[CuCl2]- why is this ion colourless?

hiky

Any help greatly appreciated
Thank you

Reply 1

charco

Study Forum Helper

The copper atom is in the +1 oxidation state in which it has a full (totally occupied) set of 'd' orbitals. There can be no transitions between the non-degenerate orbitals and so there can be no frequencies of light absorbed due to d-d transitions.

Reply 2

Nichrome

That is true for CuCl. But CuCl2 is green no? :p:

Reply 3

charco

Study Forum Helper

Nichrome

That is true for CuCl. But CuCl2 is green no? :p:

CuCl2 does not have a full set of 'd' orbitals is has a d9 configuration becuase the copper atom is in the (II) oxidation state and transitions can happen to absorb light.

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