JEE Advanced Chemistry Important Chapters

PHYSICAL CHEMISTRY 

STATES OF MATTER

Classification of matter into solid, liquid, and gaseous states.

Gaseous State: Measurable properties of gases: Gas laws - Boyle's law, Charle’s law. Graham's law of diffusion. Avogadro's law, Dalton's law of partial pressure; Concept of Absolute scale of temperature; Ideal gas equation; Kinetic theory of gases (only postulates); Concept of average, root mean square and most probable velocities; Real gases, deviation from Ideal behaviour, compressibility factor, and van der Waals equation.

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, an imperfection in solids; Electrical and magnetic properties. 

ATOMIC STRUCTURE 

Thomson and Rutherford atomic models and their limitations; Nature of electromagnetic radiation, photoelectric effect; 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's relationship. Heisenberg uncertainty principle.

Elementary ideas of quantum mechanics, quantum mechanics, the quantum mechanical model of the atom, its important features.

Concept of atomic orbitals as one-electron wave functions: Variation of  and 2 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's exclusion principle and Hund's rule, electronic configuration of elements, extra stability of half-filled and completely filled orbitals. 

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.

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; S of the universe and G of the system as criteria for spontaneity. G (Standard Gibbs energy change) and equilibrium constant. 

EQUILIBRIUM  

Meaning of equilibrium, the concept of dynamic equilibrium.

Equilibria involving physical processes: Solid-liquid, liquid - gas and solid-gas equilibria, Henry's law. General characteristics of equilibrium involving physical processes.

Equilibrium involving chemical processes: Law of chemical equilibrium, equilibrium constants (Kp and Kc) and their significance, the significance of G and G in chemical equilibrium, factors affecting equilibrium concentration, pressure, temperature, the effect of 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.

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, 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 9: CHEMICAL KINETICS 

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). 

INORGANIC CHEMISTRY

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. 

S -BLOCK ELEMENTS (ALKALI AND ALKALINE EARTH METALS) 

Group -1 and 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 and sodium hydroxide and sodium hydrogen carbonate; Industrial uses of lime, limestone. Plaster of Paris and cement: Biological significance of Na, K. Mg, and Ca. 

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 aluminum; Structure, properties, and uses of borax, boric acid, diborane, boron trifluoride, aluminum chloride, and alums.

Group -14 

The 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; Allotrophic 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 ozone: Allotropic forms of sulphur; Preparation, properties, structures, and uses of sulphuric acid (including its industrial preparation); Structures of oxoacids of sulphur.

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, colour, catalytic behaviour, magnetic properties, complex formation, interstitial compounds, alloy formation; Preparation, properties, and uses of K2Cr2O7, and KMnO4.

Inner Transition Elements: Lanthanoids - Electronic configuration, oxidation states, and lanthanoid contraction. Actinoids - Electronic configuration and oxidation states. 

ENVIRONMENTAL CHEMISTRY 

Environmental pollution: Atmospheric, water, and soil.

Atmospheric pollution: Tropospheric and Stratospheric

Tropospheric pollutants: Gaseous pollutants: Oxides of carbon, nitrogen, and sulphur, 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 the 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. 

ORGANIC CHEMISTRY

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: and those containing halogens, oxygen, nitrogen, and sulphur; 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. 

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 (Markownikoffs and peroxide effect): Ozonolysis 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 - Craft's alkylation and acylation, directive influence of the functional group in monosubstituted benzene. 

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. 

ORGANIC COMPOUNDS CONTAINING OXYGEN 

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

ALCOHOLS, PHENOLS, AND ETHERS 

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 (Wolf 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.

BIOMOLECULES

General introduction and importance of biomolecules.

Carbohydrates: Classification; aldoses and ketoses: monosaccharides (glucose and fructose) and constituent monosaccharides of oligosaccharides (sucrose, lactose, and maltose).

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.

Nucleic Acids: Chemical constitution of DNA and RNA. Biological functions of nucleic acids. 

Topics

No of Questions

Weightage of Marks (%)

The periodic table and Representative Elements

3

12

Transition Elements and Coordination Chemistry

3

12

Atomic Structure

2

8

Nuclear Chemistry And Environment

2

8

Chemical Kinetics

1

4

Solid State And Surface Chemistry

2

8

Thermodynamics And Gaseous State

2

8

Chemical Bonding

2

8

Chemical And Ionic Equilibrium

2

8

Solution and Colligative Properties

1

4

Hydrocarbon

1

4

Aromatic Compounds

1

4

Redox Reaction

1

4

Mole Concept

1

4

Alkyl Halides

1

4

Carboxylic Acid and their Derivatives

1

4

Electrochemistry

1

4

General Organic Chemistry

1

4

Stereochemistry

1

4

Carbohydrates, amino acid and Polymers

1

4