Questions

Identify the correct order of increasing ionic sizes

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{Al}^{3 +} < O^{2 -} < F^{-} < {Cl}^{-}

F^{-} < O^{2 -} < {Cl}^{-} < {Al}^{3 +}

{Al}^{3 +} < F^{-} < O^{2 -} < {Cl}^{-}

{Al}^{3 +} < F^{-} < {Cl}^{-} < O^{2 -}

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detailed solution

Correct option is C

The electronic configurations of the given ions are

${Al}^{3 +} : (1 s)^{2} (2 s)^{2} (2 p)^{6} F^{-} : (1 s)^{2} (2 s)^{2} (2 p)^{6}$

$O^{2 -} : (1 s)^{2} (2 s)^{2} (2 p)^{6} {Cl}^{-} : (1 s)^{2} (2 s)^{2} (2 p)^{6} (3 s)^{2} (3 p)^{6}$

The size of ${Cl}^{-}$ will be the largest as its outer shell belongs to the quantum number n = 3. Of the remaining species,

${Al}^{3 +}$ will have the minimum ionic size because of three positive charge and $O 2^{-}$ will have maximum ionic size because of two negative charge.

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