NCERT Chemistry Chapters List

Master the fundamental principles of chemistry: particulate nature of matter, SI base units, scientific measurements, the 5 laws of chemical combinations, Dalton’s atomic theory, mole concept, empirical formulas, and solution stoichiometry.

Master atomic theory from first principles: discovery of electron, proton, and neutron; Thomson & Rutherford nuclear models; Planck’s quantum hypothesis & photoelectric effect; Bohr’s quantized planetary model & hydrogen spectra; de Broglie matter waves & Heisenberg uncertainty principle; Schrödinger wave equation, quantum numbers (n, l, ml, ms), orbital shapes, nodes, Aufbau principle, Pauli exclusion, Hund’s rule, and electron configurations (Z = 1 to 30).

Master periodic classification from first principles: historical genesis (Dobereiner’s triads, Newlands’ octaves, Lothar Meyer, Mendeleev’s table & predictions for Ga/Ge), Moseley’s Modern Periodic Law & X-ray spectra discovery, long form 7-period/18-group architecture, IUPAC nomenclature for Z > 100, s/p/d/f block characteristics, metals/metalloids/non-metals, periodic trends in atomic & ionic radii, isoelectronic species contraction, ionization enthalpy (ΔiH) & anomalies (Be/B, N/O), electron gain enthalpy (ΔegH) & F/Cl inversion, Pauling electronegativity, oxidation states, second-period anomalous behaviors, diagonal relationships, and acid-base oxide periodicity across Period 3.

Master chemical bonding from first principles: Kössel-Lewis octet framework and Lewis dot structures, ionic bond energetics and Born-Haber lattice enthalpy (NaCl: -788 kJ/mol), bond parameters (radii, angles, average bond enthalpies, resonance hybrids), bond polarity and dipole moments (Debye units, NH3 vs NF3 vector opposition, Fajans rules), VSEPR 3D geometries and lone-pair repulsion hierarchy (CH4, NH3, H2O, PCl5 axial bond elongation, SF4, ClF3, XeF4), Valence Bond Theory potential energy curves and sigma/pi overlaps, Pauling hybridisation (sp, sp2, sp3, sp3d, sp3d2), Molecular Orbital Theory with 2s-2p mixing (Z <= 7 vs Z > 7), bond order calculation, paramagnetism of O2, double bond in C2, and hydrogen bonding (inter vs intra, ice cage density anomaly at 4°C).

Master chemical thermodynamics from first principles: open, closed, and isolated systems; state functions vs path functions; First Law of Thermodynamics and internal energy; reversible vs irreversible pressure-volume work; enthalpy, calorimetry (bomb vs constant pressure), and heat capacities (Cp - Cv = R); standard formation enthalpies, Hess’s law of heat summation, bond enthalpies, and lattice energy via Born-Haber cycle; spontaneity, entropy, Second Law, and Gibbs free energy (ΔG = ΔH - TΔS); Third Law absolute zero entropy, and the thermodynamic equilibrium constant (ΔrG° = -RT ln K).

Master dynamic chemical and ionic equilibria from first principles: dynamic phase and chemical equilibria (Haber deuterium scrambling); Law of Mass Action and equilibrium constants (Kc, Kp = Kc(RT)^Δn); reaction quotient (Qc) and thermodynamic connection (ΔrG° = -RT ln K); Le Chatelier’s principle (concentration, pressure, volume, temperature via van ’t Hoff, inert gas, and catalyst invariance); Arrhenius, Brönsted-Lowry, and Lewis acid-base theories; autoionization of water and ionic product (Kw = 1.0 × 10⁻¹⁴); logarithmic pH scale; weak acid/base ionization (Ka, Kb) and Ostwald’s dilution law; polyprotic acids and common-ion effect; salt hydrolysis in all 4 categories; buffer solutions and Henderson-Hasselbalch equations; and sparingly soluble salts, solubility product (Ksp), precipitation criteria (Qsp > Ksp), common-ion suppression, and pH-dependent solubility.