Which of the following has the smallest size?

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(B) The species $Na^{+}$,$Mg^{2+}$,$F^{-}$,and $Cl^{-}$ are not all isoelectronic. $Na^{+}$ $(10 \ e^{-})$,$Mg^{2+}$ $(10 \ e^{-})$,and $F^{-}$ $(10 \

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$Mg^{2+}$

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(B) The species $Na^{+}$,$Mg^{2+}$,$F^{-}$,and $Cl^{-}$ are not all isoelectronic. $Na^{+}$ $(10 \ e^{-})$,$Mg^{2+}$ $(10 \ e^{-})$,and $F^{-}$ $(10 \ e^{-})$ are isoelectronic,while $Cl^{-}$ $(18 \ e^{-})$ is larger due to an extra shell. Among the isoelectronic species ($Na^{+}$,$Mg^{2+}$,$F^{-}$),the size decreases as the nuclear charge increases. $Mg^{2+}$ has the highest atomic number $(Z=12)$ compared to $Na^{+}$ $(Z=11)$ and $F^{-}$ $(Z=9)$. Therefore,$Mg^{2+}$ has the strongest attraction for electrons,resulting in the smallest ionic radius.

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