📚 AQA A-Level Chemistry 1.3 Bonding: Structure, Polarity and Intermolecular Forces | AQA 化学 1.3 键合：结构、极性与分子间作用力
In AQA A-Level Chemistry, topic 1.3 Bonding explains how atoms, ions and molecules are held together. You need to link the type of bonding to structure, physical properties, shapes and intermolecular forces. This revision guide covers ionic, covalent and metallic bonding, electronegativity, polarity, shapes of molecules and the intermolecular forces that determine melting and boiling points.
在 AQA A-Level 化学中，1.3 键合一章解释原子、离子和分子如何结合在一起。你需要把键合类型与结构、物理性质、分子形状和分子间作用力联系起来。本复习指南涵盖离子键、共价键和金属键，电负性、极性、分子形状以及决定熔点和沸点的分子间作用力。
1. Types of Bonding Overview | 键合类型总览
There are three main types of strong chemical bonding: ionic, covalent and metallic. Ionic bonding occurs between metals and non-metals, covalent bonding usually occurs between non-metals, and metallic bonding occurs between metal atoms.
化学键主要有三种强键合类型：离子键、共价键和金属键。离子键通常形成于金属与非金属之间，共价键通常形成于非金属之间，金属键形成于金属原子之间。
The type of bonding and structure determines physical properties such as melting point, boiling point, electrical conductivity and solubility. You must be able to explain these properties by referring to the particles present and the forces between them.
键合类型和结构决定物理性质，如熔点、沸点、导电性和溶解性。你必须能够通过所存在的粒子以及它们之间的作用力来解释这些性质。
In addition to strong bonds, there are weak intermolecular forces between simple molecules. These weak forces must not be confused with covalent bonds inside a molecule.
除了强键之外，简单分子之间还存在弱的分子间作用力。这些弱作用力不能与分子内部的共价键混淆。
2. Ionic Bonding | 离子键
Ionic bonding is the electrostatic attraction between oppositely charged ions. It forms when a metal atom transfers one or more electrons to a non-metal atom.
离子键是带相反电荷离子之间的静电吸引力。当金属原子将一个或多个电子转移给非金属原子时形成。
The metal loses electrons to form a positive cation, such as Na⁺ or Mg²⁺. The non-metal gains electrons to form a negative anion, such as Cl⁻ or O²⁻.
金属失去电子形成阳离子，如 Na⁺ 或 Mg²⁺。非金属得到电子形成阴离子，如 Cl⁻ 或 O²⁻。
Na → Na⁺ + e⁻
Cl + e⁻ → Cl⁻
Na⁺ + Cl⁻ → NaCl
Ionic compounds form a giant ionic lattice in which each ion is surrounded by oppositely charged ions. The strong electrostatic forces act in all directions, giving high melting and boiling points.
离子化合物形成巨型离子晶格，每个离子被带相反电荷的离子包围。强大的静电作用力在所有方向上起作用，因此熔点和沸点很高。
Ionic compounds do not conduct electricity when solid because the ions cannot move. They conduct when molten or dissolved in water because the ions are free to move and carry charge.
离子化合物在固态时不导电，因为离子不能移动。它们在熔融或溶于水时导电，因为离子可以自由移动并携带电荷。
3. Covalent Bonding and Dative Covalent Bonds | 共价键与配位共价键
Covalent bonding is the electrostatic attraction between the shared pair of electrons and the positive nuclei of the bonded atoms. It usually forms between two non-metal atoms.
共价键是共用电子对与成键原子正原子核之间的静电吸引力。它通常形成于两个非金属原子之间。
A single covalent bond contains one shared pair of electrons, a double bond contains two shared pairs, and a triple bond contains three shared pairs. Examples include Cl₂, O₂ and N₂.
单键含有一对共用电子，双键含有两对共用电子，三键含有三对共用电子。例子包括 Cl₂、O₂ 和 N₂。
A dative covalent bond, also called a coordinate bond, forms when both electrons in the shared pair come from one atom. The ammonium ion NH₄⁺ and the hydronium ion H₃O⁺ contain dative covalent bonds.
配位共价键，又称 dative covalent bond，当共用电子对中的两个电子都来自同一个原子时形成。铵根离子 NH₄⁺ 和水合氢离子 H₃O⁺ 含有配位共价键。
Simple covalent molecules have strong covalent bonds inside the molecule, but weak intermolecular forces between molecules. This causes low melting and boiling points.
简单共价分子内部有强共价键，但分子之间有弱的分子间作用力。因此熔点、沸点较低。
4. Metallic Bonding | 金属键
Metallic bonding is the electrostatic attraction between positive metal ions and the delocalised electrons in a metallic lattice.
金属键是金属晶格中正金属离子与离域电子之间的静电吸引力。
The metal atoms lose their outer electrons to form a lattice of positive ions. These outer electrons become delocalised and are free to move throughout the structure.
金属原子失去外层电子，形成正离子晶格。这些外层
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