📚 Year 10 AQA Chemistry Core Knowledge Points Summary | AQA 化学核心知识点梳理
Year 10 AQA Chemistry builds the foundation for the GCSE course by covering atomic structure, bonding, quantitative calculations, chemical changes, and energy transfers. This revision guide consolidates all the core knowledge points you need to master, presented in clear, bilingual pairs. Each section reinforces key concepts with concise explanations, helping you retain the facts and apply them confidently in exams.
Year 10 AQA 化学是整个 GCSE 课程的基础，涵盖了原子结构、化学键、定量计算、化学变化和能量转移等内容。这份核心知识点梳理采用中英双语对照的方式，帮助你有条理地复习和掌握每一个考点。每个要点都用简明的英文和中文配对呈现，让你既理解学科术语，又巩固深层原理，在考试中从容应对。
1. Atomic Structure | 原子结构
All matter is made up of atoms. An atom consists of a tiny, dense nucleus containing protons and neutrons, surrounded by electrons moving in specific energy levels (shells).
所有物质都由原子构成。每个原子包含一个极小且致密的原子核（由质子和中子组成），核外有电子在特定的能层（电子层）中运动。
| Particle | Relative charge | Relative mass |
|---|---|---|
| Proton (p⁺) | +1 | 1 |
| Neutron (n⁰) | 0 | 1 |
| Electron (e⁻) | -1 | 1/1840 (negligible) |
The atomic number (Z) is the number of protons and determines which element an atom is. The mass number (A) is the total number of protons + neutrons. In a neutral atom, the number of electrons equals the number of protons.
原子序数 (Z) 是质子数，决定了元素种类。质量数 (A) 是质子数与中子数之和。中性原子里，电子数等于质子数。
Isotopes are atoms of the same element (same number of protons) but with different numbers of neutrons, so they have different mass numbers. For example, carbon-12 and carbon-14 are isotopes.
同位素是同一元素（质子数相同）但中子数不同的原子，因此质量数不同。例如碳-12 和碳-14 就是一对同位素。
Electrons occupy shells around the nucleus. The first shell holds up to 2 electrons, the second and third shells up to 8 electrons each. Electron configurations for the first 20 elements must be learned, e.g. Na: 2,8,1.
电子分布在核外电子层上。第一层最多容纳 2 个电子，第二层和第三层最多容纳 8 个电子。你需要记住前 20 号元素的电子排布，例如钠 Na：2,8,1。
2. The Periodic Table | 元素周期表
Elements are arranged in the periodic table in order of increasing atomic number. The table is organised into periods (horizontal rows) and groups (vertical columns). Elements in the same group have the same number of outer-shell electrons, which gives them similar chemical properties.
元素按照原子序数递增的顺序排列在周期表中。周期是横向的行，族是纵向的列。同一族元素原子的最外层电子数相同，因此它们的化学性质相似。
Group 1: Alkali metals (Li, Na, K, Rb, Cs) – all have one electron in their outer shell, are soft, very reactive, and reactivity increases down the group. They react vigorously with water to form a metal hydroxide and hydrogen gas, e.g. 2Na + 2H₂O → 2NaOH + H₂.
第 1 族：碱金属（锂、钠、钾、铷、铯）——最外层都只有 1 个电子，质地软，非常活泼，且活泼性沿族向下增强。它们与水剧烈反应，生成金属氢氧化物和氢气，例如 2Na + 2H₂O → 2NaOH + H₂。
Group 7: Halogens (F₂, Cl₂, Br₂, I₂) – all have 7 outer electrons, exist as diatomic molecules, and reactivity decreases down the group. A more reactive halogen can displace a less reactive one from its halide salt, e.g. Cl₂ + 2KBr → 2KCl + Br₂.
第 7 族：卤素（氟、氯、溴、碘）——最外层都有 7 个电子，以双原子分子存在，反应活性沿族向下减弱。较活泼的卤素能把较不活泼的卤素从其卤化物溶液中置换出来，例如 Cl₂ + 2KBr → 2KCl + Br₂。
Group 0 (or 8): Noble gases (He, Ne, Ar, Kr, Xe, Rn) – have full outer shells, making them extremely unreactive. Boiling points increase down the group.
第 0 族（或称第 8 族）：稀有气体（氦、氖、氩、氪、氙、氡）——最外层已满，因此性质极不活泼。沸点沿族向下逐渐升高。
Transition metals (central block) form coloured compounds, often act as catalysts, and can form ions with different charges, e.g. Fe²⁺ and Fe³⁺.
过渡金属（中间区域）常形成有色化合物，常用作催化剂，且能形成多种价态的离子，例如 Fe²⁺ 和 Fe³⁺。
3. Ionic Bonding | 离子键
Ionic bonding occurs between a metal and a non-metal. Metal atoms lose electrons to form positive ions (cations), while non-metal atoms gain electrons to form negative ions (anions). The oppositely charged ions are held together by strong electrostatic forces in a giant ionic lattice.
离子键形成于金属和非金属之间。金属原子失去电子形成阳离子，非金属原子获得电子形成阴离子。带相反电荷的离子通过强大的静电引力结合在一起，形成巨型离子晶格。
For example, sodium chloride (NaCl): sodium atoms lose one electron to become Na⁺, and chlorine atoms gain one electron to become Cl⁻. The ionic bond is the strong attraction between Na⁺ and Cl⁻ throughout the lattice.
例如氯化钠 (NaCl)：钠原子失去一个电子变成 Na⁺，氯原子得到一个电子变成 Cl⁻。整个晶格中 Na⁺ 和 Cl⁻ 之间的强烈吸引力就是离子键。
Ionic compounds have high melting and boiling points because a lot of energy is needed to overcome the strong electrostatic forces between ions. They conduct electricity only when molten or dissolved in water, as the ions are free to move. They are often soluble in water and form crystals.
离子化合物的熔点和沸点很高，因为需要大量的能量来克服离子间的强静电引力。它们只有熔融或溶于水时才能导电，此时离子可以自由移动。它们通常可溶于水，形成晶体。
4. Covalent and Metallic Bonding | 共价键与金属键
Covalent bonding forms between non-metal atoms. Atoms share pairs of electrons to achieve a full outer shell. A single covalent bond involves one shared pair of electrons, a double bond two pairs, and a triple bond three pairs.
共价键形成于非金属原子之间。原子通过共用电子对达到稳定的外层电子结构。单键共用一对电子，双键共用两对，三键共用三对。
Simple molecular substances such as H₂O, CO₂, and O₂ consist of small molecules with weak intermolecular forces. They have low melting and boiling points, do not conduct electricity, and are often gases or liquids at room temperature.
简单分子物质，例如 H₂O、CO₂ 和 O₂，由小分子构成，分子间存在微弱的分子间作用力。它们的熔点和沸点较低，不导电，常温下常为气体或液体。
Giant covalent structures (macromolecules) have many atoms linked by strong covalent bonds throughout. Diamond (each carbon forms four bonds) is extremely hard and does not conduct electricity. Graphite (each carbon forms three bonds in layers) is soft and conducts electricity due to delocalised electrons between layers. Silicon dioxide (SiO₂) is similar to diamond and has a high melting point.
巨型共价结构（大分子）中，大量原子通过强共价键连接。金刚石中每个碳原子形成四个共价键，非常坚硬，不导电。石墨中每个碳原子只形成三个键，呈层状结构，层间有离域电子，因此软而导电。二氧化硅 (SiO₂) 类似金刚石，具有极高的熔点。
Metallic bonding: metals consist of positive ions arranged in a regular lattice, surrounded by a ‘sea’ of delocalised electrons. The strong electrostatic attraction between the positive ions and the delocalised electrons explains why metals are good conductors of heat and electricity, are malleable and ductile, and have high melting points. Alloys are harder than pure metals because the different-sized atoms disrupt the layers, preventing them from sliding.
金属键：金属由规则排列的阳离子和包围它们的“离域电子气”构成。阳离子和离域电子之间的强静电引力使金属具有良好的导电导热性、延展性和较高的熔点。合金比纯金属更硬，因为不同大小的原子打乱了层状排列，使原子层难以滑动。
5. States of Matter and Properties | 物质状态与性质
The three states of matter are solid, liquid and gas. The particle model explains their behaviour: in solids, particles are closely packed in a regular arrangement and vibrate about fixed positions; in liquids, particles are close but can move past each other; in gases, particles are far apart and move rapidly in all directions.
物质有固态、液态和气态三种状态。粒子模型解释了它们的行为：固体中，粒子紧密排列，有固定位置，只在原位振动；液体中，粒子紧密但可以互相滑动；气体中，粒子相距很远，快速无规则运动。
When a substance changes state, mass is conserved. Melting and boiling are endothermic processes (energy is absorbed to overcome forces between particles), while condensing and freezing are exothermic (energy is released). The stronger the forces between particles, the higher the melting and boiling points.
物质状态变化时，质量守恒。熔化和沸腾是吸热过程（吸收能量克服粒子间作用力），而凝结和凝固是放热过程（释放能量）。粒子间作用力越强，熔点和沸点越高。
Nanoparticles are particles with sizes between 1 and 100 nanometres. They have a very high surface area to volume ratio, giving them unique properties and making them useful in medicine, cosmetics, and catalysts. However, their potential health and environmental effects are still being studied.
纳米颗粒是尺寸在 1 到 100 纳米之间的粒子。它们具有极大的比表面积，因此表现出独特的性质，在医药、化妆品和催化剂等方面有广泛应用。但它们对健康与环境的潜在影响仍在研究中。
6. Quantitative Chemistry: The Mole | 定量化学：摩尔
Relative atomic mass (Aᵣ) is the average mass of an atom of an element compared to 1/12th the mass of a carbon-12 atom. Relative formula mass (Mᵣ) is the sum of all the relative atomic masses in a compound’s formula.
相对原子质量 (Aᵣ) 是某元素原子的平均质量与碳‑12 原子质量的 1/12 的比值。相对分子质量 (Mᵣ) 是化合物化学式中所有原子的相对原子质量之和。
One mole of any substance contains exactly 6.022 × 10²³ particles (Avogadro constant). The mass of one mole of a substance in grams is equal to its Aᵣ or Mᵣ. This is called the molar mass.
任何物质的 1 摩尔都含有 6.022 × 10²³ 个微粒（阿伏伽德罗常数）。1 摩尔物质的质量（以克为单位）等于其 Aᵣ 或 Mᵣ，称为摩尔质量。
The mole equation: mass (g) = moles × Mᵣ. Rearranged, moles = mass ÷ Mᵣ. This relationship allows you to convert between mass and amount of substance.
摩尔计算公式：质量 (g) = 物质的量 (mol) × 相对分子质量 (Mᵣ)。变形后，物质的量 = 质量 ÷ Mᵣ。利用这一关系可以在质量和物质的量之间进行换算。
For solutions, concentration in mol/dm³ is calculated as: concentration = moles ÷ volume (in dm³). Volume in cm³ must be divided by 1000 to convert to dm³. You must be able to use balanced equations to calculate reacting masses and volumes of gases (at room temperature and pressure, one mole of any gas occupies 24 dm³).
对于溶液，浓度（mol/dm³）的计算公式为：浓度 = 物质的量 ÷ 体积（dm³）。体积若以 cm³ 为单位，需除以 1000 换算成 dm³。你需要能利用配平的化学方程式计算反应质量和气体体积（常温常压下，1 摩尔任何气体体积为 24 dm³）。
7. Chemical Changes: Reactions of Acids | 化学变化：酸的反应
The pH scale (0–14) measures the acidity or alkalinity of a solution. Acids have pH less than 7, alkalis have pH greater than 7, and neutral solutions have pH = 7. Acids produce H⁺ ions in water, and alkalis produce OH⁻ ions.
pH 标度（0–14）用于衡量溶液的酸碱度。酸溶液的 pH 小于 7，碱溶液的 pH 大于 7，中性溶液的 pH = 7。酸在水中产生 H⁺ 离子，碱在水中产生 OH⁻ 离子。
Acids react with metals above hydrogen in the reactivity series to form a salt and hydrogen gas: metal + acid → salt + hydrogen. For example, Mg + 2HCl → MgCl₂ + H₂.
酸能与金属活动性顺序中排在氢前面的金属反应，生成盐和氢气：金属 + 酸 → 盐 + 氢气。例如 Mg + 2HCl → MgCl₂ + H₂。
Acids are neutralised by bases (metal oxides, metal hydroxides) to form a salt and water. neutralisation: H⁺ (aq) + OH⁻ (aq) → H₂O (l). Salts can be produced by reacting an acid with an insoluble base, then filtering off excess solid and crystallising the solution. Soluble salts can also be made by titration using an indicator.
酸被碱（金属氧化物、金属氢氧化物）中和，生成盐和水。中和反应的离子方程式为：H⁺ (aq) + OH⁻ (aq) → H₂O (l)。可通过酸与不溶性碱的反应制备盐，然后过滤掉多余固体并使溶液结晶。也可使用指示剂通过滴定法制备可溶性盐。
Strong acids (e.g. HCl, H₂SO₄, HNO₃) ionise completely in water, releasing all their H⁺ ions. Weak acids (e.g. ethanoic acid, citric acid) only partially ionise, so they have a higher pH (less acidic) than a strong acid of the same concentration.
强酸（如 HCl、H₂SO₄、HNO₃）在水中完全电离，释放出全部 H⁺ 离子。弱酸（如乙酸、柠檬酸）只部分电离，因此相同浓度下弱酸的 pH 较高（酸性较弱）。
8. Electrolysis | 电解
Electrolysis is the process of using a direct electric current to decompose an ionic compound into its elements. The ionic substance must be molten or dissolved in water so that the ions are free to move and conduct electricity.
电解是利用直流电将离子化合物分解为单质的过程。离子化合物必须处于熔融状态或溶于水中，使离子能够自由移动并导电。
During electrolysis, positive ions (cations) move to the negative electrode (cathode) and gain electrons (reduction). Negative ions (anions) move to the positive electrode (anode) and lose electrons (oxidation). You can remember: PANIC – Positive Anode Negative Is Cathode.
电解时，阳离子移向负极（阴极）得到电子（还原反应）；阴离子移向正极（阳极）失去电子（氧化反应）。可记住：“阳氧阴还”谐音或 PANIC 助记。
In the electrolysis of molten binary compounds (e.g. molten lead(II) bromide, PbBr₂), a metal (Pb) is produced at the cathode and a non-metal (Br₂) at the anode. Overall: PbBr₂ (l) → Pb (l) + Br₂ (g).
电解熔融的二元化合物（如熔融溴化铅 PbBr₂）时，阴极生成金属单质（Pb），阳极生成非金属单质（Br₂）。总反应：PbBr₂ (l) → Pb (l) + Br₂ (g)。
In aqueous electrolysis, the products depend on the relative reactivity of the ions and the presence of water molecules. At the cathode, the least reactive cation (often H⁺ from water if the metal is more reactive than hydrogen) is discharged. At the anode, a halide ion will be discharged in preference to hydroxide ions; if no halide is present, oxygen gas is produced from the oxidation of water.
在水溶液电解中，产物取决于离子的相对活泼性和水的存在。在阴极，通常较不活泼的阳离子优先放电（若金属比氢活泼，水中的 H⁺ 放电析出氢气）。在阳极，卤素离子优先于氢氧根离子放电；若无卤素离子，则由水氧化产生氧气。
Aluminium is extracted by electrolysis of molten aluminium oxide (Al₂O₃) dissolved in cryolite to lower the melting point. Electroplating uses electrolysis to coat an object with a thin layer of metal, e.g. silver plating.
铝是通过电解溶解在冰晶石中的熔融氧化铝 (Al₂O₃) 来提取的，冰晶石可以降低熔点。电镀则利用电解在物体表面镀上一层薄金属，如镀银。
9. Energy Changes | 能量变化
Chemical reactions can be exothermic (transfers energy to the surroundings, usually as heat) or endothermic (takes in energy from the surroundings). Exothermic reactions include combustion, neutralisation, and respiration. Endothermic reactions include thermal decomposition and photosynthesis.
化学反应可以是放热反应（向环境释放能量，通常以热的形式）或吸热反应（从环境吸收能量）。燃烧、中和、呼吸作用属于放热反应；热分解和光合作用属于吸热反应。
Reaction profile diagrams show the energy changes during a reaction. The overall energy change (ΔH) is the difference between the energy of products and reactants. In an exothermic reaction, the products are at a lower energy level than the reactants; in an endothermic reaction, the products are at a higher energy level.
反应剖面图展示反应过程中的能量变化。总能量变化 (ΔH) 是生成物与反应物的能量差。放热反应中，生成物能量低于反应物；吸热反应中，生成物能量高于反应物。
The activation energy (Ea) is the minimum energy needed for a reaction to occur. Catalysts provide an alternative reaction pathway with lower activation energy, increasing the rate without being used up.
活化能 (Ea) 是反应发生所需的最低能量。催化剂通过提供活化能更低的反应途径，加快反应速率，而自身不被消耗。
Bond energies can be used to calculate the overall energy change for a reaction: energy change = total energy absorbed to break bonds − total energy released when forming bonds. A negative result indicates exothermic; a positive result indicates endothermic.
可利用键能计算反应的总能量变化：能量变化 = 断裂化学键吸收的总能量 – 形成化学键释放的总能量。结果为负值表示放热反应，正值表示吸热反应。
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