JEE Chemistry Syllabus: Chapter-wise Important Topics and Weightage for JEE Main 2022 Exam

The JEE Main 2022 examination has an extensive syllabus. Students preparing for the examination should entirely focus on the syllabus and their chapter-wise weightage to score high. Students must put both dedication and innovative thinking into their learning techniques to crack JEE Main 2022 Chemistry examination. Most students are seen working hard on less important topics that have low weightage in the JEE Main 2022 Chemistry examinations; these students become trapped in the JEE 2022 examination cycle and end up with low ranks. To work competently, students must understand the chapter-wise weightage and syllabus of the JEE Main 2022 examination.

Students can Get Syllabus of Chemistry for JEE Main 2022 | AESL. 

JEE Main 2022 Chemistry: Syllabus

Applicants can effectively strategise their JEE Main 2022 learning plan and preparation techniques using the JEE Main 2022 Chemistry syllabus. As the JEE 2022 examinations are around the corner, applicants can accurately plan their schedules and prepare their JEE Main 2022 Chemistry syllabus accordingly. Students can comprehend the Get Syllabus of Chemistry for JEE Main 2022 | AESL from here.

Unit 1: Some Basic Concepts of Chemistry

• Dalton’s atomic theory, matter, and its nature. 
• The concept of the molecule, atom, element, and compound.
• Physical quantities and their measurements in Chemistry, accuracy, and precision, significant figures, dimensional analysis, S.I. Units
• Laws of chemical combination
• Chemical equations and stoichiometry
• Mole concept, atomic and molecular masses, molar mass, empirical and molecular formulae, percentage composition

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Unit 2: States of Matter

• Classification of matter into solid, liquid, and gaseous states.
• Gaseous State: Measurable properties of gases; Gas laws – Graham’s law of diffusion, Boyle’s law, Charles’s law, Dalton’s law of partial pressure. Avogadro’s law
• The concept of the Absolute scale of temperature; Kinetic theory of gases (only postulates), and Ideal gas equation
• The concept of average, probable velocities, and root mean square.
• Real gases, compressibility factor, deviation from Ideal behaviour, liquefaction of gases, van der Waals equation, critical constants.
• Liquid State: Properties of liquids – vapor pressure, temperature (only qualitative treatment), viscosity, and surface tension.
• Solid State: Classification of solids-molecular, amorphous and crystalline (elementary idea), ionic, covalent and metallic solids.
• Unit cell and lattices, voids, packing in solids (bcc, fcc, and hcp lattices), calculations involving unit cell parameters, and Imperfections in solids.
• Bragg’s law and its applications
• Electrical, dielectric and magnetic properties.

Unit 3: Atomic Structure

• Discovery of subatomic particles (electron, proton, and neutron).
• Nature of electromagnetic radiation, the photoelectric effect.
• Thomson and Rutherford atomic models and their limitations.
• The spectrum of the hydrogen atom, Bohr model of the hydrogen atom – its postulates, derivation of the relations for the electron’s energy and radii of the different orbits, limitations of Bohr’s model.
• Elementary ideas of quantum mechanics, the quantum mechanical model of an atom, their features, and the concept of atomic orbitals as one-electron wave functions.
• Dual nature of matter, de-Broglie relationship, Heisenberg uncertainty principle.
• Variation of orbitals; various quantum numbers (principal, magnetic quantum numbers and angular momentum), and their significance.
• Shapes of s, p and d – orbitals, electron spin and spin quantum number.
• Rules for filling electrons in orbitals – Pauli exclusion principle, Aufbau principle and Hund’s rule, electronic configuration of elements, the extra stability of half-filled and filled orbitals.

Unit 4: Chemical Bonding and Molecular Structure

• Kossel – Lewis’s approach to chemical bond formation, the concept of ionic and covalent bonds.
• Quantum mechanical approach to covalent bonding: Valence bond theory, their features, the concept of hybridisation involving s, p, and d orbitals; Resonance.
• Molecular Orbital Theory: Their features, LCAOs, sigma and pi-bonds, types of molecular orbitals (antibonding, bonding), molecular orbital electronic configurations of homonuclear diatomic molecules, the concept of bond order, bond energy and bond length.
• Hydrogen bonding, and its applications, elementary idea of metallic bonding.

Unit 5: Chemical Thermodynamics

• Fundamentals of thermodynamics: Extensive and intensive properties, system and surroundings, types of processes, state functions.
• The first law of thermodynamics: Concept of work, internal heat energy, and enthalpy, heat capacity, molar heat capacity
• The second law of thermodynamics: Spontaneity of processes; Delta Go (Standard Gibbs energy change), Delta S of the universe and Delta G of the system as criteria for spontaneity and equilibrium constant.
• Hess’s law of constant heat summation
• Atomisation, bond dissociation enthalpies, hydration, combustion, formation, phase transition, sublimation, ionisation, and solution.

Unit 6: Solutions

• Different methods for expressing the concentration of a solution.
• Ideal and non-ideal solutions, vapour pressure – plots for ideal and non-ideal solutions, composition.
• Colligative properties of dilute solutions, relative lowering of vapour pressure, depression of freezing point, the elevation of boiling point and osmotic pressure.
• Hoff factor, its significance and abnormal value of molar mass.
• Determination of molecular mass using colligative properties.

Unit 7: Equilibrium

• Meaning of equilibrium
• Concept of dynamic equilibrium
• Equilibria involve physical processes.
• Equilibria involve chemical processes.
• Le Chatelier’s principle
• Ionic equilibrium

Unit 8: Redox Reactions and Electrochemistry

• Electronic concepts of oxidation and reduction, oxidation number, redox reactions, rules for assigning oxidation numbers, and balancing of redox reactions.
• Kohlrausch’s law and its applications
• Electrolytic and metallic conduction, conductance in electrolytic solutions, specific and molar conductivities and their variation with concentration.
• Electrochemical cells
• Relationship between cell potential and Gibbs’ energy change, Nernst equation and its applications.
• Fuel cells, dry cells and lead accumulator
• Corrosion and its prevention

Unit 9: Chemical Kinetics

• The rate of a chemical reaction affects the rate of reactions: temperature, concentration, pressure, and catalyst.
• Order and molecularity of reactions, elementary and complex reactions, rate law, differential and integral forms of zero and first-order reactions, rate constant and its units, their characteristics and half-lives, and the effect of temperature on the rate of reactions.
• Arrhenius theory, collision theory of bimolecular gaseous reactions (no derivation), activation energy, and calculation.

Unit 10: Surface Chemistry

• Adsorption
• Catalysis
• Colloidal state
• Multimolecular preparation and properties of colloids, macromolecular and associated colloids (micelles)
• Emulsions and their characteristics.

Unit 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.
• Ionisation enthalpy, periodic trends in properties of elements atomic and ionic radii.
• Electrons gain enthalpy, oxidation states, valence, and chemical reactivity.

Unit 12: General Principles and Process of Isolation of Metals

• Modes of occurrence of elements in nature, minerals, ores.
• Thermodynamic and electrochemical principles are involved in the extraction of metals.
• Steps involved in the extraction of metals.

Unit 13: Hydrogen

• The position of hydrogen in the periodic table, preparation, isotopes, properties, and uses of hydrogen.
• Chemical and physical properties of heavy water and water.
• Classification of hydrides: interstitial, ionic and covalent
• Structure, preparation, reactions, and uses of hydrogen peroxide.
• Hydrogen as a fuel.

Unit 14: S Block Elements (Alkali and Alkaline Earth Metals)

• Group 1 and Group 2 Elements
• Preparation and properties of some important compounds
• The biological significance of Na, K, Mg and Ca
• Industrial uses of lime, limestone, Plaster of Paris and cement

Unit 15: P Block Elements

• Group 13 to Group 18 Elements: General Introduction, Electronic configuration, and general trends in chemical and physical 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.

Unit 16: D and F Block Elements

• Transition Elements
• Properties, preparation, and uses of K2Cr2O7 and KMnO4.
• Inner Transition Elements

Unit 17: Coordination Compounds

• Introduction to coordination compounds, coordination number, ligands, chelation, Werner’s theory, denticity.
• Importance of coordination compounds
• IUPAC nomenclature of mononuclear coordination compounds, isomerism.
• Bonding-Valence bond approach, colour and magnetic properties, and Crystal field theory basic ideas.

Unit 18: Environmental Chemistry

• Environmental pollution
• Atmospheric pollution
• Gaseous pollutants
• Particulate pollutants
• Stratospheric pollution
• Water Pollution
• Soil pollution
• Strategies to control environmental pollution.
• Greenhouse effect and Global warming, acid rain.

Unit 19: Purification and Characterisation of Organic Compounds

• Purification: Sublimation, crystallisation, distillation, differential extraction, and chromatography principles.
• Qualitative analysis
• Quantitative analysis (basic principles only)
• Calculations of molecular formulas and empirical formulas; Numerical problems in organic quantitative analysis.

Unit 20: Some Basic Principles of Organic Chemistry

• Tetravalency of Carbon; Shapes of simple molecules – hybridisation (s and p).
• Nomenclature (Trivial and IUPAC)
• Classification of organic compounds based on functional groups
• Isomerism
• Electronic displacement in a covalent bond
• Common types of organic reactions

Unit 21: Hydrocarbons

• Classification, IUPAC nomenclature, isomerism, general preparation methods, properties and reactions.
• Alkanes
• Alkenes
• Alkynes
• Aromatic hydrocarbons
• Mechanism of electrophilic substitution
• Mechanism of electrophilic addition

Unit 23 Organic Compounds Containing Oxygen

• General methods of preparation, reactions, properties, and uses.
• Alcohols
• Phenols
• Ethers
• Aldehyde and Ketones
• Carboxylic Acids
• Chemical tests to distinguish Ketones and aldehydes
• Important reactions include nucleophilic addition reactions (addition of HCN, NH3 and its derivatives), oxidation; Grignard reagent; reduction (Wolff Kishner and Clemmensen); aldol condensation, the acidity of hydrogen, Cannizzaro reaction, and Haloform reaction.

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Unit 24: Organic Compounds Containing Nitrogen

• General methods of preparation, reactions, properties, and uses.
• Amines: Nomenclature, structure, classification, basic character and identification of primary, secondary and tertiary amines and their basic character.
• Diazonium Salts

Unit 25 Polymers

• General methods of polymerisation addition and condensation, general introduction and classification of polymers, co-polymerisation.
• Vulcanisation and natural and synthetic rubber.
• Some important polymers emphasise their monomers and uses, nylon, polyethene, polyester, and bakelite.

Unit 26: Biomolecules

• General introduction and importance of biomolecules
• Carbohydrates
• Vitamins
• Proteins
• Biological functions of nucleic acids.
• B Chemical constitution of DNA and RNA. 

Unit 27 Chemistry in Everyday Life

• Chemicals in medicines
• Chemicals in food
• Cleansing agents

Unit 28: Principles Related to Practical Chemistry

• Detection of extra elements (N, S, halogens) in organic compounds.
• Detection of the following functional groups
• The chemistry involved in the preparation of the following: Inorganic compounds: Potash alum, Mohr’s salt, and Organic compounds: p-nitro acetanilide, acetanilide, aniline yellow, iodoform.
• The chemistry involved in the titrimetric exercises: acid bases and indicators, oxalic-acid vs KMnO4, Mohr’s salt vs KMnO4.
• Chemical principles involved in the qualitative salt analysis

JEE Main 2022 Chemistry: Chapter-Wise Weightage

Conclusion

Students who are planning for the JEE Main 2022 examinations commonly question experts and subject teachers on what is the complete syllabus for the JEE 2022 examination along with the chapter-wise weightage. The JEE Main 2022 Chemistry Syllabus comprises topics from Classes 11 and 12 NCERT textbooks. Knowing the JEE Main 2022 Chemistry Syllabus and chapter-wise weightage will help students know the topics that need to be focused on and prepare accordingly. Students must completely comprehend the syllabus and design an effective study plan to achieve their desired goals with ease.

Also Read:

JEE Main 2022 Chemistry Revision: Important Notes For Students
JEE Main 2022 Chemistry Revision Notes For Session 1
JEE 2022 Main Chemistry Chapter-wise Important Questions
JEE Main Chemistry Exam 2022: How To Evaluate Your Progress?

FAQs

1. Why is it critical to comprehend the JEE Main 2022 Chemistry Syllabus?

The National Testing Agency (NTA) prescribes the JEE Main 2022 examination syllabus. The JEE Main 2022 Chemistry syllabus covers a wide range of concepts and their applications. Students are advised to review the JEE Main 2022 Chemistry to understand which chapters will be covered in the examination. Before beginning the JEE Main 2022 Chemistry preparations, students should familiarise themselves with all of the concepts covered in the syllabus and devise an appropriate study plan. Students can Get Syllabus of Chemistry for JEE Main 2022 | AESL.

2. Describe the structure of the JEE Main 2022 Chemistry questions.

The JEE Main 2022 Chemistry questions are more concerned with theories than calculations. Students preparing for the JEE Main 2022 examination find Chemistry easier than the other JEE Main subjects (Physics and Mathematics). The JEE Main 2022 Chemistry syllabus is divided into three sections: Physical Chemistry, Organic Chemistry, and Inorganic Chemistry. 

3. Suggest some of the finest reference books for completing the JEE Main 2022 Chemistry Syllabus?

JEE Main 2022 Chemistry syllabus is divided into three sections: Physical, Inorganic, and Organic. The Chemistry section involves applications of the number of reactions and formulas. Thus students need to study the subject with regular revision. The following are some of the finest reference books for effective JEE Main 2022 Chemistry preparation:

• Organic Chemistry by Morrison and Boyd
• IIT Chemistry by O P Tandon
• Physical Chemistry by O P Tandon
• Complete Chemistry for JEE Main by NCERT
• Concise Inorganic Chemistry by J D Lee
• Organic Chemistry by Solomon and Fryhle
• Numerical Chemistry by P Bahadur

4. Name the most important JEE Main 2022 Chemistry chapters.

The JEE Main 2022 Chemistry Syllabus is divided into three sections: Physical Chemistry, Organic Chemistry, and Inorganic Chemistry. Students should aim to complete the entire Chemistry paper in 40-45 minutes.

Some of the important topics in JEE Main 2022 Chemistry section are Solid State, Chemical Kinetics, Solutions, Atomic Structure, Ionic Equilibrium, Chemical Equilibrium, and Thermodynamics. Students must have a firm grasp of these chapters to score well in these units.

5. Explain why knowing the chapter-wise weightage of the JEE Main 2022 Chemistry subject is important.

Chemistry is a high-scoring and simple subject in JEE Main 2022 examination. Students must understand the concepts rather than memorise them. Students preparing for JEE Main 2022 should be aware of the chapter-wise weightage of chemistry and plan their studies accordingly. Students must begin their preparation with higher weightage topics and progress to lower weightage topics. Knowing the chapter-wise weightage can help students distribute their time effectively in important chapters rather than squandering their time in less important chapters.