Which of the following is the correct order o | vedclass

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(A) For isoelectronic species,the ionic radius decreases as the nuclear charge $(Z)$ increases.The species $Mg^{2+}$ $(Z=12)$,$Na^{+}$ $(Z=11)$,and $F

Vedclass · Accepted Answer

$Al < Mg^{2+} < Na^{+} < F^{-}$

Vedclass · Answer

(A) For isoelectronic species,the ionic radius decreases as the nuclear charge $(Z)$ increases.The species $Mg^{2+}$ $(Z=12)$,$Na^{+}$ $(Z=11)$,and $F^{-}$ $(Z=9)$ are isoelectronic,each having $10$ electrons.Since $F^{-}$ has the lowest nuclear charge $(Z=9)$,it has the largest size.$Mg^{2+}$ has the highest nuclear charge $(Z=12)$,so it has the smallest size.$Al$ is a neutral atom with $13$ electrons,which is significantly larger than the ions.Thus,the correct order of increasing size is $Al < Mg^{2+} < Na^{+} < F^{-}$.

Which of the following is the correct order of increasing size for the given species?

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