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(B) The correct order is $O^{2-} > F^{-} > Na^{+} > Mg^{2+} > Al^{3+}$.All these ions are isoelectronic species,meaning they have the same number of e

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$O^{2-} > F^{-} > Na^{+} > Mg^{2+} > Al^{3+}$

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(B) The correct order is $O^{2-} > F^{-} > Na^{+} > Mg^{2+} > Al^{3+}$.All these ions are isoelectronic species,meaning they have the same number of electrons ($10$ electrons) and the same electronic configuration $(1s^2, 2s^2, 2p^6)$.For isoelectronic species,the ionic radius decreases as the nuclear charge (atomic number) increases.The nuclear charges for these ions are: $O^{2-} (+8)$,$F^{-} (+9)$,$Na^{+} (+11)$,$Mg^{2+} (+12)$,and $Al^{3+} (+13)$.Since the nuclear charge increases from $O^{2-}$ to $Al^{3+}$,the attraction between the nucleus and the electrons increases,leading to a decrease in the ionic radius.

Which of the following represents the correct order of ionic radii?

Similar Questions

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