Question

list the following ions in order of increasing ionic radius: na+, n3−, mg2+, f−, o2−

Explanation:

Step1: Consider isoelectronic species

All these ions (\(Na^{+}\), \(N^{3 -}\), \(Mg^{2+}\), \(F^{-}\), \(O^{2 -}\)) are isoelectronic (have the same number of electrons, \(10\) electrons).

Step2: Apply the rule for ionic radius in isoelectronic species

For isoelectronic species, the ionic radius decreases as the nuclear charge (atomic number) increases. The nuclear charges (atomic numbers) are: \(Mg(12)\), \(Na(11)\), \(F(9)\), \(O(8)\), \(N(7)\).

Step3: Arrange the ions

Based on the nuclear charge, the order of increasing ionic radius is \(Mg^{2+}

Answer:

\(Mg^{2+}