JEE Mains Chemistry Syllabus 2024 (Updated), Download Detailed Syllabus PDF

1. Kossel-Lewis approach to chemical bond formation, the concept of ionic and covalent bonds.
2. Ionic Bonding: Formation of ionic bonds, factors affecting the formation of ionic bonds; calculation of lattice enthalpy.
3. 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:

1. Valence bond theory – Its important features, the concept of hybridization involving s, p, and d orbitals; Resonance.
2. 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.
3. Elementary idea of metallic bonding. Hydrogen bonding and its applications.

1. Fundamentals of thermodynamics: System and surroundings, extensive and intensive properties, state functions, types of processes.
2. 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.
3. Second law of thermodynamics: Spontaneity of processes; AS of the universe and AG of the system as criteria for spontaneity, AG” (Standard Gibbs energy change) and equilibrium constant.

1. Meaning of equilibrium is the concept of dynamic equilibrium
2. Equilibria involving physical processes: Solid-liquid, liquid – gas and solid-gas equilibria, Henry’s law, general characteristics of equilibrium involving physical processes.
3. 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.
4. 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, solubility of sparingly soluble salts and solubility products, buffer solutions.

1. Electronic concepts of oxidation and reduction, redox reactions, oxidation number, rules for assigning oxidation number, and balancing of redox reactions.
2. Electrolytic and metallic conduction, conductance in electrolytic solutions, molar conductivities and their variation with concentration: Kohlrausch’s law and its applications.
3. 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.

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.

• Group -13 to Group 18 Elements– General Introduction: Electronic configurations 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, (PC13, PCI,); Structures of oxides and oxoacids of nitrogen and phosphorus.
• Group -16 Preparation, properties, structures and uses of ozone; Allotropic forms of sulfur; Preparation, properties, structures and uses of sulphuric acid (including its industrial preparation); Structures of oxoacids of sulfur.
• Group -17– Preparation, properties and uses of hydrochloric acid; Trends in the acidic nature of hydrogen halides; Structures of Interhalogen compounds and oxides and oxoacids of halogens.
• Group-18- Occurrence and uses of noble gases; Structures of fluorides and oxides of xenon.

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 K2 Cr, 07 and Kmn04.

Inner Transition Elements

Lanthanoids – Electronic configuration, oxidation states and lanthanide contraction.

Actinides – Electronic configuration and oxidation states.

Co-Ordination 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 in biological systems).