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(C) $1$. For isoelectronic species $(O^{2-}, F^{-}, Na^{+})$,the ionic size decreases as the nuclear charge increases. Thus,the order $O^{2-} > F^{-}

Vedclass · Accepted Answer

$O^{2-} > Cl^{-} > S^{2-}$

Vedclass · Answer

(C) $1$. For isoelectronic species $(O^{2-}, F^{-}, Na^{+})$,the ionic size decreases as the nuclear charge increases. Thus,the order $O^{2-} > F^{-} > Na^{+}$ is correct.$2$. For ions in the same group $(Cl^{-}, Br^{-}, I^{-})$,the ionic size increases down the group. Thus,$I^{-} > Br^{-} > Cl^{-}$ is correct.$3$. In option $C$,$O^{2-}$ and $Cl^{-}$ are not isoelectronic,and $S^{2-}$ is larger than $O^{2-}$ because it belongs to a higher period. The correct order for these ions is $S^{2-} > Cl^{-} > O^{2-}$. Therefore,the order $O^{2-} > Cl^{-} > S^{2-}$ is incorrect.

Which of the following represents the incorrect order of ionic size?

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