Assertion : Cuprous ion (Cu^+) has unpaired e | vedclass

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(D) The electronic configuration of $Cu$ $(Z=29)$ is $[Ar] 3d^{10} 4s^1$.For $Cu^+$ $(Cu^+)$,the configuration is $[Ar] 3d^{10}$,which has no unpaired

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If both the Assertion and Reason are incorrect.

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(D) The electronic configuration of $Cu$ $(Z=29)$ is $[Ar] 3d^{10} 4s^1$.For $Cu^+$ $(Cu^+)$,the configuration is $[Ar] 3d^{10}$,which has no unpaired electrons.For $Cu^{2+}$ $(Cu^{2+})$,the configuration is $[Ar] 3d^9$,which has one unpaired electron.Therefore,the Assertion is incorrect because $Cu^+$ has no unpaired electrons,while $Cu^{2+}$ has one.Regarding the Reason,$Cu^+$ is indeed colourless due to the absence of unpaired electrons ($d^{10}$ configuration),and $Cu^{2+}$ is blue due to $d-d$ transitions facilitated by the presence of an unpaired electron.Since the Assertion is incorrect but the Reason is correct,the correct option is $D$.

Assertion : Cuprous ion $(Cu^+)$ has unpaired electrons while cupric ion $(Cu^{2+})$ does not.
Reason : Cuprous ion $(Cu^+)$ is colourless whereas cupric ion $(Cu^{2+})$ is blue in the aqueous solution.

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Assertion : Cuprous ion $(Cu^+)$ has unpaired electrons while cupric ion $(Cu^{2+})$ does not.Reason : Cuprous ion $(Cu^+)$ is colourless whereas cupric ion $(Cu^{2+})$ is blue in the aqueous solution.