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Question

In which of the following compound(s), the colour is due to charge transfer spectra?

A
KMnO4
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B
CrO3
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C
CuCl2
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D
Cu2O
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Solution

The correct option is D Cu2O
In KMnO4, Mn has a oxidation state of +7 therefore doesn't have any electron in d orbital which implies there is no d-d transition in KMnO4 and colour will appear due to ligand to metal charge transfer spectra.
Similarly, in CrO3, Cr has a oxidation state of +6 therefore doesn't have any electron in d orbital which implies there is no d-d transition in CrO3 and colour will appear due to ligand to metal charge transfer spectra.

In case of CuCl2,Cu has a oxidation state of +2 and Cu has d9 electronic configuration and therefore d-d transition can take place.

In last option Cu2O has oxidation state of +1 which recommend d10 electronic configuration for Cu2O and therefore there is no d-d transition in Cu2O.
Hence colour is arised in A, B, D due to charge transfer spectra.

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