📚 Essential Chemistry Vocabulary Quick Memory Guide for Year 12 CIE | Year 12 CIE 化学：词汇术语速记指南
Mastering the precise terminology in CIE AS Level Chemistry is crucial for interpreting questions and expressing answers accurately. This quick memory guide presents key terms organised by topic, with concise definitions in English and Chinese, along with memory hooks to speed up learning.
掌握 CIE AS 化学的精确术语对于理解题目和准确答题至关重要。本速记指南按主题组织，提供简洁的中英文定义以及记忆技巧，帮助加速学习。
1. Stoichiometry and Quantification | 化学计量与定量
Mole: r : The mole is the SI unit for amount of substance. One mole contains exactly 6.02 × 10²³ elementary entities (Avogadro's constant). Think of a mole as a 'chemical dozen' for counting atoms, molecules or ions.
摩尔： 摩尔是国际单位制中物质的量的单位。1 摩尔恰好含有 6.02 × 10²³ 个基本单元（阿伏伽德罗常数）。可以把摩尔想象成化学中的“打”，用来数原子、分子或离子。
Avogadro constant (Nₐ): copic particle scale to macroscopic laboratory quantities. Remember the number 6.02 and the spelling 'Avogadro' – it is named after the Italian scientist Amedeo Avogadro.
阿伏伽德罗常数 (Nₐ)： 6.02 × 10²³ mol⁻¹，它把微观粒子数目与宏观实验量联系起来。记住数字 6.02 和拼写“Avogadro”——以意大利科学家阿梅代奥·阿伏伽德罗命名。
Molar mass (M): The mass of one mole of a substance, expressed in g mol⁻¹. Numerically equal to the relative atomic mass (Aᵣ) or relative molecular mass (Mᵣ) but carrying the unit g mol⁻¹.
摩尔质量 (M)： 单位物质的量的物质所具有的质量，单位为 g mol⁻¹。数值上等于相对原子质量 (Aᵣ) 或相对分子质量 (Mᵣ)，但带单位 g mol⁻¹。
Molar volume (Vₘ): At room temperature and pressure (r.t.p., 25 °C, 101 kPa), one mole of any gas occupies 24 dm³. At standard temperature and pressure (s.t.p., 0 °C, 101 kPa), it is 22.4 dm³. A useful memory aid: 'room 24, standard 22.4'.
摩尔体积 (Vₘ)： 在常温常压 (r.t.p., 25 °C, 101 kPa) 下，1 摩尔任何气体占据 24 dm³；在标准状况 (s.t.p., 0 °C, 101 kPa) 下为 22.4 dm³。可借助“室温 24，标准 22.4”来记忆。
Empirical formula: The simplest whole‑number ratio of atoms of each element in a compound. Determined from experimental composition data.
实验式（最简式）： 表示化合物中各元素原子的最简整数比，可由实验组成数据确定。
Molecular formula: The actual number of atoms of each element in a molecule. It is a whole‑number multiple of the empirical formula.
分子式： 一个分子中各元素原子的实际数目，是实验式的整数倍。
Concentration: ssolved in a given volume of solution, commonly expressed in mol dm⁻³. Formula: c = n / V.
浓度： 单位体积溶液中溶质的物质的量，常用mol dm⁻³ 表示。公式：c = n/V。
2. Atomic Structure Foundations | 原子结构基础
Proton (atomic) number (Z): The number of protons in the nucleus of an atom. It defines the element and its position in the Periodic Table.
质子数（原子序数）(Z)： 原子核中质子的数目，决定元素的种类及其在周期表中的位置。
Mass (nucleon) number (A): The total number of protons and neutrons in the nucleus. Number of neutrons = A − Z.
质量数（核子数）(A)： 原子核内质子数与中子数之和。中子数 = A − Z。
Isotopes: Atoms of the same element with the same proton number but different mass numbers (different number of neutrons). They have identical chemical properties but slightly different physical properties.
同位素： 质子数相同而质量数不同（中子数不同）的同一元素的不同原子。化学性质相同，物理性质略有差异。
Orbital: A region within an atom that can hold up to two electrons with opposite spins. s‑orbitals are spherical; p‑orbitals are dumbbell‑shaped (three orientations). Remember 's‑spherical, p‑peanut' – though more accurately a peanut with two lobes.
原子轨道： 原子中一个最多容纳两个自旋相反电子的空间区域。s 轨道呈球形；p 轨道呈哑铃形（三个取向）。可记作“s 像球，p 像花生”。
Electron configuration: The arrangement of electrons in an atom. Written using principal quantum numbers (1, 2, 3,…) and orbital labels, e.g. 1s² 2s² 2p⁶. For ions, adjust electrons accordingly.
电子构型： 原子中电子的排布方式。用主量子数和轨道符号书写，如 1s² 2s² 2p⁶。离子则据此增减电子。
First ionisation energy: ole of gaseous atoms to form one mole of gaseous ions with a 1+ charge: X(g) → X⁺(g) + e⁻.
第一电离能： 从 1 摩尔气态原子中最外层移走 1 摩尔电子，生成 1 摩尔气态 1+ 离子所需的最低能量：X(g) → X⁺(g) + e⁻。
Shielding and effective nuclear charge: Inner electrons shield outer electrons from the full attraction of the nucleus. Effective nuclear charge increases across a period, pulling electrons closer and raising ionisation energy.
屏蔽效应与有效核电荷： 内层电子部分地抵消了核对外层电子的引力。同一周期，有效核电荷增大，电子被拉得更近，电离能升高。
3. Bonding, Structure, and Intermolecular Forces | 化学键、结构与分子间作用力
Ionic bond: The electrostatic attraction between oppositely charged ions formed by the transfer of electrons. Typically occurs between a metal and a non‑metal. Giant ionic lattices are strong, brittle and conduct electricity when molten or aqueous.
离子键： 阴阳离子之间的静电引力，通过电子转移形成。常见于金属与非金属之间。离子晶体是巨型结构，硬而脆，熔融或水溶液时可导电。
Covalent bond: The electrostatic attraction between a shared pair of electrons and the nuclei of the two bonding atoms. Single, double and triple covalent bonds involve 2, 4 and 6 shared electrons respectively.
共价键： 一对共用电子与两个成键原子核之间的静电引力。单键、双键和三键分别共享 2、4、6 个电子。
Dative covalent (coordinate) bond: A covalent bond in which both electrons in the shared pair come from the same atom. The donor atom must have a lone pair and the acceptor must be electron‑deficient.
配位键（配价键）： 共用电子对全部由同一原子提供的共价键。供体必须有孤对电子，受体需缺电子。
Electronegativity: The ability of an atom to attract the bonding electrons in a covalent bond. Pauling scale values increase across a period and up a group (fluorine is the most electronegative element). Difference in electronegativity determines bond polarity.
电负性： 原子在共价键中吸引电子的能力。鲍林标度值在周期表中越向右上角越高（氟的电负性最大）。电负性差决定键的极性。
VSEPR theory: Valence Shell Electron Pair Repulsion theory – electron pairs around a central atom repel one another and adopt positions that minimise repulsion. This gives the molecule its shape and bond angles (e.g. 180° for linear CO₂, 109.5° for tetrahedral CH₄, 104.5° for bent H₂O).
价层电子对互斥理论： 中心原子周围的电子对相互排斥，采取使排斥力最小的空间取向，从而决定分子的形状和键角（如 CO₂ 直线形 180°，CH₄ 四面体 109.5°，H₂O 角形 104.5°）。
Intermolecular forces: Forces between molecules (much weaker than covalent or ionic bonds). Key types: London (dispersion) forces (all molecules), permanent dipole‑dipole forces (polar molecules), and hydrogen bonding (strong dipole‑dipole when H is bonded to N, O or F). Remember 'FON' for hydrogen bonding.
分子间作用力： 分子之间的引力（远弱于共价键或离子键）。主要类型：伦敦（色散）力（所有分子）、永久偶极‑偶极力（极性分子）和氢键（H 与 N、O、F 键合时产生的强偶极力）。可记“FON”来记住氢键。
4. Energetics and Thermochemistry | 热化学
Enthalpy change (ΔH): tions release heat (ΔH negative); endothermic reactions absorb heat (ΔH positive). Memory: 'exo = exit heat, endo = enter heat'.
焓变 (ΔH)： 恒压条件下吸收或放出的热量。放热反应 ΔH 为负值；吸热反应 ΔH 为正值。可记为“exo 出热，endo 入热”。
Standard enthalpy change of formation (ΔHf°): The enthalpy change when one mole of a compound is formed from its elements in their standard states under standard conditions (298 K, 101 kPa).
标准生成焓 (ΔHf°)： 标准状态下由最稳定单质生成 1 摩尔化合物的焓变。
Standard enthalpy change of combustion (ΔHc°): The enthalpy change when one mole of a substance is completely burned in excess oxygen under standard conditions.
标准燃烧焓 (ΔHc°)： 标准状态下 1 摩尔物质在过量氧气中完全燃烧的焓变。
Hess's law: The enthalpy change for a reaction is independent of the route taken, depending only on the initial and final states. Use it to calculate unknown ΔH values by combining known enthalpy cycles.
赫斯定律： 反应焓变只取决于始态和终态，与途径无关。可利用已知焓变构建能量循环来计算未知的 ΔH。
Bond enthalpy (mean bond enthalpy): The energy required to break one mole of a specific covalent bond averaged over a range of compounds, in the gaseous state. Bond breaking is endothermic; bond forming is exothermic.
键焓（平均键焓）： 在气态下断裂 1 摩尔某指定共价键所需的平均能量。断键吸热，成键放热。
Calorimetry: e solution, c is the specific heat capacity (usually 4.18 J g⁻¹ K⁻¹ for water and dilute aqueous solutions), and ΔT is the temperature change. Then ΔH is calculated per mole.
量热法： 用量热器测量热量变化的实验方法，常用 q = mcΔT，其中 m 为溶液质量，c 为比热容（水和稀溶液通常取 4.18 J g⁻¹ K⁻¹），ΔT 为温度变化，再换算成每摩尔的 ΔH。
5. Kinetics and Reaction Rates | 动力学与反应速率
Rate of reaction: The change in concentration of a reactant or product per unit time. Typically measured in mol dm⁻³ s⁻¹. It can be determined from the gradient of a concentration‑time graph.
反应速率： 单位时间内反应物或产物浓度的变化量，通常以 mol dm⁻³ s⁻¹ 表示。可从浓度‑时间曲线的斜率求得。
Collision theory: activation energy) and in the correct orientation. Increasing concentration, pressure (for gases), temperature or surface area increases the frequency of effective collisions.
碰撞理论： 发生反应需粒子碰撞，且碰撞能量不低于活化能，方向适当。增大浓度、压强（气体）、温度或表面积可增加有效碰撞频率。
Activation energy (Eₐ): The minimum energy that colliding particles must possess for a reaction to occur. Catalysts provide an alternative pathway with a lower activation energy, increasing the proportion of successful collisions without being consumed.
活化能 (Eₐ)： 碰撞粒子发生反应所必须达到的最低能量。催化剂通过提供较低活化能的路径，提高有效碰撞比例，自身不被消耗。
Boltzmann distribution: A graph showing the distribution of kinetic energies among molecules at a given temperature. The area under the curve beyond Eₐ represents the fraction of molecules with enough energy to react; this area increases sharply with temperature.
玻尔兹曼分布： 表示某一温度下分子动能分布情况的曲线。曲线下超出 Eₐ 的面积代表具有足够反应能量的分子分数；升温使该面积显著增大。
6. Chemical Equilibria | 化学平衡
Dynamic equilibrium: A state in a closed system where the rates of the forward and reverse reactions are equal, so the macroscopic properties (concentrations, colour, pressure) remain constant. Both reactions continue at the molecular level.
动态平衡： 在封闭体系中，正向与逆向反应速率相等的状态，宏观性质（浓度、颜色、压强）保持恒定，但微观上正逆反应仍在进行。
Le Chatelier's principle: If a system at dynamic equilibrium is subjected to a change in concentration, pressure or temperature, the position of equilibrium shifts to oppose that change. Adding a catalyst does not affect the equilibrium position; it simply speeds up the attainment of equilibrium.
勒夏特列原理： 当处于动态平衡的体系受到浓度、压强或温度改变时，平衡位置将向削弱此改变的方向移动。加入催化剂不影响平衡位置，只加快到达平衡。
Equilibrium constant, Kc: For a homogeneous reversible reaction aA + bB ⇌ cC + dD, Kc is defined in terms of molar concentrations at equilibrium:
Kc = [C]
Published by TutorHao | Year 12 Chemistry Revision Series | aleveler.com 更多咨询请联系16621398022（同微信）
或截图后用「扫一扫 → 相册」选择本图