Question

The ions $O^{2–},F^{–},N{a}^{+},M{g}^{2+}$ and $A{l}^{3+}$ are isoelectronic. Their ionic radii show:

• A. A significant decrease from $O^{2–}$ to $A{l}^{3+}$
• B. A decrease from $O^{2–}$ to $F^{–}$ and then increase from $N{a}^{+}$ to$A{l}^{3+}$
• C. A significant increase from $O^{2–}$ to $A{l}^{3+}$
• D. An increase from $O^{2–}$ to $F^{–}$ and then decrease from $N{a}^{+}$ to $A{l}^{3+}$

Answer 1

The correct option is A A significant decrease from $O^{2–}$ to $A{l}^{3+}$

Amongst isoelectronic ions, ionic radii of anions is more than that of cations. Further size of the anion increases with increase in –ve charge and size of cation decreases with increase in +ve charge. Hence, correct order is $O^{2–}>F^{–}>N{a}^{+}>M{g}^{2+}>A{l}^{3+}$.