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(C) The absorption of visible light and the resulting coloured nature of transition metal complexes are due to the $d-d$ electronic transition,which r

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$[V(NH_3)_6]^{3+}$

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(C) The absorption of visible light and the resulting coloured nature of transition metal complexes are due to the $d-d$ electronic transition,which requires the presence of at least one unpaired $d$-electron.Let us analyze the electronic configuration of the metal ions in the given complexes:$1. [Sc(H_2O)_6]^{3+}: Sc^{3+} (Z=21) = [Ar] 3d^0$. No unpaired electrons.$2. [Ti(NH_3)_6]^{4+}: Ti^{4+} (Z=22) = [Ar] 3d^0$. No unpaired electrons.$3. [V(NH_3)_6]^{3+}: V^{3+} (Z=23) = [Ar] 3d^2$. Two unpaired electrons.$4. [Zn(NH_3)_6]^{2+}: Zn^{2+} (Z=30) = [Ar] 3d^{10}$. No unpaired electrons.Since $[V(NH_3)_6]^{3+}$ contains unpaired $d$-electrons,it can undergo $d-d$ transitions and is the most likely to absorb visible light.

Which one of the following complexes will most likely absorb visible light? (At. nos. $Sc = 21$,$Ti = 22$,$V = 23$,$Zn = 30$)

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