Question

Consider the isoelectronic species, \[\ce{Na+, Mg^{2+}, F–}\] and \[\ce{O2-}\]. The correct order of increasing length of their radii is ______.

Options

• \[\ce{F- < O^{2-} < Mg^{2+} < Na+}\]

• \[\ce{Mg^{2+} < Na+ < F- < O^{2-}}\]

• \[\ce{O^{2-} < F- < Na+ < Mg^{2+}}\]

• \[\ce{O^{2-} < F- < Mg^{2+} < Na+}\]

Answer 1

Consider the isoelectronic species, \[\ce{Na+, Mg^{2+}, F–}\] and \[\ce{O2-}\]. The correct order of increasing length of their radii is \[\ce{Mg^{2+} < Na+ < F- < O^{2-}}\].

Explanation:

All the given ions are isoelectronic species thus their radii depend upon the charge more the negative charge higher would be the atomic radii and higher the positive charge lesser would be the atomic radii.