Solveeit Logo
Login

Question

Chemistry Question on Classification of elements & periodicity in properties

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

A

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