Structure 1. Models of the particulate nature of matter

1.1 Introduction to the particulate nature of matter

1.2 The nuclear atom

1.3 Electron configurations

1.4 The mole

1.5 Ideal gases

Structure 2. Models of bonding and structure

2.1 The ionic model

2.2 The covalent model

2.3 The metallic model

2.4 From models to materials

Structure 3. Classification of matter

3.1 The periodic table

3.2 Functional groups: Organic compounds

Reactivity 1. What drives chemical reactions?

1.1 Measuring enthalpy changes

1.2 Energy cycles

1.3 Energy from fuels

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

2.1 Amount of chemical change

2.2 Rate of chemical change

2.3 Extent of chemical change

Reactivity 3. What are the mechanisms of chemical change?

3.1 Proton transfer reactions

3.2 Electron transfer reactions

3.2.1—Oxidation and reduction

3.2.2—Half-equations

3.2.3—Periodic trends in redox

3.2.4—Acids with reactive metals

3.2.5—Electrodes in electrochemical cells

3.2.6—Primary (voltaic) cells

3.2.7—Secondary (rechargeable) cells

3.2.8—Electrolytic cells

3.2.9—Oxidation of organic functional groups

3.2.10—Reduction of organic functional groups

3.2.11—Reduction of unsaturated compounds

3.3 Electron sharing reactions (Radicals)

3.4 Electron-pair sharing reactions

IB Chemistry HL 3.2.12 (HL)—Standard electrode potential (E⦵) Question Bank

• Hydrogen half-cell = 0 V by convention

• Ease of oxidation/reduction

• Use standard conditions and electrode potential data to compare oxidizing/reducing ability

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