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.
