UPSC Civil Services (Mains)

• Atomic structure · 1.3 Particle in a one-dimensional box · 1.1 Postulates of quantum mechanics: operators, eigenfunctions, Hermitian operators and acceptable wave functions · 1.2 Uncertainty principle, de Broglie relation and wave–particle duality · 1.4 Hydrogen atom: Schrödinger equation, quantum numbers, radial distribution, nodes and orbital shapesFreeOpen 1.3Open 1.1Open 1.2Open 1.4
• Chemical bonding · 2.2 VSEPR, hybridisation and Bent's rule · 2.11 Molecular orbital theory: LCAO, homonuclear and heteronuclear diatomics (O₂, N₂, CO, NO, CN⁻, HF), bond order and magnetism · 3.4 Ionic bonding: lattice energy, Born–Haber cycle, Born–Landé and Kapustinskii equations, Fajans’ rulesFreeOpen 2.2Open 2.11Open 3.4
• Solid state · 3.2 Defects in solids, non-stoichiometry and semiconductors · 3.1 Crystal systems, Miller indices, Bragg's law and radius ratioFreeOpen 3.2Open 3.1
• The gaseous state and transport phenomenon · 4.2 Kinetic theory of gases: Maxwell distribution, collisions, mean free path, effusion and transport · 4.1 Real gases: van der Waals equation, critical constants, Boyle temperatureFreeOpen 4.2Open 4.1
• Liquid state · 4.3 Liquid state: surface tension, Kelvin equation, capillary action, viscosity and liquid crystalsFreeOpen
• Thermodynamics · 6.1 Second and third laws: entropy, Gibbs and Helmholtz energies, Maxwell relations · 6.2 Chemical potential, partial molar quantities, Gibbs–Duhem equation, fugacity and activity · 6.3 Chemical equilibrium: ΔG° and K, Kp, Kc and Kx, van ’t Hoff isochore and isobar · 5.1 First law of thermodynamics: work, heat, enthalpy, adiabatic changes, Joule–Thomson effect, thermochemistryFreeOpen 6.1Open 6.2Open 6.3Open 5.1
• Phase equilibria and solutions · 7.1 Phase rule, phase diagrams, Clausius–Clapeyron equation, eutectics and partially miscible liquids · 7.2 Solutions: Raoult’s and Henry’s laws, colligative properties, van ’t Hoff factor and activityFreeOpen 7.1Open 7.2
• Electrochemistry · 8.2 Electrochemical cells: Nernst equation, emf and electrodes · 8.3 Electrolytes: conductance, Kohlrausch, Debye–Hückel and transport numbers · 8.4 Electrode kinetics: double layer, overpotential, Butler–Volmer and Tafel equations, polarography and voltammetryFreeOpen 8.2Open 8.3Open 8.4
• Chemical kinetics · 9.2 Theories of reaction rate: Arrhenius, collision and transition-state theory · 9.1 Rate laws and order: integrated rate equations, half-life, reversible, parallel and consecutive reactionsFreeOpen 9.2Open 9.1
• Photochemistry · 10.1 Photochemistry: quantum yield, Jablonski diagram, H₂–halogen reactionsFreeOpen
• Surface phenomena and catalysis · 11.2 Adsorption, heterogeneous catalysis and colloidsFreeOpen
• Bio-inorganic chemistry · 12.2 Bio-inorganic chemistry: haemoglobin, cytochromes, Fe–S proteinsFreeOpen
• Coordination chemistry · 13.2 Crystal field theory · 13.3 Werner theory, isomerism, IUPAC names and VBT of complexes · 13.4 Organometallics: 18-electron rule, oxidative addition, Wilkinson's catalyst · 13.5 Metal carbonyls, nitrosyls, 18-electron rule and metal clusters · 13.6 Substitution in complexes: labile and inert, trans effect, stability constants · 13.7 Electronic spectra of complexes: term symbols, selection rules, charge transferFreeOpen 13.2Open 13.3Open 13.4Open 13.5Open 13.6Open 13.7
• Main group chemistry · 2.2 VSEPR, hybridisation and Bent's rule · 14.2 Non-aqueous solvents: liquid NH₃, HF, H₂SO₄, SO₂, BrF₃ and superacids · 14.4 Main group chemistry: boranes, borazine, phosphazenes, silicates, silicones, interhalogens, xenon and S–N compoundsFreeOpen 2.2Open 14.2Open 14.4
• General chemistry of 'f' block elements · 15.1 Lanthanides and actinides: contraction, magnetism, spectra, separationFreeOpen

Free to read: 13.2 Crystal field theory, 8.4 Electrode kinetics: double layer, overpotential, Butler–Volmer and Tafel equations, polarography and voltammetry, 7.2 Solutions: Raoult’s and Henry’s laws, colligative properties, van ’t Hoff factor and activity, 4.3 Liquid state: surface tension, Kelvin equation, capillary action, viscosity and liquid crystals, 3.4 Ionic bonding: lattice energy, Born–Haber cycle, Born–Landé and Kapustinskii equations, Fajans’ rules, 14.4 Main group chemistry: boranes, borazine, phosphazenes, silicates, silicones, interhalogens, xenon and S–N compounds, 1.4 Hydrogen atom: Schrödinger equation, quantum numbers, radial distribution, nodes and orbital shapes, 2.11 Molecular orbital theory: LCAO, homonuclear and heteronuclear diatomics (O₂, N₂, CO, NO, CN⁻, HF), bond order and magnetism, 13.3 Werner theory, isomerism, IUPAC names and VBT of complexes, 2.2 VSEPR, hybridisation and Bent's rule, 1.2 Uncertainty principle, de Broglie relation and wave–particle duality, 13.6 Substitution in complexes: labile and inert, trans effect, stability constants, 6.1 Second and third laws: entropy, Gibbs and Helmholtz energies, Maxwell relations, 4.1 Real gases: van der Waals equation, critical constants, Boyle temperature, 9.2 Theories of reaction rate: Arrhenius, collision and transition-state theory, 9.1 Rate laws and order: integrated rate equations, half-life, reversible, parallel and consecutive reactions, 1.1 Postulates of quantum mechanics: operators, eigenfunctions, Hermitian operators and acceptable wave functions, 10.1 Photochemistry: quantum yield, Jablonski diagram, H₂–halogen reactions, 7.1 Phase rule, phase diagrams, Clausius–Clapeyron equation, eutectics and partially miscible liquids, 13.4 Organometallics: 18-electron rule, oxidative addition, Wilkinson's catalyst, 14.2 Non-aqueous solvents: liquid NH₃, HF, H₂SO₄, SO₂, BrF₃ and superacids, 13.5 Metal carbonyls, nitrosyls, 18-electron rule and metal clusters, 15.1 Lanthanides and actinides: contraction, magnetism, spectra, separation, 4.2 Kinetic theory of gases: Maxwell distribution, collisions, mean free path, effusion and transport, 5.1 First law of thermodynamics: work, heat, enthalpy, adiabatic changes, Joule–Thomson effect, thermochemistry, 13.7 Electronic spectra of complexes: term symbols, selection rules, charge transfer, 8.3 Electrolytes: conductance, Kohlrausch, Debye–Hückel and transport numbers, 8.2 Electrochemical cells: Nernst equation, emf and electrodes, 3.2 Defects in solids, non-stoichiometry and semiconductors, 3.1 Crystal systems, Miller indices, Bragg's law and radius ratio, 6.2 Chemical potential, partial molar quantities, Gibbs–Duhem equation, fugacity and activity, 6.3 Chemical equilibrium: ΔG° and K, Kp, Kc and Kx, van ’t Hoff isochore and isobar, 12.2 Bio-inorganic chemistry: haemoglobin, cytochromes, Fe–S proteins, 11.2 Adsorption, heterogeneous catalysis and colloids, 1.3 Particle in a one-dimensional box. Each note is one set for Civil Services, IFoS and Geo-Scientist. More topics follow, and each release is announced on Telegram. All VKC notes