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This lesson covers the properties of d-block elements, including variable oxidation states, coloured ions, complex ion formation, ligand substitution, catalysis, isomerism in complex ions, precipitation reactions for identifying ions, redox titrations, and colourimetry. The transition metals exhibit unique chemistry due to the involvement of their partially filled d orbitals. This material aligns with the AQA and OCR A specifications for A-Level Chemistry.
Key Definition: A transition metal is a d-block element that forms at least one stable ion with a partially filled d sub-shell.
Note that scandium (Sc) and zinc (Zn) are d-block elements but are not transition metals by this definition — Sc³⁺ has an empty d sub-shell (3d⁰) and Zn²⁺ has a full d sub-shell (3d¹⁰). Copper is a transition metal because, although Cu⁺ has 3d¹⁰ (full), Cu²⁺ has 3d⁹ (partially filled).
Transition metals share several characteristic properties, all arising from the involvement of the partially filled 3d sub-shell:
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