Which of the following is largest?

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(B) All the given ions are isoelectronic,meaning they all have $18$ electrons ($Na^{+}$ has $10$ electrons,so let us compare the isoelectronic series

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$S^{2-}$

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(B) All the given ions are isoelectronic,meaning they all have $18$ electrons ($Na^{+}$ has $10$ electrons,so let us compare the isoelectronic series $S^{2-}, Cl^{-}, K^{+}, Ca^{2+}$). For isoelectronic species,the ionic radius decreases as the nuclear charge (atomic number) increases. Atomic numbers are: $S$ $(16)$,$Cl$ $(17)$,$Na$ $(11)$,$F$ $(9)$. $S^{2-}$ has the lowest nuclear charge $(Z = 16)$ among the given options $S^{2-}$ and $Cl^{-}$,therefore it has the largest ionic radius.

Similar Questions

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