The ionic radii of \(\mathrm{O^{2-}}\), \(\mathrm{F^-}\), \(\mathrm{Na^+}\) and \(\mathrm{Mg^{2+}}\) are in the order :
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- \(\mathrm{O^{2-}} \gt \mathrm{F^-} \gt \mathrm{Na^+} \gt \mathrm{Mg^{2+}}\)
- \(\mathrm{Mg^{2+}} \gt \mathrm{Na^+} \gt \mathrm{F^-} \gt \mathrm{O^{2-}}\)
- \(\mathrm{O^{2-}} \gt \mathrm{F^-} \gt \mathrm{Mg^{2+}} \gt \mathrm{Na^+}\)
- \(\mathrm{F^-} \gt \mathrm{O^{2-}} \gt \mathrm{Na^+} \gt \mathrm{Mg^{2+}}\)
The Correct Option is A
Solution and Explanation
Step 2: For isoelectronic species the same electron cloud is pulled by a larger nuclear charge, so the radius decreases as Z increases.
Step 3: Order of Z: \(8 \lt 9 \lt 11 \lt 12\), so the radii follow \(\mathrm{O^{2-}} \gt \mathrm{F^-} \gt \mathrm{Na^+} \gt \mathrm{Mg^{2+}}\).
Answer: (1) \(\mathrm{O^{2-}} \gt \mathrm{F^-} \gt \mathrm{Na^+} \gt \mathrm{Mg^{2+}}\)
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