📚 Year 11 OCR Chemistry: Core Topics Checklist | Year 11 OCR 化学：核心知识点梳理
Welcome to the Year 11 OCR GCSE Chemistry revision guide. This article provides a comprehensive overview of the core topics, from atomic structure and bonding to organic chemistry and chemical analysis. Each section is presented with concise explanations in both English and Chinese, ensuring clarity and support for bilingual learners. Use this checklist to reinforce your knowledge and prepare effectively for your exams.
本文全面梳理了 Year 11 OCR GCSE 化学的核心知识点，涵盖从原子结构、化学键到有机化学和化学分析的关键概念。每个小节均以中英双语简明解释，帮助双语学习者巩固理解、高效备考。通过本文复习，你可以系统掌握考点，自如应对考试。
The checklist follows the OCR specification order and highlights the definitions, equations, practical tests and calculations that examiners return to again and again. Read each pair of paragraphs, then try to reproduce the key facts from memory before moving on to the next section.
本清单按照 OCR 考纲顺序编排，重点标出考官反复考查的定义、方程式、实验检验与计算。建议先读中英对照段落，再合上页面回忆关键事实，确认掌握后再进入下一节。
1. Atomic Structure and the Periodic Table | 原子结构与周期表
Atoms are composed of protons (p⁺), neutrons (n⁰), and electrons (e⁻). The nucleus contains protons and neutrons, where most of the mass is concentrated, while electrons occupy shells around the nucleus. A proton has a relative mass of 1 and a charge of +1; a neutron has a relative mass of 1 and no charge; an electron has a negligible mass (about 1/1836) and a charge of -1.
原子由质子(p⁺)、中子(n⁰)和电子(e⁻)构成。原子核内有质子和中子，集中了大部分质量，电子则分层排布在核外。质子相对质量为1，带+1电荷；中子相对质量为1，不带电；电子质量极小（约1/1836），带-1电荷。
| Particle 粒子 | Relative mass 相对质量 | Charge 电荷 | Location 位置 |
| Proton 质子 p⁺ | 1 | +1 | Nucleus 原子核 |
| Neutron 中子 n⁰ | 1 | 0 | Nucleus 原子核 |
| Electron 电子 e⁻ | 1/1836 (negligible 可忽略) | -1 | Shells 电子壳层 |
The atomic number (Z) equals the number of protons and defines the element. The mass number (A) is the total number of protons and neutrons. Isotopes are atoms of the same element with the same atomic number but different mass numbers. Electrons fill shells in the order 2, 8, 8 for the first three periods.
原子序数(Z)等于质子数，决定了元素种类。质量数(A)是质子数与中子数之和。同位素是质子数相同而中子数不同的原子。电子按2、8、8的规律排布前三层电子壳。
Z = 质子数 = 电子数 A = Z + n⁰ 相对原子质量 = Σ(同位素丰度 × 同位素质量)
The periodic table arranges elements by increasing atomic number. Elements in the same group have the same number of outer electrons and therefore similar chemical properties. Group 1 metals are very reactive, Group 7 halogens are diatomic non-metals, and Group 0 noble gases are unreactive because they have full outer shells.
周期表按原子序数递增排列元素。同一主族元素最外层电子数相同，因此化学性质相似。第1族金属非常活泼，第7族卤素是双原子非金属，第0族稀有气体最外层电子已排满，因而性质稳定不活泼。
Electron configuration examples worth memorising: sodium 2,8,1; chlorine 2,8,7; calcium 2,8,8,2. The group number gives the number of outer electrons and the period number gives the number of shells.
必须记住的电子排布示例：钠 2,8,1；氯 2,8,7；钙 2,8,8,2。主族序数等于最外层电子数，周期数等于电子层数。
2. Ionic Bonding and Ionic Compounds | 离子键与离子化合物
Ionic bonding happens between metals and non-metals. Electrons are transferred from the metal atom to the non-metal atom, producing positive and negative ions. The bond itself is the strong electrostatic attraction between oppositely charged ions, acting in all directions.
离子键发生在金属与非金属之间。金属原子的电子转移给非金属原子，形成正离子和负离子。离子键的实质是带相反电荷的离子之间强烈的静电引力，这种引力在各个方向同时存在。
Dot-and-cross diagrams show the outer shell electrons only. The charge on an ion can be predicted from its group: Group 1 gives 1+, Group 2 gives 2+, Group 6 gives 2⁻ and Group 7 gives 1⁻. Sodium chloride, magnesium oxide and calcium chloride are typical examples.
点叉图只画出最外层电子。离子电荷可由族序数推断：第1族形成 1+，第2族形成 2+，第6族形成 2⁻，第7族形成 1⁻。氯化钠、氧化镁和氯化钙是典型例子。
Na → Na⁺ + e⁻ Cl + e⁻ → Cl⁻ Mg²⁺ + O²⁻ → MgO
Ionic compounds form giant ionic lattices. They have high melting and boiling points because many strong electrostatic forces must be overcome. They do not conduct electricity when solid because the ions cannot move, but they do conduct when molten or dissolved in water, since the ions become free to move. Most ionic compounds are soluble in water.
离子化合物形成巨型离子晶格，熔点和沸点较高，因为
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