Which one of the ionic species will impart colour to an aqueous solution?

STATEMENT-$1$: The number of unpaired electrons in the following gaseous ions:
${\mathrm{Mn}}^{3+},{\mathrm{Cr}}^{3+},{\mathrm{V}}^{3+}$ and ${\mathrm{Ti}}^{3+}$ are $4,3,2$ and $1$, respectively.

STATEMENT-$2$: ${\mathrm{Cr}}^{3+}$ is the most stable in aqueous solution among these ions.

The correct order of ${\mathrm{E}}_{{\mathrm{M}}^{2+}/\mathrm{M}}^{\mathrm{o}}$ values with negative sign for the four successive elements $\mathrm{Cr}, \mathrm{Mn},$ $\mathrm{Fe}$ and $\mathrm{Co}$ is:

Hint:

$\begin{array}{l}{\mathrm{E}}_{{\mathrm{Mn}}^{2+ },\mathrm{Mn}}^{\mathrm{o}}=-1.18 \mathrm{V} , {\mathrm{E}}_{{\mathrm{Cr}}^{2+}, \mathrm{Cr}}^{\mathrm{o}}=-0.91 \mathrm{V}\\ {\mathrm{E}}_{{\mathrm{Fe}}^{2+}, \mathrm{Fe}}^{\mathrm{o}}=-0.44 \mathrm{V} , {\mathrm{E}}_{{\mathrm{Co}}^{2+}, \mathrm{Co}}^{\mathrm{o}}=-0.28 \text{V}\end{array}$