Which of the following compounds shows colour | vedclass

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(A) The compound $CuSO_4 \cdot 5 H_2 O$ exhibits colour due to $d-d$ transition.In $CuSO_4 \cdot 5 H_2 O$,the copper ion is in the $Cu^{2+}$ oxidation

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$CuSO_4 \cdot 5 H_2 O$

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(A) The compound $CuSO_4 \cdot 5 H_2 O$ exhibits colour due to $d-d$ transition.In $CuSO_4 \cdot 5 H_2 O$,the copper ion is in the $Cu^{2+}$ oxidation state.The electronic configuration of $Cu^{2+}$ is $[Ar] 3 d^9$.Since there is an unpaired electron in the $d$-orbital,the $d-d$ transition is possible,which results in the observed colour.In contrast,$K_2 Cr_2 O_7$,$K_2 CrO_4$,and $KMnO_4$ exhibit colour primarily due to charge transfer transitions,as the metal ions ($Cr^{6+}$ and $Mn^{7+}$) have a $d^0$ configuration.

Which of the following compounds shows colour due to $d-d$ transition?

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Reason: There is no electron present in $d$-orbitals of Manganese in $MnO_4^-$.

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