Year 13 Edexcel Chemistry: Vocabulary Quick Memory Guide | Edexcel 化学 Year 13 词汇术语速记指南

📚 Year 13 Edexcel Chemistry: Vocabulary Quick Memory Guide | Edexcel 化学 Year 13 词汇术语速记指南

Mastering the essential terminology in Year 13 Edexcel Chemistry is the key to tackling synoptic questions, calculations and organic mechanisms with confidence. This guide compiles high-frequency terms across all core topics, giving you a quick bilingual reference to reinforce understanding and memory. Each term is presented with a concise definition in English followed by its Chinese equivalent, allowing you to switch seamlessly between the two languages during revision.

掌握 Year 13 Edexcel 化学中的核心术语，是攻克综合题、计算题和有机机理的关键。本指南汇集了所有核心专题中的高频词汇，提供一份快速的双语对照表，帮助强化理解与记忆。每个术语先给出精炼的英文定义，紧接着是中文释义，让你在复习时能够在中英文之间自如切换，巩固关键概念。

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1. Thermodynamics & Energetics | 热力学与能量学

Enthalpy change (ΔH): The heat energy transferred at constant pressure; ΔH is negative for exothermic and positive for endothermic reactions.

焓变 (ΔH)：恒压条件下传递的热量；放热反应 ΔH 为负，吸热反应 ΔH 为正。

Standard enthalpy of formation (ΔHf°): The enthalpy change when one mole of a substance is formed from its elements in their standard states under standard conditions (298 K, 100 kPa).

标准生成焓 (ΔHf°)：在标准状态和标准条件 (298 K, 100 kPa) 下，由元素的单质生成 1 mol 物质时的焓变。

Standard enthalpy of combustion (ΔHc°): The enthalpy change when one mole of a substance is completely burned in oxygen under standard conditions.

标准燃烧焓 (ΔHc°)：在标准条件下，1 mol 物质在氧气中完全燃烧时的焓变。

Hess’s Law: The total enthalpy change for a reaction is independent of the route taken, provided the initial and final conditions are the same.

盖斯定律：只要始态和终态相同，反应的总焓变与途径无关。

Born–Haber cycle: A thermochemical cycle that applies Hess’s Law to calculate lattice energy by summing enthalpy changes for atomisation, ionisation, electron affinity and formation.

玻恩‑哈伯循环：应用盖斯定律通过原子化、电离、电子亲和和生成焓等多个步骤的焓变加和来计算晶格能的热化学循环。

Lattice energy (ΔHLE): The enthalpy change when one mole of an ionic solid is formed from its gaseous ions; always exothermic and a measure of ionic bond strength.

晶格能 (ΔHLE)：气态离子形成 1 mol 离子固体时的焓变；始终为负值，是离子键强度的量度。

Entropy (S): A measure of the disorder or dispersal of energy in a system; solids have lower entropy than gases.

熵 (S)：系统混乱度或能量分散程度的量度；固体的熵低于气体。

Gibbs free energy (G): The thermodynamic criterion for feasibility, combining enthalpy and entropy:

ΔG = ΔH – TΔS

吉布斯自由能 (G)：结合焓与熵的热力学判据，用于判断反应的自发性：ΔG = ΔH – TΔS。

Feasible reaction: A reaction for which ΔG < 0; the sign of ΔG predicts whether a reaction can occur under given conditions.

可行反应：ΔG < 0 的反应；ΔG 的符号可预测在给定条件下反应能否发生。

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2. Kinetics | 动力学

Rate equation: An expression linking reaction rate to the concentrations of reactants raised to powers (orders): Rate = k[A]ᵐ[B]ⁿ.

速率方程：将反应速率与反应物浓度（带幂次）联系起来的表达式：Rate = k[A]ᵐ[B]ⁿ。

Order of reaction: The power to which a reactant concentration is raised in the rate equation; can be zero, first, second, etc.

反应级数：速率方程中反应物浓度的幂指数；可为 0、1、2 等级数。

Rate constant (k): The proportionality constant in the rate equation; its value depends on temperature and the presence of a catalyst.

速率常数 (k)：速率方程中的比例常数；其值取决于温度和催化剂的存在。

Overall order: The sum of the orders of all reactants in the rate equation.

总级数：速率方程中所有反应物级数的总和。

Half-life (t½): The time taken for the concentration of a reactant to fall to half its initial value; for a first‑order reaction, half‑life is constant.

半衰期 (t½)：反应物浓度降至初始值一半所需的时间；一级反应的半衰期为常数。

Arrhenius equation: Relates the rate constant to temperature and activation energy:

k = A e^(–Eₐ/RT)

阿伦尼乌斯方程：将速率常数与温度和活化能关联：k = A e^(–Eₐ/RT)（其中 A 为指前因子，Eₐ 为活化能，R 为气体常数，T 为热力学温度）。

Activation energy (Ea): The minimum energy required for a collision to result in a reaction.

活化能 (Eₐ)：碰撞引起反应所需的最低能量。

Rate‑determining step: The slowest step in a multi‑step reaction mechanism; it governs the overall rate and determines the rate equation.

决速步骤：多步反应机理中最慢的一步；它控制总反应速率并决定速率方程。

Catalyst: A substance that increases the rate of reaction without being consumed, by providing an alternative pathway with lower activation energy.

催化剂：通过提供较低活化能的替代途径，在反应中不被消耗而提高反应速率的物质。

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3. Chemical Equilibria | 化学平衡

Dynamic equilibrium: The state in which the forward and reverse reactions proceed at the same rate, so macroscopic concentrations remain constant.

动态平衡：正反应与逆反应速率相等的状态，宏观上各物质浓度保持不变。

Le Chatelier’s principle: If a system at equilibrium is subjected to a change in concentration, pressure or temperature, the equilibrium shifts to counteract the imposed change.

勒夏特列原理：如果处于平衡的体系受到浓度、压强或温度的改变，平衡会向削弱该改变的方向移动。

Equilibrium constant Kc: For a homogeneous reversible reaction aA + bB ⇌ cC + dD,

Kc = [C]ᶜ[D]ᵈ / [A]ᵃ[B]ᵇ

平衡常数 Kc：对于均相可逆反应 aA + bB ⇌ cC + dD，Kc 的表达式为 [C]ᶜ[D]ᵈ / [A]ᵃ[B]ᵇ（方括号表示平衡浓度，单位 mol dm⁻³）。

Equilibrium constant Kp: For gaseous equilibria, partial pressures replace concentrations:

Kp = (pC)ᶜ(pD)ᵈ / (pA)ᵃ(pB)ᵇ

平衡常数 Kp：对于气体平衡，用各组分分压代替浓度：Kp = (pC)ᶜ(pD)ᵈ / (pA)ᵃ(pB)ᵇ。

Effect of temperature on Kc/Kp: Increasing temperature favours the endothermic direction; K increases for endothermic forward reactions and decreases for exothermic forward reactions.

温度对 Kc/Kp 的影响：升高温度有利于吸热方向；若正反应吸热，K 增大；若正反应放热，K 减小。

Effect of catalyst: A catalyst speeds up both forward and reverse reactions equally and does not alter the value of the equilibrium constant.

催化剂的影响：催化剂同等程度地加快正、逆反应，不改变平衡常数的数值。

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4. Acid–Base Equilibria | 酸碱平衡

Brønsted–Lowry acid: A proton (H⁺) donor.

布朗斯特‑劳里酸：质子 (H⁺) 给予体。

Brønsted–Lowry base: A proton (H⁺

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