📚 Year 11 Eduqas Chemistry: Summer Bridging and Revision Course | Year 11 Eduqas 化学：暑期预习与衔接课程
This summer bridging course is designed for Year 11 students following the Eduqas GCSE Chemistry specification. It recaps essential Year 10 topics and introduces key Year 11 concepts, helping you to consolidate understanding and build confidence before the new academic year. Through clear explanations, worked examples, and practical tips, you will strengthen your knowledge across the core areas of chemistry.
本暑期衔接课程面向学习 Eduqas GCSE 化学的 Year 11 学生，复习巩固核心的 Year 10 内容，并介绍关键的 Year 11 概念，帮助你在新学期来临前加深理解、建立信心。通过清晰的讲解、计算示范和实用建议，你将全面强化化学核心领域的知识。
1. Atomic Structure Review and Extension | 原子结构回顾与拓展
Atoms consist of a small, dense nucleus containing protons and neutrons, surrounded by electrons arranged in energy levels (shells). The atomic number (Z) tells us the number of protons, which defines the element. The mass number (A) is the total number of protons and neutrons. Isotopes are atoms of the same element with different numbers of neutrons, hence different mass numbers. The electronic configuration of the first 20 elements follows the 2,8,8 pattern, with each shell holding a maximum number of electrons. The arrangement of electrons, particularly the outer shell, determines an element's chemical reactivity and bonding behaviour.
原子由一个致密的原子核和核外电子组成，原子核包含质子和中子。原子序数（Z） 表示质子数，决定了元素的种类；质量数（A） 为质子数和中子数之和。同位素是质子数相同但中子数不同的原子。前 20 号元素的电子排布遵循 2,8,8 的规律，每一层所能容纳的电子数有限。电子排布方式，尤其最外层的电子，决定了元素的化学活泼性和成键方式。
calculation of relative atomic mass (Aᵣ) from isotopic abundances. The formula is: Aᵣ = (% s number) / 100, summed over all isotopes. For example, chlorine has two main isotopes: 75% chlorine-35 and 25% in the Periodic Table and explain why elements in the same group have similar properties.
Year 11 的一个重要拓展是利用同位素丰度计算相对原子质量 (Aᵣ)。公式为：Aᵣ = (丰度百分比 × 质量数) 之和 ÷ 100。例如，氯元素有两种主要同位素：75% 的氯-35 和 25% 的氯-37，其 Aᵣ = (75×35 + 25×37) ÷ 100 = 35.5。你还应学会根据元素在周期表中的位置推断电子排布，并解释为什么同族元素性质相似。
2. The Periodic Table and Element Properties | 周期表与元素性质
The Periodic Table arranges elements in order of increasing atomic number. Rows are called periods and columns are called groups. Elements in the same group have the same number of outer-shell electrons and therefore similar chemical properties. Group 1 (alkali metals) are soft, low-density metals that react vigorously with water, forming metal hydroxides and hydrogen gas. Reactivity increases down the group because the outer electron is more easily lost as atomic radius increases and shielding increases.
周期表按原子序数递增排列。横行称为周期，纵列称为族。同族元素具有相同的最外层电子数，因此化学性质相似。第 1 族（碱金属）是质软、密度小的金属，能与水剧烈反应生成金属氢氧化物和氢气。从上到下反应性增强，因为随着原子半径增大和屏蔽效应增强，最外层电子越来越容易失去。
Group 7 (halogens) are diatomic non-metals. Their reactivity decreases down the group as it becomes harder to gain an electron. A more reactive halogen can displace a less reactive halide from its salt solution. Group 0 (noble gases) are monatomic and unreactive due to full outer electron shells. The transition metals, found in the middle of the table, form coloured compounds, have variable oxidation states and make good catalysts.
第 7 族（卤素）是双原子非金属单质。从上到下反应性减弱，因为获得电子的难度增加。活泼的卤素单质能把较不活泼的卤素从其盐溶液中置换出来。第 0 族（稀有气体）为单原子分子，因最外层电子已满而极不活泼。位于周期表中部的过渡金属常形成有色化合物，具有可变的氧化态，并常用作催化剂。
3. Chemical Bonding: Ionic, Covalent and Metallic | 化学键合：离子键、共价键与金属键
Ionic bonding occurs between metals and non-metals. Metal atoms lose electrons to form positive ions (cations), while non-metal atoms gain electrons to form negative ions (anions). The oppositely charged ions are held together by strong electrostatic forces in a giant ionic lattice. Ionic compounds have high melting and boiling points and can conduct electricity when molten or dissolved in water because the ions become free to move. The empirical formula shows the simplest whole-number ratio of ions, e.g. NaCl, MgO, CaCl₂.
离子键形成于金属和非金属之间。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。在庞大的离子晶格中，带相反电荷的离子通过强静电引力结合在一起。离子化合物具有较高的熔沸点，在熔融或溶于水时能够导电，因为此时离子可以自由移动。其化学式表示离子的最简整数比，如 NaCl、MgO、CaCl₂。
Covalent bonding involves non-metal atoms sharing pairs of electrons to achieve noble gas configurations. Simple molecular substances (e.g. H₂O, CO₂, O₂) consist of small molecules with weak intermolecular forces, resulting in low melting and boiling points and no electrical conductivity. Giant covalent structures, such as diamond and silicon dioxide (SiO₂), have extensive networks of strong covalent bonds and therefore extremely high melting points. Graphite is a giant covalent structure in which each carbon atom is bonded to three others, forming layers that can slide over each other; delocalised electrons between the layers allow graphite to conduct electricity.
共价键由非金属原子通过共享电子对以达到稀有气体的稳定电子结构。简单分子物质（如 H₂O、CO₂、O₂）由小分子组成，分子间作用力微弱，因此熔沸点低，不导电。巨型共价结构，如金刚石和二氧化硅 (SiO₂)，拥有由强共价键构成的巨大网络，熔点极高。石墨也是一种巨型共价结构，每个碳原子与另外三个碳原子键合，形成可滑动的层状结构；层间存在离域电子，因此石墨能够导电。
Metallic bonding is the electrostatic attraction between positive metal ions and a 'sea' of delocalised electrons. This structure
Published by TutorHao | Year 11 Chemistry Revision Series | aleveler.com
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