📚 Year 10 CCEA Chemistry: Core Topics Review | Year 10 CCEA 化学：核心知识点梳理
In Year 10 CCEA Chemistry, students encounter the foundational ideas that underpin the entire GCSE course. This article brings together the core topics – from atomic structure and bonding to organic chemistry and electrolysis – into one organised revision guide. Each section presents key concepts in both English and Chinese to support bilingual learners, helping you consolidate knowledge effectively.
Year 10 CCEA 化学课程涵盖了 GCSE 化学的基石概念。本文梳理了从原子结构、化学键到有机化学和电解等核心知识点，为中英双语学习者提供系统化的复习指南，帮助大家高效巩固知识。
1. Atomic Structure | 原子结构
All substances are made from atoms. An atom has a tiny nucleus made up of protons and neutrons, surrounded by electrons arranged in shells. The nucleus is extremely small compared with the whole atom.
所有物质都由原子构成。原子拥有一个由质子和中子组成的极小原子核，电子分层排布在核外。原子核与整个原子相比非常微小。
Protons carry a relative charge of +1 and a relative mass of 1. Neutrons are neutral with a relative mass of 1. Electrons carry a charge of -1 and have a negligible relative mass (about 1/1836). The number of protons defines the element, known as the atomic number (Z). The total number of protons and neutrons is the mass number (A).
质子带 1 个单位正电荷，相对质量为 1。中子不带电，相对质量也为 1。电子带 1 个单位负电荷，相对质量极小（约 1/1836）。质子数决定元素种类，称为原子序数 (Z)；质子数与中子数之和为质量数 (A)。
Isotopes are atoms of the same element with the same number of protons but different numbers of neutrons. For example, carbon-12 (¹²C) has 6 protons and 6 neutrons, while carbon-14 (¹⁴C) has 6 protons and 8 neutrons. They have the same chemical properties but different physical properties such as density.
同位素是质子数相同而中子数不同的同种元素的原子。例如碳-12 (¹²C) 有 6 个质子和 6 个中子，碳-14 (¹⁴C) 有 6 个质子和 8 个中子。它们的化学性质相同，但密度等物理性质不同。
2. The Periodic Table | 元素周期表
Elements are arranged in the modern periodic table in order of increasing atomic number. Horizontal rows are called periods, and vertical columns are called groups. Elements in the same group have the same number of outer‑shell electrons, which gives them similar chemical properties.
现代周期表按原子序数递增顺序排列元素。横行称为周期，纵列称为族。同一族的元素最外层电子数相同，因此化学性质相似。
Metals are found on the left and centre of the table, while non‑metals occupy the upper right. Group 1 elements (alkali metals) are very reactive, with reactivity increasing down the group as the outer electron becomes easier to lose. Group 7 elements (halogens) are also highly reactive non‑metals, but reactivity decreases down the group. Group 0 (noble gases) are extremely unreactive because they have a full outer shell of electrons.
金属位于周期表左侧和中部，非金属位于右上方。第 1 族（碱金属）非常活泼，且越往下金属性越强，因为外层电子更容易失去。第 7 族（卤素）是活泼的非金属，但越往下活泼性减弱。第 0 族（稀有气体）极不活泼，因其已具有稳定的满外层电子结构。
3. Chemical Bonding | 化学键
Atoms bond to achieve a full outer shell of electrons, becoming more stable. The three main types of bonding are ionic, covalent and metallic.
原子通过成键来获得满的外层电子，变得更加稳定。三种主要化学键类型为离子键、共价键和金属键。
Ionic bonding occurs between a metal and a non‑metal. Electrons are transferred from the metal atom to the non‑metal atom, forming oppositely charged ions that are held together by strong electrostatic forces. For example, sodium chloride (NaCl) forms when a sodium atom loses one electron to become Na⁺ and a chlorine atom gains that electron to become Cl⁻. Ionic compounds have high melting and boiling points and conduct electricity when molten or dissolved in water.
离子键形成于金属与非金属之间。金属原子失去电子形成阳离子，非金属原子得到电子形成阴离子，阴阳离子通过强静电引力结合。例如氯化钠 (NaCl) 中，钠原子失去一个电子成为 Na⁺，氯原子得到电子成为 Cl⁻。离子化合物熔沸点高，熔融态或溶于水时可导电。
Covalent bonding takes place between non‑metal atoms. Electrons are shared so that each atom attains a full outer shell. Simple molecular substances like water (H₂O), carbon dioxide (CO₂) and methane (CH₄) have weak intermolecular forces and thus low melting points. Giant covalent structures such as diamond and silicon dioxide have a vast network of strong covalent bonds, making them very hard with extremely high melting points.
共价键形成于非金属原子之间。原子通过共用电子对使各自达到稳定外层。简单分子物质如水 (H₂O)、二氧化碳 (CO₂) 和甲烷 (CH₄) 分子间作用力弱，因此熔沸点低。巨型共价结构如金刚石和二氧化硅由大量强共价键连成网络，质地坚硬且熔沸点极高。
Metallic bonding involves a lattice of metal cations surrounded by a ‘sea’ of delocalised electrons. This structure allows metals to conduct heat and electricity, and to be malleable and ductile.
金属键由金属阳离子规则排列、沉浸于自由电子的“海洋”中构成。这种结构使金属能够导电导热，并具有延展性。
4. Writing Formulas and Equations | 书写化学式和化学方程式
Chemical formulas show the types and ratios of atoms in a compound. Using ion charges, we can deduce the formula: the total positive charge must balance the total negative charge. For instance, calcium chloride contains Ca²⁺ and Cl⁻ ions, so the formula is CaCl₂.
化学式表示化合物中原子种类和数量比。利用离子电荷可以推导化学式：正负总电荷必须相等。例如氯化钙中含有 Ca²⁺ 和 Cl⁻，因此化学式为 CaCl₂。
The relative atomic mass Aᵣ is the average mass of an atom of an element compared with ¹/₁₂ 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. Word equations and balanced symbol equations tell us what happens in a reaction; conservation of mass means the number of each type of atom must be the same on both sides.
相对原子质量 Aᵣ 是以一个碳-12 原子质量的 1/12 为标准，一个原子平均质量的相对值。相对式量 Mᵣ 是化学式中所有原子 Aᵣ 之和。文字方程式和配平的符号方程式描述了反应过程；质量守恒要求反应前后各原子种类和数目不变。
Example: 2H₂ + O₂ → 2H₂O
示例：2H₂ + O₂ → 2H₂O
5. The Mole Concept | 摩尔概念
One mole of a substance contains 6.02 × 10²³ particles (Avogadro’s constant). The molar mass is the mass of one mole, equal to the relative formula mass (Mᵣ) expressed in grams. The key relationship is:
一摩尔物质含有 6.02 × 10²³ 个微粒（阿伏伽德罗常数）。摩尔质量是一摩尔物质的质量，数值上等于相对式量 Mᵣ，单位为克。核心关系式为：
mass (g) = moles × molar mass (g/mol)
质量 (g) = 摩尔数 × 摩尔质量 (g/mol)
Using this formula, we can calculate the mass of reactants needed or products formed. For example, to find the mass of water produced from 2 moles of H₂: 2H₂ + O₂ → 2H₂O gives 2 moles of H₂O; Mᵣ of H₂O = 18, so mass = 2 × 18 = 36 g. Mole calculations are central to quantitative chemistry.
通过这个公式可以计算所需反应物质量或生成物质量。例如求 2 mol H₂ 可生成多少水：2H₂ + O₂ → 2H₂O 可知生成 2 mol H₂O，H₂O 的 Mᵣ = 18，因此质量 = 2 × 18 = 36 g。摩尔计算是定量化学的核心。
6. Reactivity Series and Redox | 活动性顺序与氧化还原
Metals can be placed in a reactivity series based on how readily they react with water, acids or oxygen. A more reactive metal will displace a less reactive metal from its compound. For example, zinc displaces copper from copper sulfate solution: Zn + CuSO₄ → ZnSO₄ + Cu.
金属可根据其与水、酸或氧气的反应程度排列成活动性顺序。较活泼的金属可从较不活泼金属的化合物中将后者置换出来。例如锌能从硫酸铜溶液中置换出铜：Zn + CuSO₄ → ZnSO₄ + Cu。
Oxidation is the gain of oxygen or loss of electrons; reduction is the loss of oxygen or gain of electrons. The mnemonic OIL RIG (Oxidation Is Loss, Reduction Is Gain of electrons) helps to remember electron transfer. In a displacement reaction, the metal that donates electrons is oxidised, while the metal ion that accepts electrons is reduced.
氧化是指得到氧或失去电子；还原是指失去氧或得到电子。助记口诀 OIL RIG（氧化失电子，还原则得电子）有助于记忆。在置换反应中，提供电子的金属被氧化，接受电子的金属离子被还原。
7. Acids, Bases and Salts | 酸、碱和盐
Acids are substances that release hydrogen ions (H⁺) in water. Common laboratory acids include hydrochloric acid (HCl), sulfuric acid (H₂SO₄) and nitric acid (HNO₃). Bases are substances that neutralise acids; alkalis are soluble bases that release hydroxide ions (OH⁻) in water, such as sodium hydroxide (NaOH).
酸是在水中能释放氢离子 (H⁺) 的物质。实验室常用酸有盐酸 (HCl)、硫酸 (H₂SO₄) 和硝酸 (HNO₃)。碱能中和酸；可溶性碱称作碱溶液，能在水中释放氢氧根离子 (OH⁻)，例如氢氧化钠 (NaOH)。
Neutralisation occurs when an acid and a base react to form a salt and water. The pH scale shows how acidic or alkaline a solution is: pH 7 is neutral, lower values are acidic, higher values are alkaline. Titration can be used to prepare a soluble salt from an acid and an alkali, while insoluble salts can be made by precipitation.
酸与碱反应生成盐和水，称为中和反应。pH 标度表示溶液酸碱度：7 为中性，数值越小酸性越强，越大碱性越强。滴定法可用于从酸碱制备可溶性盐，不溶性盐可通过沉淀反应制备。
8. Electrolysis | 电解
Electrolysis is the decomposition of an ionic compound by passing direct current through it when molten or in solution. The electrolyte is the substance that conducts electricity and is decomposed. Positive ions (cations) migrate to the negative cathode, where they gain electrons (reduction); negative ions (anions) migrate to the positive anode, where they lose electrons (oxidation).
电解是利用直流电使熔融态或溶液中的离子化合物分解的过程。被分解的导体称为电解质。阳离子向负极（阴极）移动，得电子被还原；阴离子向正极（阳极）移动，失电子被氧化。
In the electrolysis of molten lead bromide (PbBr₂), lead (Pb²⁺) forms at the cathode and bromine (Br₂) at the anode. In aqueous solutions, water can also be involved. For aqueous sodium chloride, chlorine gas forms at the anode, hydrogen gas at the cathode, leaving sodium hydroxide in solution. Electrolysis is used industrially to extract aluminium from aluminium oxide and to electroplate objects.
电解熔融溴化铅 (PbBr₂) 时，阴极析出金属铅，阳极生成溴。在水溶液中，水也可能参与反应。电解食盐水时，阳极产生氯气，阴极产生氢气，溶液中留下氢氧化钠。工业上用电解提取铝，并用于电镀。
Anode half‑equation: 2Cl⁻ → Cl₂ + 2e⁻ (oxidation)
阳极
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