First slide

Periodic Trends

Question

Which of the following orders of ionic radii is correctly represented?

Easy

A

$H^{-} > H > H^{+}$
B

${Na}^{+} > F^{-} > O^{2 -}$
C

$F^{-} > O^{2 -} > {Na}^{+}$
D

${Al}^{3 +} > {Mg}^{2 +} > N^{3 -}$

Solution

Cations lose electrons and are smaller in size than the parent atom, whereas anions add electrons and are larger in size than the parent atom. Hence, the order is $H^{-} > H > H^{+}$ . For isoelectronic species, the ionic radii decreases with increase in atomic number i.e. nuclear charge. Hence, the correct orders are
$O^{2 -} > F^{-} > {Na}^{+} and N^{3 -} > {Mg}^{2 +} > {Al}^{3 +}$

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