Explain: the compounds of copper (II) are colored but those of zinc are colorless?

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Explain: the compounds of copper (II) are colored but those of zinc are colorless?

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Answer 1 · 2017-08-13T16:22:43

You have a $d^9$ electronic configuration in the case of $Cu(+II)$ ..

Explanation:

...and you gots a $d^10$ electronic configuration in the case of $Zn(+II)$ .. $Cu(+II)$ has a $d^9$ electronic configuration, and the colours exhibited by transition metal complexes are in part due to $d-d$ transitions (i.e. the energy difference in orbital configuration corresponds to the visible region). These electronic transitions are not available to the $Zn(+II)$ complex, whose $"d-orbitals"$ are completely filled.

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Explain: the compounds of copper (II) are colored but those of zinc are colorless?

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