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

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

Mastering the specific vocabulary of A-Level Chemistry is just as crucial as understanding the underlying concepts. Many examination questions demand precise definitions and the correct use of scientific terms. This guide presents a structured, bilingual memory approach to the essential terminology for Year 13 CCEA Chemistry. Each term is paired with clear English explanations, Chinese translations, and effective memorisation tips.

掌握 A-Level 化学的专有词汇与理解核心概念同等重要。许多考试题目要求给出精确定义并正确使用科学术语。本指南为 Year 13 CCEA 化学课程的关键术语提供了结构化的双语记忆方法。每个术语都配有清晰的英文解释、中文翻译和高效的记忆技巧。

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

Enthalpy change (ΔH) is the heat energy transferred in a reaction at constant pressure. Standard conditions are 298 K and 100 kPa.

焓变 (ΔH) 是在恒压下反应中传递的热能。标准条件为 298 K 和 100 kPa。

Standard enthalpy of formation (ΔH_f⁰) is the enthalpy change when one mole of a compound is formed from its elements under standard conditions.

标准生成焓 (ΔH_f⁰) 是在标准条件下由元素生成一摩尔化合物时的焓变。

Bond enthalpy is the energy required to break one mole of a given covalent bond in the gaseous state, averaged over similar compounds.

键焓是断裂气态中一摩尔特定共价键所需的能量，是类似化合物中的平均值。

Term	Memory Tip
Exothermic	Ex- = exit (heat exits system), ΔH negative. Think 'EXit'.
Endothermic	En- = enter (heat enters system), ΔH positive. Think 'ENter'.

放热：ex- 表示“出”（热量离开系统），ΔH 为负。记住“EXit”。吸热：en- 表示“进”（热量进入系统），ΔH 为正。记住“ENter”。

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2. Kinetics and Reaction Rates | 动力学与反应速率

Activation energy (E_a) is the minimum energy colliding particles must possess for a reaction to occur. It is the energy barrier between reactants and products.

活化能 (E_a) 是碰撞粒子发生反应所必须具备的最低能量，是反应物与产物之间的能量壁垒。

Rate constant (k) is the proportionality constant in the rate equation; its value depends on temperature and activation energy. A large k means a fast reaction.

速率常数 (k) 是速率方程中的比例常数；其数值取决于温度和活化能。k 值大意味着反应速率快。

Catalyst provides an alternative reaction pathway with lower activation energy, without being chemically changed at the end. Homogeneous catalysts are in the same phase as reactants; heterogeneous catalysts are in a different phase.

催化剂提供活化能较低的替代反应路径，反应结束时自身不发生化学变化。均相催化剂与反应物处于同一相；多相催化剂处于不同相。

Memory strategy: 'A catalyst climbs down the activation energy hill, then goes back unchanged.'

记忆策略：催化剂先降低活化能“山峰”，反应后恢复原样。

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3. Chemical Equilibrium and Le Chatelier's Principle | 化学平衡与勒夏特列原理

Dynamic equilibrium occurs when the forward and reverse reactions proceed at equal rates, and the concentrations of reactants and products remain constant.

动态平衡在正逆反应速率相等且各物质浓度保持不变时建立。

Equilibrium constant (K_c) expresses the ratio of product concentrations to reactant concentrations at equilibrium, each raised to the power of its stoichiometric coefficient.

平衡常数 (K_c) 表示平衡时产物浓度与反应物浓度之比，各浓度以其化学计量系数为指数。

Le Chatelier's principle states that if a system at equilibrium is subjected to a change in concentration, pressure, or temperature, the position of equilibrium will shift to counteract that change.

勒夏特列原理指出：处于平衡的体系若受到浓度、压力或温度的改变，平衡将向减弱这种改变的方向移动。

Recall phrase: 'The system does the opposite of what you do.' For temperature, treat heat as a reactant (endothermic) or product (exothermic).

速记口诀：“你施加什么，体系就反对什么。” 对于温度，将热量视为反应物（吸热反应）或产物（放热反应）。

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4. Acid–Base Equilibria and pH | 酸碱平衡与 pH

A Brønsted–Lowry acid is a proton (H⁺) donor, and a base is a proton acceptor. Conjugate pairs differ by one proton.

布朗斯特-劳里酸是质子 (H⁺) 给体，碱是质子受体。共轭酸碱对相差一个质子。

pH = – solution, while a weak acid partially dissociates, having an acid dissociation constant K_a.

pH = –log₁₀[H⁺]。强酸在水溶液中完全电离，弱酸仅部分电离，具有酸解离常数 K_a。

Buffer solution resists changes in pH when small amounts of acid or base are added. It consists of a weak acid and its conjugate base, or a weak base and its conjugate acid.

缓冲溶液是加入少量酸或碱时能抵抗 pH 变化的溶液。它由弱酸及其共轭碱，或弱碱及其共轭酸组成。

Memory: 'Buffers catch extra H⁺ or OH⁻ like a sponge.' The Henderson–Hasselbalch equation is often used, but for CCEA, focus on the equilibrium shift: adding acid shifts equilibrium to the left, consuming H⁺.

记忆：缓冲液像海绵一样吸收多余的 H⁺ 或 OH⁻。CCEA 重点在于平衡移动：加酸时平衡向左移，消耗 H⁺。

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5. Redox and Electrochemistry | 氧化还原与电化学

Oxidation is loss of electrons (OIL), reduction is gain of electrons (RIG). An oxidising agent accepts electrons and is itself reduced.

氧化是失去电子 (OIL)，还原是得到电子 (RIG)。氧化剂接受电子，自身被还原。

Standard electrode potential (E⁰) measures the tendency of a half-cell to gain electrons relative to the standard hydrogen electrode. The more positive E⁰, the stronger the oxidising agent.

标准电极电势 (E⁰) 衡量半电池相对于标准氢电极得电子的趋势。E⁰ 越正，氧化剂的氧化性越强。

In an electrochemical cell, the half-cell with the more negative E⁰ undergoes oxidation (anode), and the more positive E⁰ undergoes reduction (cathode). Cell potential E⁰_cell = E⁰_cathode - E⁰_anode.

在原电池中，E⁰ 较负的半电池发生氧化（阳极），较正的半电池发生还原（阴极）。电池电动势 E⁰_cell = E⁰_阴极 - E⁰_阳极。

Memory: 'RED CAT' (REDuction at CAThode) and 'AN OX' (OXidation at ANode). Mnemonic for E⁰: higher potential = higher electron-grabbing power.

记忆口诀：RED CAT（阴极还原）和 AN OX（阳极氧化）。电势越高，得电子能力越强。

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6. Organic Chemistry: Functional Groups and Nomenclature | 有机化学：官能团与命名

Functional group: an atom or group of atoms responsible for the characteristic reactions of a compound. Knowing suffixes and prefixes is essential for IUPAC naming.

官能团：决定化合物特征反应的原子或原子团。掌握词缀对于 IUPAC 命名至关重要。

Homologous Series	Functional Group	Suffix/Prefix
Alkane	C–C, C–H only	-ane
Alkene	C=C	-ene
Alcohol	–OH	-ol
Aldehyde	–CHO	-al
Ketone	C=O between carbons	-one
Carboxylic acid	–COOH	-oic acid
Ester	–COOR	-oate
Amine	–NH₂	-amine

Memory tip: aldehydes end in '-al' (think 'al'-dehyde); ketones end in '-one' (think 'key-tone'). Esters have '-oate' – 'EAT an ester'.

记忆技巧：醛以 “-al” 结尾（联想“醛”的拼音 quán 含“a”），酮以 “-one” 结尾（酮音 tóng）。酯以 “-oate” 结尾，联想“吃酯 (eat ester)”。

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7. Organic Reaction Mechanisms: Essential Terminology | 有机反应机理：核心术语

Homolytic fission: covalent bond breaks so each atom takes one electron, forming two free radicals. Heterolytic fission: one atom takes both electrons, forming a cation and an anion.

均裂：共价键断裂时每个原子各取一个电子，形成两个自由基。异裂：一个原子带走两个电子，形成正离子和负离子。

Electrophile: electron-pair acceptor (e.g. NO₂⁺, Br⁺). Nucleophile: electron-pair donor (e.g. OH⁻, CN⁻, NH₃).

亲电试剂是电子对受体（如 NO₂⁺、Br⁺），亲核试剂是电子对给体（如 OH⁻、CN⁻、NH₃）。

Curly arrows in mechanisms show the movement of an electron pair. A full arrowhead represents movement of two electrons, a half-headed arrow (single electron) is used for radical reactions.

机理中的弯箭头表示电子对移动。实心箭头代表一对电子的移动，单箭头（半箭头）用于自由基反应。

Recall: 'Electrophile loves electrons (seeks negative charge), nucleophile loves nuclei (seeks positive charge).'

记忆：亲电试剂爱电子（寻找负电荷），亲核试剂爱核（寻找正电荷）。

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8. Spectroscopy and Analytical Techniques | 光谱学与分析技术

causes bond vibrations. Peaks are reported as wavenumber (cm⁻¹). A broad peak around 2500–3300 cm⁻¹ indicates O–H in carboxylic acids; a sharp peak at about 1700 cm⁻¹ indicates C=O.

红外光谱通过吸收红外辐射引起键的振动来鉴别官能团。峰位置以波数 (cm⁻¹) 表示。2500–3300 cm⁻¹ 附近的宽峰指示羧酸中的 O–H；约 1700 cm⁻¹ 的尖峰指示 C=O。

Mass spectrometry determines the relative molecular mass (M_r) through the molecular ion peak (M⁺). Fragmentation patterns give structural information.

质谱通过分子离子峰 (M⁺) 确定相对分子质量 (M_r)。碎片离子峰提供结构信息。

NMR spectroscopy (¹³C and ¹H) provides information about the number and environment of carbon and hydrogen atoms. Chemical shift (δ) is measured in ppm. The integrated trace of ¹H NMR shows relative number of protons.

核磁共振波谱（碳谱和氢谱）提供碳原子和氢原子数目及化学环境的信息。化学位移 (δ) 以 ppm 为单位。氢谱的积分曲线显示氢原子的相对个数。

Memory aid: 'IR sees bonds, MS sees mass, NMR sees neighbours.' For ¹H NMR splitting patterns: n+1 rule, where n = number of hydrogens on adjacent carbon.

记忆口诀：红外看键，质谱看质量，核磁看邻居。氢谱分裂遵循 n+1 规则，n 为相邻碳上的氢原子数。

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9. Transition Metal Chemistry | 过渡金属化学

A transition element is a d-block element that forms at least one stable ion with an incomplete d-orbital. Key properties include variable oxidation states, coloured ions, and catalytic activity.

过渡元素是能形成至少一种具有未填满 d 轨道离子的 d 区元素。主要特性包括可变化合价、有色离子和催化活性。

Ligand: an ion or molecule with a lone pair of electrons that forms a coordinate bond with a central metal ion. Bidentate ligands (e.g. ethane-1,2-diamine, ethanedioate) bond through two atoms.

配体：含有孤电子对的离子或分子，与中心金属离子形成配位键。双齿配体（如 1,2-乙二胺、乙二酸根离子）通过两个原子配位。

Coordination number: the number of coordinate bonds formed to the central metal ion. Common numbers are 4 (tetrahedral or square planar) and 6 (octahedral).

配位数：中心金属离子形成的配位键数目。常见配位数为 4（四面体或平面正方形）和 6（八面体）。

Stereoisomerism in complexes: cis–trans (geometric) isomerism occurs in square planar and octahedral complexes, and optical isomerism occurs with bidentate ligands forming non-superimposable mirror images.

配合物的立体异构：平面正方形和八面体配合物存在顺反异构，双齿配体可形成不能重叠的镜像光学异构体。

Ligand substitution and chelate effect: bidentate and polydentate ligands displace monodentate ligands because the reaction produces more particles, increasing entropy (ΔS positive).

配体取代与螯合效应：双齿或多齿配体能取代单齿配体，因为反应后粒子数增多，熵增加 (ΔS > 0)。

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10. Lattice Enthalpy and Born–Haber Cycles | 晶格焓与玻恩-哈伯循环

Lattice enthalpy (ΔH_L) is the enthalpy change when one mole of an ionic solid is formed from its gaseous ions. It is always exothermic and reflects the strength of ionic bonding.

晶格焓 (ΔH_L) 是由气态离子形成一摩尔离子固体时的焓变。该过程总是放热的，反映了离子键的强度。

Born–Haber cycle is an energy cycle that applies Hess's law to calculate lattice enthalpy using atomisation, ionisation, electron affinity, and formation energies. Steps follow the acronym 'F A I E L' – Formation, Atomisation, Ionisation, Electron affinity, Lattice.

玻恩-哈伯循环是运用盖斯定律计算晶格焓的能量循环，涉及生成焓、原子化焓、电离能、电子亲和能和晶格焓。步骤可用缩写“FAIEL”记忆。

Standard enthalpy of solution (ΔH_sol) is the sum of lattice enthalpy (endothermic breaking of lattice) and hydration enthalpy (exothermic hydration of ions). If the overall process is exothermic, the salt is likely soluble.

标准溶解焓 (ΔH_sol) 是晶格焓（破坏晶格吸热）与水合焓（离子水合放热）之和。若总过程放热，盐通常易溶。

Memory: 'Lattice LEaves (breaks) taking energy in, Hydration Hugs ions releasing energy.' Remember that polarising power of cation and polarisability of anion affect thermal stability of compounds like carbonates.

记忆：晶格离开（断裂）需吸热，水合拥抱离子放出能量。阳离子的极化能力和阴离子的变形性影响碳酸盐等化合物的热稳定性。

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11. Entropy and Free Energy | 熵与自由能

Entropy (S) is a measure of the disorder or randomness of a system. Total entropy change ΔS_total = ΔS_system + ΔS_surroundings. For a reaction to be feasible, ΔS_total > 0.

熵 (S) 是体系混乱度或随机性的量度。总熵变 ΔS_total = ΔS_system + ΔS_surroundings。反应自发进行的条件是 ΔS_total > 0。

Gibbs free energy change ΔG = ΔH – and pressure, a reaction is thermodynamically feasible when ΔG < 0. ΔG = 0 at equilibrium.

吉布斯自由能变 ΔG = ΔH – TΔS。在恒温恒压下，反应热力学可行当 ΔG < 0。平衡时 ΔG = 0。

Calculation tip: always convert ΔS from J K⁻¹ mol⁻¹ to kJ K⁻¹ mol⁻¹ to match ΔH in kJ mol⁻¹. Temperature T must be in Kelvin.

计算提示：务必把 ΔS 的单位从 J K⁻¹ mol⁻¹ 转换成 kJ K⁻¹ mol⁻¹ 以匹配 ΔH 的 kJ mol⁻¹。温度 T 必须使用开尔文。

Memory phrase: 'Spontaneous reactions increase the total entropy of the universe.' When ΔH is negative and ΔS positive, reaction is always feasible.

记忆口诀：自发反应增加宇宙总熵。当 ΔH 为负、ΔS 为正时，反应在任何温度都可行。

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12. Practical Vocabulary and Key Terms | 实验词汇与关键术语

Standard solution: a solution of accurately known concentration. Prepared using a volumetric flask. Primary standards (e.g. anhydrous Na₂CO₃) must be pure, stable, and have a high molar mass to minimise weighing errors.

标准溶液：浓度精确已知的溶液，用容量瓶配制。基准物质（如无水 Na₂CO₃）必须纯净、稳定且摩尔质量大以减少称量误差。

Back titration: used when the substance is insoluble, volatile, or reacts slowly. An excess of reagent is added, and the unreacted portion is titrated.

返滴定：用于反应物难溶、易挥发或反应缓慢的场合。加入过量试剂，再滴定剩余部分。

Accuracy refers to how close a measurement is to the true value, while precision refers to the reproducibility of measurements. Systematic errors affect accuracy, random errors affect precision.

准确度指测量值接近真实值的程度，精密度指测量结果的重现性。系统误差影响准确度，随机误差影响精密度。

Reflux: continuous boiling and condensing of a reaction mixture to prevent loss of volatile components. Distillation separates liquids based on boiling points.

回流：反应混合物持续沸腾并冷凝，防止挥发性成分损失。蒸馏根据沸点不同分离液体。

Quenching: rapid cooling to stop a reaction, often used in kinetics experiments. Titration with sodium thiosulfate can quench iodine clock reactions.

淬灭：快速冷却以终止反应，常用于动力学实验。用硫代硫酸钠滴定可淬灭碘钟反应。

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