The ionic radii of F$-$ and O2$-$ respectively are 1.33$\mathop A\limits^o$ and 1.4$\mathop A\limits^o$, while the covalent radius of N is 0.74$\mathop A\limits^o$.
The correct statement for the ionic radius of N3$-$ from the following is :
Solution
F<sup>$-$</sup>, O<sup>2$-$</sup> and N<sup>3$-$</sup> all are isoelectronic species in which N<sup>3$-$</sup> have least number of protons due to which it's size increases as least nuclear attraction is experienced by the outer shell electrons. Size order<br><br>N<sup>3$-$</sup> > O<sup>2$-$</sup> > F<sup>$-$</sup>
About this question
Subject: Chemistry · Chapter: Periodic Table and Periodicity · Topic: Periodic Trends
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