CHEMISTRY SYLLABUS JEE (MAIN)
PHYSICAL CHEMISTRY
UNIT I: SOME BASIC CONCEPTS IN CHEMISTRY
Matter and its nature, Dalton's atomic theory, Concept of atom, molecule, element, and compound Laws of chemical combination, Atomic and molecular masses, mole concept, molar mass, percentage composition, empirical and molecular formulae, Chemical equations and stoichiometry.
UNIT 2: ATOMIC STRUCTURE
Nature of electromagnetic radiation, photoelectric effect, spectrum of the hydrogen atom, Bohr model of 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, Heisenberguncertainty principle, elementary ideas of quantum mechanics, the quantum mechanical model of the atom and 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 andHund'srule, electronic configuration of elements and extra stability of half-filled and completely filled orbitals.
UNIT 3: 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, and 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, and 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.
UNIT 4: CHEMICAL THERMODYNAMICS
Fundamentals of thermodynamics: system and surroundings, extensive and intensive properties, state functions, entropy, and types of processes. The first law of thermodynamics is the 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, ΔS of the universe, and ΔG of the system as criteria for spontaneity. ΔG° (standard Gibbs energy change) and equilibrium constant.
UNIT 5: SOLUTIONS
Different methods for expressing the concentration of a solution—molality, molarity, mole fraction, and 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—a relative lowering of vapor pressure, depression of freezing point, elevation of boiling point, and osmotic pressure; determination of molecular mass using colligative properties; abnormal value of molar mass; van’t Hoff factor and its significance.
UNIT 6: EQUILIBRIUM
The meaning of equilibrium is the concept of dynamic equilibrium. Equilibria involving physical processes: solid-liquid, liquid-gas, gas-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 ΔG and ΔG° in chemical equilibrium, factors affecting equilibrium concentration, pressure, temperature, the effect of a catalyst, and 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, solubility products, and 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, and fuel cells.
UNIT 8: 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 bi-molecular gaseous reactions (no derivation).
INORGANIC CHEMISTRY
UNIT 9: 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
UNIT 10: 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.
UNIT 11: 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
Lanthanoids—electronic configuration, oxidation states, and lanthanoid contraction.
Actinoids—Electronic configuration and oxidation states
UNIT 12: 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), basic ideas of crystal field theory, color and magnetic properties, and importance of coordination compounds (in qualitative analysis, extraction of metals, and in biological systems).
ORGANIC CHEMISTRY
UNIT 13: PURIFICATION AND CHARACTERIZATION 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, and phosphorus. Calculations of empirical formulas and molecular formulas, numerical problems in organic quantitative analysis,
UNIT 14: 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 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 are substitution, addition, elimination, and rearrangement.
UNIT 15: 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, 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, and nitration. Friedel-Crafts alkylation and acylation, directive influence of the functional group in mono-substituted benzene.
UNIT 16: ORGANIC COMPOUNDS CONTAINING HALOGENS
General methods of preparation, properties and reactions, nature of the C-X bond, and mechanisms of substitution reactions. Uses and environmental effects of chloroform, iodoform, freons, and DDT.
UNIT 17: 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, sulfonation, and the Reimer-Tiemann reaction. Ethers: Structure. Aldehydes and Ketones: Nature of the carbonyl group, nucleophilic addition to the >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), and the acidity of the hydrogen. Aldol condensation, Cannizzaro reaction, haloform reaction, and chemical tests to distinguish between aldehydes and ketones. Carboxylic Acids: Acidic Strength and Factors Affecting It.
UNIT 18: 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
UNIT 19: 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 bonds, 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. Hormones (General Introduction)
UNIT 20: PRINCIPLES RELATED TO PRACTICAL CHEMISTRY
Detection of extra elements (nitrogen, sulfur, halogens) in organic compounds; detection of the following functional groups: hydroxyl (alcoholic and phenolic), carbonyl (aldehyde and ketones), and carboxyl and amino groups in organic compounds.
- The chemistry involved in the preparation of the following:
Inorganic compounds: Mohr’s salt, potash alum. Organic compounds: acetanilide, p-nitro acetanilide, aniline yellow, and iodoform. The chemistry involved in the titrimetric exercises—acids, bases, and the use of indicators, oxalic acid vs. KMnO₄, and Mohr’s salt vs. KMnO₄.
• Chemical principles involved in the qualitative salt analysis:
Cations: Pb²⁺, Cu²⁺, Al³⁺, Fe³⁺, Zn²⁺, Ni²⁺, Ca²⁺, Ba²⁺, Mg²⁺, NH₄⁺ Anions: CO₃²⁻, S²⁻, SO₄²⁻, NO₃⁻, NO₂⁻, Cl⁻, Br⁻, and I⁻ (insoluble salts excluded)
- (Insoluble salts excluded). Chemical principles involved in the following experiments:
1. Enthalpy of solution of CuSO₄
2. Enthalpy of neutralization of strong acid and strong base.
3. Preparation of lyophilic and lyophobic sols.
4. Kinetic study of the reaction of iodide ions with hydrogen peroxide at room temperature.
CHEMISTRY SYLLABUS JEE (ADVANCED)
CHEMISTRY
1. General topics
Concept of atoms and molecules; Dalton’s atomic theory; mole concept; chemical formulae; balanced chemical equations; calculations (based on the mole concept and stoichiometry) involving common oxidation-reduction-neutralization and displacement reactions; concentration in terms of mole fraction, molality, and normality.
2. States of Matter: Gases and Liquids
Gas laws and ideal gas equation, absolute scale of temperature; Deviation from ideality, van der Waals equation, kinetic theory of gases, average, square, mean square, and most probable velocities and their relation with temperature; Law of partial pressures; diffusion of gases. Intermolecular interactions: types, distance dependence, and their effect on property values: vapor pressure, surface tension, and viscosity.
3. Atomic Structure
Bohr model, spectrum of hydrogen atom; wave-particle duality, de Broglie hypothesis; uncertainty principle; qualitative quantum mechanical picture of the hydrogen atom: energies, quantum functions, wave functions, and probabilities; ity (plots, p, l, y), shapes of s, p, and d orbitals; Aufbau principle; Pauli’s exclusion principle; and Hund’s rule.
4. Chemical Bonding and Molecular Structure
Orbital overlap hybridization bond; hybridization involving s, p, and d orbitals only; molecular orbital energy diagrams for homonuclear dNe₂); c species (up to Ne₂); Hydrogen bond; Polarity in molecules, dipole moment; VSEPR model and shapes of molecules (linear, angular, triangular, square planar, pyramidal, square pyramidal, tetrahedral, bipyramidal, tetrahedral, and octahedral).
5. Chemical Thermodynamics
Intensive and extensive properties, state functions, and the first law of thermodynamics; internal energy only; work (pressure-volume only); and heat. Enthalpy, heat capacity, standard state, Hess’s law, enthalpy of vaporization and fusion and vaporization, and lattice enthalpy; the second law of thermodynamics; entropy, Gibbs energy, and criteria of equilibrium and spontaneity.
6. Chemical and Ionic Equilibrium
La∆Gof ma∆G⊖action; Significance of ∆G and ∆G⊖ in chemical equilibrium; Equilibrium constant (Kp and Kc) and reaction quotient, Le Chatelier’s principle, effect of concentration, temperature, and pressure; Solubility product and pH, applications, common ion effect, pH, and buffer solutions; Acids and bases (Brønsted and Lewis concepts); hydrolysis of salts.
7. Electrochemistry
Electrochemical cells and cell reactions; standard electrode potentials; Electrochemical work, Nernst equation; electrochemical series, EMF of galvanic cells; Faraday’s laws of electron equivalence, electrolytic conductance, specific, equivalent, and molar conductivity; Kohlrausch’s law; Batteries: Primary and Secondary Fuel Cells; Corrosion.
8. Chemical Kinetics
Rates of chemical reactions; order and molecularity of reactions; rate law, rate constant, half-life; different first-order rate expressions for zero- and first-order reactions; temperature dependence of rate constant (Arrhenius equation) and heterogeneous energy; Catalysis: Homogeneous and heterogeneous, act catalysis, selectivity of solid catalysts, enzyme catalysis, and its mechanism.
9. Solid State
Classification of solids, crystalline state, seven close-packed ems (cell parameters) a, b, c, α, β, γ), close-packed structure of solids (cubic and hexagonal neighbors) in FCC, BCC, and HCP lattices; nearest neighbors, ionic radii, and radius ratio, poisolutions:
10. Solutions
Henry’s law; Raoult’s law of vapor solutions; colligative properties: lowering of vapor pressure, elevation of boiling point, depression of freezing point, and osmotic pressure; van’t Hoff factor.
11. Surface Chemistry
Elementary concepts of adsorption: physisorption and chemisorption, preparation, and ion isotherm; Colloids: types, methods of prep surfactants, general properties; elementary ideas of emulsions, surfactants, and micelles (Only definitions and examples.).
12. Classification of Elements and Periodic Properties
Modern periodic law and the present form of the periodic table; electronic configuration of elements; periodic trends in atomic radius, ionic radius, ionization enthalpy, electron gain enthalpy, valence, oxidation states, electrons, the periodic table, and chemical reactivity.
13. Hydrogen
Posi Properties of hydrogen in the periodic table, hydrides, isocovalent bonds, and reparation; properties and uses of hydrogen; hydrides—ionic, covalent, and interest peroxide preparation; preparation of chemical properties of water, heavy water; hydrogen peroxide preparation, reactions, and uses; and metals: reactivity as a fuel.
14. s-Block Elements
Alkali and alkaline earth metals—reactivity towards air, water, dihydrogen, halogens, and acids; their reducing nature, including solutions in liquid ammonia; uses of these elements; general characteristics of their oxides, hydroxides, halides, and salts of oxoacids; anomalous behavior of lithium and beryllium; preparation, properties, and uses of compounds of sodium (sodium carbonate, sodium chloride, sodium hydroxide, and sodium hydrogen carbonate) and calcium (calcium oxide, calcium hydroxide, calcium carbonate, and calcium sulfate).
15. p-Block Elements
Oxidation state and trends in chemical reactivity of elements of groups 13-17; anomalous properties of boron, carbon, nitrogen, oxygen, and fluorine with respect to other elements in their respective groups.
Group 13: Reactivity towards acids, alkalis, and halogens; preparation, properties, and uses of borax, orthoboric acid, diborane, boron trifluoride, aluminum chloride, and alums; uses of boron and aluminum.
Group 14: Reactivity towards water and halogen; allotropes of carbon and uses of carbon; preparation, properties, and uses of carbon monoxide, carbon dioxide, silicon dioxide, silicones, silicates, and zeolites.
Group 15: Reactivity towards hydrogen, oxygen, and halogen; allotropes of phosphorous; preparation, properties, and uses of dinitrogen, ammonia, and nitric acid, phosphine, phosphorus trichloride, phosphorus pentachloride; oxides of nitrogen and oxoacids of phosphorus.
Group 16: Reactivity towards hydrogen, oxygen, and halogen; simple oxides; allotropes of sulfur; preparation/manufacture, properties, and uses of dioxygen, ozone, sulfur dioxide, and sulfuric acid; oxoacids of sulfur.
Group 17: Reactivity towards hydrogen, oxygen, and metals; preparation/manufacture, properties, and uses of chlorine and hydrogen chloride and interhalogen compounds; oxoacids of halogens; bleaching powder.
Group 18: Chemical properties and uses; compounds of xenon with fluorine and oxygen.
16. d-Block Elements
Oxidation states and their stability; standard electrode potentials; interstitial compounds; alloys; catalytic properties; applications; preparation, structure, and reactions of oxoanions of chromium and manganese.
17. f-Block Elements
Lanthanoid and actinoid contractions; oxidation states; general characteristics.
18. Coordination Compounds
Werner’s theory, nomenclature, cis-trans and ionization isomerism, hybridization and geometries (linear, tetrahedral, square planar, and octahedral) of mononuclear coordination compounds; Bonding [VBT and CFT (octahedral and tetrahedral fields)]; magnetic properties (spin-only) and color of 3D-series coordination compounds; ligands and spectrochemical series; stability; importance and applications; metal carbonyls.
19. Isolation of Metals
Metal ores and their concentration; extraction of crude metal from concentrated ores: thermodynamic (iron, copper, zinc) and electrochemical (aluminum) principles of metallurgy; cyanide process (silver and gold); refining.
20. Principles of Qualitative Analysis
Groups I to V (only Ag⁺, Hg₂⁺, Cu₂⁺, Pb₂⁺, Fe³⁺, Cr³⁺, Al³⁺, Ca²⁺, Ba²⁺, Zn²⁺, Mn²⁺, and Mg²⁺); nitrate, halides (excluding fluoride), carbonate, bicarbonate, sulfate, and sulfide.
21. Environmental Chemistry
Atmospheric pollution, water pollution, soil pollution, industrial waste, strategies to control environmental pollution, and green chemistry. Basic Principles of Organic Chemistry Hybridization of carbon; σ and π-bonds; Shapes of simple organic molecules; aromaticity; structural and geometrical isomerism; stereoisomers; and
stereochemical relationship (enantiomers, diastereomers, meso) of compounds containing only up to two asymmetric centers (R, S, and E, Z configurations) excluded); determination of empirical and molecular formulae of simple compounds by combustion method only; IUPAC nomenclature of organic molecules (hydrocarbons, including simple cyclic hydrocarbons and their mono-functional and bi-functional derivatives only); hydrogen bonding effects; inductive, resonance, and hyperconjugative effects; acidity and basicity of organic compounds; reactive intermediates produced during homolytic and heterolytic bond cleavage; formation, structure, and stability of carbocations, carbanions, and free radicals.
22. Alkanes
Homologous series; physical properties (melting points, boiling points, and density) and effect of branching on them; Conformations of ethane and butane (Newman projections only); Preparation from alkyl halides and aliphatic carboxylic acids; Reactions: combustion, halogenation (including allylic and benzylic halogenation), and oxidation.
23. Alkenes and Alkynes
Physical properties (boiling points, density, and dipole moments); preparation by elimination reactions; acid-catalyzed hydration (excluding the stereochemistry of addition and elimination); metal acetylides; reactions of alkenes with KMnO₄ and ozone; reduction of alkenes and alkynes; electrophilic addition reactions of alkenes with X₂, HX, HOX (X=halogen); Effect of peroxide on addition reactions: cyclic polymerization reaction of alkynes.
24. Benzene
Structure: Electrophilic substitution reactions: halogenation, nitration, sulfonation, Friedel-Crafts alkylation, and acylation; effect of directing groups (monosubstituted benzene) in these reactions.
25. Phenols
Physical properties: preparation, electrophilic substitution reactions of phenol (halogenation, nitration, sulfonation); Reimer-Tiemann reaction, Kolbe reaction; esterification; etherification; aspirin synthesis; and oxidation and reduction reactions of phenol.
26. Alkyl Halides
Rearrangement reactions of alkyl carbocations; Grignard reactions; nucleophilic substitution reactions and their stereochemical aspects.
27. Alcohols
Physical properties: Reactions: esterification, dehydration (formation of alkanes and ethers); Reactions with sodium, phosphorus halides, ZnCl₂/concentrated HCl, and thionyl chloride; conversion of alcohols into aldehydes, ketones, and carboxylic acids.
28. Ethers
Preparation by Williamson’s synthesis: C-O bond cleavage reactions.
29. Aldehydes and Ketones
Preparation of aldehydes and ketones from acid chlorides and nitriles; aldehydes from esters; benzaldehyde from toluene and benzene; Reactions: oxidation, reduction, oxime and hydrazone formation; aldol condensation, Cannizzaro reaction; haloform reaction; nucleophilic addition reaction with RMgX, NaHSO₃, HCN, alcohol, and amine.
30. Carboxylic Acids
Physical properties: Preparation: from nitriles, Grignard reagents, hydrolysis of esters and amides; preparation of benzoic acid from alkylbenzenes; Reactions: reduction, halogenation, and formation of esters, acid chlorides, and amides.
31. Amines
Preparation from nitro compounds, nitriles, and amides; Reactions: Hoffmann bromamide degradation, Gabriel phthalimide synthesis, reaction with nitrous acid, azo coupling reaction of diazonium salts of aromatic amines, Sandmeyer and related reactions of diazonium salts, carbylamine reaction, Hinsberg test, and alkylation and acylation reactions.
32. Haloarenes
Reactions: Fittig, Wurtz-Fittig; nucleophilic aromatic substitution in haloarenes and substituted haloarenes (excluding benzyne mechanism and cine substitution).
33. Biomolecules
Carbohydrates: Classification; mono- and di-saccharides (glucose and sucrose); oxidation; reduction; glycoside formation; hydrolysis of disaccharides (sucrose, maltose, lactose); and anomers. Proteins: Amino acids; peptide linkage; structure of peptides (primary and secondary); types of proteins (fibrous and globular). Nucleic acids: Chemical composition and structure of DNA and RNA.
34. Polymers
Types of polymerization (addition, condensation); homo- and copolymers; natural rubber, cellulose, nylon, Teflon, Bakelite, PVC, biodegradable polymers; applications of polymers.
35. Chemistry in Everyday Life
Drug-target interaction, therapeutic action, and examples (excluding structures) of antacids, antihistamines, tranquilizers, analgesics, antimicrobials, and antifertility drugs; artificial sweeteners (names only); soaps, detergents, and cleansing action.
36. Practical Organic Chemistry
Detection of elements (N, S, halogens); detection and identification of the following functional groups: hydroxyl (alcoholic and phenolic), carbonyl (aldehyde and ketone), carboxyl, amino, and nitro.
