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

3.1.1—Brønsted-Lowry theory

3.1.2—Conjugate acid-base pairs

3.1.3—Amphiprotic species

3.1.4—pH scale

3.1.5—Ion product of water (Kw)

3.1.6—Strong vs. weak acids/bases

3.1.7—Neutralization reactions

3.1.8—pH curves

3.1.9 (HL)—pOH scale

3.1.10 (HL)—Acid/base strength constants

3.1.11 (HL)—Conjugate pair relationship

3.1.12 (HL)—Salt hydrolysis

3.1.13 (HL)—pH curves for weak acids/bases

3.1.14 (HL)—Acid-base indicators

3.1.15 (HL)—Indicator selection

3.1.16 (HL)—Buffer solutions

3.1.17 (HL)—Buffer pH and composition

3.2 Electron transfer reactions

3.3 Electron sharing reactions (Radicals)

3.4 Electron-pair sharing reactions

IB Chemistry HL 3.1.16 (HL)—Buffer solutions Question Bank

• Resist pH change

• Acidic buffers: weak acid + conjugate base

• Basic buffers: weak base + conjugate acid

• Explain buffer action using weak acid/base conjugate systems

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