Year 13 CCEA Chemistry: Core Knowledge Checklist | Year 13 CCEA 化学：核心知识点梳理

📚 Year 13 CCEA Chemistry: Core Knowledge Checklist | Year 13 CCEA 化学：核心知识点梳理

This revision guide outlines the essential topics in the AS-level CCEA Chemistry specification. It covers atomic theory, bonding, energetics, kinetics, equilibrium, inorganic trends, organic chemistry and spectroscopy. Use it alongside past papers and your class notes to consolidate understanding.

这份复习指南梳理了 CCEA 化学 AS 阶段的必考知识点，涵盖原子理论、化学键、能量学、动力学、平衡、无机规律、有机化学和光谱分析。请结合真题和课堂笔记，巩固理解。

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1. Atomic Structure and Electron Configuration | 原子结构与电子排布

Atoms consist of a tiny, dense nucleus containing protons and neutrons, surrounded by electrons arranged in shells and orbitals.

原子由一个致密的小原子核（含质子和中子）和分层排布的电子组成。

The atomic number (Z) is the number of protons; the mass number (A) is protons + neutrons.

相对质量：质子 ≈ 1，中子 ≈ 1，电子 ≈ 1/1836。原子序数 (Z) 是质子数；质量数 (A) 是质子数 + 中子数。

Electrons occupy orbitals in the order 1s, 2s, 2p, 3s, 3p, 4s, 3d. The 4s orbital fills before 3d, and empties before 3d when forming ions.

电子按顺序占据轨道：1s, 2s, 2p, 3s, 3p, 4s, 3d。填充时 4s 先于 3d，形成离子时 4s 先失去电子。

Shorthand electron configurations use the nearest noble gas core. For example, Fe: [Ar] 4s² 3d⁶, Fe²⁺: [Ar] 3d⁶.

电子排布简写使用最近的稀有气体核心。如 Fe: [Ar] 4s² 3d⁶；Fe²⁺: [Ar] 3d⁶。

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2. Bonding and Intermolecular Forces | 化学键与分子间作用力

Ionic bonding involves electron transfer between a metal and a non-metal, forming a giant ionic lattice with strong electrostatic attraction between oppositely charged ions.

离子键是金属与非金属之间的电子转移，形成带相反电荷的离子间强静电吸引的巨型离子晶格。

Covalent bonding is the sharing of electron pairs between non-metal atoms. Dative covalent bonds occur when one atom provides both electrons.

共价键是非金属原子间共用电子对。配位共价键是其中一个原子提供孤对电子而形成的。

Electronegativity is the power of an atom to attract the bonding pair of electrons. A difference >1.7 often leads to ionic bonding, while a difference of 0–1.7 leads to polar covalent bonding.

电负性是原子吸引共用电子对的能力。差值大于 1.7 通常形成离子键，0–1.7 形成极性共价键。

Intermolecular forces: London dispersion forces exist in all molecules; permanent dipole–dipole interactions occur in polar molecules; hydrogen bonding occurs when H is bonded to N, O or F.

分子间作用力：所有分子都有伦敦色散力；极性分子存在永久偶极-偶极作用；氢键存在于与 N、O 或 F 相连的氢上。

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3. Shapes of Molecules and Ions | 分子与离子的形状

Valence-shell electron-pair repulsion (VSEPR) theory states that electron pairs around a central atom repel each other and arrange as far apart as possible.

价层电子对互斥理论 (VSEPR) 指出，中心原子周围的电子对互相排斥，尽可能远离。

Common shapes: 2 bonding pairs – linear (180°); 3 bonding pairs – trigonal planar (120°); 4 bonding pairs – tetrahedral (109.5°); 2 bonding + 2 lone pairs – bent (104.5°); 3 bonding + 1 lone pair – trigonal pyramidal (107°).

常见形状：2 对成键电子——直线型 (180°)；3 对——平面三角形 (120°)；4 对——四面体形 (109.5°)；2 对成键 + 2 对孤对电子——弯曲形 (104.5°)；3 对成键 + 1 对孤对电子——三角锥形 (107°)。

Lone pairs repel more strongly than bonding pairs, reducing bond angles.

孤对电子的排斥力强于成键电子，会使键角减小。

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4. Redox Reactions and Oxidation Numbers | 氧化还原反应与氧化数

Oxidation is loss of electrons; reduction is gain of electrons. These always occur together in redox reactions.

氧化是失去电子，还原是得到电子。两者总是同时发生，称为氧化还原反应。

Oxidation numbers are assigned using rules: free elements = 0; oxygen in compounds = – cept peroxides); hydrogen = +1 (except metal hydrides); the sum equals the overall charge.

氧化数规则：游离态元素为 0；化合物中氧通常为 –2（过氧化物除外）；氢为 +1（金属氢化物除外）；元素氧化数总和等于所带电荷。

An increase in oxidation number is oxidation; a decrease is reduction. Oxidising agents are reduced; reducing agents are oxidised.

氧化数升高是氧化，降低是还原。氧化剂本身被还原，还原剂本身被氧化。

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5. The Mole and Stoichiometry | 摩尔与化学计量

the SI unit for amount of substance, containing 6.02 × 10²³ particles (Avogadro’s number).

摩尔是物质的量的单位，1 mol 物质含有 6.02 × 10²³ 个粒子（阿伏伽德罗常数）。

n = m / M, c = n / V, n = V / 24 dm³ (at RTP)

Key equations link mass (m), molar mass (M), concentration (c), volume (V) and molar gas volume (24 dm³ mol⁻¹ at RTP).

关键公式联立了质量 (m)、摩尔质量 (M)、浓度 (c)、体积 (V) 以及室温常压下气体摩尔体积 (24 dm³ mol⁻¹)。

Empirical formula is the simplest whole‑number ratio; molecular formula is the actual number of atoms. Calculate them from composition data.

实验式是最简整数比，分子式表示实际原子数目。通过组成数据可以计算两者。

Reacting mass calculations follow balanced equations and ratios of moles.

反应质量计算依据配平方程式和各物质的摩尔比。

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6. Energetics: Enthalpy Changes | 能量学：焓变

Enthalpy change (ΔH) is the heat energy transferred under constant pressure. Exothermic reactions release heat (ΔH negative); endothermic reactions absorb heat (ΔH positive).

焓变 (ΔH) 是恒压下的热传递。放热反应放出热量（ΔH 为负）；吸热反应吸收热量（ΔH 为正）。

q = m c ΔT, ΔH = –q / n

Calorimetry uses q = m c ΔT to calculate heat exchange, then ΔH = –q / n (where n is moles of limiting reactant).

量热法采用 q = m c ΔT 计算热量变化，再根据 ΔH = –q / n 求焓变（n 为限制反应物的物质的量）。

Standard enthalpy changes: ΔH° of formation, combustion, neutralisation and reaction. Hess’s law states that ΔH is independent of the pathway taken.

标准焓变包括标准生成焓、燃烧焓、中和焓和反应焓。盖斯定律指出，焓变与路径无关。

Mean bond enthalpies can be used to estimate ΔH, but they are averages and less accurate for specific molecules.

平均键焓可用于估算 ΔH，但它是平均值，对特定分子不够精确。

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7. Kinetics: Rates of Reaction | 动力学：反应速率

n collision frequency and the fraction of collisions with energy ≥ activation energy (Eₐ).

反应速率取决于碰撞频率以及能量大于等于活化能 (Eₐ) 的碰撞比例。

Maxwell– distribution shows the spread of molecular energies. Only molecules with E ≥ Eₐ can react.

麦克斯韦–玻尔兹曼分布展示了分子能量的分布情况。只有能量达到或超过 Eₐ 的分子才能反应。

temperature increases the proportion of molecules with E ≥ Eₐ, raising rate dramatically.

升高温度会增加能量达到活化能的分子比例，显著加快反应速率。

Increasing concentration, pressure (for gases) or surface area (for solids) increases collision frequency, thus elevating rate.

提高浓度、压强（对气体）或增大固体表面积会增加碰撞频率，从而加快反应速率。

Catalysts provide an alternative pathway with lower activation energy, increasing the proportion of effective collisions without being consumed.

催化剂提供一条活化能更低的反应路径，增加有效碰撞的比例，而本身不被消耗。

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8. Chemical Equilibrium | 化学平衡

Dynamic equilibrium occurs in a closed system when the forward and reverse reactions proceed at the same rate, with constant macroscopic properties.

动态平衡发生在封闭系统中，正逆反应速率相等，宏观性质恒定。

Le Chatelier’s principle: if a system at equilibrium is subjected to a change in concentration, temperature or pressure, the position of equilibrium shifts to oppose the change.

勒夏特列原理：如果改变平衡系统的浓度、温度或压强，平衡将向削弱该改变的方向移动。

For exothermic reactions, increasing temperature shifts equilibrium towards reactants; for endothermic, towards products.

放热反应升温时，平衡向反应物方向移动；吸热反应升温则向产物方向移动。

Catalysts do not affect the position of equilibrium; they only speed up the attainment of equilibrium.

催化剂不影响平衡位置，仅加快达到平衡的速率。

cts] / [reactants], raised to appropriate stoichiometric coefficients. Kc is constant at a given temperature.

平衡常数 Kc = [产物] / [反应物]，各浓度以方程式中系数为指数。Kc 在温度一定时为常数。

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9. Group 2 and Group 7 Chemistry | 第2族和第7族化学

Group 2 elements (Be–Ba) are reducing agents, losing two electrons to form M²⁺ ions. Reactivity increases down the group due to decreasing ionisation energy.

第2族元素（铍至钡）是还原剂，失去两个电子形成 M²⁺ 离子。自上而下电离能降低，反应活性增强。

Group 2 oxides and hydroxides are basic; solubility of hydroxides and sulfates shows opposite trends: hydroxide solubility increases down the group, sulfate solubility decreases.

第2族氧化物和氢氧化物显碱性；氢氧化物溶解度自上而下增大，硫酸盐溶解度自上而下减小。

Group 7 (halogens) exist as diatomic molecules. Reactivity decreases down the group as atomic radius increases and electronegativity falls.

第7族（卤素）以双原子分子存在。自上而下原子半径增大、电负性下降，反应活性减弱。

more reactive halogen displaces a less reactive halide ion, e.g. Cl₂ + 2Br⁻ → 2Cl⁻ + Br₂.

卤素是氧化剂。较活泼的卤素能置换较不活泼的卤离子，例如 Cl₂ + 2Br⁻ → 2Cl⁻ + Br₂。

Halide ions are reducing agents; reducing power increases down the group. Concentrated sulfuric acid reactions with NaBr and NaI produce bromine and iodine, along with reduction products like SO₂ and H₂S.

卤离子是还原剂，还原性自上而下增强。浓硫酸与 NaBr 和 NaI 反应生成溴和碘，同时生成 SO₂、H₂S 等还原产物。

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10. Introduction to Organic Chemistry: Alkanes and Alkenes | 有机化学入门：烷烃与烯烃

Organic compounds are based on carbon chains. Homologous series share the same functional group and a general formula, differing by CH₂ units.

有机化合物基于碳链。同系列具有相同的官能团和通式，相邻成员相差一个 CH₂。

Naming follows IUPAC conventions: identify the longest carbon chain, apply functional-group suffixes/prefixes, and number to give the lowest locants.

命名遵循 IUPAC 规则：选定最长碳链，使用官能团词尾/词头，以最低位序编号。

Alkanes undergo free‑radical substitution with halogens, initiated by UV light. The mechanism includes initiation, propagation and termination steps.

烷烃与卤素在紫外光下发生自由基取代反应，历经链引发、链增长和链终止步骤。

Alkenes contain a C=C double bond; they react by electrophilic addition. With H–X, the major product follows Markovnikov’s rule.

烯烃含有 C=C 双键，发生亲电加成反应。与 H–X 加成时，主要产物遵循马氏规则。

Addition of bromine (Br₂) to an alkene decolourises bromine water, a test for unsaturation.

烯烃与溴加成可使溴水褪色，这是不饱和键的检验方法。

Isomerism: structural isomers have different carbon skeletons or functional groups; E/Z (geometric) isomerism occurs in alkenes due to restricted rotation about the double bond.

同分异构：构造异构体具有不同碳骨架或官能团；烯烃因双键旋转受阻而产生 E/Z（几何）异构。

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11. Halogenoalkanes and Alcohols | 卤代烃与醇

Halogenoalkanes contain a polar C–X bond, making the carbon susceptible to nucleophilic attack. Undergo nucleophilic substitution with OH⁻, CN⁻ or NH₃.

卤代烃含有极性的 C–X 键，碳原子易受亲核试剂进攻，可与 OH⁻、CN⁻ 或 NH₃ 发生亲核取代反应。

Primary halogenoalkanes undergo S_N2 mechanism; tertiary halogenoalkanes prefer S_N1. Reaction rate depends on the strength of the C–X bond (C–I > C–Br > C–Cl).

伯卤代烃以 S_N2 机理进行，叔卤代烃倾向 S_N1。反应速率取决于 C–X 键强度 (C–I > C–Br > C–Cl)。

Elimination to form alkenes occurs with hot ethanolic KOH, in competition with substitution.

在热乙醇 KOH 作用下，卤代烃发生消除反应生成烯烃，与取代反应竞争。

Alcohols contain the –OH group. They are classified as primary, secondary or tertiary. Oxidation of primary alcohols yields aldehydes, then carboxylic acids; secondary alcohols give ketones; tertiary alcohols resist oxidation.

醇含有 –OH 官能团，可分为伯、仲、叔醇。伯醇氧化生成醛，进而生成羧酸；仲醇氧化成酮；叔醇不被氧化。

Alcohols can be dehydrated to alkenes using concentrated sulfuric acid or heated Al₂O₃.

醇可用浓硫酸或加热 Al₂O₃ 脱水生成烯烃。

Infrared spectroscopy identifies the –OH group by a broad peak around 3200–3600 cm⁻¹ (see Analytical Techniques).

红外光谱中，–OH 基团在 3200–3600 cm⁻¹ 附近呈现宽峰（参见分析技术节）。

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12. Analytical Techniques: IR and Mass Spectrometry | 分析技术：红外光谱与质谱

Infrared (IR) spectroscopy identifies functional groups by characteristic absorption frequencies due to bond vibrations.

红外光谱根据化学键振动产生的特征吸收频率来识别官能团。

Key absorptions: C=O (1650–1750 cm⁻¹), O–H (2500–3300 cm⁻¹ broad in carboxylic acids, 3200–3600 cm⁻¹ in alcohols), C–O (1000–1300 cm⁻¹), N–H (3300–3500 cm⁻¹).

关键吸收峰：C=O (1650–1750 cm⁻¹)，O–H (羧酸中 2500–3300 cm⁻¹ 宽峰，醇中 3200–3600 cm⁻¹)，C–O (1000–1300 cm⁻¹)，N–H (3300–3500 cm⁻¹)。

Mass spectrometry determines relative atomic/molecular mass. The molecular ion peak (M⁺) gives the relative molecular mass.

质谱可测定相对原子/分子质量。分子离子峰 (M⁺) 的质荷比即为相对分子质量。

Fragmentation patterns produce characteristic peaks that help deduce structure. The base peak is the most abundant fragment, set to 100% relative abundance.

碎片离子峰提供结构信息。基峰是最强的碎片峰，相对丰度定为 100%。

The M+1 peak arises from ¹³C isotope, and its intensity relates to the number of carbon atoms.

M+1 峰由 ¹³C 同位素引起，其强度可用于估算碳原子数。

High-resolution mass spectrometry can distinguish between molecules with the same nominal mass but different exact masses.

高分辨质谱能区分名义质量相同而精确质量不同的分子。

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