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

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

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If the Assertion is incorrect but the Reason is correct.

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(D) The electronic configuration of $Cu$ is $[Ar] 3d^{10} 4s^1$.For $Cu^{+}$ (cuprous ion),the configuration is $[Ar] 3d^{10}$,which has no unpaired electrons.For $Cu^{2+}$ (cupric ion),the configuration is $[Ar] 3d^9$,which has one unpaired electron.Therefore,the Assertion is incorrect because it states the opposite.$Cu^{+}$ is colourless due to the absence of unpaired electrons,while $Cu^{2+}$ is blue in aqueous solution due to $d-d$ transitions in the presence of water ligands. Thus,the Reason is correct.The correct option is $D$.

List-$I$	List-$II$
$(1) \ \text{Cr}$	$(A) \ [\text{Ar}] \ 3d^8 4s^0$
$(2) \ \text{Fe}^{2+}$	$(B) \ [\text{Ar}] \ 3d^{10} 4s^1$
$(3) \ \text{Ni}^{2+}$	$(C) \ [\text{Ar}] \ 3d^6 4s^0$
$(4) \ \text{Cu}$	$(D) \ [\text{Ar}] \ 3d^5 4s^1$
	$(E) \ [\text{Ar}] \ 3d^6 4s^2$

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.