JEE Main Chemistry Syllabus 2025 (Available) – Get Syllabus PDF Here

The JEE Main 2024 Chemistry syllabus, set by the National Testing Agency (NTA), is designed to evaluate students’ understanding of Chemistry concepts from both Class XI and XII. The examination, conducted twice a year, aims to provide admission to various Engineering and Technology courses across India. The syllabus is meticulously structured to cover key areas of Physical and Chemical Chemistry, ensuring comprehensive preparation for candidates.

The syllabus is divided into three main sections. Section A focuses on Physical Chemistry and comprises 10 units, covering essential topics such as Atomic Structure, Chemical Bonding, States of Matter, and Thermodynamics. This section emphasizes the theoretical and quantitative aspects of Chemistry, requiring students to master concepts and solve numerical problems effectively.

Section B addresses Organic Chemistry, with 8 units dedicated to understanding compounds, reactions, and mechanisms. Topics include the Classification of Organic Compounds, Nomenclature, and Functional Groups, emphasizing the structure and behaviour of organic molecules. Section C encompasses Chemical Chemistry, including 10 units that deal with Environmental Chemistry, Solutions, and Equilibrium, among other critical areas. This section integrates various aspects of Chemistry, highlighting both practical and theoretical knowledge essential for the JEE Main examination.

JEE Main 2025 Chemistry Syllabus – Released

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JEE Main 2024 Chemistry Syllabus 

The JEE Main 2024 Chemistry syllabus, set by the National Testing Agency (NTA), covers key concepts from both Class XI and XII, divided into three sections: Physical Chemistry, Organic Chemistry, and Chemical Chemistry. This comprehensive syllabus is designed to assess students’ understanding of fundamental and advanced Chemistry topics essential for engineering and technology admissions.

Physical Chemistry

Unit 1- Some Basic Concepts in Chemistry

Unit I of the JEE Main 2024 Chemistry syllabus introduces fundamental concepts essential for understanding chemistry. It begins with the nature of matter, exploring how matter is composed of atoms and molecules and the foundational ideas of Dalton’s atomic theory. This theory describes atoms as indivisible particles that combine to form molecules, elements, and compounds.

Key concepts covered include the laws of chemical combination, which explain how elements combine to form compounds in fixed proportions. The unit also addresses atomic and molecular masses, emphasizing the mole concept, which relates the amount of a substance to its mass in grams. Students will learn about molar mass, percentage composition, and the difference between empirical and molecular formulae.

Chemical equations and stoichiometry are central to this unit, teaching students how to write and balance chemical equations and perform calculations to determine the quantities of reactants and products involved in chemical reactions. Mastery of these concepts is crucial for solving more complex problems in chemistry.

Unit 2- Atomic Structure

Unit II of the JEE Main 2024 Chemistry syllabus delves into atomic structure and the fundamental principles of quantum mechanics. It starts with the nature of electromagnetic radiation and the photoelectric effect, laying the groundwork for understanding atomic spectra. The spectrum of the hydrogen atom is explored, highlighting how it provides evidence for quantized energy levels in atoms.

A key focus is the Bohr model of the hydrogen atom, which introduces postulates about electron orbits and energy levels. The unit covers the derivation of equations for electron energy and orbit radii, while also addressing the model’s limitations. The dual nature of matter, represented by de Broglie’s relationship, and the Heisenberg uncertainty principle are discussed, emphasizing the shift from classical to quantum mechanical views of atoms.

The quantum mechanical model is introduced, explaining atomic orbitals as one-electron wave functions. This section includes the concept of quantum numbers (principal, angular momentum, and magnetic) and their significance in defining electron positions and energies. The shapes of s, p, and d orbitals, electron spin, and the principles for electron configuration—Aufbau principle, Pauli’s exclusion principle, and Hund’s rule—are covered. These principles explain the arrangement of electrons in atoms and the stability associated with half-filled and fully filled orbitals.

Unit 3: Chemical Bonding and Molecular Structutre

Unit III of the JEE Main 2024 Chemistry syllabus explores the fundamental concepts of chemical bonding and molecular structure. It begins with the Kossel-Lewis approach, which simplifies the understanding of ionic and covalent bond formation. Ionic bonding is covered through its formation, factors influencing bond strength, and lattice enthalpy calculations, providing insight into the energy involved in forming ionic compounds.

The unit further examines covalent bonding, introducing the concept of electronegativity and Fajan’s rule, which helps in understanding the polarization of ionic bonds. The dipole moment is discussed to explain the distribution of electrical charge in molecules. Valence Shell Electron Pair Repulsion (VSEPR) theory is introduced to predict the shapes of simple molecules based on the repulsion between electron pairs in the valence shell.

A detailed quantum mechanical approach to covalent bonding is provided through Valence Bond Theory, including hybridization of s, p, and d orbitals and resonance, which explains the delocalization of electrons in molecules. Molecular Orbital Theory is also covered, focusing on Linear Combination of Atomic Orbitals (LCAOs), types of molecular orbitals (bonding and antibonding), and the significance of sigma and pi bonds. This theory helps in understanding the electronic configurations of homonuclear diatomic molecules, bond order, bond length, and bond energy. The unit concludes with an introduction to metallic bonding and hydrogen bonding, including their basic principles and applications.

Unit 4- Chemical Thermodynamics

Unit IV of the JEE Main 2024 Chemistry syllabus covers the principles of thermodynamics, focusing on the energy changes involved in chemical processes. Here’s a detailed breakdown of the key topics:

Fundamentals of Thermodynamics

• System and Surroundings: Understanding the system (the part of the universe we are studying) and its surroundings (everything else). Systems can be open, closed, or isolated based on their interaction with surroundings.
• Extensive and Intensive Properties: Extensive properties depend on the amount of matter (e.g., volume, mass), while intensive properties do not (e.g., temperature, pressure).
• State Functions: Properties that depend only on the state of the system, not on the path taken to reach that state. Examples include internal energy, enthalpy, and entropy.
• Entropy (S): A measure of the disorder or randomness in a system. It helps determine the feasibility of a process.
• Types of Processes: Includes isothermal (constant temperature), adiabatic (no heat exchange), isobaric (constant pressure), and isochoric (constant volume) processes.

The First Law of Thermodynamics

• Concepts:
  • Work (W): Energy transferred by the system to its surroundings or vice versa.
  • Heat (q): Energy transferred due to temperature difference.
  • Internal Energy (U): The total energy contained within a system.
  • Enthalpy (H): The total heat content of a system, defined as H=U+PVH = U + PVH=U+PV, where P is pressure and V is volume.
  • Heat Capacity (C): The amount of heat required to change the temperature of a substance by one degree Celsius.
  • Molar Heat Capacity: Heat capacity per mole of substance.
• Hess’s Law of Constant Heat Summation: The total enthalpy change of a reaction is the same regardless of whether it occurs in one step or multiple steps.
• Enthalpies:
  • Bond Dissociation: Energy required to break a bond.
  • Combustion: Energy released when a substance burns.
  • Formation: Energy change when one mole of a compound is formed from its elements.
  • Atomization: Energy required to convert a substance into its atomic form.
  • Sublimation: Energy required to convert a solid to a gas.
  • Phase Transition: Energy changes during changes in states (e.g., melting, boiling).
  • Hydration: Energy change when ions interact with water.
  • Ionization: Energy required to remove an electron from an atom or ion.
  • Solution: Energy change when a solute dissolves in a solvent.

The Second Law of Thermodynamics

• Spontaneity of Processes: Determines whether a process occurs spontaneously under given conditions.
  • ΔS of the Universe: Entropy change of the universe, which must increase for a spontaneous process.
  • ΔG of the System: Gibbs free energy change, which indicates spontaneity. A negative ΔG indicates a spontaneous process.
  • ΔG° (Standard Gibbs Energy Change): Gibbs free energy change under standard conditions (1 atm, 298 K).
  • Equilibrium Constant (K): Reflects the ratio of concentrations of products to reactants at equilibrium. The relationship between ΔG° and K is given by ΔG°=−RTln⁡KΔG° = -RT \ln KΔG°=−RTlnK, where R is the gas constant and T is the temperature.

This unit provides the foundation for understanding energy transformations in chemical reactions and helps in predicting the direction and extent of chemical processes.

Unit 5- Solutions

• Different methods for expressing the concentration of 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, the elevation of boiling point and osmotic pressure; Determination of molecular mass using colligative properties; Abnormal value of molar mass, van Hoff factor and its significance.

Unit 6- Equilibrium

• The meaning of equilibrium is the concept of dynamic balance.
• Equilibria involving physical processes: Solid-liquid, liquid-gas, and solid-gas equilibria, Henry’s law, general characteristics of equilibrium involving physical processes.
• Equilibria involving chemical processes: Law of chemical equilibrium, equilibrium constants (Kp and Kc) and their significance, the significance of AG and AG” in chemical equilibria, factors affecting equilibrium concentration, pressure, temperature, the effect of catalyst; Le Chatelier’s principle.
• Ionic equilibrium: Weak and robust 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.

Unit 7- Redox Reactions and Electrochemistry

• Electronic concepts of oxidation and reduction, redox reactions, oxidation number, rules for assigning oxidation number, and balancing of redox reactions.
• Electrolytic and metallic conduction, conductance in electrolytic solutions, 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.

Unit 8- Chemical Kinetics

• Rate of a chemical reaction, factors affecting the price of reactions: concentration, temperature, pressure, and catalyst; elementary and complex results, order and molecularity of results; 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 responses.
• Arrhenius theory, activation energy, and its calculation, collision theory of bimolecular gaseous reactions (no derivation).

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Inorganic Chemistry

Inorganic Chemistry is part of Section B, containing 8 Units.

Unit 9- Classification of Elements and Periodicity in Properties

Modem 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, electron gain enthalpy, valence, oxidation states, and chemical reactivity.

Unit 10: P-Block Elements

Group 13 to Group 18 Elements:
The p-block elements, from Group 13 to Group 18, show distinct trends in physical and chemical properties as one moves across periods or down groups. Each group has unique characteristics, with notable differences in behavior observed in the first element of each group due to their smaller size and higher electronegativity.

Unit 11: d- and f-Block Elements

Transition Elements: Transition metals, located in the d-block, are recognized for their diverse properties such as varying oxidation states, catalytic behavior, and colorful compounds. Key features include their ionization enthalpies, atomic radii, and magnetic properties. Important compounds like potassium dichromate (K2Cr2O7) and potassium permanganate (KMnO4) are discussed for their preparation and applications.

Inner Transition Elements: The f-block elements consist of lanthanoids and actinoids. Lanthanoids are noted for their similar electronic configurations and lanthanoid contraction, influencing their properties and applications. Actinoids, characterized by their radioactive nature and various oxidation states, are significant in nuclear chemistry and energy production.

Unit 12: Coordination Compounds

Introduction to Coordination Compounds: Coordination compounds, also known as complex compounds, are formed by the coordination of metal ions with ligands. The study begins with Werner’s theory, which laid the foundation for understanding these compounds. Key concepts include the coordination number (the number of ligand attachments to a central metal), denticity (the number of bonds a ligand can form), and chelation (the formation of ring structures by multidentate ligands).

IUPAC Nomenclature and Isomerism: The unit covers the IUPAC rules for naming mononuclear coordination compounds, which involve naming the metal center and the ligands in a specific order. It also explores isomerism in these compounds, including structural isomers and stereoisomers, which result from different spatial arrangements of ligands.

Bonding and Theoretical Approaches: The bonding in coordination compounds is explained through the Valence Bond Theory and an introduction to Crystal Field Theory. Crystal Field Theory helps explain the color and magnetic properties of these compounds, based on the interaction between the metal ion’s d-orbitals and the surrounding ligands.

Applications and Importance: Coordination compounds play significant roles in various fields, such as qualitative analysis for identifying metal ions, metal extraction processes, and biological systems, including enzyme function and oxygen transport in hemoglobin.

Organic Chemistry

Unit 13: Purification and Characterisation of Organic Compounds

Purification Techniques: This unit covers various methods for purifying organic compounds. Crystallization involves forming pure crystals from a solution, while sublimation is used for substances that transition directly from solid to gas. Distillation separates liquids based on boiling points, and differential extraction uses solvents to separate components of a mixture. Chromatography, including techniques like paper and column chromatography, helps in separating and analyzing mixtures based on the movement of compounds through a medium.

Qualitative Analysis: Qualitative analysis focuses on detecting the presence of specific elements in organic compounds. Methods are discussed for identifying nitrogen, sulfur, phosphorus, and halogens through specific tests and reactions that reveal the presence of these elements.

Quantitative Analysis: Basic principles of quantitative analysis are introduced, including methods to estimate the amounts of carbon, hydrogen, nitrogen, halogens, sulfur, and phosphorus in organic compounds. This section also includes calculations for determining empirical and molecular formulae, involving numerical problems to understand the composition and structure of organic compounds.

Unit 14: Some Basic Principles of Organic Chemistry

Tetravalency and Molecular Shapes: This unit explores the tetravalency of carbon, which allows it to form four covalent bonds. The shapes of simple molecules are discussed, with a focus on hybridization involving s and p orbitals, which explains the geometric arrangements of atoms in organic compounds.

Classification and Nomenclature: Organic compounds are classified based on their functional groups, including those containing halogens, oxygen, nitrogen, and sulfur. The concept of homologous series is introduced, alongside isomerism, which includes structural and stereoisomerism. The unit covers both trivial and IUPAC nomenclature systems for naming organic compounds.

Bond Fission and Electronic Displacement: The types of covalent bond fission are explained, including homolytic and heterolytic cleavage, which produce free radicals and ions. The stability of carbocations and free radicals, as well as the concepts of electrophiles and nucleophiles, are discussed. Electronic displacement effects, such as inductive, electromeric, resonance, and hyperconjugation effects, are explored to understand how they influence the behavior of organic molecules.

Types of Organic Reactions: Common types of organic reactions are introduced, including substitution, addition, elimination, and rearrangement reactions. The principles and mechanisms of these reactions are examined to understand how organic compounds undergo chemical transformations.

Unit 15: Hydrocarbons

Classification and Nomenclature: Hydrocarbons are classified into alkanes, alkenes, alkynes, and aromatic hydrocarbons. The unit covers the general methods of preparation, properties, and reactions of each class. The IUPAC nomenclature for naming hydrocarbons is discussed to standardize the naming conventions of organic compounds.

Alkanes: The focus is on the conformations of alkanes, including the sawhorse and Newman projections for ethane. The mechanism of halogenation of alkanes is examined to understand how these hydrocarbons react with halogens.

Alkenes: This section addresses geometrical isomerism in alkenes and the mechanism of electrophilic addition reactions. It includes the addition of hydrogen, halogens, water, and hydrogen halides, along with the Markovnikov’s rule and peroxide effect. Additionally, ozonolysis and polymerization of alkenes are covered.

Alkynes: The acidic character of alkynes is explored, along with their reactions, including addition of hydrogen, halogens, water, and hydrogen halides. Polymerization of alkynes is also discussed.

Aromatic Hydrocarbons: The nomenclature and structure of benzene, as well as its aromaticity, are reviewed. The mechanism of electrophilic substitution in aromatic hydrocarbons is studied, including reactions such as halogenation and nitration. Friedel-Craft’s alkylation and acylation processes are discussed, along with the directive influence of functional groups in monosubstituted benzene derivatives.

Unit 16: Organic Compounds Containing Halogens

General Methods of Preparation and Properties: This unit covers the preparation, properties, and reactions of organic compounds containing halogens. It examines various methods for synthesizing these compounds and their chemical behavior in different reactions. The nature of the carbon-halogen (C-X) bond is discussed, highlighting how it influences the reactivity and stability of these compounds.

Mechanisms of Substitution Reactions: The mechanisms of substitution reactions involving halogenated organic compounds are explored. This includes understanding the different types of substitution reactions, such as nucleophilic substitution, and how the C-X bond affects the reaction pathway.

Uses and Environmental Effects: The practical applications of halogenated organic compounds are discussed, including their uses in industrial and household products. Additionally, the environmental impact of certain halogenated compounds, such as chloroform, iodoform, freons, and DDT, is addressed, focusing on their effects on ecosystems and human health.

Unit 17: Organic Compounds Containing Oxygen

General Methods of Preparation, Properties, Reactions, and Uses: This unit covers the preparation, properties, reactions, and uses of organic compounds containing oxygen, focusing on alcohols, phenols, ethers, aldehydes, ketones, and carboxylic acids.

Alcohols, Phenols, and Ethers:

• Alcohols: Discusses the identification and classification of primary, secondary, and tertiary alcohols, and explores the mechanism of alcohol dehydration.
• Phenols: Examines the acidic nature of phenols, their electrophilic substitution reactions including halogenation, nitration, and sulphonation, and the Reimer-Tiemann reaction.
• Ethers: Covers the structure of ethers and their general properties.

Aldehydes and Ketones:

• Carbonyl Group: Analyzes the nature of the carbonyl group and its role in nucleophilic addition reactions.
• Reactivity: Compares the relative reactivities of aldehydes and ketones and their important reactions, including nucleophilic additions (e.g., with HCN and NH3), Grignard reagent reactions, oxidation, reduction (e.g., Wolf-Kishner and Clemmensen), and aldol condensation.
• Reactions: Describes Cannizzaro reaction, haloform reaction, and chemical tests for distinguishing between aldehydes and ketones.

Carboxylic Acids: Explores the acidic strength of carboxylic acids and the factors affecting it.

Unit 18: Organic Compounds Containing Nitrogen

General Methods of Preparation, Properties, Reactions, and Uses: This unit addresses the preparation, properties, reactions, and applications of organic compounds containing nitrogen, focusing on amines and diazonium salts.

Amines:

• Nomenclature and Classification: Covers the naming and classification of amines into primary, secondary, and tertiary types.
• Structure and Basic Character: Examines the structure of amines and their basicity, including factors influencing their basic character.
• Identification: Discusses methods for identifying primary, secondary, and tertiary amines based on their properties.

Diazonium Salts:

• Importance: Highlights the significance of diazonium salts in synthetic organic chemistry, including their role in various chemical reactions and applications.

Unit 19: Biomolecules

General Introduction and Importance: This unit provides an overview of biomolecules, emphasizing their critical roles in biological systems and their classification.

Carbohydrates:

• Classification: Differentiates between aldoses and ketoses.
• Monosaccharides: Focuses on glucose and fructose.
• Oligosaccharides: Discusses sucrose, lactose, and maltose, including their constituent monosaccharides.

Proteins:

• α-Amino Acids and Peptide Bond: Introduces the structure and bonding of α-amino acids and peptide bonds.
• Polypeptides and Protein Structure: Explains primary, secondary, tertiary, and quaternary structures (qualitative overview).
• Denaturation and Enzymes: Covers protein denaturation and the role of enzymes.

Vitamins:

• Classification and Functions: Outlines the types of vitamins and their physiological roles.

Nucleic Acids:

• Chemical Constitution: Describes the structure of DNA and RNA.
• Biological Functions: Discusses the roles of nucleic acids in biological processes.

Hormones:

• General Introduction: Provides an overview of hormones and their functions in the body.

Unit 20: Principles Related to Practical Chemistry

Detection of Extra Elements and Functional Groups:

• Extra Elements: Methods for identifying nitrogen, sulfur, and halogens in organic compounds.
• Functional Groups: Techniques for detecting hydroxyl (alcoholic and phenolic), carbonyl (aldehyde and ketones), carboxyl, and amino groups.

Chemistry of Preparation:

• Inorganic Compounds: Preparation and chemistry of Mohr’s salt and potash alum.
• Organic Compounds: Synthesis of acetanilide, p-nitro acetanilide, aniline yellow, and iodoform.

Titrimetric Exercises:

• Acids and Bases: Techniques for titration involving acids, bases, and indicators.
• Oxalic Acid vs. KMnO4: Specific procedures and principles.
• Mohr’s Salt vs. KMnO4: Titrimetric analysis methods.

Qualitative Salt Analysis:

• Cations: Principles of detecting Pb²⁺, Cu²⁺, Al³⁺, Fe³⁺, Zn²⁺, Ni²⁺, Ca²⁺, Ba²⁺, Mg²⁺, and NH₄⁺.
• Anions: Techniques for identifying CO₃²⁻, S²⁻, SO₄²⁻, NO₃⁻, NO₂⁻, Cl⁻, Br⁻, and I⁻ (excluding insoluble salts).

Chemical Principles in Experiments:

• Enthalpy of Solution: Measuring the enthalpy change during the dissolution of CuSO₄.
• Enthalpy of Neutralization: Evaluating the enthalpy change when a strong acid reacts with a strong base.
• Preparation of Sols: Making lyophilic and lyophobic sols.
• Kinetic Study: Investigating the reaction kinetics of iodide ions with hydrogen peroxide at room temperature.

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