SQA Higher Chemistry: Vocabulary and Terminology Memorization Guide | SQA 高等化学：词汇术语速记指南

📚 SQA Higher Chemistry: Vocabulary and Terminology Memorization Guide | SQA 高等化学：词汇术语速记指南

Mastering the key vocabulary is half the battle in SQA Higher Chemistry. From bonding to reaction kinetics, terminology builds the foundation for understanding concepts and answering exam questions accurately. This guide provides essential terms grouped by topic, along with memory tricks to help you retain them and apply them confidently in assessments.

掌握关键词汇是 SQA 高等化学成功的一半。从化学键到反应动力学，术语是理解概念和准确答题的基础。本指南按主题归类核心术语，并提供记忆技巧，助你牢固掌握并在考试中自信运用。

1. Bonding and Structure Terminology | 化学键与结构术语

A solid grasp of bonding terms is essential for explaining physical properties of substances, such as melting points and conductivity. SQA Higher papers often ask you to describe bonding in terms of electronegativity and intermolecular forces, so familiarise yourself with the language of structure.

扎实掌握化学键术语，对于解释物质的物理性质（如熔点和导电性）至关重要。SQA 高等考试常要求你用电负性和分子间作用力来描述键合，因此要熟悉结构语言。

Electronegativity – a measure of the attraction of an atom for the bonding electrons in a covalent bond. Values increase across a period and decrease down a group.

电负性 – 衡量原子在共价键中对键合电子吸引能力的尺度。同周期从左到右递增，同族从上到下递减。

Ionic bond – the electrostatic attraction between oppositely charged ions formed when a metal transfers electrons to a non-metal. Requires a large electronegativity difference (usually >1.7).

离子键 – 金属向非金属转移电子后，阴阳离子间的静电引力。通常要求电负性差值较大（>1.7）。

Covalent bond – a shared pair of electrons between two non-metal atoms. Non-polar when atoms have identical electronegativity; polar when there is a difference, creating partial charges δ⁺ and δ⁻.

共价键 – 两个非金属原子间共享一对电子。原子电负性相同时为非极性键；存在差异时为极性键，产生部分电荷 δ⁺ 和 δ⁻。

Hydrogen bonding – a strong dipole-dipole attraction between a lone pair on N, O or F and a hydrogen atom covalently bonded to N, O or F. Crucial for explaining the higher boiling points of H₂O, NH₃ and HF.

氢键 – N、O 或 F 上的孤对电子与另一分子中与 N、O 或 F 成键的氢原子之间强烈的偶极-偶极吸引。可用于解释 H₂O、NH₃ 和 HF 的沸点偏高。

Metallic bonding – the attraction between delocalised electrons and positive metal ions. Explains electrical conductivity and malleability.

金属键 – 离域电子与正金属离子间的吸引力。可解释导电性与可延展性。

Van der Waals forces – temporary instantaneous dipole-induced dipole attractions that exist between all atoms and molecules. Increase with molecular size and shape, affecting boiling points of non-polar substances.

范德华力 – 所有原子和分子间存在的瞬时偶极-诱导偶极引力。随分子大小和形状增加，影响非极性物质的沸点。

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2. Organic Chemistry Foundations | 有机化学基础术语

SQA Higher organic chemistry relies heavily on systematic naming and recognising families of compounds. Knowing the basic vocabulary allows you to decode any structure and identify reaction pathways.

SQA 高等有机化学高度依赖系统命名和化合物族的识别。掌握基础词汇可以让你解析任何结构并识别反应途径。

Hydrocarbon – a compound containing only carbon and hydrogen atoms. Saturated hydrocarbons contain only single bonds (alkanes); unsaturated contain double or triple bonds (alkenes, alkynes).

烃 – 仅含碳和氢的化合物。饱和烃只含单键（烷烃）；不饱和烃含有双键或三键（烯烃、炔烃）。

Homologous series – a family of organic compounds with the same general formula, functional group and similar chemical properties, where each member differs by a CH₂ unit.

同系物 – 具有相同通式、官能团和相似化学性质的一系列有机化合物，相邻成员相差一个 CH₂ 单元。

Functional group – an atom or group of atoms that gives a molecule its characteristic reactions. Examples: hydroxyl –OH (alcohols), carboxyl –COOH (carboxylic acids), carbonyl C=O (aldehydes and ketones).

官能团 – 赋予分子特征反应的原子或原子团。例如：羟基 –OH（醇类）、羧基 –COOH（羧酸）、羰基 C=O（醛和酮）。

Isomer – molecules with the same molecular formula but different structural arrangements. Structural isomers have different bonds; stereoisomers have the same connectivity but differ in spatial arrangement (geometric isomers require a double bond and two different groups on each carbon).

异构体 – 分子式相同但结构排列不同的分子。构造异构体的键合不同；立体异构体连接方式相同但空间排列不同（几何异构要求有双键且每个碳上连有两个不同基团）。

Alkyl group – an alkane with one hydrogen removed, e.g. methyl –CH₃, ethyl –C₂H₅. Used as branches in nomenclature.

烷基 – 烷烃去掉一个氢原子形成的基团，如甲基 –CH₃、乙基 –C₂H₅。命名中用作支链。

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3. Functional Groups and Homologous Series | 官能团与同系物速记

You must be able to name and draw structures for key functional groups. A clever mnemonic helps: ‘Monkeys Eat Peeled Bananas’ for methyl, ethyl, propyl, butyl, but many prefer learning the suffixes directly: -ol (alcohol), -al (aldehyde), -one (ketone), -oic acid (carboxylic acid).

你必须能够命名和绘制关键官能团的结构。用口诀记忆：’Monkeys Eat Peeled Bananas’ 对应甲基、乙基、丙基、丁基，但许多人更倾向直接记后缀：-ol（醇）、-al（醛）、-one（酮）、-oic acid（羧酸）。

Alkanes: suffix -ane, general formula CₙH₂ₙ₊₂. Methane CH₄, ethane C₂H₆.

烷烃：后缀 -ane，通式 CₙH₂ₙ₊₂。如甲烷 CH₄、乙烷 C₂H₆。

Alkenes: suffix -ene, general formula CₙH₂ₙ. Ethene C₂H₄, propene C₃H₆. The double bond location needs the smallest number.

烯烃：后缀 -ene，通式 CₙH₂ₙ。如乙烯 C₂H₄、丙烯 C₃H₆。须用最小数字标出双键位置。

Alcohols: suffix -ol, general formula CₙH₂ₙ₊₁OH. Ethanol C₂H₅OH. Primary, secondary or tertiary based on the carbon bearing the –OH.

醇：后缀 -ol，通式 CₙH₂ₙ₊₁OH。如乙醇 C₂H₅OH。根据与 –OH 相连的碳原子的类别分为伯、仲、叔醇。

Aldehydes: suffix -al, carbonyl group at the end of the chain, e.g. ethanal CH₃CHO.

醛：后缀 -al，羰基在碳链末端，如乙醛 CH₃CHO。

Ketones: suffix -one, carbonyl group on an interior carbon, e.g. propanone CH₃COCH₃.

酮：后缀 -one，羰基在非末端碳上，如丙酮 CH₃COCH₃。

Carboxylic acids: suffix -oic acid, functional group –COOH, e.g. ethanoic acid CH₃COOH.

羧酸：后缀 -oic acid，官能团 –COOH，如乙酸 CH₃COOH。

Esters: formed from an alcohol and a carboxylic acid; named as alkyl alkanoate, e.g. ethyl ethanoate CH₃COOC₂H₅. ‘RCOOR’ is a handy general formula.

酯：由醇和羧酸反应生成；命名为某酸某酯，如乙酸乙酯 CH₃COOC₂H₅。通式简记为 RCOOR。

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4. Reaction Types and Mechanisms | 反应类型与机理术语

Understanding reaction mechanisms is a key skill. SQA Higher requires you to describe the movement of electrons using curly arrows and classify reactions as addition, substitution, elimination, condensation or hydrolysis, often with specific reagents.

理解反应机理是一项关键技能。SQA 高等化学要求你用弯箭头描述电子移动，并将反应分类为加成、取代、消除、缩合或水解，通常涉及特定试剂。

Addition reaction – two molecules combine to form a single product. Typical for alkenes with H₂ (hydrogenation), H₂O (hydration) or halogens, following the electrophilic addition mechanism.

加成反应 – 两个分子结合生成一个产物。典型例子为烯烃与 H₂（加氢）、H₂O（水合）或卤素的反应，遵循亲电加成机理。

Substitution reaction – one atom or group is replaced by another. Halogenoalkanes undergo nucleophilic substitution with OH⁻, CN⁻ or NH₃. The term ‘nucleophile’ means ‘nucleus-loving’ – a species that donates an electron pair.

取代反应 – 一个原子或基团被另一个替换。卤代烷与 OH⁻、CN⁻ 或 NH₃ 发生亲核取代。’亲核试剂’意为’亲核’——提供电子对的物种。

Elimination reaction – removal of a small molecule (often H–X from a halogenoalkane) to form an alkene. Uses a strong base such as ethanolic KOH.

消除反应 – 脱去一个小分子（常见为卤代烷脱 H–X）生成烯烃。使用强碱如氢氧化钾的乙醇溶液。

Condensation reaction – two molecules join with the elimination of a small molecule like water. Esterification is a classic condensation between an acid and alcohol.

缩合反应 – 两个分子结合，同时脱去一个小分子（如水）。酯化反应是酸与醇之间经典的缩合反应。

Hydrolysis – breakdown of a compound by reaction with water. Esters hydrolyse to acid and alcohol; amides hydrolyse to carboxylic acid and amine. Acid or base catalysis is common.

水解反应 – 化合物与水反应而分解。酯水解生成酸和醇；酰胺水解生成羧酸和胺。常用酸或碱催化。

Electrophile – an electron-deficient species that accepts a pair of electrons (e.g. H⁺, Brδ⁺–Brδ⁻). Memory trick: ‘electro’ = electrons, ‘phile’ = loving.

亲电试剂 – 缺电子物种，能接受电子对（如 H⁺、Brδ⁺–Brδ⁻）。速记：’electro’ 指电子，’phile’ 意为喜好。

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5. Kinetics and Reaction Rate Vocabulary | 动力学与反应速率术语

Kinetics terminology helps you interpret Maxwell-Boltzmann distributions and enthalpy profiles. Knowing the language of collisions and activation energy is vital for explaining why temperature, concentration and catalysts affect rate.

动力学术语有助于你解释麦克斯韦-玻尔兹曼分布和焓变图。掌握碰撞和活化能的语言，对解释温度、浓度和催化剂如何影响反应速率至关重要。

Activation energy (Ea) – the minimum kinetic energy required for colliding particles to react. On a Maxwell-Boltzmann distribution, it is the energy threshold shown by the area under the curve to the right of Ea.

活化能 (Ea) – 碰撞粒子发生反应所需的最低动能。在麦克斯韦-玻尔兹曼分布中，是指分布曲线下方 Ea 右侧的面积。

Successful collision – a collision with energy ≥ Ea and correct orientation that leads to product formation. Increasing concentration or pressure raises collision frequency.

有效碰撞 – 能量不低于活化能且取向正确的碰撞，能生成产物。增加浓度或压强可提高碰撞频率。

Transition state – the unstable arrangement of atoms at the top of the energy barrier, showing partial bond breaking and forming. Represented as the peak in an enthalpy profile.

过渡态 – 能垒顶点处不稳定的原子排列，显示化学键部分断裂与形成。在焓图中位于峰顶。

Catalyst – a substance that increases the rate of reaction by providing an alternative pathway with lower activation energy, without being consumed. In a Maxwell-Boltzmann diagram, this lowers the Ea line, so a higher proportion of particles have sufficient energy.

催化剂 – 通过提供更低活化能的替代路径来加快反应速率，而自身不被消耗的物质。在麦克斯韦-玻尔兹曼图中，Ea 线下移，因此有足够能量的粒子比例增大。

Rate determining step – the slowest step in a multi-step reaction mechanism that determines the overall rate. SQA Higher links this to reaction profiles but does not require detailed rate equations.

决速步骤 – 多步反应机理中最慢的一步，决定总反应速率。SQA 高等化学将其与反应焓图联系，但不要求复杂的速率方程。

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6. Chemical Equilibrium Terms | 化学平衡术语

Equilibrium concepts are central to industrial processes like the Haber and Contact processes. SQA expects you to distinguish between static and dynamic equilibrium and apply Le Chatelier’s principle to predict shifts in equilibrium position.

平衡概念是哈伯法和接触法等工业过程的核心。SQA 要求你区分静态平衡与动态平衡，并运用勒夏特列原理预测平衡移动方向。

Dynamic equilibrium – a state in a closed system where the forward and reverse reactions occur at equal rates, so macroscopic properties remain constant. It is dynamic, not static.

动态平衡 – 在封闭系统中，正反应与逆反应速率相等、宏观性质保持恒定的状态。这是动态而非静态的。

Le Chatelier’s principle – if a system at equilibrium is subjected to a change in concentration, pressure or temperature, the position of equilibrium moves to oppose the change. Increase concentration of reactants → shifts to products; increase pressure → shifts to side with fewer gas moles; increase temperature → shifts in endothermic direction.

勒夏特列原理 – 若平衡系统受到浓度、压强或温度变化，平衡位置会朝着减弱该变化的方向移动。增大反应物浓度 → 向产物方向移动；增大压强 → 向气体分子数少的方向移动；升温 → 向吸热方向移动。

Equilibrium constant (Kc) – for a homogeneous reaction aA + bB ⇌ cC + dD, Kc = [C]^c [D]^d / [A]^a [B]^b. Kc is temperature-dependent only; its value indicates the position of equilibrium. Kc > 1 means product-favoured.

平衡常数 (Kc) – 对于均相反应 aA + bB ⇌ cC + dD，Kc = [C]^c [D]^d / [A]^a [B]^b。Kc 仅与温度有关；其值可指示平衡位置，Kc > 1 表示产物占优势。

Position of equilibrium – describes whether the equilibrium lies to the left (more reactants) or right (more products). Changes in concentration or pressure shift the position but do not change Kc (temperature change does).

平衡位置 – 描述平衡是偏左（反应物较多）还是偏右（产物较多）。浓度或压强的改变会移动平衡位置但不改变 Kc，温度改变会同时改变 Kc。

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7. Enthalpy and Thermochemistry | 焓变与热化学术语

Calorimetry and Hess’s law questions require precise use of enthalpy vocabulary. You must be able to define terms like standard enthalpy of combustion and calculate ΔH using bond enthalpies or experimental data.

量热法与盖斯定律的题目需要精确使用焓变词汇。你必须能够定义标准燃烧焓等术语，并利用键焓或实验数据计算 ΔH。

Enthalpy change (ΔH) – the heat energy change at constant pressure. Exothermic: ΔH negative, heat released; endothermic: ΔH positive, heat absorbed. Unit: kJ mol⁻¹.

焓变 (ΔH) – 恒压下的热量变化。放热：ΔH 为负，释放热量；吸热：ΔH 为正，吸收热量。单位：kJ mol⁻¹。

Standard enthalpy of combustion (ΔH°c) – the enthalpy change when one mole of a substance is completely burned in oxygen under standard conditions. E.g. C₂H₅OH(l) + 3O₂(g) → 2CO₂(g) + 3H₂O(l). Always exothermic.

标准燃烧焓 (ΔH°c) – 在标准条件下，1 摩尔物质在氧气中完全燃烧时的焓变。如 C₂H₅OH(l) + 3O₂(g) → 2CO₂(g) + 3H₂O(l)。总是放热。

Standard enthalpy of formation (ΔH°f) – the enthalpy change when one mole of a compound is formed from its elements in their standard states. ΔH°f of any element in its standard state is zero.

标准生成焓 (ΔH°f) – 由标准状态下的元素生成 1 摩尔化合物时的焓变。标准状态下任何元素的 ΔH°f 为零。

Hess’s law – the enthalpy change for a reaction is independent of the route taken

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