transition metals electron configuration
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Copper is one of the few period 4 transition metals to form a +1 oxidation state. Explain why in terms of its electron configuration
Cu [Ar] 4s1 3d10 Has 1 electron in the 4s sub-shell that can be lost. Most transition metals have 2
Write the full electron configuration for Sc and Sc3+ The definition of a transition metal is that it forms at least 1 stable ion with an incomplete d sub-shell. Use this to explain why Sc does not have typical properties of a transition metal
Sc [Ar] 4s2 3d1 Sc3+ [Ar] 4s0 3d0 Does not form an ion with an incomplete d sub-shell
Write the full electron configuration for Fe2+ and Fe3+. Use these to predict and explain which oxidation state of iron is more stable
Fe2+ [Ar] 4s0 3d6 Fe3+ [Ar] 4s0 3d5 Fe3+ has a half filled d sub-shell (no electrons are paired in an orbital) this is more stable
Zinc only forms a Zn2+ ion and is resistant to further reduction. Explain why in terms of its electron configuration
Zn2+ [Ar] 4s0 3d10 Completely filled 3d sub-shell is more stable
Zinc does not form coloured compounds. Explain why in terms of its electron configuration
Requires a partially filled 3d sub-shell (to absorb photons in the visible part of the spectrum). Zn has 3d10 electron configuration (full)