📚 Year 13 AQA Chemistry: Key Terms & Vocabulary Quick Memory Guide | 词汇术语速记指南
Mastering the precise language of AQA Year 13 Chemistry is one of the most effective ways to lift your exam performance. This guide presents essential terms from every major topic, with paired English and Chinese explanations, designed to speed up your memorisation. Whether you are tackling thermodynamics, aromatic mechanisms or transition metal complexes, these concise definitions and memory hooks will help you recall the right vocabulary at the right time.
精准掌握 AQA Year 13 化学的语言是提升考试成绩最有效的途径之一。本指南整理了每个重要主题的核心术语，提供英文与中文的配对解释，帮助你快速记忆。无论是热力学、芳烃机理还是过渡金属配合物，这些简洁的定义和记忆线索都能让你在需要的时刻准确调取正确的词汇。
1. Organic Reaction Mechanisms: Electrophiles, Nucleophiles & Radicals | 有机反应机理：亲电试剂、亲核试剂与自由基
An electrophile is an electron‑deficient species that accepts an electron pair to form a new covalent bond. It is attracted to regions of high electron density. Typical examples include H⁺, NO₂⁺, and SO₃.
亲电试剂是缺电子的物种，通过接受一对电子形成新的共价键。它被高电子密度区域所吸引。常见的亲电试剂有 H⁺、NO₂⁺ 和 SO₃。
A nucleophile donates a lone pair of electrons to an electron‑deficient centre. Nucleophiles are often negatively charged or contain lone‑pair atoms. Examples: OH⁻, CN⁻, NH₃ and H₂O.
亲核试剂提供孤对电子给缺电子中心。亲核试剂通常带负电荷或含有孤对电子的原子，例如 OH⁻、CN⁻、NH₃ 和 H₂O。
A radical (free radical) is a species possessing an unpaired electron, making it extremely reactive. In AQA mechanisms, radicals are shown with a single dot, e.g. Cl• from homolytic fission of Cl₂.
自由基是带有一个不成对电子的物种，反应活性极高。在 AQA 的机理中，自由基用单个点表示，例如 Cl₂ 均裂产生的 Cl•。
Memory aid: Think 'electrophile = electron lover' and 'nucleophile = nucleus lover'. Radicals are the lone‑wolf species with a single unpaired electron.
记忆技巧：把 "electrophile" 想象成“爱电子者”，"nucleophile" 是“爱核者”。自由基则是那个带着单电子的“独狼”。
2. Functional Groups and Reaction Types | 官能团与反应类型
Addition reaction: two reactant molecules combine to form one product. Characteristic of alkenes and carbonyls, where a π‑bond is broken and two σ‑bonds are formed.
加成反应：两个反应物分子结合生成一个产物。多见于烯烃和羰基化合物，反应中一个 π 键断裂并生成两个 σ 键。
Substitution reaction: an atom or group is replaced by another. Halogenoalkanes undergo nucleophilic substitution; arenes undergo electrophilic substitution.
取代反应：一个原子或基团被另一个取代。卤代烷发生亲核取代，芳烃发生亲电取代。
Elimination reaction: a small molecule (often H₂O or HX) is removed, forming an unsaturated product. Base‑induced elimination from halogenoalkanes yields alkenes.
消除反应：脱去一个小分子（常为 H₂O 或 HX），生成不饱和产物。卤代烷在碱的作用下发生消除反应得到烯烃。
Condensation: two molecules join with the elimination of a small molecule, e.g. esterification forming an ester and water.
缩合反应：两个分子结合同时脱去一个小分子，如酯化反应生成酯和水。
Hydrolysis: splitting a bond by reaction with water. Often acid‑ or base‑catalysed, such as hydrolysis of esters producing alcohol and carboxylic acid.
水解反应：通过与水反应使化学键断裂。通常在酸或碱催化下进行，如酯水解生成醇和羧酸。
3. Thermodynamics: Enthalpy, Entropy & Gibbs Free Energy | 热力学：焓、熵与吉布斯自由能
Standard enthalpy change (ΔH⦵) refers to the heat transferred under standard conditions (100 kPa, 298 K) with substances in their standard states. ΔH⦵f means formation, ΔH⦵c means combustion.
标准焓变 (ΔH⦵) 指在标准条件 (100 kPa, 298 K) 下，反应物和产物均处于标准态时的热量变化。ΔH⦵f 表示生成焓，ΔH⦵c 表示燃烧焓。
Entropy (S) measures the dispersal of energy or disorder in a system. Gases have higher entropy than liquids, which have higher entropy than solids. ΔS⦵ is the standard entropy change.
熵 (S) 衡量系统中能量的分散程度或无秩序的程度。气体的熵高于液体，液体的熵高于固体。ΔS⦵ 表示标准熵变。
ΔG⦵ = ΔH⦵ – TΔS⦵
Gibbs free energy change determines reaction feasibility. A reaction becomes feasible when ΔG⦵ < 0. Temperature T must be in kelvin.
吉布斯自由能变判断反应是否可行。当 ΔG⦵ < 0 时反应可行。温度 T 必须使用开尔文温标。
Memory: 'If Gibbs is negative, the reaction is active.' Also recall ΔG⦵ = ΔH⦵ – TΔS⦵ as the 'Goldilocks equation' balancing enthalpy and entropy.
记忆口诀：“吉布斯为负，反应自有路。”同时将 ΔG⦵ = ΔH⦵ – TΔS⦵ 视作平衡焓与熵的“金凤花方程”。
4. Kinetics: Rate Equations, Orders and Arrhenius | 动力学：速率方程、级数与阿伦尼乌斯
ate = k[A]ᵐ[B]ⁿ. m and n are the orders with respect to A and B, determined experimentally—not from the stoichiometric equation.
速率方程将反应速率与反应物浓度关联：速率 = k[A]ᵐ[B]ⁿ。m 和 n 分别是对 A 和 B 的反应级数，由实验确定，不能从化学反应计量方程式直接获得。
The rate constant k is temperature‑dependent. Its units vary with the overall order of reaction, e.g. for second order overall: mol⁻¹ dm³ s⁻¹.
速率常数 k 随温度变化。其单位取决于总反应级数，例如总反应为二级时：mol⁻¹ dm³ s⁻¹。
k = A exp(−Eₐ/RT)
The Arrhenius equation shows the exponential relationship between k and temperature. Eₐ is the activation energy, A is the pre‑exponential factor, R is the gas constant (8.31 J mol⁻¹ K⁻¹).
阿伦尼乌斯方程表明 k 与温度之间呈指数关系。Eₐ 为活化能，A 为指前因子，R 为摩尔气体常数 (8.31 J mol⁻¹ K⁻¹)。
A catalyst provides an alternative pathway with a lower activation energy. It increases k but does not affect equilibrium position or the overall enthalpy change.
催化剂提供一条活化能较低的反应路径。它增大速率常数 k，但不改变平衡位置或总焓变。
5. Chemical Equilibria: Kc, Kp and Le Chatelier’s Principle | 化学平衡：Kc、Kp 与勒夏特列原理
For a general reaction aA + bB ⇌ cC + dD, the equilibrium constant in terms of concentration:
对于一般反应 aA + bB ⇌ cC + dD，浓度平衡常数表示为：
Kc = [C]c [D]d / [A]a [B]b
Kc is constant at a given temperature. Only temperature changes shift its value; concentration or pressure changes do not.
在给定温度下
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