📚 Year 11 SQA Chemistry: Fast-Track Terminology Memorisation Guide | SQA Year 11 化学：术语速记指南
Mastering the language of chemistry is half the battle in SQA exams. This guide breaks down essential terms by topic, pairing each definition with a memory hook, word root, or simple analogy. You will find the most tested vocabulary for Year 11 (National 5 equivalent), from atomic structure to reaction rates, presented in bite-sized English-Chinese pairs.
掌握化学的语言是 SQA 考试成功的一半。本指南按主题拆分必考术语，为每个定义配上记忆线索、词根或简单类比。从原子结构到反应速率，你都能看到 Year 11（相当于苏格兰 National 5）最高频的词汇，以英中配对形式呈现，帮助你速记速查。
1. Atomic Structure & Periodicity | 原子结构与周期律术语
Atom – the smallest neutral particle of an element that still shows the chemical properties of that element. Every atom has a tiny, dense nucleus and shells of electrons around it.
Atom（原子） – 元素保持其化学性质的最小电中性粒子。每个原子都有一个微小致密的核和环绕的电子层。
Proton (p⁺) – a subatomic particle found in the nucleus; it carries a positive charge of +1 and a relative mass of 1. The number of protons defines the element (atomic number, Z).
Proton（质子，p⁺） – 位于原子核内的亚原子粒子，带 +1 正电荷，相对质量约为 1。质子数决定了元素种类（原子序数 Z）。
Neutron (n⁰) – a neutral subatomic particle in the nucleus with a relative mass of 1. Neutrons help stabilise the nucleus; their number can vary in isotopes.
Neutron（中子，n⁰） – 原子核中不带电的亚原子粒子，相对质量约为 1。中子帮助稳定原子核，其数目不同会形成同位素。
Electron (e⁻) – nucleus in energy levels (shells). Electrons have almost no mass (relative mass ≈ 1/1840).
Electron（电子，e⁻） – 带负电荷的粒子，在能级（电子层）中绕核高速运动。电子的相对质量极小（约 1/1840）。
Isotope – atoms of the same element (same proton number) but with different numbers of neutrons, hence different mass numbers. Isotopes have identical chemical properties but different physical ones.
Isotope（同位素） – 质子数相同但中子数不同的同种元素原子，因此质量数不同。同位素化学性质几乎相同，物理性质有所差异。
Ion – atoms loses or gains electrons (lose → positive ion, cation; gain → negative ion, anion).
Ion（离子） – 原子或原子团失去或得到电子后形成的带电粒子（失电子→正离子/阳离子；得电子→负离子/阴离子）。
Relative Atomic Mass (Aᵣ) – the weighted mean mass of an atom of an element compared to 1/12th the mass of a carbon‑12 atom.
Relative Atomic Mass（相对原子质量，Aᵣ） – 某元素一个原子的加权平均质量与碳‑12 原子质量的 1/12 之比值。
2. Chemical Bonding & Structures | 化学键与结构
Covalent bond – a shared pair of electrons between two non-metal atoms, held together by the attraction between the nuclei and the shared electrons. Word root: co- (together) + valent (strength).
Covalent bond（共价键） – 两个非金属原子间共用一对电子，依靠原子核对共用电子对的吸引而形成。词根：co- 意为“共同”，valent 意为“力量”。
Ionic bond – the strong electrostatic attraction between oppositely charged ions, typically formed when a metal transfers electrons to a non-metal.
Ionic bond（离子键） – 带相反电荷离子之间的强静电引力，通常在金属向非金属转移电子时形成。
Metallic bonding – the attraction between a lattice of positive metal ions and a sea of delocalised electrons, which explains conductivity and malleability.
Metallic bonding（金属键） – 正金属离子晶格与离域电子海之间的吸引力，解释了金属的导电性与延展性。
Molecule – a discrete group of atoms held together by covalent bonds. Diatomic molecules include H₂, O₂, N₂ and the halogens.
Molecule（分子） – 由共价键结合在一起的独立原子团。双原子分子包括 H₂, O₂, N₂ 和卤素单质。
Lattice – a regular, repeating three-dimensional arrangement of atoms, ions or molecules. Giant ionic lattices (e.g. NaCl) and giant covalent networks (e.g. diamond, SiO₂) are key examples.
Lattice（晶格） – 原子、离子或分子规则重复的三维排列。重要实例有巨型离子晶格（如 NaCl）和巨型共价网络（如金刚石、SiO₂）。
3. Formulae & Reaction Types | 化学式与反应类型
Molecular formula – shows the actual number of each type of atom in a molecule, e.g. C₂H₆.
Molecular formula（分子式） – 表示分子中每种原子的实际数目，如 C₂H₆。
Empirical formula – the simplest whole-number ratio of atoms in a compound. For ethane (C₂H₆) the empirical formula is CH₃.
Empirical formula（最简式/实验式） – 化合物中各原子最简整数比。乙烷 (C₂H₆) 的最简式为 CH₃。
Word equation – tive summary of reactants and products, e.g. sodium + water → sodium hydroxide + hydrogen.
Word equation（文字方程式） – 用物质名称描述反应物和生成物，如：钠 + 水 → 氢氧化钠 + 氢气。
Balanced symbol equation – e quantitative relationship; total mass and atoms are conserved. Example: 2H₂ + O₂ → 2H₂O.
Balanced symbol equation（配平的化学方程式） – 使用化学符号和系数表示数量关系，体现质量与原子守恒。如 2H₂ + O₂ → 2H₂O。
Neutralisation – n an acid and a base (or alkali) to produce a salt and water. Key pattern: H⁺ + OH⁻ → H₂O.
Neutralisation（中和反应） – 酸与碱（或可溶性碱）反应生成盐和水。核心离子式：H⁺ + OH⁻ → H₂O。
Precipitation – formation of an insoluble solid (precipitate) when two solutions are mixed, often shown by a state symbol (s).
Precipitation（沉淀反应） – 两种溶液混合时生成不溶性固体（沉淀），常用状态符号 (s) 表示。
4. The Mole Concept & Calculations | 摩尔概念与计算
Mole (mol) – bstance that contains exactly 6.02 × 10²³ elementary entities (Avogadro’s constant). Think ‘a mole is a chemist’s dozen’.
Mole（摩尔，mol） – 包含恰好 6.02 × 10²³ 个基本单元（阿伏伽德罗常数）的物质的量。可记作“化学家的‘打’”。
Molar mass (M) – the mass of one mole of a substance, numerically equal to the relative formula mass but expressed in g mol⁻¹.
Molar mass（摩尔质量，M） – 1 摩尔物质的质量，数值上等于相对式量，但单位是 g mol⁻¹。
n = m ÷ M
摩尔数 (n) = 质量 (m) ÷ 摩尔质量 (M)
Concentration (c) – olved in 1 dm³ of solution. Formula: c = n ÷ V, where V is in dm³. Common units: mol dm⁻³.
Concentration（浓度，c） – 每立方分米 (1 dm³) 溶液中溶解的溶质的物质的量。公式：c = n ÷ V，V 单位 dm³。常用单位：mol dm⁻³。
Limiting reactant – the reactant that is completely used up first, determining the amount of product formed. The other reactants are in excess.
Limiting reactant（限量反应物） – 最先被完全消耗的反应物，决定了产物的最大量；其余反应物过量。
Percentage composition – the mass percentage of each element in a compound, useful for identifying purity or deducing empirical formulae.
Percentage composition（百分含量） – 化合物中每种元素的质量百分比，常用于判断纯度或推导最简式。
5. Acids, Bases & pH Scale | 酸、碱与 pH 标度
Acid – a substance that donates hydrogen ions (H⁺) in aqueous solution. Common lab acids: HCl, H₂SO₄, HNO₃. pH < 7.
Acid（酸） – 在水溶液中能给出氢离子 (H⁺) 的物质。常见实验室酸：HCl, H₂SO₄, HNO₃。pH 值小于 7。
Base – a substance that accepts H⁺ ions; metal oxides and hydroxides are typical bases.
Base（碱） – 能接受 H⁺ 的物质；金属氧化物和氢氧化物是典型碱。
Alkali – a soluble base that releases hydroxide ions (OH⁻) in water, raising the pH above 7. NaOH and KOH are strong alkalis.
Alkali（碱溶液/可溶性碱） – 溶于水并能释放氢氧根离子 (OH⁻) 的碱，使 pH 大于 7。NaOH 和 KOH 是强碱。
pH scale – a logarithmic measure of the concentration of H⁺ ions; from 0 (strongly acidic) to 14 (strongly alkaline), with 7 being neutral.
pH scale（pH 标度） – 氢离子浓度的对数度量；范围 0（强酸）到 14（强碱），7 为中性。
Salt – an ionic compound formed when the H⁺ of an acid is replaced by a metal ion (or ammonium). E.g., NaCl, KNO₃.
Salt（盐） – 酸中的 H⁺ 被金属离子（或铵根）取代后生成的离子化合物，如 NaCl, KNO₃。
6. Hydrocarbons & Homologous Series | 碳氢化合物与同系列
Hydrocarbon – a compound containing only carbon and hydrogen atoms. Alkanes and alkenes are the two main families in N5.
Hydrocarbon（碳氢化合物） – 只含碳和氢原子的化合物。National 5 两大族：烷烃和烯烃。
Homologous series – a family of compounds with the same general formula, similar chemical properties, and a graduation in physical properties (e.g., boiling points increase with chain length).
Homologous series（同系列） – 具有相同通式、相似化学性质且物理性质随碳链增长呈递变规律的一族化合物。
Alkane – saturated hydrocarbons with single C–C bonds only; general formula CₙH₂ₙ₊₂. Methane (CH₄), ethane (C₂H₆), propane (C₃H₈).
Alkane（烷烃） – 只含 C-C 单键的饱和烃，通式 CₙH₂ₙ₊₂。如甲烷 (CH₄)、乙烷 (C₂H₆)、丙烷 (C₃H₈)。
Alkene – aining at least one C=C double bond; general formula CₙH₂ₙ. Ethene (C₂H₄), propene (C₃H₆).
Alkene（烯烃） – 含至少一个 C=C 双键的不饱和烃，通式 CₙH₂ₙ。如乙烯 (C₂H₄)、丙烯 (C₃H₆)。
Isomer – molecules with the same molecular formula but different structural arrangements (different displayed formulae). For example, butane and methylpropane (C₄H₁₀ isomers).
Isomer（同分异构体） – 分子式相同但原子排列方式不同的分子（结构式不同）。例如丁烷和甲基丙烷是 C₄H₁₀ 的同分异构体。
Addition reaction – a reaction in which an unsaturated molecule (alkene) opens its double bond to add atoms, turning into a saturated compound. Test: bromine water decolorises from orange to colourless.
Addition reaction（加成反应） – 不饱和分子（烯烃）打开双键加上原子，变成饱和化合物的反应。检验：溴水由橙黄色褪为无色。
7. Energy Changes & Reaction Rates | 能量变化与反应速率
Exothermic reaction – a reaction that releases heat energy to the surroundings, causing the temperature to rise. Examples: combustion, neutralisation. ΔH is negative.
Exothermic reaction（放热反应） – 向周围环境释放热量的反应，会使温度升高。实例：燃烧、中和反应。ΔH 为负。
Endothermic reaction – a reaction that absorbs heat energy from the surroundings, leading to a temperature drop. Examples: photosynthesis, thermal decomposition of carbonates. ΔH positive.
Endothermic reaction（吸热反应） – 从周围环境吸收热量的反应，导致温度下降。实例：光合作用、碳酸盐热分解。ΔH 为正。
Activation energy (Eₐ) – the minimum energy colliding particles must have for a reaction to occur. It is the energy barrier that must be overcome.
Activation energy（活化能，Eₐ） – 反应物粒子发生有效碰撞所必须具备的最低能量，相当于必须跨越的能垒。
Catalyst – a substance that speeds up a chemical reaction without being used up or changed permanently. It provides an alternative pathway with lower activation energy.
Catalyst（催化剂） – 能加快化学反应速率而本身不被消耗或发生永久性变化的物质。它通过提供活化能更低的替代途径起作用。
Rate of reaction – the change in concentration of a reactant or product per unit time. Can be increased by: higher temperature, higher concentration, larger surface area, or use of a catalyst.
Rate of reaction（反应速率） – 单位时间内反应物或生成物浓度的变化速率。可通过升高温度、增大浓度、增加表面积或使用催化剂来提高。
Collision theory – for a reaction to happen, particles must collide with the correct orientation and with energy equal to or greater than the activation energy.
Collision theory（碰撞理论） – 反应发生的条件是粒子必须以正确取向碰撞，且碰撞能量达到或超过活化能。
8. Chemical Analysis & Instrumental Methods | 化学分析与仪器方法
Flame test – a qualitative method to identify metal ions by the colour they impart to a Bunsen flame: red (lithium), orange (sodium), lilac (potassium), brick-red (calcium), blue-green (copper).
Flame test（焰色反应） – 通过金属离子在本生灯焰中产生的特征颜色进行定性鉴定的方法：锂（红）、钠（黄-橙）、钾（淡紫）、钙（砖红）、铜（蓝绿）。
Precipitation test – adding a reagent to form a characteristic insoluble salt. E.g., AgNO₃ for halides: white (Cl⁻), cream (Br⁻), yellow (I⁻).
Precipitation test（沉淀检验） – 加入试剂形成特征不溶性盐。例如用 AgNO₃ 检验卤离子：Cl⁻ 白色，Br⁻ 奶油色，I⁻ 黄色。
pH meter – an electronic instrument that gives a precise pH reading; more accurate than universal indicator.
pH meter（pH 计） – 能给出精确 pH 读数的电子仪器，比通用指示剂更准。
Chromatography – a mobile phase. Rf value = distance moved by substance ÷ distance moved by solvent front.
Chromatography（色谱法） – 基于各组分在固定相和流动相之间分配不同而实现分离的技术。比移值 Rf = 物质移动距离 ÷ 溶剂前沿移动距离。
Titration – a quantitative method to determine the concentration of an unknown solution by reacting it with a solution of known concentration, using an indicator to find the end point.
Titration（滴定） – 用已知浓度溶液与待测液反应，借助指示剂确定终点，从而定量测定未知液浓度的分析方法。
9. Electrochemistry & Metals | 电化学与金属
Oxidation – loss of electrons by a substance; oxidation number increases. Mnemonic: OIL – Oxidation Is Loss (of electrons).
Oxidation（氧化） – 物质失去电子的过程，氧化数升高。记忆术：OIL – Oxidation Is Loss。
Reduction – gain of electrons; oxidation number decreases. Mnemonic: RIG – Reduction Is Gain.
Reduction（还原） – 物质得到电子的过程，氧化数降低。记忆术：RIG – Reduction Is Gain。
Redox reaction – a reaction where both reduction and oxidation occur simultaneously. One species is oxidised while another is reduced.
Redox reaction（氧化还原反应） – 还原和氧化同时发生的反应。一种物质被氧化，另一种被还原。
Electrochemical series – a list of metals (and hydrogen/non-metals) arranged by their standard electrode potentials. More reactive metals are higher in the series and lose electrons more readily.
Electrochemical series（电化序/金属活动性顺序） – 根据标准电极电势排列的金属（及氢/非金属）列表。位置越靠上的金属越易失电子、越活泼。
Electrolysis – the use of a direct electric current to drive a non-spontaneous chemical reaction, splitting ionic compounds into their elements.
Electrolysis（电解） – 利用直流电驱动非自发的化学反应，将离子化合物分解为单质。
Alloy – a mixture of a metal with one or more other elements (often other metals) to improve properties, e.g., steel (iron + carbon).
Alloy（合金） – 由一种金属与其他元素（常为其他金属）形成的混合物，用于改善性能，例如钢铁（铁 + 碳）。
10. Memory Tools & Exam Tips | 记忆工具与应试技巧
Acronyms for diatomic elements: BrINClHOF – Bromine, Iodine, Nitrogen, Chlorine, Hydrogen, Oxygen, Fluorine. The ‘magic seven’ that exist as diatomic molecules (Br₂, I₂, N₂, Cl₂, H₂, O₂, F₂).
双原子元素助记口诀： BrINClHOF – 溴、碘、氮、氯、氢、氧、氟。记住这“魔力七种”以双原子分子存在。
OILRIG for redox: Oxidation Is Loss, Reduction Is Gain of electrons. Every time the question mentions electron transfer, recall OILRIG.
氧化还原的 OILRIG： 氧化失电子，还原得电子。每当题目提到电子转移，立刻想到 OILRIG。
Mole map mnemonic: ‘Divide by M, multiply by 24 (or Vₘ)’ – es at room temperature, n = volume (dm³) ÷ 24. For mass, n = m ÷ M. Practise the triangle.
摩尔图记忆： “除以 M，乘以 24（或 Vₘ）”——室温下气体摩尔数 n = 体积 (dm³) ÷ 24。质量则 n = m ÷ M。多练习公式三角。
Value of the mole: er 6.02 × 10²³ by heart. Compare: one mole of water is 18 g, about the size of a mouthful.
摩尔数数值： 熟记阿伏伽德罗常数 6.02 × 10²³。可类比：1 摩尔水约 18 g，正好一小口。
pH colour drills: Universal indicator – red (0-3), orange (4-5), green (7), blue (8-11), violet (12-14). Visualise a rainbow from acid to base.
pH 颜色速记： 通用指示剂 – 红 (0-3)，橙 (4-5)，绿 (7)，蓝 (8-11)，紫 (12-14)。想象一条从酸到碱的彩虹。
Command word check: In SQA papers, ‘name’ requires a single word, ‘describe’ needs details, ‘explain’ requires reasoning. Underline the command words.
指令词核对： SQA 试卷中，“name” 只需一词，“describe” 需要细节，“explain” 要求因果推理。圈出指令词再答题。
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