Consider the isoelectronic species,Na^{+},Mg^ | vedclass

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Question

(B) For isoelectronic species,the ionic radius decreases as the nuclear charge (atomic number) increases.$1$. All given species ($Na^{+}$,$Mg^{2+}$,$F

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

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(B) For isoelectronic species,the ionic radius decreases as the nuclear charge (atomic number) increases.$1$. All given species ($Na^{+}$,$Mg^{2+}$,$F^{-}$,$O^{2-}$) have $10$ electrons.$2$. Their atomic numbers are: $O (8)$,$F (9)$,$Na (11)$,$Mg (12)$.$3$. As the nuclear charge increases,the attraction of the nucleus for the electrons increases,causing the ionic radius to decrease.$4$. The order of increasing atomic number is $O^{2-} (8) $5$. Therefore,the order of increasing ionic radii is $Mg^{2+} < Na^{+} < F^{-} < O^{2-}$.

Consider the isoelectronic species,$Na^{+}$,$Mg^{2+}$,$F^{-}$,and $O^{2-}$. The correct order of increasing ionic radii is:

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