Last-Minute Revision Notes for IB & AQA Chemistry | IB AQA 化学：考前冲刺笔记

📚 Last-Minute Revision Notes for IB & AQA Chemistry | IB AQA 化学：考前冲刺笔记

Preparing for the IB or AQA Chemistry exam requires a solid grasp of fundamental concepts, quick recall of definitions, and the ability to apply knowledge to unfamiliar problems. These last-minute revision notes condense the most critical topics from atomic structure to organic chemistry, helping you strengthen your weak areas before the final test.

准备IB或AQA化学考试需要扎实掌握基本概念、快速回忆定义，并能够将知识应用于陌生问题。这些考前冲刺笔记浓缩了从原子结构到有机化学的最关键主题，帮助你在最终考试前强化薄弱环节。

1. Atomic Structure and Periodic Trends | 原子结构与周期趋势

Atoms consist of protons, neutrons and electrons. The atomic number Z defines the element; mass number A = protons + neutrons. Isotopes have the same Z but different A. Electron configuration follows the Aufbau principle: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ and so on. Across a period, atomic radius decreases while ionisation energy and electronegativity increase due to greater nuclear charge.

原子由质子、中子和电子组成。原子序数Z决定元素种类；质量数A = 质子数 + 中子数。同位素的Z相同而A不同。电子排布遵循构造原理：1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 等。同一周期从左到右，原子半径递减，而电离能和电负性递增，这是因为核电荷增大。

2. Stoichiometry and Mole Concept | 化学计量与摩尔概念

One mole contains 6.02 × 10²³ entities. Molar mass M in g·mol⁻¹ links mass and moles: n = m / M. The ideal gas law pV = nRT is essential for gas calculations (R = 8.31 J·K⁻¹·mol⁻¹). In titrations, use n = cV (with V in dm³) to relate concentration and volume at the equivalence point. Always balance equations first to convert between moles of reactants and products.

1摩尔含有6.02 × 10²³个微粒。摩尔质量M的单位是g·mol⁻¹，将质量与物质的量联系起来：n = m / M。理想气体状态方程pV = nRT是气体计算的核心（R = 8.31 J·K⁻¹·mol⁻¹）。在滴定中，运用n = cV（V单位为dm³）在等当点关联浓度与体积。务必先配平方程式，再在反应物与产物之间进行物质的量换算。

3. Chemical Bonding and Structure | 化学键与结构

Ionic bonding involves electron transfer to form cations and anions held by electrostatic forces. Covalent bonding arises from electron sharing; polarity is determined by electronegativity difference. Metallic bonding is a lattice of cations in a sea of delocalised electrons. VSEPR theory predicts molecular shapes: e.g. 4 electron pairs give tetrahedral (109.5°), 3 give trigonal planar (120°). Intermolecular forces include London dispersion, dipole-dipole and hydrogen bonding, which affect boiling points.

离子键通过电子转移形成阳离子与阴离子，以静电引力结合。共价键由共享电子形成；极性取决于电负性差值。金属键是阳离子晶格浸泡在离域电子海中。VSEPR理论预测分子形状：例如4对电子呈四面体（109.5°），3对呈平面三角形（120°）。分子间作用力包括伦敦色散力、偶极-偶极力和氢键，它们影响沸点高低。

4. Energetics and Thermochemistry | 能量学与热化学

Enthalpy change ΔH is measured at constant pressure. Exothermic reactions have ΔH < 0; endothermic have ΔH > 0. Hess’s law states that the total enthalpy change is path-independent. Bond enthalpy calculations: ΔH ≈ Σ(bonds broken) − Σ(bonds formed). In IB HL, Born-Haber cycles link lattice enthalpy, ionisation energies and electron affinity. Standard conditions are 298 K, 100 kPa, with all substances in their standard states.

焓变ΔH在恒压下测定。放热反应ΔH < 0；吸热反应ΔH > 0。盖斯定律指出总焓变与途径无关。键能估算：ΔH ≈ Σ（断裂键能）− Σ（形成键能）。在IB HL中，玻恩-哈伯循环将晶格焓、电离能和电子亲和能联系起来。标准条件为298 K、100 kPa，所有物质处于标准状态。

5. Chemical Kinetics | 化学动力学

Rate of reaction is change in concentration per unit time. The rate equation rate = k[A]ᵐ[B]ⁿ is determined experimentally; m and n are orders, k is the rate constant. Factors affecting rate: concentration, temperature (Arrhenius equation k = Ae^(−Eₐ/RT)), surface area and catalysts. Catalysts provide an alternative pathway with lower activation energy Eₐ, speeding up both forward and reverse reactions equally.

反应速率是单位时间内浓度的变化。速率方程 rate = k[A]ᵐ[B]ⁿ 由实验确定；m和n为反应级数，k为速率常数。影响速率的因素：浓度、温度（阿伦尼乌斯方程 k = Ae^(−Eₐ/RT)）、表面积和催化剂。催化剂通过提供较低活化能Eₐ的替代途径，同等程度地加快正、逆反应。

6. Chemical Equilibrium | 化学平衡

Dynamic equilibrium: rate of forward reaction equals rate of reverse. Le Chatelier’s principle: if a system at equilibrium is disturbed, it shifts to counteract the change. Equilibrium constant Kc = [C]ᶜ[D]ᵈ / [A]ᵃ[B]ᵇ for aA + bB ⇌ cC + dD. Kc is affected only by temperature. For gases, Kp uses partial pressures. Reaction quotient Q indicates direction: Q < Kc shifts right, Q > Kc shifts left.

动态平衡：正反应速率等于逆反应速率。勒夏特列原理：如果平衡体系受到扰动，平衡会朝减弱该改变的方向移动。平衡常数Kc = [C]ᶜ[D]ᵈ / [A]ᵃ[B]ᵇ，对应 aA + bB ⇌ cC + dD。Kc仅受温度影响。对气体，Kp用分压表示。反应商Q指示方向：Q < Kc向右移动，Q > Kc向左移动。

7. Acids, Bases and pH | 酸、碱与pH

Bronsted-Lowry acids donate protons, bases accept protons. pH = −log[H⁺]; pOH = −log[OH⁻]; pH + pOH = 14 at 298 K. Strong acids fully dissociate; weak acids have Ka = [H⁺][A⁻]/[HA] and pKa = −log Ka. Buffer solutions resist pH change; for an acid buffer, pH ≈ pKa + log([base]/[acid]) (Henderson-Hasselbalch). Titration curves show equivalence points where pH changes sharply; indicator choice depends on the pH range.

布朗斯特-劳里酸是质子给体，碱是质子受体。pH = −log[H⁺]；pOH = −log[OH⁻]；298 K时pH + pOH = 14。强酸完全解离；弱酸有Ka = [H⁺][A⁻]/[HA]，pKa = −log Ka。缓冲溶液能抵抗pH变化；对酸性缓冲，pH ≈ pKa + log([碱]/[酸])（亨德森-哈塞尔巴尔赫方程）。滴定曲线在等当点pH突跃；指示剂的选择取决于pH突变范围。

8. Redox Processes | 氧化还原过程

Oxidation is loss of electrons (increase in oxidation number), reduction is gain. Balance redox using half-equations. In electrochemical cells, the cell potential E°cell = E°cathode − E°anode. A positive E°cell indicates a spontaneous reaction. Standard electrode potentials are measured against the standard hydrogen electrode (0 V). The Nernst equation relates E to concentrations: E = E° − (RT/nF)lnQ.

氧化是失去电子（氧化数升高），还原是得到电子。用半反应配平氧化还原方程式。在原电池中，电池电动势E°cell = E°阴极 − E°阳极。正的E°cell表明反应自发。标准电极电势以标准氢电极（0 V）为参比。能斯特方程关联电势与浓度：E = E° − (RT/nF)lnQ。

9. Organic Chemistry Basics | 有机化学基础

Organic molecules are built on carbon skeletons. Functional groups determine reactivity: alkanes (C-C), alkenes (C=C), alcohols (-OH), aldehydes (-CHO), ketones (C=O), carboxylic acids (-COOH), amines (-NH₂). IUPAC nomenclature requires identification of the longest chain, suffixes and prefixes. Key reaction types: substitution (alkanes with halogens UV), addition (alkenes with H₂, Br₂, HBr), oxidation (alcohols → aldehydes → carboxylic acids), esterification and condensation polymerisation.

有机分子建立在碳骨架上。官能团决定反应活性：烷烃 (C-C)、烯烃 (C=C)、醇 (-OH)、醛 (-CHO)、酮 (C=O)、羧酸 (-COOH)、胺 (-NH₂)。IUPAC命名需确定最长碳链、后缀和前缀。关键反应类型：取代（烷烃与卤素需紫外光）、加成（烯烃与H₂, Br₂, HBr）、氧化（醇 → 醛 → 羧酸）、酯化和缩聚。

10. Analytical Techniques | 分析技术

Infrared (IR) spectroscopy identifies bonds by characteristic absorption ranges (e.g. O–H broad ~3200–3600 cm⁻¹, C=O sharp ~1700 cm⁻¹). Mass spectrometry gives the molecular ion peak (M⁺) and fragmentation pattern. NMR (¹H and ¹³C) reveals hydrogen/carbon environments; chemical shift, integration and splitting provide structural details. Chromatography (TLC, GC) separates mixtures based on affinity to stationary and mobile phases.

红外（IR）光谱通过特征吸收范围鉴定化学键（如O–H宽峰约3200–3600 cm⁻¹，C=O尖峰约1700 cm⁻¹）。质谱给出分子离子峰 (M⁺) 和碎片模式。核磁共振（¹H和¹³C）揭示氢/碳环境；化学位移、积分和裂分提供结构细节。色谱法（TLC、GC）基于组分对固定相和流动相亲和力的差异分离混合物。

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Last-Minute Revision Notes for IB & AQA Chemistry | IB AQA 化学：考前冲刺笔记