When the permanganate ion, $Mn{O}_4^{-}$, acts as an oxidizing agent it forms different products depending on the $\mathrm{pH}$ of the solution. Which species correspond to the conditions listed?

	Acidic	Basic	Neutral
A	$M{n}^{2+}$	$Mn(OH{)}_2$	$Mn{O}_2$
B	$M{n}^{2+}$	$Mn{O}_{\mathit{4}}^{\mathit{2}\mathit{-}}$	$Mn{O}_2$
C	$Mn{O}_2$	$Mn{O}_{\mathit{4}}^{\mathit{2}\mathit{-}}$	$Mn(OH{)}_2$
D	$M{n}^{2+}$	$Mn(OH{)}_2$	$Mn{O}_{\mathit{4}}^{\mathit{2}\mathit{-}}$

Since tendency to accept electron increases $M{n}^{2+}$ is acidic in nature.

Since the permanganate (VII) ion is a strong oxidizing agent it is basic in nature.

Manganese has a +7-oxidation state, which indicates a high oxidation state and an acidic oxide. Manganese's oxidation state in $\text{ MnO| }$ is +2, which denotes a low oxidation state and basic oxide status.

Hence, option B is correct.