Cuprous ion (Cu^+) is colourless while cupric | vedclass

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(D) The electronic configuration of $Cu$ is $[Ar] 3d^{10} 4s^1$. For the cuprous ion $(Cu^+)$,the configuration is $[Ar] 3d^{10}$. Since the $d-$ orbi

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Cuprous ion has a complete $d-$ orbital and cupric ion has an incomplete $d-$ orbital

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(D) The electronic configuration of $Cu$ is $[Ar] 3d^{10} 4s^1$. For the cuprous ion $(Cu^+)$,the configuration is $[Ar] 3d^{10}$. Since the $d-$ orbital is completely filled,there are no unpaired electrons available for $d-d$ transition,making it colourless. For the cupric ion $(Cu^{2+})$,the configuration is $[Ar] 3d^9$. Since the $d-$ orbital is incompletely filled,it contains one unpaired electron,which allows for $d-d$ transition,making it coloured.

Cuprous ion $(Cu^+)$ is colourless while cupric ion $(Cu^{2+})$ is coloured because

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