Which of the following pairs exhibit color in | vedclass

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(A) In aqueous medium,transition metal ions exhibit color due to $d-d$ transitions if they have unpaired electrons in their $d$-orbitals.$1$. $VOCl_2$

Vedclass · Accepted Answer

$VOCl_2, \, FeCl_2$

Vedclass · Answer

(A) In aqueous medium,transition metal ions exhibit color due to $d-d$ transitions if they have unpaired electrons in their $d$-orbitals.$1$. $VOCl_2$: $V$ is in $+4$ oxidation state $(3d^1)$,which has $1$ unpaired electron.$2$. $FeCl_2$: $Fe$ is in $+2$ oxidation state $(3d^6)$,which has $4$ unpaired electrons.$3$. $CuCl_2$: $Cu$ is in $+2$ oxidation state $(3d^9)$,which has $1$ unpaired electron.$4$. $MnCl_2$: $Mn$ is in $+2$ oxidation state $(3d^5)$,which has $5$ unpaired electrons.All the given compounds contain transition metal ions with unpaired electrons,thus all pairs exhibit color. However,in standard multiple-choice contexts for this specific question,all options provided contain colored ions. Given the options,all pairs are colored. If this is a single-choice question,there may be an error in the question design,but $VOCl_2$ $(3d^1)$,$FeCl_2$ $(3d^6)$,$CuCl_2$ $(3d^9)$,and $MnCl_2$ $(3d^5)$ are all colored.

Which of the following pairs exhibit color in aqueous medium?

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