Among the isoelectronic ions (O^{2-}, N^{3-}, | vedclass

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(A) For isoelectronic species,the ionic radius decreases as the nuclear charge (number of protons) increases because the electrons are more strongly a

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$Mg^{2+}, N^{3-}$

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(A) For isoelectronic species,the ionic radius decreases as the nuclear charge (number of protons) increases because the electrons are more strongly attracted to the nucleus.						$Species$			$N^{3-}, O^{2-}, Na^{+}, Mg^{2+}$							$Number$ of electrons			$10, 10, 10, 10$							$Number$ of protons			$7, 8, 11, 12$			As the number of protons increases,the effective nuclear charge increases,leading to a smaller ionic radius.The order of ionic radius is: $Mg^{2+} Thus,$Mg^{2+}$ has the least ionic radius and $N^{3-}$ has the highest ionic radius.

Among the isoelectronic ions $(O^{2-}, N^{3-}, Mg^{2+}, Na^{+})$,the ions with the least and the highest ionic radius are,respectively

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