AS Chemistry: Coordination Chemistry Key Points | AS 化学：配位化学 考点精讲

📚 AS Chemistry: Coordination Chemistry Key Points | AS 化学：配位化学 考点精讲

Transition metals form a fascinating array of complex ions and compounds due to their ability to form dative covalent bonds with ligands. Understanding coordination chemistry is essential for mastering topics such as colour, isomerism, and reactivity in AS Chemistry. This article provides a focused revision of key concepts, common pitfalls, and exam strategies to help you excel.

过渡金属由于其能与配体形成配位键，可生成一系列迷人的配离子和配合物。理解配位化学对于掌握 AS 化学中的颜色、异构现象和反应性等主题至关重要。本文针对考点进行重点梳理，包括核心概念、常见误区和考试策略，助你取得优异成绩。

1. Introduction to Transition Metals | 过渡金属简介

A transition metal is defined as an element that forms at least one stable ion with a partially filled d-subshell. Common examples include iron (Fe), copper (Cu), and chromium (Cr). This partial filling of d-orbitals gives rise to characteristic properties such as variable oxidation states, catalytic activity, and the formation of coloured compounds.

过渡金属的定义是：能形成至少一种具有部分填充 d 亚层的稳定离子的元素。常见例子有铁(Fe)、铜(Cu)和铬(Cr)。d 轨道的部分填充导致了其典型性质，如可变氧化态、催化活性及形成有色化合物。

In AS Chemistry, the focus is on the first row of the d-block: Sc to Zn. However, scandium and zinc are not transition metals under this definition because Sc³⁺ has an empty d-subshell ([Ar]) and Zn²⁺ has a full d-subshell ([Ar]3d¹⁰). Thus, they do not exhibit typical transition metal properties.

在 AS 化学中，重点放在 d 区第一行：Sc 到 Zn。然而，根据定义，钪和锌不属于过渡金属，因为 Sc³⁺ 的 d 亚层为空([Ar])，而 Zn²⁺ 的 d 亚层全满([Ar]3d¹⁰)。因此，它们并不表现典型的过渡金属性质。

2. The Nature of Dative Covalent Bonds | 配位键的本质

In a coordination complex, the bond between the central metal ion and a ligand is a dative covalent bond (also called a coordinate bond). Both electrons in the bond are donated by the ligand to the empty orbitals of the metal ion. The metal ion acts as a Lewis acid (electron pair acceptor), and the ligand acts as a Lewis base (electron pair donor).

在配合物中，中心金属离子与配体之间的键为配位键（也称配位共价键）。键中的两个电子均由配体提供，进入金属离子的空轨道。金属离子充当路易斯酸（电子对接受体），配体充当路易斯碱（电子对给予体）。

For example, when ammonia (NH₃) coordinates to Cu²⁺, the lone pair on nitrogen is donated to the copper ion, forming [Cu(NH₃)₄]²⁺. The overall charge of a complex ion is the sum of the metal ion’s oxidation state and the charges on the ligands.

例如，当氨(NH₃)与 Cu²⁺ 配位时，氮原子上的孤对电子给予铜离子，形成 [Cu(NH₃)₄]²⁺。配离子的总电荷是金属离子氧化态与配体电荷的代数和。

3. Ligands: Monodentate, Bidentate and Polydentate | 配体：单齿、双齿和多齿配体

Ligands are classified by the number of donor atoms they use to bond to the central metal ion. Monodentate ligands bind through one donor atom; examples include H₂O:, NH₃, and Cl⁻. Bidentate ligands have

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