Which of the following compounds is expected | vedclass

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(C) The colour of transition metal compounds is generally due to the presence of unpaired electrons in the $d$-orbitals,which allow for $d-d$ transiti

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$CuCl_2$

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(C) The colour of transition metal compounds is generally due to the presence of unpaired electrons in the $d$-orbitals,which allow for $d-d$ transitions.In $CuCl_2$,copper exists as $Cu^{2+}$ ions with a $3d^9$ electronic configuration.Due to the presence of $1$ unpaired electron in the $3d$-orbital,$CuCl_2$ exhibits colour.In contrast,$Zn^{2+}$ $(3d^{10})$,$Mg^{2+}$ $(2p^6)$,and $Ag^+$ $(4d^{10})$ have fully filled orbitals and no unpaired electrons,making their compounds colourless.Therefore,$CuCl_2$ is the expected coloured compound.

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

Which of the following compounds is expected to be coloured?

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