Question

The ionic radii (in $\stackrel{o}{\text{A}}$) of $N^{3-},O^{2-}\text{and}{F}^{-}$ are respectively:

• A. $1.71,1.40\text{and}1.36$
• B. $1.71,1.36\text{and}1.40$
• C. $1.36,1.40\text{and}1.71$
• D. $1.36,1.71\text{and}1.40$

Answer 1

The correct option is A $1.71,1.40\text{and}1.36$

For isoelectronic species, size of anion increases as negative charge increases and ionic radius icreases with increase in size. Thus the correct order is.

$\begin{array}{c}{N}^{-3}\\ 1.71\end{array}>\begin{array}{c}{O}^{2-}\\ 1.40\end{array}>\begin{array}{c}{F}^{-}\\ 1.36\end{array}$

Hence, correct Answer is (a).