IB Sciences • SL

Chemistry SL

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Structure 1. Models of the particulate nature of matter

S1.1 Introduction to the particulate nature of matter

S1.1.1 Elements, Compounds and Mixtures

S1.1.2 The Kinetic Molecular Theory

S1.1.3 Temperature and Kinetic Energy

Structure 2. Models of bonding and structure

S2.1 The ionic model

S2.1.1 Formation of ions

S2.1.2 Ionic bonds and binary compounds

S2.1.3 Lattice structures and properties

S2.2 The covalent model

S2.2.1 Formation of covalent bonds

S2.2.2 Single, double and triple bonds

S2.3 The metallic model

S2.3.1 Metallic bonding and properties of metals

S2.3.2 Strength of metallic bonds

S2.4 From models to materials

S2.4.1 Bonding as a continuum

S2.4.2 Position in the bonding triangle

Structure 3. Classification of matter

S3.1 The periodic table: classification of elements

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

S3.2 Functional groups: classification of organic compounds

S3.2.1 Representation of organic compounds

S3.2.2 Functional groups

Reactivity 1. What drives chemical reactions?

R1.1 Measuring enthalpy change

R1.1.1 Energy transfer in chemical reactions

R1.1.2 Endothermic and exothermic reactions

R1.1.3 Energy profiles

R1.1.4 Standard enthalpy change

R1.1.5 Practical considerations

R1.2 Energy cycles in reactions

R1.2.1 Bond enthalpy

R1.2.2 Hess's Law

R1.3 Energy from fuels

R1.3.1 Combustion fuels

R1.3.2 Incomplete combustion

R1.3.3 Fossil fuels

Reactivity 2. How much, how fast and how far?

R2.1 How much? The amount of chemical change

R2.1.1 Chemical equations and stoichiometry

R2.1.2 Using the mole ratio

R2.1.3 Limiting and excess reactants

R2.1.4 Percentage yield

R2.1.5 Atom economy

R2.2 How fast? The rate of chemical change

R2.2.1 Rate of reaction

R2.2.2 Collision theory

R2.3 How far? The extent of chemical change

R2.3.1 Dynamic equilibrium

R2.3.2 The equilibrium law and constant

Reactivity 3. What are the mechanisms of chemical change?

R3.1 Proton transfer reactions

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

R3.2 Electron transfer reactions

R3.2.1 Oxidation and reduction definitions

R3.2.2 Redox half-equations

R3.3 Electron sharing reactions

R3.3.1 Radicals

R3.3.2 Homolytic fission

R3.3.3 Substitution reactions with alkanes

R3.4 Electron pair sharing reactions

R3.4.1 Nucleophiles

R3.4.2 Nucleophilic substitution reactions

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

S2.4.3 Alloys

S2.4.4 Polymers

S2.4.5 Addition polymers

S3.2.3 Homologous series

S3.2.4 Physical trends in homologous series

S3.2.5 IUPAC nomenclature

S3.2.6 Structural isomers

R1.3.4 Biofuels

R1.3.5 Fuel cells

R2.2.3 Factors affecting the rate of reaction

R2.2.4 Activation energy

R2.2.5 Catalysts

R2.3.3 Magnitude of K and temperature dependence

R2.3.4 Le Châtelier’s principle

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

R3.4.3 Heterolytic fission

R3.4.4 Electrophiles

R3.4.5 Electrophilic attack

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