📚 Year 13 SQA Chemistry: Essential Terminology Memory Guide | SQA 高级化学核心术语速记指南
Mastering the precise language of Advanced Higher Chemistry is half the battle. This guide presents the most frequently examined terms, grouped by topic, with clear definitions in English immediately followed by Chinese explanations to speed up your recall. Use the memory hooks, patterns, and comparative tables to anchor each concept firmly.
掌握 SQA 高级化学的精确语言是成功的一半。本指南按主题分组，列出最高频的考点术语，英文定义后紧跟中文解释，帮助快速记忆。利用记忆钩子、规律和对比表格，将每个概念牢牢锁定在脑海中。
1. Reaction Types and Mechanisms | 反应类型与机理
Nucleophile – an electron‑pair donor that attacks electron‑deficient carbon centres, e.g. OH⁻, CN⁻, NH₃. ‘Nucleus‑loving’ species seek positive charge.
亲核试剂 – 电子对供体，进攻缺电子碳中心，例如 OH⁻、CN⁻、NH₃。可记为“亲核”即亲近原子核（正电中心）。
Electrophile – an electron‑pair acceptor attracted to regions of high electron density, e.g. NO₂⁺, Br₂ (polarised). Electrophiles are Lewis acids.
亲电试剂 – 电子对受体，被高电子密度区域吸引，例如 NO₂⁺、Br₂（极化后）。亲电试剂通常属于路易斯酸。
Free radical – a species with an unpaired electron, formed by homolytic fission. Highly reactive; three steps: initiation, propagation, termination.
自由基 – 带有未成对电子的物种，由均裂产生。反应活性极高；反应三步：引发、增长、终止。
Homolytic vs heterolytic fission – homolytic: each atom takes one electron from the covalent bond, producing radicals. Heterolytic: one atom takes both electrons, forming ions.
均裂与异裂 – 均裂：每个原子从共价键中各取一个电子，生成自由基。异裂：一个原子拿去两个电子，生成离子。
Sₙ1 and Sₙ2 – Sₙ1: two‑step, carbocation intermediate, rate = k[halogenoalkane], racemisation possible. Sₙ2: one‑step concerted, rate = k[halogenoalkane][nucleophile], inversion of configuration.
Sₙ1 与 Sₙ2 – Sₙ1 分两步，碳正离子中间体，速率方程 rate = k[卤代烷]，可能外消旋。Sₙ2 一步协同过程，速率 = k[卤代烷][亲核试剂]，构型翻转。
2. Organic Functional Groups and Nomenclature | 有机官能团与命名
Alkane – saturated hydrocarbon, CₙH₂ₙ₊₂. Suffix ‘‑ane’. Example: propane, CH₃CH₂CH₃.
烷烃 – 饱和烃，通式 CₙH₂ₙ₊₂，词尾“‑烷”。如丙烷 CH₃CH₂CH₃。
Alkene – contains C=C double bond, unsaturated, CₙH₂ₙ. Suffix ‘‑ene’. Geometric isomerism (E/Z) arises from restricted rotation.
烯烃 – 含碳碳双键，不饱和，通式 CₙH₂ₙ，词尾“‑烯”。因旋转受限产生 E/Z 几何异构。
Alcohol – hydroxyl group –OH; suffix ‘‑ol’. Primary, secondary, tertiary based on carbon attached to –OH.
醇 – 羟基 –OH，词尾“‑醇”。根据 –OH 所连碳的类型分为伯、仲、叔醇。
Aldehyde and ketone – both contain C=O. Aldehyde: at end of chain, suffix ‘‑al’. Ketone: C=O in middle, suffix ‘‑one’.
醛与酮 – 均含羰基 C=O。醛基在碳链末端，词尾“‑醛”。酮基在链中，词尾“‑酮”。
Carboxylic acid and ester – acid: –COOH, suffix ‘‑oic acid’. Ester: –COO–, suffix ‘‑oate’. Esters are sweet‑smelling, used as solvents and plasticisers.
羧酸与酯 – 羧酸含 –COOH，词尾“‑酸”。酯含 –COO–，词尾“‑酸酯”。酯有果香味，用作溶剂和增塑剂。
3. Spectroscopy and Analytical Techniques | 光谱与分析方法
Infrared (IR) spectroscopy – detects bond vibrations. Wavenumber range 400–4000 cm⁻¹. Key absorptions: O–H (broad, 3200–3550 cm⁻¹), C=O (sharp, 1680–1750 cm⁻¹), C–O (1000–1300 cm⁻¹).
红外光谱 (IR) – 检测化学键振动。波数范围 400–4000 cm⁻¹。特征吸收：O–H 键宽峰 3200–3550 cm⁻¹，C=O 尖峰 1680–1750 cm⁻¹，C–O 在 1000–1300 cm⁻¹。
Mass spectrometry – molecular ion peak M⁺ gives relative molecular mass. Fragmentation patterns help identify structure. Also used to detect isotopes.
质谱 – 分子离子峰 M⁺ 给出相对分子质量。碎片峰有助于推断结构，也可检测同位素。
NMR (nuclear magnetic resonance) – ¹³C NMR gives number of unique carbon environments. ¹H NMR: chemical shift (δ, ppm), integration (proton count), splitting (n+1 rule).
核磁共振 (NMR) – ¹³C NMR 显示不同化学环境的碳原子数。¹H NMR：化学位移 δ（ppm）、积分（氢原子数）、裂分（n+1 规律）。
Chemical shift (δ) – electron‑withdrawing groups deshield protons, shifting signal to higher ppm. Reference TMS at 0 ppm.
化学位移 (δ) – 吸电子基团去屏蔽质子，使信号移向高 ppm 值。以四甲基硅烷 TMS (0 ppm) 为参考。
Chromatography – separates mixtures. TLC (thin‑layer), GC (gas‑liquid), HPLC (high‑performance liquid). Rf value and retention time used for identification.
色谱法 – 分离混合物。TLC 薄层色谱、GC 气液色谱、HPLC 高效液相色谱。利用Rf值或保留时间进行鉴定。
4. Thermodynamics and Energetics | 热力学与能量学
Enthalpy change (ΔH) – heat change at constant pressure, units kJ mol⁻¹. Exothermic: ΔH < 0; endothermic: ΔH > 0.
焓变 ΔH – 恒压下的热效应，单位 kJ mol⁻¹。放热反应 ΔH < 0，吸热反应 ΔH > 0。
Hess’s Law – total enthalpy change is independent of route. Use enthalpy of formation, combustion, or bond enthalpies to calculate ΔH.
盖斯定律 – 总焓变与路径无关。可利用生成焓、燃烧焓或键能计算反应焓变。
Bond enthalpy – energy required to break 1 mol of bonds in gaseous molecules (average). Bond breaking endothermic, bond making exothermic.
键焓 – 气态分子中断裂 1 mol 化学键所需能量（平均值）。断键吸热，成键放热。
Entropy (S) – measure of disorder, units J K⁻¹ mol⁻¹. Gases have higher S than liquids > solids. ΔSₜₒₜₐₗ = ΔSₛᵧₛ + ΔSₛᵤᵣᵣ > 0 for spontaneous change.
熵 (S) – 混乱度的量度，单位 J K⁻¹ mol⁻¹。气态熵 > 液态 > 固态。总熵变 ΔSₜₒₜₐₗ = ΔSₛᵧₛ + ΔSₛᵤᵣᵣ > 0 时过程自发。
Gibbs free energy – ΔG = ΔH – TΔS. Spontaneous when ΔG < 0. At equilibrium, ΔG = 0. ΔG° relates to equilibrium constant K.
吉布斯自由能 – ΔG = ΔH – TΔS。ΔG < 0 反应自发；平衡时 ΔG = 0。标准 ΔG° 与平衡常数 K 相关：ΔG° = –RT ln K。
5. Chemical Equilibrium | 化学平衡
Dynamic equilibrium – rate of forward = rate of reverse reaction, concentrations constant, closed system. Le Chatelier’s principle predicts shift when conditions change.
动态平衡 – 正逆反应速率相等，各物质浓度恒定，需在封闭体系中。勒夏特列原理可预测条件改变时平衡移动的方向。
Equilibrium constant Kc – Kc = [products]ᵖ / [reactants]ʳ, each raised to stoichiometric coefficients. Only temperature changes Kc.
平衡常数 Kc – Kc = [产物]ᵖ/[反应物]ʳ，幂次为计量系数。仅温度可改变 Kc 值。
Kp and partial pressure – for gas reactions, Kp uses partial pressures. Mole fraction × total pressure = partial pressure.
Kp 与分压 – 气相反应使用 Kp，以分压代替浓度。分压 = 摩尔分数 × 总压。
Acid dissociation constant Ka – Ka = [H⁺][A⁻]/[HA]. pKa = –log₁₀ Ka. Smaller pKa means stronger acid.
酸解离常数 Ka – Ka = [H⁺][A⁻]/[HA]，pKa = –log₁₀ Ka。pKa 越小，酸性越强。
Buffer solutions – resist pH change. Made from weak acid + its conjugate base, or weak base + its conjugate acid. Henderson–Hasselbalch: pH = pKa + log([A⁻]/[HA]).
缓冲溶液 – 能抵抗 pH 变化。通常由弱酸与其共轭碱（或弱碱与其共轭酸）组成。亨德森‑哈塞尔巴尔赫方程：pH = pKa + log([A⁻]/[HA])。
6. Kinetics | 化学动力学
Rate of reaction – change in concentration per unit time (mol dm⁻³ s⁻¹). Measured by following volume of gas, mass loss, colour change, or pH.
反应速率 – 单位时间内浓度的变化，单位 mol dm⁻³ s⁻¹。可通过气体体积、质量减少、颜色变化或 pH 来跟踪。
Rate equation – rate = k[A]ᵐ[B]ⁿ. m, n are orders of reaction determined experimentally, not from stoichiometry. Overall order = m + n.
速率方程 – rate = k[A]ᵐ[B]ⁿ。m、n 为反应级数，须由实验测定而非从化学计量式得到。总级数 = m + n。
Rate constant k – temperature‑dependent, units vary with overall order. Larger k → faster reaction. Arrhenius: k = Ae^(–Eₐ/RT).
速率常数 k – 随温度变化，单位取决于总级数。k 越大反应越快。阿伦尼乌斯公式：k = Ae^(–Eₐ/RT)。
Activation energy Eₐ – minimum energy needed for a collision to lead to reaction. Catalysts lower Eₐ.
活化能 Eₐ – 有效碰撞所需的最低能量。催化剂通过提供替代路径降低活化能。
Reaction mechanisms and rate‑determining step – the slowest step dictates the rate law. Species in the rate equation must appear in or before the RDS.
反应机理与速控步 – 最慢的一步决定速率方程。速率方程中出现的物种必须出现在速控步或其之前的步骤中。
7. Redox and Electrochemistry | 氧化还原与电化学
Oxidation and reduction – OIL RIG: Oxidation Is Loss (of electrons), Reduction Is Gain. Oxidation number rules determine electron transfer.
氧化与还原 – 记忆口诀 OIL RIG：氧化失电子，还原得电子。利用氧化数规则判断电子转移。
Oxidising and reducing agents – oxidising agent gains electrons, itself reduced. Reducing agent loses electrons, itself oxidised. E.g., dichromate(VI) is an oxidising agent.
氧化剂与还原剂 – 氧化剂得电子，自身被还原。还原剂失电子，自身被氧化。例如重铬酸根(VI)为氧化剂。
Standard electrode potential E° – measured under standard conditions (298 K, 1 mol dm⁻³, 100 kPa) against standard hydrogen electrode (0.00 V). More positive E° means stronger oxidising agent.
标准电极电势 E° – 在标准条件（298 K, 1 mol dm⁻³, 100 kPa）下以标准氢电极(0.00 V)为参考测定。E° 越正，氧化性越强。
Cell potential E°cₑₗₗ – E°cₑₗₗ = E°(cathode) – E°(anode) where reduction occurs at cathode. Positive E°cₑₗₗ → feasible reaction. ΔG° = –nFE°.
电池电动势 E°cₑₗₗ – E°cₑₗₗ = E°(正极) – E°(负极)，正极发生还原。E°cₑₗₗ > 0 反应可行。ΔG° = –nFE°。
Electrolysis – non‑spontaneous redox driven by external e.m.f. Cations migrate to cathode, anions to anode. Quantitative electrolysis: Q = It, and Faraday’s laws.
电解 – 由外加电源驱动的非自发氧化还原。阳离子移向阴极，阴离子移向阳极。定量电解：电荷 Q = It，应用法拉第定律计算质量。
8. Atomic Structure and Periodicity | 原子结构与周期性
Atomic orbitals – s (spherical), p (dumbbell, 3 orientations), d (5 orientations). Electrons fill according to Aufbau principle, Hund’s rule, Pauli exclusion principle.
原子轨道 – s 轨道球形，p 轨道哑铃形（三个方向），d 轨道五种取向。电子按构造原理、洪特规则和泡利不相容原理填充。
Ionisation energy – energy to remove 1 mol of electrons from gaseous atoms. Trend across period increases (greater nuclear charge), down group decreases (increased shielding and distance).
电离能 – 气态原子移除 1 mol 电子所需能量。同周期从左到右增大（核电荷增加），同族从上到下减小（屏蔽和距离增加）。
Electronegativity – ability of an atom to attract bonding electrons. Pauling scale; increases across period, decreases down group. Polar bonds result from ΔEN.
电负性 – 原子吸引键合电子的能力（鲍林标度）。同周期递增，同族递减。电负性差产生极性键。
Intermolecular forces – London dispersion (all molecules), permanent dipole–dipole, hydrogen bonding (H with N, O, or F). Hydrogen bonding strongly affects boiling point and solubility.
分子间作用力 – 伦敦色散力（所有分子）、永久偶极‑偶极作用、氢键（与 N、O、F 成键的 H）。氢键显著影响沸点和溶解度。
9. Transition Metals and Complexes | 过渡金属与配合物
Transition metal – d‑block element forming one or more stable ions with partially filled d‑orbitals. Characteristic properties: variable oxidation states, coloured compounds, catalytic activity, complex formation.
过渡金属 – 能形成一种或多种具有部分填充 d 轨道稳定离子的 d 区元素。特征：变价、有色化合物、催化活性、形成配合物。
Complex and ligand – a complex has a central metal ion surrounded by ligands. Ligand is an electron‑pair donor (Lewis base) that forms coordinate bond. Monodentate (one donor atom): H₂O, NH₃, Cl⁻. Bidentate: 1,2‑diaminoethane (en), ethanedioate ion.
配合物与配体 – 配合物由中心金属离子与周围配体组成。配体为电子对供体（路易斯碱），形成配位键。单齿配体：H₂O、NH₃、Cl⁻；双齿配体：1,2‑二氨基乙烷 (en)、乙二酸根。
Coordination number and shape – number of coordinate bonds from ligands. CN = 6 → octahedral; CN = 4 → tetrahedral or square planar (e.g. cisplatin).
配位数与空间构型 – 配体提供的配位键数目。配位数 6 → 八面体；配位数 4 → 四面体或平面正方形（如顺铂）。
Crystal field splitting and colour – ligands split d‑orbitals into two energy levels. The energy gap ΔE corresponds to visible light; absorbed wavelength gives complementary colour. Strength of ligand affects ΔE (spectrochemical series).
晶体场分裂与颜色 – 配体使 d 轨道分裂为两组能级。能级差 ΔE 对应可见光波长，吸收光的补色就是观测到的颜色。配体强弱影响 ΔE（光谱化学序列）。
Transition metal catalysis – heterogeneous (surface adsorption) and homogeneous (intermediate formation). Examples: Fe in Haber, V₂O₅ in Contact, Pd in hydrogenation.
过渡金属催化 – 多相催化（表面吸附）和均相催化（中间产物形成）。典型例子：哈伯法用 Fe，接触法用 V₂O₅，加氢用 Pd。
10. Organic Synthesis and Reaction Routes | 有机合成路线
Functional group interconversion – alkanes → haloalkanes (free radical substitution); haloalkanes → alcohols (Sₙ1/Sₙ2 with aqueous NaOH); primary alcohols → aldehydes → carboxylic acids (oxidation); carboxylic acid + alcohol ⇌ ester (esterification, H⁺ catalyst). Learn the ladder!
官能团互变 – 烷烃 → 卤代烷（自由基取代）；卤代烷 → 醇（Sₙ1/Sₙ2，NaOH 水溶液）；伯醇 → 醛 → 羧酸（氧化）；羧酸 + 醇 ⇌ 酯（酯化，酸催化）。掌握转化阶梯是关键。
Condensation polymers – polyesters (diol + dicarboxylic acid) and polyamides (diamine + dicarboxylic acid). Release small molecule like H₂O. Hydrolysed back to monomers.
缩合聚合物 – 聚酯（二醇 + 二酸）和聚酰胺（二胺 + 二酸），缩合时放出小分子（如 H₂O）并可水解回单体。
Important reagents – HCN for hydroxynitriles (nucleophilic addition); LiAlH₄ for deep reduction; PCl₅, SOCl₂ for converting –OH to –Cl; 2,4‑DNP for detecting C=O; Tollens’ for aldehydes.
重要试剂 – HCN 制备羟基腈（亲核加成）；LiAlH₄ 深度还原；PCl₅、SOCl₂ 将 –OH 转为 –Cl；2,4‑二硝基苯肼检测羰基；托伦斯试剂鉴别醛基。
Reaction conditions matter – temperature, solvent, catalyst. E.g., halogenoalkane with NaOH (aq) → alcohol, but with NaOH (alc) → alkene (elimination).
反应条件至关重要 – 温度、溶剂、催化剂不同，产物迥异。如卤代烷与 NaOH 水溶液得醇，与 NaOH 醇溶液则发生消除生成烯。
Synthetic routes and yield – plan retrosynthetically; aim for high atom economy and minimal steps. Percentage yield = (actual/theoretical) × 100.
合成路线与产率 – 采用逆合成分析，追求高原子经济性和最少步骤。产率 = (实际产量/理论产量) × 100。
11. Properties of Materials | 材料性质
Polymers: thermoplastics vs thermosets – thermoplastics soften on heating, can be remoulded (weak intermolecular forces between chains). Thermosets do not soften, decompose instead (extensive cross‑links).
热塑性塑料与热固性塑料 – 热塑性加热软化可重塑（链间弱分子间力）；热固性加热不软化而分解（高度交联）。
Metallic bonding and alloys – delocalised electrons hold metal cations in lattice. Explains conductivity, malleability. Alloys disrupt regular lattice, making them harder.
金属键与合金 – 离域电子将金属阳离子固定在晶格中，解释导电性和延展性。合金引入异种原子打乱规则排列，使硬度增大。
Ionic and covalent lattices – ionic: high m.p., brittle, conduct when molten/aqueous. Covalent network: e.g. diamond (hard, insulator), graphite (conducts along layers, lubricant).
离子与共价晶格 – 离子晶体：高熔点，脆，熔融或水溶液导电。共价网络：金刚石（坚硬、绝缘），石墨（层间导电、润滑剂）。
Conductors, insulators, semiconductors – band theory: metals have overlapping conduction and valence bands; insulators have large gap; semiconductors have small gap, doping creates n‑type/p‑type.
导体、绝缘体与半导体 – 能带理论：金属的导带与价带重叠；绝缘体带隙大；半导体带隙小，掺杂可形成 n 型或 p 型半导体。
12. Laboratory Techniques and Measurements | 实验技术与测量
Volumetric analysis – titration: accurate measurement of solution volume using burette (0.05 cm³ uncertainty), pipette (0.04 cm³), and volumetric flask (0.08/0.2 cm³). Concordant titres ± 0.1 cm³.
容量分析 – 滴定：用滴定管（±0.05 cm³）、移液管（±0.04 cm³）、容量瓶（±0.08/0.2 cm³）准确量取溶液。平行滴定结果误差 ±0.1 cm³ 以内。
Colorimetry – measures absorbance proportional to concentration (Beer–Lambert). Choose complementary filter for maximum sensitivity.
比色法 – 吸光度与浓度成正比（比尔‑朗伯定律）。选择互补滤光片以获得最大灵敏度。
Melting point determination – pure substance has sharp m.p. range (≤ 0.5 °C) while impurities broaden and depress the range.
熔点测定 – 纯物质熔点范围尖锐（≤0.5 °C），杂质使范围变宽且下降。
Separation techniques – distillation (simple vs fractional for close‑boiling liquids), recrystallisation (dissolve in minimum hot solvent, cool, filter crystals).
分离技术 – 蒸馏（简单蒸馏与分馏用于沸点接近的液体），重结晶（以最少热溶剂溶解，冷却，过滤晶体）。
Uncertainty and error – random error reduced by replicates; systematic error affects accuracy. % uncertainty = (apparatus uncertainty / measured value) × 100.
误差与不确定度 – 随机误差通过重复实验减少；系统误差影响准确度。百分不确定度 = (仪器误差 / 测量值) × 100。
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