A) \[O_{2}^{-}<{{F}^{-}}<N{{a}^{+}}<M{{g}^{2+}}<A{{l}^{3+}}\]
B) \[O_{2}^{-}>{{F}^{-}}>N{{a}^{+}}>M{{g}^{2+}}>A{{l}^{3+}}\]
C) \[O_{2}^{-}>{{F}^{-}}<N{{a}^{+}}<M{{g}^{2+}}<A{{l}^{3+}}\]
D) \[{{F}^{-}}>O_{2}^{-}>N{{a}^{+}}>A{{l}^{3+}}>M{{g}^{2+}}\]
Correct Answer: B
Solution :
Isoelectronic species are elements or ions that have the same, or equal number of electrons. Among isoelectronic species \[Ionic\text{ }radius\propto \frac{1}{nuclear\,\,ch\arg e}\] Hence, the correct order of radii of these given isoelectronic species \[\operatorname{O}_{2}^{-}>{{F}^{-}}\,>\,\,N{{a}^{+}}\,>\,\,M{{g}^{2+}}\,>\,\,A{{l}^{3+}}\]
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