Description
Core Topics (SL & HL)
- Stoichiometric Relationships
- Mole concept & Avogadro’s constant
- Reacting masses and volumes (moles, molar mass, limiting reagent, % yield)
- Solutions and concentrations
- Ideal gas law (PV = nRT)
- Empirical & molecular formulae
- Balanced equations & stoichiometry calculations
- Atomic Structure
- Structure of the atom (protons, neutrons, electrons)
- Isotopes & mass spectrometry
- Electron configuration (s, p, d, f orbitals)
- Emission & absorption spectra (hydrogen atom line spectrum)
- Ionization energy trends
- Periodicity
- Periodic table organization (groups & periods)
- Periodic trends: atomic radius, ionization energy, electronegativity
- Oxides & chlorides across period 3
- Metallic, non-metallic, and amphoteric behavior
- Bonding & Structure
- Ionic, covalent, and metallic bonding
- Intermolecular forces (London dispersion, dipole-dipole, hydrogen bonding)
- Lewis structures, resonance, exceptions to octet rule
- Molecular geometry (VSEPR theory)
- Hybridization (sp, sp2, sp3)
- Polarity and molecular interactions
- Giant structures: diamond, graphite, graphene, fullerene, silica
- Energetics (Thermochemistry)
- Exothermic & endothermic reactions
- Enthalpy changes of combustion, neutralization, formation
- Hess’s Law & enthalpy cycles
- Bond enthalpy calculations
- Lattice enthalpy (HL)
- Entropy and Gibbs free energy (HL)
- Kinetics
- Collision theory and factors affecting rate (temperature, concentration, surface area, catalysts)
- Rate expressions and rate constants
- Determination of rate from experimental data
- Reaction mechanisms (slow step, rate-determining step)
- Activation energy & Arrhenius equation (HL)
- Equilibrium
- Dynamic equilibrium in closed systems
- Le Chatelier’s Principle (temperature, concentration, pressure effects)
- The equilibrium constant Kc
- The equilibrium constant Kp (HL)
- Relationship between Gibbs free energy and equilibrium constant (HL)
- Acids and Bases
- Definitions (Arrhenius, Brønsted–Lowry, Lewis)
- Strong vs. weak acids/bases
- pH, pOH, [H+], [OH–] calculations
- Acid–base titrations and indicators
- Buffer solutions (HL)
- Acid deposition and environmental impact
- Redox Processes
- Oxidation and reduction (electron transfer, oxidation numbers)
- Balancing redox equations
- Reactivity of metals and halogens
- Activity series and redox reactions
- Electrochemical cells (voltaic and electrolytic)
- Electrolysis (applications: electroplating, extraction of metals)
- Standard electrode potentials (E° values) (HL)
- Nernst equation (HL)
- Organic Chemistry
- Hydrocarbons: alkanes, alkenes, alkynes
- Functional groups (alcohols, halogenoalkanes, aldehydes, ketones, carboxylic acids, esters, amines, nitriles)
- Isomerism (structural, stereoisomers, cis/trans, E/Z, optical)
- Organic reaction pathways (substitution, addition, elimination, oxidation, reduction, esterification)
- Reaction mechanisms (SN1, SN2, electrophilic addition) (HL)
- Benzene and aromatic chemistry (HL)
- Polymers (addition & condensation)
- Measurement and Data Processing
- Uncertainty and error analysis
- Significant figures
- Graphical techniques and best-fit lines
- Experimental design and evaluation
- Use of data book for constants & standard values
Additional HL Extension Topics
- Atomic Structure: More detail on electron configuration, sublevels, and ionization trends across periods.
- Bonding: Hybridization in detail (sp, sp2, sp3, dsp3, d2sp3), molecular orbital theory.
- Energetics: Lattice enthalpy, entropy, Gibbs free energy (ΔG = ΔH – TΔS).
- Kinetics: Arrhenius equation, advanced reaction mechanisms, rate-determining steps.
- Equilibrium: Kp (gas equilibria), ΔG° = –RT lnK.
- Acids & Bases: pKa, pKb, Kw, buffer calculations, titration curves.
- Redox: Standard electrode potentials, Nernst equation, fuel cells.
- Organic: Aromatic chemistry (benzene), electrophilic substitution, condensation polymers, stereoisomerism (optical activity).
- Data Processing: Advanced error analysis and uncertainty propagation.
