The ionic sizes decrease in the order :-

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(A) The species $S^{2-}, K^{+}, Sc^{3+}, V^{5+},$ and $Mn^{7+}$ are isoelectronic,as they all contain $18$ electrons.For isoelectronic species,the ion

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$S^{2-} > K^{+} > Sc^{3+} > V^{5+} > Mn^{7+}$

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(A) The species $S^{2-}, K^{+}, Sc^{3+}, V^{5+},$ and $Mn^{7+}$ are isoelectronic,as they all contain $18$ electrons.For isoelectronic species,the ionic size is inversely proportional to the effective nuclear charge $(Z_{eff})$.As the atomic number $(Z)$ increases,the effective nuclear charge increases,which leads to a decrease in ionic size.Since the atomic numbers are $S(16), K(19), Sc(21), V(23),$ and $Mn(25)$,the effective nuclear charge increases in the order $S^{2-} Therefore,the ionic size decreases in the order: $S^{2-} > K^{+} > Sc^{3+} > V^{5+} > Mn^{7+}$.

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