d-d transition occurs in . . . . . . . | vedclass

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(C) For a $d-d$ transition to occur,the metal ion must have a partially filled $d$-orbital (i.e.,$d^1$ to $d^9$ configuration).$1$. $Cu^{+}$: Electron

Vedclass · Accepted Answer

$Mn^{3+}$

Vedclass · Answer

(C) For a $d-d$ transition to occur,the metal ion must have a partially filled $d$-orbital (i.e.,$d^1$ to $d^9$ configuration).$1$. $Cu^{+}$: Electronic configuration is $[Ar] 3d^{10}$. It has a fully filled $d$-orbital,so no $d-d$ transition is possible.$2$. $Zn^{2+}$: Electronic configuration is $[Ar] 3d^{10}$. It has a fully filled $d$-orbital,so no $d-d$ transition is possible.$3$. $Mn^{3+}$: Electronic configuration is $[Ar] 3d^4$. It has a partially filled $d$-orbital,allowing for $d-d$ transition.$4$. $Sc^{3+}$: Electronic configuration is $[Ar] 3d^0$. It has an empty $d$-orbital,so no $d-d$ transition is possible.Therefore,the correct option is $C$.

$d-d$ transition occurs in . . . . . . .

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