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Question: Consider the isoelectronic species, \(Na^{+},Mg^{2 +},F^{-}\) and \(O^{2 -}\) the correct order of i...

Consider the isoelectronic species, Na+,Mg2+,F−Na^{+},Mg^{2 +},F^{-} and O2−O^{2 -} the correct order of increasing length of their radii is.

A

F1<O2−<Mg2+<Na+F^{1} < O^{2 -} < Mg^{2 +} < Na^{+}

B

Mg2+<Na+<F−<O2−Mg^{2 +} < Na^{+} < F^{-} < O^{2 -}

C

O2−<F−<Na+<Mg2+O^{2 -} < F^{-} < Na^{+} < Mg^{2 +}

D

O2−<F−<Mg2+<Na+O^{2} - < F^{-} < Mg^{2 +} < Na^{+}

Answer

Mg2+<Na+<F−<O2−Mg^{2 +} < Na^{+} < F^{-} < O^{2 -}

Explanation

Solution

: For isoelectronic species, ionic radii decrease with increase in nuclear charge (i.e., no. of protons). Thus, the cation with greater +ve charge will have a smaller radius and the anion with greater – ve charge will have a larger radius. Thus, the correct order of increasing ionic radii isMg2+<Na+<F−<O2−Mg^{2 +} < Na^{+} < F^{-} < O^{2 -}