Chemistry — NEET
20 Units (Physical · Inorganic · Organic)
Physical Chemistry
Unit 1: 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 a hydrogen atom — postulates, derivation of relations for energy of the electron and radii of orbits, limitations of Bohr's model; dual nature of matter, de Broglie's relationship. Heisenberg uncertainty principle. Quantum mechanical model of the atom; atomic orbitals as one-electron wave functions; variation of ψ and ψ² with r for 1s and 2s orbitals; quantum numbers (principal, angular momentum and magnetic) and their significance; shapes of s, p and d orbitals; electron spin and spin quantum number. Aufbau principle, Pauli's exclusion principle and Hund's rule; electronic configuration of elements; extra stability of half-filled and completely filled orbitals.
Unit 3: Chemical Bonding and Molecular Structure
Kossel–Lewis approach to chemical bond formation; 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; VSEPR theory and shapes of simple molecules. Quantum mechanical approach: valence bond theory, hybridization involving s, p and d orbitals; resonance. Molecular orbital theory — LCAOs, types of molecular orbitals, sigma and pi bonds, molecular orbital electronic configurations of homonuclear diatomic molecules, 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, types of processes. 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. Second law of thermodynamics — spontaneity of processes; ΔS of the universe and ΔG of the system as criteria for spontaneity. ΔG° and equilibrium constant.
Unit 5: Solutions
Different methods for expressing concentration of solution — molality, molarity, mole fraction, percentage (by volume and mass). Vapour pressure of solutions and Raoult's law; ideal and non-ideal solutions, vapour pressure–composition plots. Colligative properties of dilute solutions — relative lowering of vapour 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
Meaning of equilibrium, concept of dynamic equilibrium. Equilibria involving physical processes: solid-liquid, liquid-gas and solid-gas equilibria; Henry's law. Law of chemical equilibrium, equilibrium constants (Kp and Kc) and their significance; factors affecting equilibrium — concentration, pressure, temperature, effect of catalyst; Le Chatelier's principle. Ionic equilibrium: weak and strong electrolytes, ionization of electrolytes; various concepts of acids and bases (Arrhenius, Brønsted–Lowry and Lewis); 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.
Unit 7: 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 8: Chemical Kinetics
Rate of a chemical reaction; factors affecting the rate — 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; 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
Unit 9: Classification of Elements and Periodicity in Properties
Modern 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. 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.
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, 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.
Unit 12: 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; colour and magnetic properties; importance of coordination compounds (in qualitative analysis, extraction of metals and in biological systems).
Organic Chemistry
Unit 13: Purification and Characterisation of Organic Compounds
Purification — crystallization, sublimation, distillation, differential extraction and chromatography; principles and their applications. Qualitative analysis — detection of nitrogen, sulphur, phosphorus and halogens. Quantitative analysis (basic principles only) — estimation of carbon, hydrogen, nitrogen, halogens, sulphur and phosphorus. Calculations of empirical and molecular formulae; 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: 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.
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. Alkenes — geometrical isomerism; mechanism of electrophilic addition; addition of hydrogen, halogens, water, hydrogen halides (Markovnikov'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, nitration, Friedel–Crafts alkylation and acylation, directive influence of the functional group in monosubstituted benzene.
Unit 16: 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.
Unit 17: Organic Compounds Containing Oxygen
General methods of preparation, properties, reactions and uses. 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. Aldehydes and ketones: nature of carbonyl group; nucleophilic addition to >C=O group, relative reactivities; important reactions — nucleophilic addition (HCN, NH₃ and its derivatives), Grignard reagent; oxidation; reduction (Wolff–Kishner and Clemmensen); acidity of α-hydrogen, aldol condensation, Cannizzaro reaction, haloform reaction; 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; 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 α-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. Hormones (general introduction).
Unit 20: Principles Related to Practical Chemistry
Detection of extra elements (nitrogen, sulphur, halogens) in organic compounds; detection of hydroxyl (alcoholic and phenolic), carbonyl (aldehyde and ketone), carboxyl and amino groups in organic compounds. Chemistry involved in the preparation of: inorganic compounds — Mohr's salt, potash alum; organic compounds — acetanilide, p-nitroacetanilide, aniline yellow, iodoform. Chemistry involved in titrimetric exercises — acids, bases and indicators, oxalic acid vs KMnO₄, Mohr's salt vs KMnO₄. Qualitative salt analysis: cations — Pb²⁺, Cu²⁺, Al³⁺, Fe³⁺, Zn²⁺, Ni²⁺, Ca²⁺, Ba²⁺, Mg²⁺, NH₄⁺; anions — CO₃²⁻, S²⁻, SO₄²⁻, NO₃⁻, NO₂⁻, Cl⁻, Br⁻, I⁻ (insoluble salts excluded). Experiments: enthalpy of solution of CuSO₄, enthalpy of neutralization of strong acid and strong base, preparation of lyophilic and lyophobic sols, kinetic study of iodide ion reaction with hydrogen peroxide.