📚 IGCSE CIE Chemistry: Final Exam Revision Outline | IGCSE CIE 化学：期末复习提纲
This comprehensive revision guide covers all key topics in the IGCSE CIE Chemistry syllabus, from atomic structure to organic chemistry. It is designed to help you consolidate essential concepts, master formulas, and approach the final exam with confidence. Each section pairs an English explanation with a Chinese translation for bilingual learners. Use this outline to check your understanding, fill gaps, and practise targeted questions.
这份综合复习提纲涵盖了IGCSE CIE化学课程的所有核心主题，从原子结构到有机化学。它旨在帮助你巩固基本概念、掌握公式，并自信地应对期末考试。每一部分都用英文解释配合中文翻译，方便双语学习者使用。利用这份提纲检查你的理解、填补知识漏洞并进行针对性练习。
1. Atomic Structure and the Periodic Table | 原子结构与元素周期表
An atom consists of a central nucleus containing protons and neutrons, surrounded by electrons in shells. The atomic number (proton number) defines the element, while the mass number is the sum of protons and neutrons. Isotopes have the same atomic number but different mass numbers due to varying neutron counts. Electrons fill shells in the order 2,8,8… and the outer shell electrons determine chemical properties.
原子由包含质子和中子的原子核以及核外分层排布的电子组成。原子序数（质子数）决定了元素种类，质量数是质子数与中子数之和。同位素具有相同的原子序数，但因中子数不同而质量数不同。电子按照2、8、8……的规则填充电子层，最外层电子决定化学性质。
- Relative charges and masses: proton (1, +1), neutron (1, 0), electron (1/1840, -1).
- 相对电荷与质量：质子（1, +1），中子（1, 0），电子（1/1840, -1）。
The Periodic Table arranges elements by increasing atomic number, with groups (vertical columns) and periods (horizontal rows). Group number often equals the number of outer electrons. Metals are on the left, non‑metals on the right. Trends down a group include increasing reactivity for metals (Group 1) but decreasing reactivity for non‑metals (Group 17).
元素周期表按原子序数递增排列，分为族（纵列）和周期（横行）。族数通常等于最外层电子数。金属位于左边，非金属位于右边。同一族从上到下，金属（第1族）反应性增强，而非金属（第17族）反应性减弱。
2. Chemical Bonding and Structure | 化学键与结构
Ionic bonding occurs between metals and non‑metals via electron transfer, forming giant ionic lattices. These compounds have high melting points, are often soluble in water, and conduct electricity when molten or in solution. Covalent bonding involves sharing electron pairs between non‑metals, producing simple molecules (e.g. H₂, CO₂) or giant covalent structures (e.g. diamond, SiO₂). Simple molecular substances have low melting points; giant covalent ones have very high melting points and are usually insoluble.
离子键形成于金属和非金属之间，通过电子转移形成巨大的离子晶格。这类化合物熔点高，通常溶于水，熔融或溶解时能导电。共价键涉及非金属原子间共用电子对，生成简单分子（如H₂, CO₂）或巨型共价结构（如金刚石, SiO₂）。简单分子物质熔点低；巨型共价结构熔点极高且通常不溶于水。
Metallic bonding is the attraction between positive metal ions and a ‘sea’ of delocalised electrons. This explains malleability, ductility, and electrical conductivity. Alloys are mixtures of metals with other elements and are often stronger than pure metals because the added atoms disrupt the regular lattice.
金属键是正金属离子与“电子海”之间的吸引力。这解释了金属的延展性、可塑性和导电性。合金是金属与其他元素的混合物，通常比纯金属更强韧，因为添加的原子扰乱了规则的晶格排列。
3. Stoichiometry and Moles | 计量化学与摩尔
The mole is the amount of substance containing 6.02 × 10²³ particles (Avogadro constant). Essential formulas include:
摩尔是含有6.02 × 10²³个微粒（阿伏伽德罗常数）的物质的量。基本公式包括：
n = m / M (moles = mass / molar mass)
n = V / 24 dm³ (for gases at r.t.p., 24 dm³ mol⁻¹)
concentration = n / V (mol/dm³)
n = m / M（摩尔 = 质量 / 摩尔质量）
n = V / 24 dm³（常温常压下气体，24 dm³ mol⁻¹）
浓度 = n / V（mol/dm³）
Use balanced equations to calculate reacting masses, volumes of gases, and concentrations. The limiting reactant is the one used up first, determining the amount of product. Percentage yield = (actual yield / theoretical yield) × 100%. Empirical formula can be found from mass or percentage composition by dividing by atomic masses and finding the simplest ratio.
利用配平方程式计算反应质量、气体体积和浓度。限量反应物是最先消耗完的物质，决定产物的量。产率百分比 =（实际产量 / 理论产量）× 100%。经验式可通过质量或百分组成除以相对原子质量并化为最简整数比求得。
4. States of Matter and Changes of State | 物质状态与状态变化
The kinetic particle theory explains the properties of solids, liquids, and gases in terms of particle arrangement and motion. Solids have fixed shape, liquids take the shape of a container, and gases fill the container. Changes of state (melting, boiling, condensing, freezing, sublimation) occur at specific temperatures and involve energy transfer without temperature change.
粒子运动论从粒子的排列和运动角度解释固体、液体和气体的性质。固体有固定形状，液体随容器成形，气体充满整个容器。状态变化（熔化、沸腾、冷凝、凝固、升华）在特定温度发生，并伴随能量转移而温度不变。
Diffusion is the random movement of particles from a region of higher concentration to a region of lower concentration. Heavier particles diffuse more slowly (Graham’s law). Evidence for diffusion can be seen in the bromine‑air experiment or the ammonia‑hydrogen chloride ring demonstration.
扩散是粒子从高浓度区域向低浓度区域的随机运动。较重的粒子扩散较慢（格雷姆定律）。溴与空气实验或氨气与氯化氢的‘白烟环’演示提供了扩散的证据。
| State | Particle arrangement | Motion |
| Solid | Orderly, close | Vibrate in fixed positions |
| Liquid | Random, close | Slide past each other |
| Gas | Random, far apart | Fast, random |
| 状态 | 粒子排列 | 运动方式 |
| 固体 | 有序，紧密 | 在固定位置振动 |
| 液体 | 无序，紧密 | 相互滑动 |
| 气体 | 无序，远离 | 快速、随机 |
5. Acids, Bases and Salts | 酸、碱与盐
Acids are proton (H⁺) donors; bases are proton acceptors. Common acids include HCl, H₂SO₄, HNO₃. Alkalis are soluble bases that release OH⁻ ions in water. The pH scale (0‑14) measures acidity: below 7 is acidic, 7 neutral, above 7 alkaline. Universal indicator or pH probes can be used.
酸是质子（H⁺）的供体；碱是质子的受体。常见酸有HCl、H₂SO₄、HNO₃。碱是溶于水释放OH⁻离子的物质。pH标度（0‑14）测量酸碱度：低于7为酸性，7为中性，高于7为碱性。可使用通用指示剂或pH计测定。
Reactions of acids: with metals → salt + H₂; with metal oxides/hydroxides → salt + water; with carbonates → salt + water + CO₂. Preparation of soluble salts can be done by reacting an acid with excess insoluble base/metal/carbonate, followed by filtration and crystallisation. Titration is used for soluble reactants (e.g. NaOH + HCl).
酸的反应：与金属反应→盐 + H₂；与金属氧化物/氢氧化物反应→盐 + 水；与碳酸盐反应→盐 + 水 + CO₂。可溶性盐的制备可用酸与过量不溶性碱/金属/碳酸盐反应，然后过滤、结晶。滴定用于可溶性反应物之间的反应（如NaOH + HCl）。
- Neutralisation: H⁺ + OH⁻ → H₂O
- 中和反应：H⁺ + OH⁻ → H₂O
6. Reactivity Series and Metal Extraction | 反应性顺序与金属提取
The reactivity series ranks metals by their tendency to form positive ions. Key order: K, Na, Ca, Mg, Al, (C), Zn, Fe, (H), Cu, Ag, Au. Carbon and hydrogen are included as references. More reactive metals displace less reactive metals from their compounds; e.g. zinc displaces copper from CuSO₄ solution.
金属活动性顺序根据金属形成阳离子的倾向排列。主要顺序：K, Na, Ca, Mg, Al, (C), Zn, Fe, (H), Cu, Ag, Au。碳和氢作为参考。活泼金属能从化合物中置换出不活泼金属；例如锌能从CuSO₄溶液中置换出铜。
Extraction methods depend on the metal’s position in the series: Electrolysis for K‑Al; reduction with carbon/carbon monoxide for Zn‑Fe; occurrence uncombined for Ag and Au. In the blast furnace, iron is extracted from haematite (Fe₂O₃) using coke (C) and limestone:
提取方法取决于金属在活动性顺序中的位置：K‑Al用电解法；Zn‑Fe用碳/一氧化碳还原；Ag和Au天然存在。在高炉中，用焦炭(C)和石灰石从赤铁矿(Fe₂O₃)中提取铁：
Fe₂O₃ + 3CO → 2Fe + 3CO₂
Aluminium is extracted by electrolysis of alumina (Al₂O₃) dissolved in molten cryolite to lower the melting point.
铝通过电解溶解在熔融冰晶石中的氧化铝(Al₂O₃)来提取，冰晶石可降低熔点。
7. Electrochemistry | 电化学
Electrolysis is the decomposition of an ionic compound by passing direct current through its molten or dissolved state. The cathode (negative electrode) attracts cations; the anode (positive electrode) attracts anions. Products depend on the electrolyte and electrode material. For molten binary compounds, metal is at cathode, non‑metal at anode. In aqueous solutions, the reactivity of the metal and the concentration of halide ions determine discharge (e.g. Cu²⁺ rather than H⁺; Cl⁻ rather than OH⁻).
电解是通过向熔融或溶液态的离子化合物通直流电使其分解的过程。阴极（负极）吸引阳离子；阳极（正极）吸引阴离子。产物取决于电解质和电极材料。对于熔融二元化合物，金属在阴极生成，非金属在阳极生成。在水溶液中，金属的活动性与卤离子浓度共同决定放电顺序（如Cu²⁺先于H⁺放电；Cl⁻先于OH⁻放电）。
Simple cells consist of two different metals in an electrolyte; the more reactive metal acts as the negative electrode and releases electrons. Fuel cells like the hydrogen‑oxygen cell produce electricity cleanly: 2H₂ + O₂ → 2H₂O. Electroplating uses electrolysis to coat an object with a layer of metal.
简单电池由两种不同金属置于电解质中构成；较活泼的金属作为负极并释放电子。燃料电池如氢氧燃料电池清洁地产生电能：2H₂ + O₂ → 2H₂O。电镀利用电解在物体表面镀上一层金属。
8. Chemical Energetics | 化学能量学
Exothermic reactions release energy to the surroundings (temperature increase); examples include combustion, neutralisation, and dissolving anhydrous salts. Endothermic reactions absorb energy (temperature decrease); examples include photosynthesis, thermal decomposition of CaCO₃, and dissolving certain ammonium salts.
放热反应向环境释放能量（温度升高）；例子有燃烧、中和反应和溶解无水盐。吸热反应吸收能量（温度降低）；例子有光合作用、碳酸钙热分解以及溶解某些铵盐。
Energy change (ΔH) can be calculated from bond energies: ΔH = sum of bonds broken − sum of bonds formed. A negative ΔH means exothermic; positive means endothermic. Simple calorimetry experiments measure temperature change to calculate heat transferred: q = mcΔT. Reaction profiles show energy levels of reactants and products, and activation energy (Eₐ).
能量变化（ΔH）可通过键能计算：ΔH = 断裂键的总能量 − 形成键的总能量。ΔH为负表示放热；为正表示吸热。简单量热计实验通过测量温度变化来计算传递的热量：q = mcΔT。反应过程图展示反应物和产物的能量水平以及活化能(Eₐ)。
9. Reaction Rates and Equilibrium | 反应速率与平衡
Rate of reaction is measured by the change in concentration of a reactant or product per unit time. Factors affecting rate: surface area (smaller particles → faster), concentration/pressure (increased → faster), temperature (higher → faster), and catalysts (provide alternative pathway with lower Eₐ). The collision theory states that particles must collide with sufficient energy (≥ activation energy) and correct orientation.
反应速率通过单位时间内反应物或产物浓度的变化来衡量。影响速率的因素：表面积（颗粒越小→越快），浓度/压强（增大→越快），温度（升高→越快），以及催化剂（提供更低Eₐ的替代路径）。碰撞理论指出，粒子必须发生碰撞且具有足够能量（≥活化能）和正确的取向。
Reversible reactions reach dynamic equilibrium in a closed system when forward and reverse rates are equal. Le Chatelier’s principle: if a system at equilibrium is subjected to a change in concentration, pressure, or temperature, the equilibrium shifts to oppose the change. In the Haber process (N₂ + 3H₂ ⇌ 2NH₃), high pressure favours product but high temperature decreases yield (compromise conditions: 450 °C, 200 atm, iron catalyst).
可逆反应在密闭系统中达到动态平衡时，正向和逆向速率相等。勒夏特列原理：如果处于平衡的体系受到浓度、压强或温度变化的影响，平衡会向削弱该变化的方向移动。在哈伯法中（N₂ + 3H₂ ⇌ 2NH₃），高压有利于产率但高温降低产率（采用折衷条件：450 °C、200 atm、铁催化剂）。
10. Organic Chemistry | 有机化学
Organic chemistry centres on carbon compounds. Homologous series have the same general formula, functional group, and similar chemical properties. Key series:
有机化学以碳的化合物为核心。同系物具有相同的通式、官能团和相似的化学性质。主要系列：
| Series | Functional group | General formula |
| Alkanes | C−C single bonds | CₙH₂ₙ₊₂ |
| Alkenes | C=C double bond | CₙH₂ₙ |
| Alcohols | −OH | CₙH₂ₙ₊₁OH |
| Carboxylic acids | −COOH | CₙH₂ₙ₊₁COOH |
Alkanes undergo combustion and substitution (e.g. Cl₂, UV light). Alkenes undergo addition reactions (e.g. with Br₂, turning bromine water colourless). Ethanol can be produced by fermentation (glucose → ethanol + CO₂) or by hydration of ethene (C₂H₄ + H₂O → C₂H₅OH). Carboxylic acids react with alcohols to form esters (e.g. ethyl ethanoate) with concentrated H₂SO₄ as catalyst.
烷烃发生燃烧和取代反应（如Cl₂、紫外光）。烯烃发生加成反应（如与Br₂反应，使溴水褪色）。乙醇可通过发酵（葡萄糖 → 乙醇 + CO₂）或乙烯水合（C₂H₄ + H₂O → C₂H₅OH）制取。羧酸与醇在浓H₂SO₄催化下反应生成酯（如乙酸乙酯）。
Polymers: Addition polymerisation of alkenes forms long chains (e.g. poly(ethene), poly(propene)). Condensation polymerisation involves monomers with two functional groups (e.g. nylon, PET). Recycling and disposal problems are important environmental issues.
聚合物：烯烃的加成聚合形成长链（如聚乙烯、聚丙烯）。缩合聚合涉及带有两个官能团的单体（如尼龙、PET）。回收利用和处置问题是重要的环境议题。
11. Experimental Techniques and Chemical Analysis | 实验技术与化学分析
Common separation methods: filtration (insoluble solid from liquid), crystallisation (obtaining soluble salt), simple and fractional distillation (liquid from solution / separating liquids with different boiling points), chromatography (separating mixtures of soluble substances using a mobile and stationary phase), and sublimation (for substances like iodine). Rf value = distance moved by spot / distance moved by solvent front.
常用分离方法：过滤（从液体中分离不溶固体），结晶（获得可溶性盐），简单蒸馏和分馏（从溶液中蒸出液体/分离不同沸点液体），色谱法（利用流动相和固定相分离可溶混合物），以及升华（适用于碘等物质）。Rf值 = 斑点移动距离 / 溶剂前沿移动距离。
Identification tests: Cations can be tested with NaOH (aq) to form coloured precipitates; e.g. Cu²⁺ gives blue, Fe²⁺ green, Fe³⁺ brown. Anions: Cl⁻ gives white ppt with AgNO₃/HNO₃, soluble in NH₃; SO₄²⁻ gives white ppt with BaCl₂/HCl; CO₃²⁻ effervesces with acid, gas turns limewater milky. Flame tests: Li⁺ red, Na⁺ yellow, K⁺ lilac, Ca²⁺ orange‑red, Ba²⁺ green.
鉴定测试：阳离子可用NaOH溶液检验，生成有色沉淀；如Cu²⁺蓝色，Fe²⁺绿色，Fe³⁺棕色。阴离子：Cl⁻遇AgNO₃/HNO₃生成白色沉淀，溶于NH₃；SO₄²⁻遇BaCl₂/HCl生成白色沉淀；CO₃²⁻与酸反应产生气泡，气体使石灰水变浑浊。焰色反应：Li⁺红色，Na⁺黄色，K⁺紫色，Ca²⁺橙红色，Ba²⁺绿色。
Gases: H₂ pops with lighted splint; O₂ relights glowing splint; CO₂ turns limewater milky; Cl₂ bleaches damp litmus paper; NH₃ turns damp red litmus blue. Volumetric analysis (titration) uses a burette and pipette to find unknown concentration using a standard solution and an indicator (e.g. methyl orange).
气体：H₂用点燃的木条检验发出爆鸣声；O₂使余烬木条复燃；CO₂使石灰水变浑浊；Cl₂使湿润的石蕊试纸漂白；NH₃使湿润的红色石蕊试纸变蓝。容量分析（滴定）使用滴定管和移液管，用标准溶液和指示剂（如甲基橙）测定未知浓度。
Published by TutorHao | Chemistry Revision Series | aleveler.com
更多咨询请联系16621398022（同微信）
屏轩国际教育cambridge primary/secondary checkpoint, cat4, ukiset,ukcat,igcse,alevel,PAT,STEP,MAT, ibdp,ap,ssat,sat,sat2课程辅导，国外大学本科硕士研究生博士课程论文辅导Cancel reply