Actinoids: Electronic configuration and oxidation states.

17. Coordination Compounds

Introduction to coordination compounds, Werner’s theory.

ligands, coordination number, denticity, chelation.

IUPAC nomenclature of mononuclear coordination compounds, isomerism.

Bonding-Valence bond approach and basic ideas of Crystal field theory, color, and magnetic properties.

Importance of coordination compounds (in qualitative analysis, extraction of metals, and biological systems).

18. Environmental Chemistry

Environmental pollution: Atmospheric, water, and soil.

Atmospheric pollution: Tropospheric and stratospheric.

Gaseous pollutants: Oxides of carbon, nitrogen, and sulfur, hydrocarbons; their sources, harmful effects, and prevention.

Greenhouse effect and Global warming, acid rain.

Particulate pollutants: Smoke, dust, smog, fumes, mist; their sources, harmful effects, and prevention.

Stratospheric pollution: Formation and breakdown of ozone, depletion of ozone layer its mechanism and effects.

Water Pollution: Major pollutants such as pathogens, organic wastes, and chemical pollutants; their harmful effects and prevention.

Soil pollution: Major pollutants such as Pesticides (insecticides, herbicides and fungicides) their harmful effects and prevention.

Strategies to control environmental pollution.

Section C: Organic Chemistry
Unit Number Topic Sub-topics
19.

Purification and Characterisation of Organic Compounds

Purification: Crystallization, sublimation, distillation, differential extraction, and chromatography principles and their applications.

Qualitative analysis: Detection of nitrogen, sulfur, phosphorus, and halogens.

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

Calculations of empirical formula and molecular formulae; Numerical problems in organic quantitative analysis.

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.

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.

22.

Organic Compounds Containing Halogens

General methods of preparation, properties, and reactions.

Nature of C-X bond.

Mechanisms of substitution reactions.

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

23.

Organic Compounds Containing Oxygen

General methods of preparation, properties, reactions, and uses.

Alcohols: Identification of primary, secondary and tertiary alcohols; mechanism of dehydration.

Phenols: Acidic nature, electrophilic substitution reactions: halogenation, nitration, and sulphonation, Reimer Tiemann reaction.

Ethers: Structure.

Aldehyde and Ketones: Nature of carbonyl group; Nucleophilic addition to >C=O group, relative reactivities of aldehydes and ketones.

Important reactions such as Nucleophilic addition reactions (addition of HCN, 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.

24.

Organic Compounds Containing Nitrogen

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.

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.

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.

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.

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.


Topic-wise Weightage of JEE Main Chemistry Syllabus

The topic-wise weightage of chemistry questions with regard to number of questions and marks is as follows:

TopicsNumber of QuestionsMarks
Transition Elements and Coordination Chemistry312
Periodic table and Representative Elements312
Thermodynamics And Gaseous State28
Atomic Structure28
Chemical Bonding28
Chemical And Ionic Equilibrium28
Solid State And Surface Chemistry28
Nuclear Chemistry And Environment28
Mole Concept14
Redox Reaction14
Electrochemistry14
Chemical Kinetics14
Solution and Colligative Properties14
General Organic Chemistry14
Stereochemistry14
Hydrocarbon14
Alkyl Halides14
Carboxylic Acid and their Derivatives14
Carbohydrates,amino acid and Polymers14
Aromatic Compounds14

Online Mock Tests for JEE Main Chemistry

One of the most essential components of preparation is analysing your exam strategy. Using mock exams, one must continuously assess the accuracy of their exam preparation strategies and the degree to which they understand various concepts.

NTA helps candidates by offering official practise exams. The NTA’s official website, nta.ac.in, is where the official mock tests can be found. On the NTA’s official website, a total of 18 mock exams have been made available, 15 of which are for Paper 1 and 3 for Paper 2. You can access mock exams in Gujarati, Hindi, and English.


Chemistry Video Lectures for JEE Main Preparation

For the preparation of the JEE Main Chemistry section, NTA has made available online video lectures by IIT faculty and experts. The following are the steps to access the video lectures:

  • Go to the NTA’s official website at nta.ac.in.
  • Then select “CONTENT BASED LECTURES – FOR JEE MAIN AND NEET-UG BY IIT PROFESSORS / SUBJECT EXPERTS” from the list of options.
  • You will be taken to a page with the names of various subjects.
  • By selecting the subject, you can select the video lecture.

Analysis of Difficulty Level of JEE Main Chemistry

During different sessions, the JEE Main Chemistry section’s level of difficulty changes. The following table provides a basic breakdown of the number of questions on the B.E./ B. Tech paper for the JEE Main 2020 January session for the candidates’ understanding:

SectionsToughMediumEasy
Chemistry41110
Mathematics21013
Physics2716

Although chemistry appears to be the most difficult section in the B.E./B.Tech paper based on the analysis above, candidates must remember that level of difficulty is a subjective issue and chemistry still ranks among the easiest sections to attempt and score well in.


Why should applicants try the chemistry section of the JEE Main B.E./ B. Tech paper first?

  • Experts frequently recommend that, of the three sections of the B.E./B. Tech paper for JEE Main, chemistry be attempted first.
  • Fact-based questions make up a large portion of the chemistry exam. Therefore, it will be simple to solve them first. The remaining time can then be applied to the physics and math sections, which are thought to take more time.
  • Starting with inorganic chemistry questions is a wise course of action in chemistry as well. For instance, read carefully through chapters on the P, S-block, classification of elements, and periodicity in property. Direct inquiries from these areas can be answered by directly putting concept knowledge to use.
  • According to experts, you should finish the JEE Main Chemistry section in no more than 40 to 45 minutes.
  • The B.E./B.Tech paper’s chemistry section should be studied in the following order: inorganic chemistry (6–8 minutes), organic chemistry (12–15 minutes), and physical chemistry ( 15 – 17 min). The remaining 40 to 45 minutes must be used to answer the five questions that are based on numerical values.

Section-wise Tips by IITians to maximize your score in JEE Main Chemistry

For Physical Chemistry

  • As it doesn’t necessitate intensive memorization of chemical reactions, physical chemistry is almost universally regarded as the section of chemistry that students enjoy the most. The key to succeeding in physical chemistry is to practise as much as you can because the subject involves many constants and calculations.
  • 11th grade Comparatively speaking, physical chemistry is more difficult than class twelve. The hardest topics to master on exam day are ones like Ionic Equilibrium and Thermodynamics, which call for in-depth theoretical understanding as well as practise. The NCERT textbook is the best for theory for both of these chapters, though N. Avasthi’s books can be helpful for problem-solving.
  • Atomic structure, chemical equilibrium, the gaseous state, and mole concepts are simple subjects that also score well. Because the same chapter is covered in class 12 physics as well and the content is nearly identical, atomic structure needs to be the focus of increased attention.
  • In contrast to class 11, physical chemistry in class 12 is much simpler and also scores better. It is simple to score well in physical chemistry because chapters like Solid State, Solutions, and Chemical Kinetics are simple. In the 12th grade, only the chapter on electrochemistry is interesting. You can only answer the questions in this chapter if you have a thorough understanding of the theory. In N. Avasthi’s book, the Level-2 problems are really excellent and will help you lay a solid foundation for this chapter.
  • Last but not least, the chapter Surface Chemistry is entirely theoretical but very rewarding because one question from this chapter that was taken directly from the NCERT textbook was included in both the JEE Mains and the JEE Advanced.
  • Class 12 is more significant than class 11. Topics like solid state, solutions, chemical kinetics, and atomic structure are simple, and each of these chapters typically contains two questions on a competitive exam. Since electrochemistry, ionic equilibrium, and thermodynamics are challenging concepts, you should practise them more frequently.

Since practise is the key to success in physical chemistry, books with quality questions become crucial. Read NCERT textbooks and class notes (from school or coaching) only for theory preparation because side books contain additional topics that are not on any exam’s syllabus. Refer to these books for practise questions:

  • O.P. Tandon
  • P.Bahadur
  • R.C Mukharjee
  • N. Avasthi

For Organic Chemistry

  • According to the class XI and XII syllabus, organic chemistry makes up about 33% of the chemistry questions in the JEE Main exam. Even though some people may find the questions in this section challenging, if one has a thorough understanding of this area of the subject, they take very little time to complete.
  • When answering questions, students should have a firm grasp of the facts and ideas of organic chemistry because frequently the options are unclear and people err due to a lack of knowledge of the material. As a result, the first and most important thing we should do is thoroughly study NCERT and finish all the exercises with full dedication because many questions come directly from NCERT.
  • General Organic Chemistry is the most crucial topic in the course because it introduces the ideas, mechanisms, and exceptions that are used throughout the remaining chapters of Organic Chemistry.
  • Even if one studies for a month prior to the exams, there are some very simple topics in the JEE Mains syllabus that can earn one points. These subjects include classification of elements in organic compounds, chemistry in daily life, and biomolecules and polymers.
  • Due to the variety of questions, organic chemistry also necessitates a lot of practise. However, because the questions in this section take up so little time, we can practise a lot of them. Because these ideas are used in almost every chapter of Organic Chemistry and because it is frequently necessary to determine the order of acidity or basicity in questions, it is essential to fully comprehend resonance, acidity, and basicity as well as practise all types of questions relating to these concepts.
  • “One thing that I would advise everyone to do is to compile a list of reagent and substrate exceptional behaviours after each chapter, as it would be a very helpful tool when revising the chapters. To fully master the subjects, I would also advise practising answering questions about organic chemistry for at least 30 to 45 minutes each day. ”
  • Understanding the mechanisms of reactions and the reagents used in the reactions—which determine what product would be formed in the reactions—is the most crucial factor that can fetch very good marks in Organic Chemistry in both JEE Advanced and JEE Mains. Every year, questions about aromatic compounds and their reactions appear on the test.
  • In addition to the NCERT textbook, one can use “Organic Chemistry for JEE Main and Advanced by Ranjeet Shahi” or “GRB Organic Chemistry by OP Tandon” for theory. These books contain a wide range of questions that can aid in gaining a thorough understanding of the topics. Every student should also complete the past year’s questions in addition to these books.

For Inorganic Chemistry

  • Even though inorganic chemistry makes up almost half of the plus two chemistry curriculum, it is a subject that receives little attention because, unlike the organic portion, it requires memorization of countless facts and exceptions rather than core ideas.
  • If one can master it, this component also ensures an advantage over the other participants. Contrary to organic chemistry, which contains hundreds of complex reaction mechanisms, understanding a few key ideas and regularly reviewing exceptions will ensure a smooth passage through the inorganic chapters.
  • For the higher secondary exam, the 39/70 mark distribution for classes 11 and 12 is essentially unchanged. Because the inorganic section takes up more than half the paper, students who were savvy enough to prepare it can actually score well on it.
  • Regarding the study plan, all you require is the two-part NCERTS for classes 11 and 12, along with one reliable reference book.
  • The NCERTs clearly explain all the fundamental ideas, and you should read each line of the book several times to ensure that you understand it. It’s a good idea to keep highlighters on hand to mark the key passages, as many students do. Keep a notebook nearby to make notes on crucial details, responses, and exceptions that you can later review. It is better to use sticky notes and keep them inside the chapters of the book itself because this will facilitate quick review whenever you open the books to skim through the chapters before your big day.
  • Drawing important reactions, such as those from salt analysis, redox chapters, and periodic tables, on sheets and sticking them on the walls can also help the memory retain information better.
  • The next question is how much time should be allotted for this section. This simpler section only requires patience and memory. Throughout the year, revise the chapters as they are taught in your schools or coaching centre (p.s. don’t save for last-minute revisions), and then continue to go over them on the weekends.
  • After the course is finished, set aside at least an hour each day to review the chapters, paying particular attention to the exceptions. Over time, it will take less time, perhaps as little as 30 to 45 minutes. Since questions about exceptions and reactions are frequently asked in competitive exams, they should take precedence.
  • J.D. Lee and O.P. Tandon are two examples of reference books recommended by top students. You can also consult a book by Cengage Publishing or VK Jaiswal’s “Problems in Inorganic Chemistry” for help with problem-solving. Anyone, and remember that one is sufficient.
  • For JEE Main, there are typically only 17–18 questions asked, so two preparations—exceptions, most importantly—along with plenty of MCQ practise will be sufficient. Make notes of key points as you answer MCQs; this will allow you to cover more material in less time. If reading is ineffective, one may also consult the best two online videos, produced by Byju’s and Kaysons.
  • Your NCERTs should serve as your Bible with a healthy dose of problem-solving. You will undoubtedly receive a perfect score in the subject if you consistently review all the concepts and exceptions.

Preparation and Paper Attempting Tips for JEE Main 2022 Chemistry

Chemistry, the most highly scored section, frequently proves to be a significant rank raiser for one’s overall JEE Main performance. However, candidates find that chemistry can be challenging when it comes to preparation. The following advice can help candidates with their JEE Main Chemistry preparation:

Utilize precise, constrained resources: Don’t try to cover the syllabus from several different sources; instead, concentrate on mastering NCERT. Apart from that, you can read various ideas from a few reliable sources. Write down or record notes, then review them frequently.

Solve Questions Everyday: Retention is one of the factors that contributes to a successful attempt on the chemistry section, and retention can only be ensured through practise. Candidates should establish a daily habit of answering 40–50 questions. It is entirely up to you whether you mix questions from different topics or deal with questions from a single topic every day. Making sure that your memorization and analytical abilities are in balance will help you to get the best possible grade in Chemistry.

Identify answers through approximations: It is not a good idea to test your mathematical prowess while answering the chemistry questions. Instead, find answers through approximations. You must keep in mind that there is a time limit and find solutions accordingly. Unless the choices are extremely close to one another, candidates can obtain a rough answer and select the option that comes the closest to it.

Practice with past year’s test questions and mock exams: According to all experts, practising is the most important part of your preparation. To determine the effectiveness of your current plan, continuously practise and evaluate your performance.

Invest your time wisely: Candidates can use the time they save on direct questions to spend on questions that will take longer to complete. Time management is crucial for the chemistry paper.


Best Books to Cover JEE Main Chemistry Syllabus 2022

While the class XI and XII NCERT textbooks are recommended as the best preparation for the JEE Main Chemistry Section because so many direct questions are drawn from them, the following list of additional books may be useful to applicants:

Authors/PublishersBooks
P BahadurConcept of Physical Chemistry for JEE Main & Advanced 
N AwasthiPhysical Chemistry
Solomons and FryhleOrganic Chemistry
Morrison and BoydOrganic Chemistry
R.K GuptaArihant’s Practice Book Chemistry for JEE Main And Advanced
J D LeeConcise Inorganic Chemistry
Freedman and YoungUniversity Chemistry
MS ChauhanElementary problems in Organic Chemistry
O.P. TandonPhysical Chemistry; Organic Chemistry
P.W.AtkinsPhysical Chemistry
R.C. MukherjeeModern Approach to Chemical Calculations


Frequently Asked Questions

Ques. Is NCERT enough for the chemistry portion of the JEE mains?

Ans. For JEE Mains Chemistry preparation, NCERT books are extremely helpful. But it is not enough.
The part with the highest scores is inorganic chemistry. And NCERT books are a requirement for this section. In previous years, NCERT-approved questions were included. But you should also read your textbooks and class notes.
NCERT is insufficient for Physical and Inorganic Chemistry. In order to have a strong command of these sections, you must practise a lot. Go through the NCERT for these sections, make notes for key passages, and complete practise exercises.

Ques. How do I get a 250 on the JEE Mains?

Ans. You must use wise preparation methods if you want to achieve a JEE Main score of 250 or higher. Utilize your time wisely and revise each section thoroughly. For a thorough understanding of the subject, you must solve two papers per day.
For the JEE Mains, chemistry scores quite well. You must strive for a 90–100 overall score.
NCERT is sufficient for Physical Chemistry.
You must practise in order to perform well in math. You can easily achieve a high grade if you put in the extra effort. For JEE Mains, the coordinate geometry section has a high passing rate.
It can be challenging to achieve a physics score of 70 to 90. Learn to use shortcuts and tricks to finish the task faster. You can study NCERT to understand physics concepts, and books like HCV can help you solve problems.
Browse through last two months’ exam papers to see how various topics were weighted. To solve issues faster, use shortcuts and tricks.


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