📚 Year 10 Edexcel Chemistry: Key Terms Memorisation Guide | Year 10 Edexcel 化学：关键术语速记指南
Mastering the vocabulary of chemistry is half the battle in your Edexcel Year 10 course. This guide groups essential terms by topic, provides clear definitions, and includes memory tricks to help you recall them fast in exams.
掌握化学词汇是你在 Edexcel 十年级课程中成功的一半。本指南按专题归类关键术语，提供清晰定义，并附加记忆技巧，帮助你在考试中快速回想。
1. Atomic Structure & the Periodic Table | 原子结构与周期表基础
The atom is the smallest unit of an element that retains its chemical properties. It contains a nucleus (protons and neutrons) surrounded by electrons.
原子是保持元素化学性质的最小单元。它包含原子核（质子和中子），外部围绕电子。
Protons have a relative mass of 1 and a charge of +1. Neutrons have a mass of 1 and no charge. Electrons have a mass of 1/1836 and a charge of -1.
质子相对质量1，电荷+1。中子相对质量1，不带电。电子质量1/1836，电荷-1。
The atomic number (Z) is the number of protons, defining the element. The mass number (A) is the total protons plus neutrons.
原子序数 (Z) 是质子数，决定元素。质量数 (A) 是质子数加中子数。
In a neutral atom, the number of electrons equals the number of protons. Ions form by loss or gain of electrons.
中性原子中，电子数等于质子数。失去或得到电子形成离子。
Isotopes are atoms of the same element with the same number of protons but different numbers of neutrons (different mass numbers).
同位素是同一元素原子，质子数相同但中子数不同（质量数不同）。
Electron shells fill according to the 2,8,8 scheme for the first 20 elements. The electronic configuration of sodium (Na) is 2,8,1.
电子层按2,8,8规则填充前20种元素。钠(Na)的电子排布为2,8,1。
The periodic table is arranged by increasing atomic number. Horizontal rows are periods, vertical columns are groups. Elements in the same group have similar chemical properties because they have the same number of outer-shell electrons.
周期表按原子序数递增排列。横行称为周期，纵列称为族。同族元素化学性质相似，因为最外层电子数相同。
Memory trick: Use 'A.P.E.' – Atomic number = Protons = Electrons (neutral atom). Use 'M.A.N.' – Mass number – up 1 is very reactive alkali metals, Group 7 halogens, Group 0 noble gases are unreactive.
记忆技巧： 'A.P.E.' – 原子序数 = 质子数 = 电子数（中性原子）。'M.A.N.' – 质量数 – 原子序数 = 中子数。族：第1族高活性碱金属，第7族卤素，第0族稀有气体不活泼。
2. Ions and Ionic Bonding | 离子与离子键
An ion is a charged particle formed when an atom gains or loses electrons. Metals lose electrons to form positive cations, while non-metals gain electrons to form negative anions.
离子是原子获得或失去电子时形成的带电粒子。金属失去电子形成正阳离子，非金属获得电子形成负阴离子。
Ionic bonding is the strong electrostatic attraction between oppositely charged ions. It typically occurs between a metal and a non-metal.
离子键是带相反电荷离子之间的强静电引力。通常发生在金属与非金属之间。
Common cation examples: Na⁺, Mg²⁺, Al³⁺. Common anions: Cl⁻, O²⁻, N³⁻.
常见阳离子：Na⁺, Mg²⁺, Al³⁺。常见阴离子：Cl⁻, O²⁻, N³⁻。
Ionic compounds form a giant ionic lattice, a regular repeating arrangement of oppositely charged ions.
离子化合物形成巨型离子晶格，即带相反电荷离子的规则重复排列。
Properties of ionic compounds: high melting and boiling points due to strong ionic bonds; they conduct electricity only when molten or dissolved in water because the ions are free to move.
离子化合物的性质：因离子键强，熔点和沸点高；仅在熔融或溶于水时导电，因为离子可自由移动。
You can deduce the formula of an ionic compound by balancing the charges, e.g. sodium chloride is NaCl (Na⁺ and Cl⁻ in a 1:1 ratio).
可以通过平衡电荷推导离子化合物的化学式，例如氯化钠为 NaCl (Na⁺ 与 Cl⁻ 比例 1:1)。
Memory trick: Think 'Cat-ions are Paws-itive' (cations are positive). 'ANion' starts with 'A N' for 'A Negative Ion'. Formula-writing: swap the charge numbers to become subscripts after cross-multiplying.
记忆技巧： 想象 'Cat-ions 是正电'（cations 正离子）。'ANion' 可记为 'A Negative ion'。化学式书写：将电荷数交叉相乘后成为右下角下标。
3. Covalent Bonding and Simple Molecules | 共价键与简单分子
Covalent bonding occurs between non-metal atoms when they share one or more pairs of electrons to achieve a full outer shell.
共价键发生在非金属原子之间，它们共享一对或多对电子以达到稳定的最外层。
A single covalent bond is one shared pair (e.g. H– bond is two shared pairs (e.g. O=O in O₂), and a triple bond is three shared pairs (e.g. N≡N).
单键共享一对电子（如 H₂ 中的 H–H）。双键共享两对（如 O₂ 中的 O=O），三键共享三对（如 N≡N）。
A molecule is a group of atoms held together by covalent bonds. Common examples: H₂O, CO₂, CH₄, NH₃.
分子是由共价键结合在一起的原子团。常见例子：H₂O, CO₂, CH₄, NH₃。
Simple molecular substances have low melting and boiling points because the intermolecular forces between molecules are weak, even though the covalent bonds inside the molecules are strong.
简单分子物质熔点和沸点较低，因为分子间的分子间力较弱，尽管分子内部的共价键很强。
These substances do not conduct electricity in any state as they have no free ions or delocalised electrons.
这些物质在任何状态下均不导电，因为它们没有自由离子或离域电子。
The molecular formula gives the actual number of atoms of each element in a molecule, while the empirical formula shows the simplest whole-number ratio of atoms.
分子式给出分子中每种原子的实际数目，而实验式显示最简单的整数比。
Memory tip: 'COVALENT = CO llaborative VAlence Electrons Nudged Together'. In simple molecules, separate 'Molecules' with weak forces between them – that's why they are 'simple'.
记忆点： '共价'可理解为协同共享价电子。对于简单分子，分子之间作用力弱——因此它们是“简单”分子。
4. Metallic Bonding | 金属键
Metallic bonding occurs between metal atoms. The metal atoms lose their outer-shell electrons to become positive ions, and these delocalised electrons form a 'sea' of free electrons that holds the ions together.
金属键发生在金属原子之间。金属原子失去最外层电子形成正离子，这些离域电子形成自由电子“海洋”，将离子结合在一起。
This strong electrostatic attraction between the positive metal ions and the sea of delocalised electrons is metallic bonding.
正金属离子与离域电子海之间的强静电引力即为金属键。
Metals are good conductors of electricity and heat because the delocalised electrons can move freely and carry charge or thermal energy.
金属是电和热的良导体，因为离域电子可自由移动并携带电荷或热能。
Metals are malleable and ductile because the layers of ions can slide over each other without breaking the metallic bonds; the electron sea quickly adjusts.
金属具有延展性和可锻造性，因为离子层可以相互滑动而不会破坏金属键；电子海能迅速调整。
Most metals have high melting and boiling points due to the strong metallic bonds, though mercury (Hg) is an exception.
大多数金属因金属键强而具有高熔点和沸点，汞 (Hg) 例外。
An alloy is a mixture of a metal with other elements; its properties differ because the regular layers are disrupted, making it harder.
合金是金属与其他元素的混合物；因其规则的离子层被破坏，性质改变，通常更硬。
Quick recall: Picture a 'sea of electrons' gluing positive metal ions together. 'Metals are seaside' – positive ions in a sea of electrons.
快速记忆： 想象正离子漂浮在电子海里。'金属键 = 离子在电子海中'。
5. Types of Substances – Giant Structures vs Simple Molecules | 物质类型对比 – 巨型结构与简单分子
Ionic compounds form giant ionic lattices. They have high melting points and conduct electricity when molten or in aqueous solution because ions are free to move.
离子化合物形成巨型离子晶格。它们熔点高，在熔融或水溶液中因离子自由移动而导电。
Giant covalent structures (e.g. diamond, graphite, silicon dioxide SiO₂) have many atoms joined by covalent bonds in a continuous lattice. They generally have very high melting points and are hard.
巨型共价结构（如金刚石、石墨、二氧化硅 SiO₂）由共价键在连续晶格中连接许多原子。它们通常熔点极高且硬度大。
In diamond, each carbon atom is covalently bonded to four others, making it extremely hard and an electrical insulator.
金刚石中，每个碳原子与另外四个碳原子以共价键相连，使其极硬且绝缘。
In graphite, each carbon atom bonds to three others, forming layers; one delocalised electron per atom allows graphite to conduct electricity along the layers.
石墨中，每个碳原子与另外三个成键，形成层状结构；每个原子提供一个离域电子，使石墨沿层状方向导电。
Metals have giant metallic structures with delocalised electrons, making them conductors, malleable, and ductile.
金属具有含离域电子的巨型金属结构，使其导电，并具有延展性和可锻造性。
Simple molecular substances, like water and carbon dioxide, consist of small molecules. They have low melting points and do not conduct electricity because there are no free ions or delocalised electrons.
简单分子物质，如水和二氧化碳，由小分子构成。它们熔点低且不导电，因为没有自由离子或离域电子。
explain differences in properties by referring to the type of bonding and structure: e.g. 'Giant structure + strong bonds → high melting point'.
你可以通过键型和结构解释性质差异：例如“巨型结构 + 强键 → 高熔点”。
6. Chemical Equations and State Symbols | 化学方程式与状态符号
ions using the names of reactants and products, e.g. magnesium + oxygen → magnesium oxide.
文字方程式用反应物和产物的名称表示反应，例如 镁 + 氧 → 氧化镁。
Symbol equations use chemical formulae and must be balanced so that atoms are conserved. Never change the formula; only place coefficients in front.
符号方程式使用化学式且必须配平，使原子守恒。切勿改变化学式本身，只能添加化学式前的系数。
State symbols indicate the physical state: (s) solid, (l) liquid, (g) gas, (aq) aqueous (dissolved in water).
状态符号表示物理状态：(s) 固体, (l) 液体, (g) 气体, (aq) 水溶液（溶于水）。
Example balanced equation with state symbols: 2H₂(g) + O₂(g) → 2H₂O(l).
带状态符号的配平方程式示例：2H₂(g) + O₂(g) → 2H₂O(l)。
ange are omitted. For example, the reaction of acid and alkali: H⁺(aq) + OH⁻(aq) → H₂O(l).
离子方程式只显示实际反应的粒子。不参与反应的过程中离子（旁观离子）被省略。例如酸与碱的反应：H⁺(aq) + OH⁻(aq) → H₂O(l)。
ransfer in redox reactions, e.g.: Na → Na⁺ + e⁻ (oxidation); Cl₂ + 2e⁻ → 2Cl⁻ (reduction).
半方程式表示氧化还原反应中的电子转移，例如：Na → Na⁺ + e⁻（氧化）；Cl₂ + 2e⁻ → 2Cl⁻（还原）。
Memory aid: Remember 'SLGA' – Solid, Liquid, Gas, Aqueous. For balancing, use 'MACHO': Metals, Ammonium, Carbonates, Hydroxides, then Others (a counting strategy).
记忆辅助： 记住 'SLGA' – 固体、液体、气体、水溶液。配平时采用 MACHO 方法：先配金属，然后铵根，碳酸根，氢氧根，最后其他原子。
7. Quantitative Chemistry: Moles, Ar, Mr | 定量化学：摩尔、相对原子质量、相对分子质量
The relative atomic mass (Ar) is the average mass of an atom of an element compared to 1/12 the mass of carbon-12. It has no units.
相对原子质量 (Ar) 是元素的平均原子质量与碳-12原子质量的1/12之比，无单位。
The relative formula mass (Mr) applies
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