Which of the following may be colourless?

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Question

(B) The colour of transition metal ions is generally due to $d-d$ transitions,which require the presence of unpaired electrons in the $d$-orbitals.$1$

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$Cu^{+}$

Vedclass · Answer

(B) The colour of transition metal ions is generally due to $d-d$ transitions,which require the presence of unpaired electrons in the $d$-orbitals.$1$. $Cr^{3+}$ has an electronic configuration of $[Ar] 3d^3$,which contains $3$ unpaired electrons.$2$. $Cu^{+}$ has an electronic configuration of $[Ar] 3d^{10}$,which has a completely filled $d$-subshell with no unpaired electrons.$3$. $Fe^{3+}$ has an electronic configuration of $[Ar] 3d^5$,which contains $5$ unpaired electrons.$4$. $Cu^{2+}$ has an electronic configuration of $[Ar] 3d^9$,which contains $1$ unpaired electron.Since $Cu^{+}$ has a $d^{10}$ configuration,it has no unpaired electrons to undergo $d-d$ transitions,making it colourless.Therefore,the correct option is $(B)$.

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

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