Consider the isoelectronic species, Na^(+),Mg^(2+),F^(-) and O^(2-). The correct order of increasing length of their radii is:

Consider the isoelectronic species, Na^(+),Mg^(2+),F^(-) and O^(2-). T

1.	Consider the isoelectronic species, Na^(+),Mg^(2+),F^(-) and O^(2-). The correct order of increasing length of their radii is:
Answer» `F^(-)O^(2-)ltMg^(2+)ltNa^(+)` `Mg^(2+)ltNa^(+)ltF^(-)LTO^(2-)` `O^(2-)ltF^(-)ltNa^(+)ltMg^(2+)` `O^(2-)ltF^(-)ltMg^(2+)ltNa^(+)` 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 `Mg^(2+)ltNa^(+)ltF^(-)ltO^(2-)`