The correct arrangement for the ions in the i | vedclass

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Question

(A) The ions $Ca^{2+}, K^{+},$ and $S^{2-}$ are isoelectronic species,as they all contain $18$ electrons. For isoelectronic species,the ionic radius d

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$Ca^{2+}, K^{+}, S^{2-}$

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(A) The ions $Ca^{2+}, K^{+},$ and $S^{2-}$ are isoelectronic species,as they all contain $18$ electrons. For isoelectronic species,the ionic radius decreases as the atomic number $(Z)$ increases due to the increase in effective nuclear charge. The atomic numbers are: $S = 16, K = 19, Ca = 20$. Since the nuclear charge increases from $S$ to $Ca$,the ionic radius decreases in the order $S^{2-} > K^{+} > Ca^{2+}$. Therefore,the increasing order of radii is $Ca^{2+} < K^{+} < S^{2-}$.

The correct arrangement for the ions in the increasing order of their radii is

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