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(A) All these ions are isoelectronic,meaning they all have $10$ electrons.For isoelectronic species,the ionic radius decreases as the nuclear charge (

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$Mg^{2+} < Na^{+} < F^{-} < O^{2-}$

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(A) All these ions are isoelectronic,meaning they all have $10$ electrons.For isoelectronic species,the ionic radius decreases as the nuclear charge (atomic number) increases.The atomic numbers are: $O (8), F (9), Na (11), Mg (12)$.As the nuclear charge increases,the electrons are pulled more strongly towards the nucleus,resulting in a smaller ionic radius.Therefore,the order of increasing ionic radii is: $Mg^{2+} < Na^{+} < F^{-} < O^{2-}$.

Arrange the following in increasing order of ionic radii: $O^{2-}, Na^{+}, F^{-}, Mg^{2+}$

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