AP Chemistry AP化学
📌 Course at a glance
· 9 units · key topics drilled across the official outline
· Next exam: 2026-05-04 · 2026-05-04
📝 Full chapter-by-chapter lecture walkthroughs are being written. This page is the course outline — every unit and topic that will be covered, with key concepts you can already start to recognise. Use it as a study map; the chapter notes drop in over the coming weeks.
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Course outline
Unit 1 · Atomic Structure and Properties 原子结构与性质
Exam weight: 7-9%
1.1 — Moles and Molar Mass 摩尔与摩尔质量
· Definition of the mole and Avogadro's number · Calculating molar mass · Converting between mass and moles
1.2 — Mass Spectroscopy of Elements 元素的质谱分析
· Basic principles of mass spectrometry · Relative abundance of isotopes · Calculating average atomic mass from mass spectrum data
1.3 — Elemental Composition of Pure Substances 纯物质的元素组成
· Mass percent composition · Determining empirical and molecular formulas · Stoichiometric relationships
1.4 — Composition of Mixtures 混合物的组成
· Distinction between mixtures and pure substances · Mass fraction of components in a mixture · Quantitative analysis of mixture composition
1.5 — Atomic Structure and Electron Configuration 原子结构与电子构型
· Basic atomic structure (protons, neutrons, electrons) · Rules for writing electron configurations · Electron arrangement (Aufbau principle, Hund's rule, Pauli exclusion principle)
1.6 — Photoelectron Spectroscopy 光电子能谱
· Basic principles of photoelectron spectroscopy · Determining electron configuration from PES spectra · Relationship between ionization energy and electron subshells
1.7 — Periodic Trends 元素周期律
· Periodic trends in ionization energy · Periodic trends in atomic radius · Periodic trends in electronegativity · Effective nuclear charge and shielding effect
1.8 — Valence Electrons and Ionic Compounds 价电子与离子化合物
· Determining valence electrons · Formation and charge of ions · Composition and naming of ionic compounds · Coulomb's law and lattice energy
Unit 2 · Molecular and Ionic Compound Structure and Properties 分子与离子化合物的结构和性质
Exam weight: 7-9%
2.1 — Types of Chemical Bonds 化学键的类型
· Comparison of ionic, covalent, and metallic bonds · Electronegativity difference and bond type · Bond polarity
2.2 — Intramolecular Force and Potential Energy 分子内作用力与势能
· Bond energy of covalent bonds · Relationship between bond length and bond energy · Analysis of potential energy curves
2.3 — Structure of Ionic Solids 离子固体的结构
· Structural features of ionic crystals · Lattice energy and its influencing factors · Physical properties of ionic solids
2.4 — Structure of Metals and Alloys 金属与合金的结构
· Metallic bonding and the electron sea model · Physical properties of metals · Types and properties of alloys
2.5 — Lewis Diagrams 路易斯结构图
· Rules for drawing Lewis structures · Lone pairs and bonding pairs · Octet rule and its exceptions
2.6 — Resonance and Formal Charge 共振与形式电荷
· Drawing resonance structures · Calculating formal charge · Determining the best Lewis structure
2.7 — VSEPR and Bond Hybridization VSEPR理论与杂化轨道
· VSEPR model for predicting molecular geometry · Hybridization theory (sp, sp2, sp3) · Determining molecular polarity
Unit 3 · Intermolecular Forces and Properties 分子间作用力与性质
Exam weight: 18-22%
3.1 — Intermolecular Forces 分子间作用力
· London dispersion forces · Dipole-dipole interactions · Hydrogen bonding and conditions for formation
3.2 — Properties of Solids 固体的性质
· Ionic, molecular, covalent network, and metallic crystals · Comparing physical properties of different solid types · Relationship between crystal structure and properties
3.3 — Solids, Liquids, and Gases 固体、液体和气体
· Microscopic characteristics of three states of matter · Phase transitions and energy changes · Effect of intermolecular forces on states of matter
3.4 — Ideal Gas Law 理想气体定律
· Applications of PV = nRT · Molar volume of gases · Gas mixtures and Dalton's law of partial pressures
3.5 — Kinetic Molecular Theory 分子运动论
· Basic assumptions of kinetic molecular theory · Relationship between temperature and average kinetic energy · Maxwell-Boltzmann speed distribution
3.6 — Deviation from Ideal Gas Law 对理想气体定律的偏离
· Deviations of real gases from ideal behavior · Van der Waals equation · Deviations at high pressure and low temperature
3.7 — Solutions and Mixtures 溶液与混合物
· Types of solutions · Expressing concentration (molarity, mass fraction) · Dissolution process and intermolecular forces
3.8 — Representations of Solutions 溶液的表示
· Particulate representations of solutions · Solute-solvent interactions · Electrolyte and nonelectrolyte solutions
3.9 — Separation of Solutions and Mixtures Chromatography 溶液和混合物的分离——色谱法
· Basic principles of chromatography · Distillation and filtration · Selecting appropriate separation methods
3.10 — Solubility 溶解度
· Factors affecting solubility · Like dissolves like principle · Effect of temperature and pressure on solubility
3.11 — Spectroscopy and the Electromagnetic Spectrum 光谱学与电磁波谱
· Regions of the electromagnetic spectrum · Relationship between photon energy and frequency · Absorption and emission spectra
3.12 — Photoelectric Effect 光电效应
· Basic principles of the photoelectric effect · Photon energy and work function · Analysis of photoelectric effect experimental data
3.13 — Beer-Lambert Law 比尔-朗伯定律
· Linear relationship between absorbance and concentration · Application of A = ebc · Spectrophotometric determination of solution concentration
Unit 4 · Chemical Reactions 化学反应
Exam weight: 7-9%
4.1 — Introduction for Reactions 化学反应导论
· Basic concepts of chemical reactions · Reactants and products · Writing and balancing chemical equations
4.2 — Net Ionic Equations 离子净方程式
· Complete ionic and net ionic equations · Identifying spectator ions · Steps for writing ionic equations
4.3 — Representations of Reactions 化学反应的表示
· Particulate-level reaction diagrams · Multiple representations of chemical equations · Correspondence between macroscopic and microscopic reactions
4.4 — Physical and Chemical Changes 物理变化与化学变化
· Distinction between physical and chemical changes · Evidence of chemical change · Changes in properties of matter
4.5 — Stoichiometry 化学计量学
· Mole ratios in chemical equations · Determining the limiting reagent · Theoretical yield and actual yield
4.6 — Introduction to Titration 滴定简介
· Basic principles and procedure of titration · Determining the equivalence point · Titration calculations
4.7 — Types of Chemical Reactions 化学反应的类型
· Synthesis and decomposition reactions · Single and double replacement reactions · Precipitation reactions
4.8 — Introduction to Acid-Base Reactions 酸碱反应简介
· Basic definitions of acids and bases · Acid-base neutralization reactions · Predicting products of acid-base reactions
4.9 — Oxidation-Reduction (Redox) Reactions 氧化还原反应
· Determining oxidation numbers · Identifying oxidizing and reducing agents · Balancing redox reaction equations
Unit 5 · Kinetics 化学动力学
Exam weight: 7-9%
5.1 — Reaction Rates 反应速率
· Definition and representation of reaction rate · Average rate and instantaneous rate · Graphical analysis of concentration vs. time
5.2 — Introduction to Rate Law 速率定律简介
· Rate law expression · Determining reaction order · Meaning of the rate constant k
5.3 — Concentration Changes Over Time 浓度随时间的变化
· Integrated rate laws for zero, first, and second order reactions · Concept and calculation of half-life · Determining reaction order using graphs
5.4 — Elementary Reactions 基元反应
· Definition of elementary reactions · Relationship between molecularity and reaction order · Rate laws for elementary reactions
5.5 — Collision Model 碰撞模型
· Conditions for effective collisions · Concept of activation energy · Relationship between temperature and collision frequency
5.6 — Reaction Energy Profile 反应能量曲线
· Interpreting reaction energy diagrams · Activation energy and enthalpy of reaction · Transition state and activated complex
5.7 — Introduction to Reaction Mechanisms 反应机理简介
· Basic concepts of reaction mechanisms · Difference between intermediates and transition states · Overall reaction and elementary steps
5.8 — Reaction Mechanism and Rate Law 反应机理与速率定律
· Rate-determining step · Deriving rate law from mechanism · Verifying consistency of mechanism with experimental rate law
5.9 — Steady-State Approximation 稳态近似法
· Basic assumptions of the steady-state approximation · Steady-state treatment of intermediate concentrations · Deriving rate laws for complex reactions
5.10 — Multistep Reaction Energy Profile 多步反应能量曲线
· Drawing and analyzing multistep reaction energy diagrams · Comparing activation energies of individual steps · Identifying the rate-determining step on energy diagrams
5.11 — Catalysis 催化作用
· Principles of how catalysts work · Homogeneous and heterogeneous catalysis · Effect of catalysts on activation energy and reaction rate
Unit 6 · Thermodynamics 热力学
Exam weight: 7-9%
6.1 — Endothermic and Exothermic Processes 吸热过程与放热过程
· Definitions of endothermic and exothermic reactions · Meaning of positive and negative enthalpy change (delta H) · Conservation of energy and the system-surroundings concept
6.2 — Energy Diagrams 能量图
· Graphical representation of enthalpy change · Relative energy of reactants and products · Interpreting energy diagrams
6.3 — Heat Transfer and Thermal Equilibrium 热传递与热平衡
· Direction of heat transfer · Establishing thermal equilibrium · Quantitative calculation of heat: q = mc delta T
6.4 — Heat Capacity and Calorimetry 热容与量热法
· Difference between specific heat and heat capacity · Principles and calculations of calorimetry experiments · Coffee cup calorimeter and bomb calorimeter
6.5 — Energy of Phase Changes 相变能量
· Enthalpy of fusion and enthalpy of vaporization · Why temperature remains constant during phase changes · Analysis of heating curves
6.6 — Introduction to Enthalpy of Reaction 反应焓变简介
· Definition of enthalpy of reaction · Standard enthalpy of reaction · Relationship between enthalpy change and stoichiometric coefficients
6.7 — Bond Enthalpies 键焓
· Definition of bond energy · Estimating enthalpy of reaction using bond energies · Limitations of bond energy data
6.8 — Enthalpy of Formation 生成焓
· Definition of standard enthalpy of formation · Calculating enthalpy of reaction using standard enthalpies of formation · Standard enthalpy of formation of elements is zero
6.9 — Hess's Law 赫斯定律
· Statement of Hess's Law · Calculating enthalpy changes using Hess's Law · Path independence of enthalpy
Unit 7 · Equilibrium 化学平衡
Exam weight: 7-9%
7.1 — Introduction to Equilibrium 化学平衡简介
· Concept of dynamic equilibrium · Characteristics of reversible reactions · Macroscopic and microscopic descriptions of equilibrium
7.2 — Direction of Reversible Reactions 可逆反应的方向
· Comparing forward and reverse reaction rates · Determining the direction toward equilibrium · Analysis of concentration-time graphs
7.3 — Reaction Quotient and Equilibrium Constant 反应商与平衡常数
· Writing equilibrium constant expressions Kc and Kp · Calculating the reaction quotient Q · Comparing Q and K to determine reaction direction
7.4 — Calculating the Equilibrium Constant 平衡常数的计算
· Using ICE tables · Calculating K from equilibrium concentrations · Calculating K from initial and equilibrium conditions
7.5 — Magnitude of the Equilibrium Constant 平衡常数的大小
· Physical meaning of the magnitude of K · Meaning of K >> 1 and K << 1 · Determining the position of equilibrium
7.6 — Properties of the Equilibrium Constant 平衡常数的性质
· Effect of changing the equation on K · Relationship between K and temperature · Calculating K for multi-step reactions
7.7 — Calculating Equilibrium Concentrations 平衡浓度的计算
· Calculating equilibrium concentrations using ICE tables · Simplification using approximations · Solving quadratic equations
7.8 — Representations of Equilibrium 平衡的表示
· Particulate-level representations of equilibrium · Concentration-time graphs and equilibrium · Analyzing the composition of equilibrium mixtures
7.9 — Introduction to Le Chatelier's Principle 勒夏特列原理简介
· Statement of Le Chatelier's Principle · Effect of concentration changes on equilibrium · Effect of temperature changes on equilibrium
7.10 — Reaction Quotient and Le Chatelier's Principle 反应商与勒夏特列原理
· Using Q and K to explain equilibrium shifts · Effect of pressure and volume changes · Quantitative analysis of equilibrium shifts
7.11 — Introduction to Solubility Equilibria 溶解平衡简介
· Definition of the solubility product constant Ksp · Writing Ksp expressions · Relationship between solubility and Ksp
7.12 — Common-Ion Effect 同离子效应
· Effect of the common-ion effect on solubility · Quantitative calculations involving the common-ion effect · Application of the common-ion effect in equilibrium
7.13 — pH and Solubility pH与溶解度
· Effect of pH on solubility of sparingly soluble salts · Dissolution of salts with basic anions in acid · Relationship between solubility and acidity/basicity
7.14 — Free Energy of Dissolution 溶解自由能
· Gibbs free energy change for the dissolution process · Entropy and enthalpy changes of dissolution · Thermodynamic conditions for spontaneous dissolution
Unit 8 · Acids and Bases 酸与碱
Exam weight: 11-15%
8.1 — Introduction to Acids and Bases 酸碱简介
· Arrhenius acid-base theory · Bronsted-Lowry acid-base theory · Conjugate acid-base pairs
8.2 — pH and pOH of Strong Acids and Bases 强酸强碱的pH和pOH
· Definition and calculation of pH and pOH · Complete ionization of strong acids and bases · Relationship pH + pOH = 14
8.3 — Weak Acid and Base Equilibria 弱酸弱碱的平衡
· Acid dissociation constant Ka · Base dissociation constant Kb · Calculating pH of weak acid and weak base solutions
8.4 — Acid-Base Reactions and Buffers 酸碱反应与缓冲溶液
· Nature of acid-base neutralization reactions · Composition of buffer solutions · How buffer solutions work
8.5 — Acid-Base Titrations 酸碱滴定
· Features of titration curves · Determining pH at the equivalence point · Selecting indicators
8.6 — Molecular Structure of Acids and Bases 酸碱的分子结构
· Effect of molecular structure on acid strength · Acid strength trends in oxyacids · Relationship between bond polarity and acidity
8.7 — pH and pKa pH与pKa
· Definition and significance of pKa · Relationship between pH and pKa · Comparing relative acid strengths
8.8 — Properties of Buffers 缓冲溶液的性质
· Ability of buffers to resist pH changes · pH range of buffer solutions · Preparation of buffer solutions
8.9 — Henderson-Hasselbalch Equation 亨德森-哈塞尔巴尔赫方程
· Derivation of the Henderson-Hasselbalch equation · Calculating buffer pH using the equation · Determining component ratios of buffer solutions
8.10 — Buffer Capacity 缓冲容量
· Definition of buffer capacity · Factors affecting buffer capacity · Conditions for buffer failure
Unit 9 · Applications of Thermodynamics 热力学的应用
Exam weight: 7-9%
9.1 — Introduction to Entropy 熵的简介
· Concept and microscopic interpretation of entropy · Relationship between entropy and disorder · Qualitative prediction of entropy changes
9.2 — Absolute Entropy and Entropy Change 绝对熵与熵变
· Third Law of Thermodynamics · Standard molar entropy · Calculating reaction entropy change (delta S standard)
9.3 — Gibbs Free Energy and Thermodynamic Favorability 吉布斯自由能与热力学可行性
· Application of delta G = delta H - T delta S · Criteria for spontaneous reactions · Effect of temperature on spontaneity
9.4 — Thermodynamic and Kinetic Control 热力学控制与动力学控制
· Thermodynamic products vs. kinetic products · Distinction between reaction rate and thermodynamic favorability · Effect of temperature on product distribution
9.5 — Free Energy and Equilibrium 自由能与平衡
· Relationship between delta G standard and K · Application of delta G standard = -RT ln K · Calculating delta G under non-standard conditions
9.6 — Coupled Reactions 耦合反应
· Concept of coupled reactions · Driving non-spontaneous reactions · Coupled reactions in biological systems (ATP)
9.7 — Galvanic (Voltaic) and Electrolytic Cells 原电池与电解池
· How galvanic (voltaic) cells work · How electrolytic cells work · Comparison of the two cell types
9.8 — Cell Potential and Free Energy 电池电势与自由能
· Standard electrode potentials · Application of delta G standard = -nFE standard · Cell potential and spontaneity of reactions
9.9 — Cell Potential Under Nonstandard Conditions 非标准条件下的电池电势
· Application of the Nernst equation · Effect of concentration on cell potential · Concentration cells
9.10 — Electrolysis and Faraday's Law 电解与法拉第定律
· Basic principles of electrolysis · Application of Faraday's law · Quantitative calculations of electrolysis products