📚 Year 12 CCEA Chemistry: Core Knowledge Review | 12年级CCEA化学：核心知识点梳理
Year 12 CCEA Chemistry lays the foundation for A-level understanding by covering core physical, inorganic, and organic topics. This revision guide summarises essential concepts, from atomic structure and bonding to energetics, kinetics, equilibrium, redox, and organic chemistry, along with analytical techniques. Mastering these fundamentals is crucial for success in the AS units and beyond.
12年级CCEA化学通过涵盖核心的物理化学、无机化学和有机化学主题，为A-level学习打下基础。本复习指南总结了从原子结构、化学键合到能量学、动力学、平衡、氧化还原和有机化学以及分析技术的关键概念。掌握这些基础知识对于成功应对AS单元及更深入的学习至关重要。
1. Atomic Structure and the Periodic Table | 原子结构与周期表
Atoms consist of a nucleus containing protons (Z) and neutrons, surrounded by electrons in energy levels. The atomic number (Z) defines the element, while the mass number (A) is the sum of protons and neutrons. Isotopes are atoms of the same element with different numbers of neutrons.
原子由包含质子（Z）和中子的原子核以及分布在能级上的电子组成。原子序数（Z）定义了元素，而质量数（A）是质子与中子数之和。同位素是同一元素中具有不同中子数的原子。
Electrons occupy shells and subshells (s, p, d). The first ionisation energy is the energy required to remove one mole of electrons from one mole of gaseous atoms. Trends across a period (general increase) and down a group (decrease) are explained by nuclear charge, shielding, and atomic radius.
电子占据电子层和亚层（s、p、d）。第一电离能是从一摩尔气态原子中移除一摩尔电子所需的能量。周期内（总体增加）和族内（递减）的趋势可用核电荷、屏蔽效应和原子半径来解释。
Atomic radius decreases across a period and increases down a group. Electronegativity increases across a period and decreases down a group. Successive ionisation energies provide evidence for electron shells.
原子半径在同一周期内减小，在同一族内增大。电负性在周期内增大，在族内减小。逐级电离能为电子层的存在提供了证据。
2. Chemical Bonding and Structure | 化学键合与结构
Ionic bonding is the electrostatic attraction between oppositely charged ions, formed when metals transfer electrons to non-metals. Ionic compounds have high melting points, conduct electricity when molten or in solution, and form giant ionic lattices.
离子键是带相反电荷离子之间的静电吸引力，在金属向非金属转移电子时形成。离子化合物具有高熔点，在熔融或溶液状态下可导电，并形成巨型离子晶格。
Covalent bonding involves the sharing of electron pairs between non-metal atoms. Molecules can be simple (e.g., H₂O, CO₂) or giant covalent (e.g., diamond, graphite). Metallic bonding is the attraction between positive metal ions and delocalised electrons, explaining malleability and conductivity.
共价键涉及非金属原子之间共用电子对。分子可以是简单分子（如H₂O、CO₂）或巨型共价结构（如金刚石、石墨）。金属键是正金属离子与自由电子之间的吸引力，解释了金属的展性和导电性。
Intermolecular forces include London (dispersion) forces, permanent dipole–dipole interactions, and hydrogen bonding. Hydrogen bonding, found in molecules containing H bonded to N, O, or F, strongly influences boiling points and solubility.
分子间力包括伦敦（色散）力、永久偶极-偶极相互作用和氢键。氢键存在于含有与N、O或F键合的氢原子的分子中，对沸点和溶解度有显著影响。
3. Stoichiometry and the Mole Concept | 化学计量与摩尔概念
The mole is the amount of substance containing Avogadro's number (6.02 × 10²³) of particles. Molar mass (g mol⁻¹) links mass to number of moles.
摩尔是包含阿伏伽德罗常数（6.02 × 10²³）个微粒的物质的量。摩尔质量（g mol⁻¹）将质量与物质的量联系起来。
n = m / M, c = n / V, V(gas
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