Calculate the number of unpaired electrons in the following gaseous ions: $Mn^{3+}, Cr^{3+}, V^{3+}$ and $Ti^{3+}$. Which one of these is the most stable in aqueous solution?
(B)
$Cr^{3+}$ is the most stable in aqueous solutions owing to a $t_{2g}^3$ configuration,which corresponds to a half-filled $t_{2g}$ subshell in an octahedral field.
| Gaseous ions | Number of unpaired electrons |
|---|---|
| $(i). Mn^{3+}, [Ar] \, 3d^4$ | $4$ |
| $(ii). Cr^{3+}, [Ar] \, 3d^3$ | $3$ |
| $(iii). V^{3+}, [Ar] \, 3d^2$ | $2$ |
| $(iv). Ti^{3+}, [Ar] \, 3d^1$ | $1$ |
$Cr^{3+}$ is the most stable in aqueous solutions owing to a $t_{2g}^3$ configuration,which corresponds to a half-filled $t_{2g}$ subshell in an octahedral field.
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