GCSE Edexcel Chemistry: End-of-Term Revision Outline | GCSE Edexcel 化学：期末复习提纲

📚 GCSE Edexcel Chemistry: End-of-Term Revision Outline | GCSE Edexcel 化学：期末复习提纲

Welcome to your end-of-term revision outline for GCSE Edexcel Chemistry. This guide summarises the key topics you need to master, including atomic structure, bonding, quantitative chemistry, chemical changes, energy, rates, organic chemistry, analysis, the atmosphere, and resources. Use this outline to check your understanding and focus your revision.

欢迎查阅 GCSE Edexcel 化学期末复习提纲。本指南总结了你需要掌握的关键主题，包括原子结构、化学键、定量化学、化学变化、能量、反应速率、有机化学、化学分析、大气化学和资源利用。请使用本提纲检查你的理解并集中复习。

1. Atomic Structure and the Periodic Table | 原子结构与周期表

All substances are made of atoms. An atom contains a tiny nucleus with protons and neutrons, surrounded by electrons arranged in shells.

所有物质都由原子构成。原子包含一个极小的原子核，核内有质子和中子，核外电子分布在壳层中。

The atomic number (Z) is the number of protons, which determines the element. The mass number (A) is the total number of protons and neutrons.

原子序数(Z)是质子数，决定了元素种类。质量数(A)是质子和中子数的总和。

Isotopes are atoms of the same element with the same number of protons but different numbers of neutrons. They have the same chemical properties but different physical properties such as mass.

同位素是质子数相同但中子数不同的同种元素的原子。它们的化学性质相同，但物理性质（如质量）不同。

Electrons occupy shells (energy levels), and the electronic configuration for the first 20 elements follows the pattern 2,8,8,2.

电子占据壳层（能级），前20种元素的电子排布遵循2,8,8,2的模式。

The periodic table arranges elements in order of increasing atomic number. Groups (vertical columns) contain elements with similar chemical properties because they have the same number of outer-shell electrons.

周期表按原子序数递增的顺序排列元素。族（纵列）包含化学性质相似的元素，因为它们具有相同的最外层电子数。

Metals are on the left and centre, non-metals on the right. Metals tend to lose electrons to form positive ions; non-metals gain electrons to form negative ions.

金属位于左侧和中部，非金属位于右侧。金属容易失去电子形成阳离子；非金属容易得到电子形成阴离子。

2. Bonding, Structure and Properties of Matter | 物质的结构、键合与性质

Ionic bonding occurs between metals and non-metals. Electrons are transferred from the metal to the non-metal, forming oppositely charged ions that attract each other in a giant ionic lattice.

离子键形成于金属和非金属之间。电子从金属转移到非金属，形成带相反电荷的离子，这些离子在巨型离子晶格中相互吸引。

Covalent bonding occurs between non-metal atoms. Atoms share pairs of electrons to achieve a full outer shell. Covalent substances can exist as simple molecules (e.g. H₂O, CO₂) or giant covalent structures (e.g. diamond, silicon dioxide).

共价键形成于非金属原子之间。原子共用电子对以达到满壳层。共价物质可以是简单分子（如 H₂O, CO₂）或巨型共价结构（如金刚石、二氧化硅）。

Metallic bonding involves a lattice of positive ions surrounded by a sea of delocalised electrons. This explains the properties of metals: electrical conductivity, malleability, and ductility.

金属键涉及正离子晶格被离域电子的海洋所包围。这解释了金属的性质：导电性、延展性和韧性。

The physical properties of substances—melting point, boiling point, and electrical conductivity—depend on their structure and bonding type. For example, ionic compounds conduct electricity when molten or dissolved, while simple molecular substances do not.

物质的物理性质—熔点、沸点和导电性—取决于其结构和键合类型。例如，离子化合物在熔融或溶解时导电，而简单分子物质不导电。

3. Quantitative Chemistry | 定量化学

Relative atomic mass (Aᵣ) is the average mass of an atom compared to 1/12th of the mass of a carbon-12 atom. Relative formula mass (Mᵣ) is the sum of Aᵣ for all atoms in a formula.

相对原子质量(Aᵣ)是一个原子的平均质量与碳-12原子质量的1/12相比较的值。相对化学式量(Mᵣ)是化学式中所有原子Aᵣ的总和。

The mole is the unit for amount of substance. One mole contains 6.02 × 10²³ particles (Avogadro constant). The number of moles can be calculated using:

摩尔是物质的量的单位。一摩尔物质含有6.02 × 10²³ 个粒子（阿伏伽德罗常数）。摩尔数可用如下公式计算：

n = m ÷ Mᵣ

where n is the number of moles, m is mass in grams, and Mᵣ is the relative formula mass.

其中 n 是摩尔数，m 是质量（克），Mᵣ 是相对化学式量。

Concentration of a solution is measured in mol/dm³ or g/dm³ and can be found using c = n ÷ V (volume in dm³).

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