Subject content
Fundamental particles
Mass number and isotopes
Electron configuration
Relative atomic mass and relative molecular mass
The mole and the Avogadro constant
The ideal gas equation
Empirical and molecular formula
Balanced equations and associated calculations
Ionic bonding
Nature of covalent and dative covalent bonds
Metallic bonding
Bonding and physical properties
Shapes of simple molecules and ions
Bond polarity
Forces between molecules
Enthalpy change
Calorimetry
Applications of Hess’s Law
Bond enthalpies
Collision theory
Maxwell-Boltzmann distribution
Effect of temperature on reaction rate
Effect of concentration and pressure
Catalysts
Equilibrium constant Kc for homogeneous systems
Born-Haber Cycles
Gibbs free-energy change, deltaG, and entropy change, deltaS
Rate equations
Determination of rate equation
Electrode potentials and cells
Commercial applications of electrochemical cells
Bronsted-Lowry acid-base equilibria in aqueous solution
Definition and determination of pH
The ionic product of water, Kw
Weak acids and bases Ka for weak acids
pH curves, titrations and indicators
Buffer action
Classification
Physical properties of Period 3 elements
Trends in properties
Uses of chlorine and chlorate(I)
General properties of transition metals
Substitution reactions
Shapes of complex ions
Formation of coloured ions
Variable oxidation states
catalysts
Nomenclature
Reaction mechanisms
isomerism
Fractional distillation of crude oil
Modification of alkanes by cracking
Combustion of alkanes
Chlorination of alkanes
Nucleophilic substitution
Elimination
Ozone depletion
Structure, bonding and reactivity
Addition reactions of alkenes
Addition polymers
Alcohol production
Oxidation of alcohols
Elimination
Identification of functional groups by test-tube reactions
Mass spectrometry
Infrared spectroscopy
Carboxylic acids and esters
Acylation
Bonding
Electrophilic substitution
Preparation
Base properties
Nucleophilic properties
Condensation polymers
Biodegradability and disposal of polymers
Amino acids
Proteins
Enzymes
DNA
AS Level subject content Candidates for Cambridge International AS Level Chemistry study the following topics: A Level subject content Candidates for Cambridge International A Level Chemistry study the AS topics and the following topics:
Physical chemistry
AS Level candidates also study practical skills.
Physical chemistry
~9–10 5
1.1 Moles and Molar Mass 5
1.2 Mass Spectra of Elements 2
1.3 Elemental Composition of Pure Substances 5
1.4 Composition of Mixtures 1
1.5 Atomic Structure and Electron Configuration 4
1.6 Photoelectron Spectroscopy 4
1.7 Periodic Trends 4
1.8 Valence Electrons and Ionic Compounds
~12–13 Class Periods 7–9% 6
2.1 Types of Chemical Bonds 3
2.2 Intramolecular Force and Potential Energy 4
2.3 Structure of Ionic Solids 4
2.4 Structure of Metals and Alloys 3
2.5 Lewis Diagrams 6
2.6 Resonance and Formal Charge 6
2.7 VSEPR and Hybridization
~14–15 Class Periods 18–22% AP Exam Weighting 4
3.1 Intermolecular and Interparticle Forces 4
3.2 Properties of Solids 3
3.3 Solids, Liquids, and Gases 5
3.4 Ideal Gas Law 4
3.5 Kinetic Molecular Theory 6
3.6 Deviation from Ideal Gas Law 5
3.7 Solutions and Mixtures 3
3.8 Representations of Solutions 2
3.9 Separation of Solutions and Mixtures 4
3.10 Solubility 4
3.11 Spectroscopy and the Electromagnetic Spectrum 5
3.12 Properties of Photons 2
3.13 Beer-Lambert Law
~14–15 Class Periods 7–9% AP Exam Weighting 2
4.1 Introduction for Reactions 5
4.2 Net Ionic Equations 3
4.3 Representations of Reactions 6
4.4 Physical and Chemical Changes 5
4.5 Stoichiometry 3
4.6 Introduction to Titration 1
4.7 Types of Chemical Reactions 1
4.8 Introduction to Acid-Base Reactions 5
4.9 Oxidation-Reduction (Redox) Reactions
~13–14 Class Periods 7–9% AP Exam Weighting 6
5.1 Reaction Rates 5
5.2 Introduction to Rate Law 5
5.3 Concentration Changes Over Time 5
5.4 Elementary Reactions 6
5.5 Collision Model 3
5.6 Reaction Energy Profile 1
5.7 Introduction to Reaction Mechanisms 5
5.8 Reaction Mechanism and Rate Law 5
5.9 Pre-Equilibrium Approximation 3
5.10 Multistep Reaction Energy Profile 6
5.11 Catalysis
~10–11 Class Periods 7–9% AP Exam Weighting 6
6.1 Endothermic and Exothermic Processes 3
6.2 Energy Diagrams 6
6.3 Heat Transfer and Thermal Equilibrium 2
6.4 Heat Capacity and Calorimetry 1
6.5 Energy of Phase Changes 4
6.6 Introduction to Enthalpy of Reaction 5
6.7 Bond Enthalpies 5
6.8 Enthalpy of Formation 5
6.9 Hess’s Law
~13–15 Class Periods 7–9% AP Exam Weighting 6
7.1 Introduction to Equilibrium 4
7.2 Direction of Reversible Reactions 3
7.3 Reaction Quotient and Equilibrium Constant 5
7.4 Calculating the Equilibrium Constant 6
7.5 Magnitude of the Equilibrium Constant 5
7.6 Properties of the Equilibrium Constant 3
7.7 Calculating Equilibrium Concentrations 3
7.8 Representations of Equilibrium 6
7.9 Introduction to Le Châtelier’s Principle 5
7.10 Reaction Quotient and Le Châtelier’s Principle 5
7.11 Introduction to Solubility Equilibria 2
7.12 Common-Ion Effect
~14–16 Class Periods 11–15% 5
8.1 Introduction to Acids and Bases 5
8.2 pH and pOH of Strong Acids and Bases 5
8.3 Weak Acid and Base Equilibria 5
8.4 Acid-Base Reactions and Buffers 5
8.5 Acid-Base Titrations 6
8.6 Molecular Structure of Acids and Bases 2
8.7 pH and pKa 6
8.8 Properties of Buffers 5
8.9 Henderson-Hasselbalch Equation 6
8.10 Buffer Capacity 2
8.11 pH and Solubility
~10–13 Class Periods 7–9% AP Exam Weighting 6
9.1 Introduction to Entropy 5
9.2 Absolute Entropy and Entropy Change 6
9.3 Gibbs Free Energy and Thermodynamic Favorability 6
9.4 Thermodynamic and Kinetic Control Thermodynamics and Electrochemistry 6
9.5 Free Energy and Equilibrium Thermodynamics and Electrochemistry 4
9.6 Free Energy of Dissolution 4
9.7 Coupled Reactions 2
9.8 Galvanic (Voltaic) and Electrolytic Cells 5
9.9 Cell Potential and Free Energy 6
9.10 Cell Potential Under Nonstandard Conditions 5
9.11 Electrolysis and Faraday’s Law
hl
Core
Additional higher level (AHL)
Option (Choice of one out of four) A. Materials B. Biochemistry C. Energy D. Medicinal chemistry
Structure 1. Models of the particulate nature of matter
Structure 1.1—Introduction to the particulate nature of matter Structure 1.2—The nuclear atom Structure 1.3—Electron configurations Structure 1.4—Counting particles by mass: The mole Structure 1.5—Ideal gases 17 21
Structure 2. Models of bonding and structure Structure
2.1—The ionic model Structure 2.2—The covalent model Structure 2.3—The metallic model Structure 2.4—From models to materials 20 30
Structure 3. Classification of matter Structure
3.1—The periodic table: Classification of elements Structure 3.2—Functional groups: Classification of organic compounds 16 31
Reactivity 1. What drives chemical reactions?
Reactivity 1.1—Measuring enthalpy change Reactivity 1.2—Energy cycles in reactions Reactivity 1.3—Energy from fuels Reactivity 1.4—Entropy and spontaneity (Additional higher level) 12 22
Reactivity 2. How much, how fast and how far?
Reactivity 2.1—How much? The amount of chemical change Reactivity 2.2—How fast? The rate of chemical change Reactivity 2.3—How far? The extent of chemical change
蛋白质的结构与功能
核酸的结构与功能
酶与酶促反应
聚糖的结构与功能
糖代谢
生物氧化
脂质代谢
蛋白质消化吸收和氨基酸代谢
核苷酸代谢
代谢的整合与调节
真核基因与基因组
DNA的合成
DNA损伤和损伤修复
RNA的合成
蛋白质的合成
基因表达调控
细胞信号转导的分子机制
血液的生物化学
肝的生物化学
维生素
钙、磷、微量元素
癌基因和抑癌基因
DNA重组和重组DNA技术
常用分子生物学技术原理应用
基因结构功能分析和疾病相关基因鉴定克隆
基因诊断和基因治疗
组学与系统生物医学