The ionic radii of ${{\rm{N}}^{3 - }},{{\rm{O}}^{2 - }}{\rm{and}}\,{{\rm{F}}^ - }$ are respectively given by:

$\begin{array}{*{20}{l}} {1.71,{\rm{ }}1.40,{\rm{ }}1.36} \end{array}$

$\begin{array}{*{20}{l}} {1.36,{\rm{ }}1.40,{\rm{ }}1.71} \end{array}$

$\begin{array}{*{20}{l}} {1.36,{\rm{ }}1.71,{\rm{ }}1.40} \end{array}$

$\begin{array}{*{20}{l}} {1.71,{\rm{ }}1.36,{\rm{ }}1.40} \end{array}$

NEET UG CHEMISTRY MCQ: CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES

1 Easy

1 of 1

Understanding +4 | -1

The ionic radii of

{\mathrm{N}^{3 - }},{\mathrm{O}^{2 - }}\mathrm{and}\,{\mathrm{F}^ - }

are respectively given by:

View answer and explanation

Correct option: C

\begin{array}{llllllllllllllllllll} {1.71,\mathrm{ }1.40,\mathrm{ }1.36} \end{array}

Option C (

\begin{array}{llllllllllllllllllll}{1.71,\mathrm{ }1.40,\mathrm{ }1.36}\end{array}

) is correct because as the negative charge increases, the ionic radii increase due to greater electron repulsion, and all are isoelectronic.