📚 Year 10 AQA Chemistry: Core Knowledge Organiser | Year 10 AQA 化学：核心知识点梳理
Welcome to your core knowledge organiser for Year 10 AQA Chemistry. This article pulls together the most vital concepts you will encounter across the first year of the GCSE course — from atomic structure and bonding to quantitative chemistry, acids, electrolysis and energy changes. Each section is written in clear, syllabus‑specific language to support your revision, homework and end‑of‑topic tests.
欢迎阅读 Year 10 AQA 化学核心知识点梳理。本文汇集了 GCSE 课程第一年最重要的概念——从原子结构和化学键，到定量化学、酸、电解和能量变化。每一节都用清晰且紧扣考纲的语言写成，帮助你复习、完成作业以及准备单元测验。
1. Atomic Structure | 原子结构
All substances are made of atoms. An atom contains a tiny, dense nucleus composed of protons and neutrons, surrounded by electrons arranged in shells. The nucleus holds virtually all the mass of the atom, while the electrons occupy most of the volume.
所有物质都由原子构成。原子含有一个非常小且致密的原子核，核由质子和中子组成，核外电子分层排布。原子几乎全部质量集中在核上，而电子占据了原子绝大部分体积。
- Proton: relative mass 1, relative charge +1.
- 质子：相对质量 1，相对电荷 +1。
- Neutron: relative mass 1, relative charge 0.
- 中子：相对质量 1，相对电荷 0。
- Electron: relative mass 1/1840 (negligible), relative charge –1.
- 电子：相对质量 1/1840（可忽略），相对电荷 –1。
The atomic number (Z) is the number of protons and determines the element. The mass number (A) is the total number of protons plus neutrons. Atoms are electrically neutral because the number of protons equals the number of electrons. Isotopes are atoms of the same element with different numbers of neutrons (same Z, different A).
原子序数（Z）等于质子数，决定了元素种类。质量数（A）等于质子数与中子数之和。原子呈电中性，因为质子数等于电子数。同位素是同种元素的不同原子，它们的中子数不同（Z 相同，A 不同）。
Electrons occupy the lowest available energy levels (shells). The first shell holds up to 2 electrons, the second up to 8, and the third up to 8 (in the first 20 elements). Electronic configurations follow the pattern 2.8.8 for elements up to calcium.
电子优先填入能量最低的电子层（电子壳层）。第一层最多容纳 2 个电子，第二层最多 8 个，第三层在最初 20 号元素中最多 8 个。电子排布遵循 2.8.8 的规律（适用于钙及之前的元素）。
2. The Periodic Table | 元素周期表
Elements are arranged in the modern periodic table by increasing atomic number. Vertical columns are called groups; horizontal rows are called periods. Elements in the same group have the same number of electrons in their outer shell, giving them similar chemical properties.
现代周期表按原子序数递增排列元素。纵列称为族，横排称为周期。同族元素最外层电子数相同，因此具有相似的化学性质。
- Group 1 – alkali metals: one electron in outer shell, very reactive, reactivity increases down the group. They form 1⁺ ions.
- 第 1 族——碱金属：最外层一个电子，非常活泼，活泼性自上而下增强。它们形成 1⁺ 离子。
- Group 7 – halogens: seven electrons in outer shell, reactive non‑metals, reactivity decreases down the group. They form 1⁻ ions and exist as diatomic molecules (F₂, Cl₂, Br₂, I₂).
- 第 7 族——卤素：最外层七个电子，活泼的非金属，活泼性自上而下减弱。它们形成 1⁻ 离子，以双原子分子存在（F₂, Cl₂, Br₂, I₂）。
- Group 0 – noble gases: full outer shells (8 electrons, except helium with 2), making them extremely unreactive. They exist as single atoms and have low boiling points that increase down the group.
- 第 0 族——稀有气体：最外层全满（8 电子，氦为 2），因此极不活泼。它们以单原子形式存在，沸点很低且自上而下升高。
Between Group 2 and Group 3 lies the block of transition metals. They form ions with different charges, are often good catalysts, and form coloured compounds.
在第 2 族与第 3 族之间是过渡金属区。过渡金属可形成不同电荷的离子，常用作催化剂，并能形成有色化合物。
3. Ionic Bonding | 离子键
Ionic bonding occurs when a metal atom transfers electrons to a non‑metal atom. The metal loses electrons to become a positively charged cation; the non‑metal gains electrons to become a negatively charged anion. The oppositely charged ions are held together by strong electrostatic forces called ionic bonds.
离子键形成于金属原子向非金属原子转移电子的过程中。金属失去电子成为带正电的阳离子，非金属得到电子成为带负电的阴离子。带相反电荷的离子通过强大的静电引力（即离子键）结合在一起。
For example, sodium (Na) loses one electron to become Na⁺, and chlorine (Cl) gains one electron to become Cl⁻, forming sodium chloride (NaCl). Magnesium oxide (MgO) is formed when magnesium loses two electrons (Mg²⁺) and oxygen gains two electrons (O²⁻).
例如，钠（Na）失去一个电子形成 Na⁺，氯（Cl）得到一个电子形成 Cl⁻，结合为氯化钠（NaCl）。镁失去两个电子形成 Mg²⁺，氧得到两个电子形成 O²⁻，生成氧化镁（MgO）。
Ionic compounds have a giant lattice structure: a regular, repeating arrangement of ions. This structure explains their high melting and boiling points and their ability to conduct electricity when molten or dissolved in water (because the ions are free to move).
离子化合物具有巨型离子晶格结构：离子按规则重复排列。这种结构解释了它们的高熔点、高沸点，以及在熔融或溶于水时能够导电（因为离子可以自由移动）。
4. Covalent and Metallic Bonding | 共价键与金属键
Covalent bonding forms between non‑metal atoms when they share pairs of electrons to achieve a full outer shell. The shared pair is attracted to the nuclei of both atoms, which holds the atoms together strongly. A single covalent bond involves one shared pair; double bonds involve two shared pairs (e.g. O₂, CO₂).
共价键形成于非金属原子之间，它们通过共用电子对达到满外层结构。共用电子对同时受到两个原子核的吸引，从而将原子牢固结合。单键共用一对电子，双键共用两对电子（如 O₂、CO₂）。
Small covalent molecules have strong covalent bonds within the molecule but weak intermolecular forces between molecules. This gives them low melting and boiling points. Examples include H₂O, NH₃, CH₄.
简单共价分子内部有很强的共价键，但分子之间只有微弱的分子间作用力。因此它们的熔点和沸点较低，例如 H₂O、NH₃、CH₄。
Giant covalent structures, such as diamond, graphite and silicon dioxide (SiO₂), consist of a huge network of covalent bonds. Diamond has each carbon atom bonded to four others in a rigid 3‑D tetrahedral structure, making it extremely hard. Graphite has layers of hexagonally arranged carbon atoms; the weak forces between layers allow them to slide, making graphite slippery and a good lubricant. Graphite can conduct electricity because of delocalised electrons between the layers.
巨型共价结构（如金刚石、石墨和二氧化硅 SiO₂）由庞大的共价键网络构成。金刚石中每个碳原子与另外四个碳原子以四面体结构成键，因此极硬。石墨由六边形排列的碳原子层组成，层间作用力弱，使得层与层可以滑动，因此石墨润滑且可用作润滑剂。石墨层间有离域电子，故能导电。
Metallic bonding arises from the electrostatic attraction between a regular arrangement of positive metal ions and a 'sea' of delocalised electrons. This 'sea' model explains why metals are good conductors of heat and electricity, are malleable (layers of ions can slide over each other) and ductile.
金属键源于规则排列的金属正离子与离域电子“海洋”之间的静电引力。这种离域电子模型解释了为什么金属是热和电的良导体、具有延展性（离子层可以在彼此之上滑动）和韧性。
5. Structures and Properties | 结构与性质
The bulk properties of a substance are determined by its structure and bonding. A summary of the main structure types is given below.
物质的宏观性质由结构和键型决定。以下是主要结构类型的小结。
| Structure type 结构类型 | Particles 微粒 | Bonding 键型 | Melting/boiling points 熔沸点 | Electrical conductivity 导电性 |
| Giant ionic 巨型离子 | Ions 离子 | Ionic bonds 离子键 | High 高 | When molten/aqueous 熔融或水溶液时导电 |
| Small covalent molecules 简单分子 | Molecules 分子 | Strong covalent bonds, weak intermolecular forces 强共价键，弱分子间力 | Low 低 | Do not conduct 不导电 |
| Giant covalent 巨型共价 | Atoms 原子 | Covalent bonds 共价键 | Very high 极高 | Most do not (graphite conducts) 多数不导电（石墨导电） |
| Metallic 金属 | Positive ions and delocalised electrons 阳离子与离域电子 | Metallic bonding 金属键 | High 高 | Good conductor 良导体 |
Alloys are mixtures of metals with other elements, designed to disrupt the regular layers of metal ions, making it harder for layers to slide. This makes alloys harder and less malleable than pure metals.
合金是金属与其他元素混合而成的物质，用来打乱金属离子的规则层排列，使层间更难滑动。因此合金比纯金属更硬、延展性更差。
6. Quantitative Chemistry — Formula Mass and the Mole | 定量化学——式量与摩尔
The relative atomic mass (Aᵣ) is the average mass of an atom of an element compared to 1/12 of the mass of a carbon‑12 atom. The relative formula mass (Mᵣ) is the sum of the Aᵣ values of all atoms in the formula of a compound.
相对原子质量（Aᵣ）是一个元素的原子平均质量相对于碳‑12 原子质量的 1/12 的比值。相对式量（Mᵣ）是化合物化学式中所有原子 Aᵣ 的总和。
One mole of a substance contains 6.02 × 10²³ particles (Avogadro' e in grams is numerically equal to its Mᵣ. The key equation linking mass, moles and Mᵣ is:
1 摩尔物质含有 6.02 × 10²³ 个粒子（阿伏伽德罗常数）。1 摩尔物质的质量（以克计）在数值上等于其 Mᵣ。连接质量、摩尔和 Mᵣ 的关键方程式为：
moles = mass (g) / Mᵣ
摩尔数 = 质量 (g) / Mᵣ
You can use moles to balance equations and calculate reacting masses. The limiting reactant is the one that is completely used up in a reaction, determining the maximum amount of product formed.
可利用摩尔来配平方程式和计算反应质量。限量反应物是在反应中完全消耗掉的反应物，它决定了最多能生成多少产物。
Concentration of a solution can be expressed in g/dm³ or mol/dm³. The relationship is:
溶液的浓度可用 g/dm³ 或 mol/dm³ 表示，关系如下：
concentration (mol/dm³) = moles / volume (dm³)
浓度 (mol/dm³) = 摩尔数 / 体积 (dm³)
Always convert volumes to dm³ when working with concentrations (1000 cm³ = 1 dm³).
涉及浓度计算时务必把体积单位转换为 dm³（1000 cm³ = 1 dm³）。
7. Reactivity of Metals and Redox | 金属反应性与氧化还原
The reactivity series lists metals in order of their tendency to lose electrons and form positive ions. A more reactive metal will displace a less reactive metal from a solution of its salt. Potassium, sodium, lithium and calcium are very reactive, reacting vigorously with water. Magnesium, aluminium, zinc and iron react with acids to release hydrogen gas. Copper, silver and gold are unreactive.
金属活动性顺序按金属失去电子形成阳离子的倾向排列。活泼性较强的金属能将活泼性较弱的金属从其盐溶液中置换出来。钾、钠、锂和钙非常活泼，与水反应剧烈。镁、铝、锌和铁能与酸反应放出氢气。铜、银和金不活泼。
Oxidation is the loss of electrons; reduction is the gain of electrons. In a displacement reaction, the metal atom is oxidised (loses electrons) and the metal ion in the compound is reduced (gains electrons). OIL RIG is a useful memory aid: Oxidation Is Loss, Reduction Is Gain of electrons.
氧化是失去电子，还原是得到电子。在置换反应中，金属原子被氧化（失去电子），化合物中的金属离子被还原（得到电子）。可借助“OIL RIG”记忆：氧化是失电子，还原是得电子。
Metals can be extracted from their ores by reduction with carbon or by electrolysis, depending on their position in the reactivity series. Metals above carbon in the series (e.g. aluminium) are extracted by electrolysis; those below carbon (e.g. iron) can be extracted by heating with carbon.
金属可通过碳还原或电解的方法从其矿石中提取，具体取决于金属在活动性顺序中的位置。排在碳之前的金属（如铝）需用电解提取；排在碳之后的金属（如铁）可用碳加热还原。
8. Acids, Bases and Salts | 酸、碱和盐
Acids are substances that release hydrogen ions (H⁺) in aqueous solution. Common laboratory acids include hydrochloric acid (HCl), sulfuric acid (H₂SO₄) and nitric acid (HNO₃). Alkalis are soluble bases that release hydroxide ions (OH⁻) in water. The pH scale measures acidity or alkalinity: pH less than 7 is acidic, pH 7 is neutral, pH greater than 7 is alkaline.
酸是在水溶液中释放氢离子（H⁺）的物质。常见实验室酸有盐酸（HCl）、硫酸（H₂SO₄）和硝酸（HNO₃）。碱是能够中和酸的物质，可溶性的碱称为碱溶液，在水中释放氢氧根离子（OH⁻）。pH 标度衡量酸碱度：pH 小于 7 为酸性，pH 等于 7 为中性，pH 大于 7 为碱性。
er: H⁺(aq) + OH⁻(aq) → H₂O(l). The specific salt formed depends on the acid and base used.
中和反应是酸与碱生成盐和水的反应：H⁺(aq) + OH⁻(aq) → H₂O(l)。生成的盐取决于所使用的酸和碱。
- Acid + metal oxide → salt + water
- 酸 + 金属氧化物 → 盐 + 水
- Acid + metal hydroxide → salt + water
- 酸 + 金属氢氧化物 → 盐 + 水
- Acid + metal carbonate → salt + water + carbon dioxide
- 酸 + 金属碳酸盐 → 盐 + 水 + 二氧化碳
- Acid + metal → salt + hydrogen (only for metals above hydrogen in reactivity series)
- 酸 + 金属 → 盐 + 氢气（仅适用于活动性顺序中排在氢前面的金属）
Making pure, dry soluble salts often uses the technique of crystallisation: react an excess of a solid base with the acid, filter off the excess, and evaporate the water slowly to obtain crystals.
制备纯净干燥的可溶盐常用结晶法：用过量的固体碱与酸反应，过滤掉过量固体，缓慢蒸发水分以析出晶体。
9. Electrolysis | 电解
Electrolysis is the process of using direct current to break down an ionic substance into its elements. An electrolytic cell consists of two electrodes (anode positive, cathode negative) dipped into an electrolyte — either the molten ionic compound or its aqueous solution.
电解是利用直流电将离子化合物分解为相应单质的过程。电解池包含两个电极（阳极接正极，阴极接负极），浸入电解质中——电解质可以是熔融的离子化合物或其水溶液。
Positive ions (cations) move to the negative cathode and gain electrons (reduction). Negative ions (anions) move to the positive anode and lose electrons (oxidation).
阳离子移向负极阴极并得到电子（还原）。阴离子移向正极阳极并失去电子（氧化）。
In the electrolysis of molten PbBr₂, lead is produced at the cathode and bromine gas at the anode. When the solution is aqueous, water molecules also can be discharged. The reactivity of the metal and the concentration of ions affect the products formed at the electrodes.
电解熔融 PbBr₂ 时，铅在阴极生成，溴气在阳极生成。若电解水溶液，水分子也可能参与放电。金属的活泼性和离子浓度会影响电极产物。
Electrolysis is used industrially to extract reactive metals such as aluminium from aluminium oxide (dissolved in molten cryolite to lower the melting point). It is also used in the purification of copper and in electroplating.
工业上用电解提取活泼金属，如从氧化铝（溶于熔融冰晶石以降低熔点）中制取铝。电解还用于铜的精炼和电镀。
10. Energy Changes | 能量变化
Chemical reactions involve energy transfers. In an exothermic reaction, energy is transferred to the surroundings, usually making the reaction mixture feel hotter. Examples include combustion, neutralisation and many oxidation reactions. In an endothermic reaction, energy is taken in from the surroundings, causing a temperature drop. Thermal decomposition and the reaction of citric acid with sodium hydrogencarbonate are endothermic.
化学反应伴随能量转移。放热反应向环境释放能量，通常使反应混合物的温度升高。例如燃烧、中和反应以及许多氧化反应。吸热反应从环境吸收能量，导致温度下降。热分解反应和柠檬酸与碳酸氢钠的反应属于吸热反应。
Reaction profile diagrams show the energy changes. The difference in energy between reactants and products is the overall energy change (ΔH). For an exothermic reaction, the products have lower energy than the reactants (ΔH negative). In an endothermic reaction, products have higher energy (ΔH positive). The diagram also shows the activation energy (Eₐ), which is the minimum energy needed for particles to collide successfully and react.
反应剖面图展示能量变化。反应物与生成物的能量差即为总能量变化（ΔH）。放热反应的生成物能量低于反应物（ΔH 为负），吸热反应生成物能量更高（ΔH 为正）。图中还标出活化能（Eₐ），即粒子发生有效碰撞并反应所需的最低能量。
Bond breaking is endothermic — energy must be supplied to break bonds. Bond making is exothermic — energy is released when new bonds form. In a reaction, if the energy released in forming new bonds is greater than the energy needed to break existing bonds, the reaction is exothermic overall; otherwise it is endothermic.
断裂化学键需要吸热——必须提供能量才能断开化学键。形成化学键则放热——新键形成时释放能量。在反应中，若形成新键释放的能量大于断裂原有化学键所需的能量，整个反应为放热反应；反之则为吸热反应。
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