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S2.2.1 Formation of covalent bonds
S2.2.2 Single, double and triple bonds
S2.2.3 Coordination bonds
S2.2.4 VSEPR theory
S2.2.5 Bond polarity
S2.2.6 Molecular polarity
S2.2.7 Covalent network structures
S2.2.8 Intermolecular forces
S2.2.9 Intermolecular forces and physical properties
S2.2.10 Chromatography
S2.2.11 Resonance structures (HL only)
S2.2.12 Benzene (HL only)
S2.2.13 Expanded Octet of Electrons (HL only)
S2.2.14 Formal Charge and Lewis Formulas (HL only)
S2.2.15 Sigma and Pi Bonds (HL only)
S2.2.16 Hybridization and Bonding (HL only)
S3.1.1 The structure of the periodic table
S3.1.2 Electron configuration and group trends
S3.1.3 Periodicity of properties
S3.1.4 Trends in chemical reactivity
S3.1.5 Metallic and non-metallic oxides
S3.1.6 Oxidation states
S3.1.7 Discontinuities in ionization energy trends (HL only)
S3.1.8 Properties of transition elements (HL only)
S3.1.9 Oxidations states of transition elements (HL only)
S3.1.10 Color of transition metal complexes (HL only)
S3.2.1 Representation of organic compounds
S3.2.2 Functional groups
S3.2.3 Homologous series
S3.2.4 Physical trends in homologous series
S3.2.5 IUPAC nomenclature
S3.2.6 Structural isomers
S3.2.7 Stereoisomers (HL only)
S3.2.8 Mass spectrometry (HL only)
S3.2.9 Infrared spectra (HL only)
S3.2.10 Proton nuclear magnetic resonance spectroscopy (HL only)
S3.2.11 H NMR spectra interpretation (HL only)
S3.2.12 Structural analysis (HL only)
R2.2.1 Rate of reaction
R2.2.2 Collision theory
R2.2.3 Factors affecting the rate of reaction
R2.2.4 Activation energy
R2.2.5 Catalysts
R2.2.6 Reaction mechanisms and rate-determining steps (HL only)
R2.2.7 Energy profiles and transition states (HL only)
R2.2.8 Molecularity (HL only)
R2.2.9 Rate equations (HL only)
R2.2.10 Order of a reaction (HL only)
R2.2.11 Rate constant (HL only)
R2.2.12 Arrhenius equation (HL only)
R2.2.13 Arrhenius factor (HL only)
R3.1.1 Brønsted–Lowry acid-base theory
R3.1.2 Conjugate acid-base pairs
R3.1.3 Amphiprotic species
R3.1.4 pH and the hydrogen ion concentration
R3.1.5 The ion product of water (Kw)
R3.1.6 Strong and weak acids and bases
R3.1.7 Neutralization reactions
R3.1.8 pH curves for neutralization
R3.1.9 pOH scale (HL only)
R3.1.10 Acid and base strength and constants (HL only)
R3.1.11 Conjugate Acid-Base pair (HL only)
R3.1.12 The pH of a salt solution (HL only)
R3.1.13 pH curves of Acid-Base combinations (HL only)
R3.1.14 Acid-Base indicators and pH changes (HL only)
R3.1.15 Appropriate indicators for titration (HL only)
R3.1.16 Buffer solutions (HL only)
R3.1.17 The pH of a buffer solution (HL only)
R3.2.1 Oxidation and reduction definitions
R3.2.2 Redox half-equations
R3.2.3 Reactivity of elements based on periodic trends
R3.2.4 Acid-metal reactions
R3.2.5 Electrochemical cells: Oxidation and reduction
R3.2.6 Primary (voltaic) cells
R3.2.7 Secondary (rechargeable) cells
R3.2.8 Electrolytic cells
R3.2.9 Oxidation of organic compounds
R3.2.10 Reduction of functional groups
R3.2.11 Reduction of unsaturated compounds
R3.2.12 Standard electrode potentials (HL only)
R3.2.13 Standard cell potential (HL only)
R3.2.14 Gibbs free energy and cell potential (HL only)
R3.2.15 Electrolysis of aqueous solutions (HL only)
R3.2.16 Electroplating (HL only)
R3.4.1 Nucleophiles
R3.4.2 Nucleophilic substitution reactions
R3.4.3 Heterolytic fission
R3.4.4 Electrophiles
R3.4.5 Electrophilic attack
R3.4.6 Lewis acid (HL only)
R3.4.7 Lewis acid-base reaction (HL only)
R3.4.8 Ligands and coordination bond (HL only)
R3.4.9 SN1 and SN2 mechanisms (HL only)
R3.4.10 Rate of the substitution reactions (HL only)
R3.4.11 Electrophilic addition (HL only)
R3.4.12 The relative stability of carbocations (HL only)
R3.4.13 Reactions between benzene and electrophiles (HL only)