📚 Year 12 Edexcel Chemistry: Vocabulary & Terminology Quick Memorisation Guide | Year 12 Edexcel 化学：词汇术语速记指南
For Year 12 Edexcel Chemistry students, a secure grip on subject terminology is the foundation for understanding complex concepts and explaining answers precisely. This bilingual guide walks you through essential vocabulary, topic by topic, pairing clear English definitions with Chinese translations and clever memory hooks.
对于 Year 12 Edexcel 化学的同学来说，牢固掌握学科术语是理解复杂概念、准确作答的基础。这份双语指南按主题梳理核心词汇，每个术语都配有清晰的英文定义、中文翻译和巧妙的记忆钩子，助你高效消化。
1. Atomic Structure and Isotopes | 原子结构与同位素
Atom: The smallest particle of an element that can participate in a chemical reaction. It contains a tiny, dense nucleus surrounded by electrons.
原子: 元素中能参与化学反应的最小粒子。它包含一个微小致密的原子核和绕核运动的电子。
Proton: charged subatomic particle found in the nucleus. Relative mass ≈ 1, relative charge = +1.
质子: 位于原子核内带正电荷的亚原子粒子，相对质量约为1，相对电荷为+1。
Neutron: ative mass ≈ 1, charge = 0. It stabilises the nucleus by reducing proton-proton repulsion.
中子: 原子核内不带电的亚原子粒子，相对质量约为1，电荷为0。它通过减弱质子间的排斥力使原子核稳定。
Atomic Number (Z): The number of protons in the nucleus – it defines the element and determines its position in the periodic table.
原子序数 (Z): 核内质子数 – 决定元素种类和在周期表中的位置。
Mass Number (A): The total number of protons and neutrons in an atom. A = Z + number of neutrons.
质量数 (A): 原子中质子数与中子数之和。A = Z + 中子数。
Isotopes: Atoms of the same element with the same atomic number but different mass numbers (different neutron count). They exhibit identical chemical behaviour but differ in physical properties such as mass.
同位素: 同一元素中质子数相同但中子数不同（即质量数不同）的原子。它们的化学性质几乎完全一样，但物理性质（如质量、密度）有差异。
💡 Quick memory: 'Iso' = same, 'topos' = place → same position on the periodic table. Protons start with 'p' like 'positive'; neutrons are 'neutral'.
💡 速记: 'Iso' 意为相同，'topos' 意为位置 → 周期表中的同一位置。 Proton 和 Positive 都以 'p' 开头，Neutron 和 Neutral 都以 'n' 开头。
2. Electron Configuration and Orbitals | 电子排布与轨道
Principal quantum shell (n): The main energy level of an electron, labelled n = 1, 2, 3… The further from the nucleus, the higher the energy.
主量子壳层 (n): 电子的主要能级，标记为n=1,2,3…离核越远，能量越高。
Sub-shell: A group of orbitals of the same type within a shell, designated s, p, d. s holds up to 2 electrons, p holds up to 6, d holds up to 10.
亚层: 同一壳层内同类型的轨道集合，分为s, p, d。s最多容纳2个电子，p最多6个，d最多10个。
Orbital: A region within an atom where there is a high probability (∼95%) of finding an electron. Each orbital can hold a maximum of two electrons with opposite spins.
轨道: 原子内电子出现概率很高（约95%）的空间区域。每个轨道最多容纳两个自旋相反的电子。
s-orbital: Spherical in shape. Each shell has one s-orbital.
s轨道: 球状。每个壳层只有一个s轨道。
p-orbital: ng x, y, z axes (px, py, pz). Each shell from n=2 onwards has three degenerate p-orbitals.
p轨道: 哑铃形，分别沿x, y, z轴方向（pₓ, pᵧ, pₚ）。从n=2开始，每个壳层有三个简并的p轨道。
Electron configuration: The distribution of electrons among the orbitals of an atom, e.g., 1s² 2s² 2p⁶ 3s² for Mg. Aufbau principle: electrons fill lowest energy orbitals first.
电子排布: 电子在原子轨道上的分布，例如镁：1s² 2s² 2p⁶ 3s²。构造原理（Aufbau principle）：电子优先填充能量最低的轨道。
Hund's rule: Electrons occupy degenerate orbitals singly with parallel spins before pairing up.
洪特规则: 电子填入简并轨道时，会先以自旋平行的方式单独占据各轨道，然后才配对。
💡 Quick memory: 'Smart People Don't Forget' for s, p, d, f. Picture s as Sphere, p as Peanut (dumbbell). Hund's rule: empty seats on a bus – passengers sit alone before sharing.
💡 速记: s,p,d 可记为“Smart People Don't”。s轨道想象成球(Sphere)，p轨道像花生(Peanut)。洪特规则：公交车空位 – 乘客先各占一排，再允许同坐。
3. Types of Chemical Bonding | 化学键类型
Ionic bond: The electrostatic attraction between oppositely charged ions, formed by electron transfer from a metal to a non-metal. Giant ionic lattice with high melting points.
离子键: 带相反电荷离子间的静电吸引力，由金属向非金属转移电子形成。形成巨型离子晶格，熔点高。
Covalent bond: The strong electrostatic attraction between a shared pair of electrons and the nuclei of two atoms. Found in non-metal−non-metal combinations.
共价键: 一对共享电子与两个原子核之间的强静电吸引力，通常存在于非金属原子之间。
Dative covalent (coordinate) bond: A covalent bond in which both electrons in the shared pair come from the same atom. Example: NH₃ donating a lone pair to H⁺ to form NH₄⁺.
配位共价键: 共享电子对中的两个电子均来自同一个原子的共价键。例如NH₃向H⁺提供孤对电子形成NH₄⁺。
Metallic bond: The electrostatic attraction between a lattice of positive metal ions and a 'sea' of delocalised electrons. Explains conductivity and malleability.
金属键: 正金属离子晶格与离域电子“海洋”之间的静电吸引力，解释了金属的导电性和延展性。
Electronegativity: Published by TutorHao | Year 12 Chemistry Revision Series | aleveler.com
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