📚 Subject Specific Vocabulary for AQA A-Level Chemistry | AQA A-Level 化学学科专用词汇
In AQA A-Level Chemistry, precise subject specific vocabulary is essential for interpreting exam questions and writing definitions that meet mark scheme requirements. Many marks depend on using the correct scientific terms in the correct context.
在 AQA A-Level 化学中，准确的学科专用词汇对于理解考题和写出符合评分标准的定义至关重要。许多分数取决于能否在正确语境中使用正确的科学术语。
1. Amount of Substance and Equations | 物质的量与方程式
The relative atomic mass (Aᵣ) of an element is the weighted mean mass of an atom relative to 1/12th the mass of one atom of carbon-12.
元素的相对原子质量 (Aᵣ) 是原子加权平均质量相对于一个碳-12原子质量的1/12的比值。
Relative molecular mass (Mᵣ) is the sum of the relative atomic masses of the atoms in one molecule; for ionic compounds the term relative formula mass is used instead.
相对分子质量 (Mᵣ) 是一个分子中原子的相对原子质量之和；离子化合物则使用相对式量。
t contains exactly 6.022 × 10²³ elementary entities; this number is the Avogadro constant.
摩尔是所含基本单元数恰好为 6.022 × 10²³ 的物质的量；这一数值称为阿伏伽德罗常数。
The empirical formula is the simplest whole-number ratio of atoms of each element in a compound, while the molecular formula gives the actual number of each type of atom.
实验式是化合物中各元素原子的最简整数比，而分子式给出每种原子的实际个数。
Atom economy measures the percentage of reactants that become useful products, while percentage yield compares actual yield to the theoretical yield.
原子经济性衡量反应物转化为有用产物的百分比，而产率则是实际产量与理论产量的比值。
2. Atomic Structure and Ionisation Energy | 原子结构与电离能
First ionisation energy is the energy required to remove one mole of electrons from one mole of gaseous atoms to form one mole of gaseous 1+ ions.
第一电离能是指从一摩尔气态原子中移走一摩尔电子形成一摩尔气态 +1 离子所需的能量。
Second ionisation energy refers to removing one mole of electrons from one mole of gaseous 1+ ions to form one mole of gaseous 2+ ions.
第二电离能是指从一摩尔气态 +1 离子中移走一摩尔电子形成一摩尔气态 +2 离子所需的能量。
Shielding is the repulsion between inner-shell electrons and outer-shell electrons, which reduces the effective nuclear charge experienced by outer electrons.
屏蔽效应是内层电子与外层电子之间的排斥作用，它降低了外层电子所感受到的有效核电荷。
An orbital is a region of space around the nucleus where there is a high probability of finding up to two electrons with opposite spins.
轨道是原子核周围空间中发现最多两个自旋相反电子的概率较高的区域。
Electron configuration shows the distribution of electrons among subshells; AQA uses notation such as 1s² 2s² 2p⁶.
电子构型表示电子在各亚层中的分布；AQA 使用 1s² 2s² 2p⁶ 这类表示法。
Time of flight mass spectrometry provides relative abundance data and can determine relative atomic mass from the m/z values of ions.
飞行时间质谱可提供相对丰度数据，并根据离子的质荷比 (m/z) 确定相对原子质量。
3. Bonding, Structure and Intermolecular Forces | 化学键、结构与分子间力
Ionic bonding is the electrostatic attraction between positive and negative ions formed by electron transfer from a metal to a non-metal.
离子键是金属向非金属转移电子后形成的正、负离子之间的静电引力。
Covalent bonding is the electrostatic attraction between a shared pair of electrons and the positively charged nuclei of two atoms.
共价键是共用电子对与两个原子带正电的核之间的静电引力。
A dative covalent bond, also called a coordinate bond, forms when both electrons in the shared pair come from one atom only.
配位共价键（又称配位键）是指共用电子对完全由一个原子提供而形成的共价键。
Electronegativity is the power of an atom to attract the shared pair of electrons in a covalent bond toward itself.
电负性是原子吸引共价键中共享电子对的能力。
Permanent dipole-dipole forces act between polar molecules; hydrogen bonding is a particularly strong dipole-dipole interaction involving H bonded to N, O or F.
永久偶极-偶极力存在于极性分子之间；氢键是涉及与 N、O 或 F 成键的 H 的特别强的偶极-偶极相互作用。
London dispersion forces, also called instantaneous dipole-induced dipole forces, exist between all molecules and atoms and increase with molecular size.
伦敦色散力又称瞬时偶极-诱导偶极力，存在于所有分子和原子之间，并随分子大小增大而增强。
4. Energetics and Hess's Law | 能量学与盖斯定律
Standard enthalpy of formation (ΔHf⦵) is the enthalpy change when one mole of a compound is formed from its elements under standard states and standard conditions.
标准生成焓 (ΔHf⦵) 是在标准态和标准条件下，由元素生成一摩尔化合物时的焓变。
Standard enthalpy of combustion (ΔHc⦵) is the enthalpy change when one mole of a substance completely burns in oxygen under standard conditions.
标准燃烧焓 (ΔHc⦵) 是在标准条件下，一摩尔物质在氧气中完全燃烧时的焓变。
Hess's law states that the total enthalpy change for a reaction is independent of the route taken, provided the initial and final conditions are the same.
盖斯定律指出，只要
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