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(D) All the given ions are isoelectronic,meaning they have the same number of electrons ($10$ electrons each).For isoelectronic species,the ionic radi

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$Na^{+}$

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(D) All the given ions are isoelectronic,meaning they have the same number of electrons ($10$ electrons each).For isoelectronic species,the ionic radius decreases as the nuclear charge (atomic number) increases.$N^{3-}$ $(Z=7)$,$O^{2-}$ $(Z=8)$,$F^{-}$ $(Z=9)$,$Na^{+}$ $(Z=11)$.Since $Na^{+}$ has the highest atomic number $(Z=11)$,it has the strongest nuclear attraction for the electrons,making it the smallest in size.

$Column\, A$ (ion)	$Column\, B$ (radius)
$(i)$ $Li^{+}$	$(p)$ $216\, pm$
$(ii)$ $Na^{+}$	$(q)$ $195\, pm$
$(iii)$ $Br^{-}$	$(r)$ $60\, pm$
$(iv)$ $I^{-}$	$(s)$ $95\, pm$

Which of the following is the smallest in size?

Similar Questions

Which of the following is the correct order of increasing size?

Match $Column\, A$ with $Column\, B$:
$Column\, A$ (ion) $Column\, B$ (radius)
$(i)$ $Li^{+}$ $(p)$ $216\, pm$
$(ii)$ $Na^{+}$ $(q)$ $195\, pm$
$(iii)$ $Br^{-}$ $(r)$ $60\, pm$
$(iv)$ $I^{-}$ $(s)$ $95\, pm$

The unit representing atomic radii and ionic radii is

Atomic radii of $Be, O, C, N, B$ are respectively (in $pm$):

The increasing order of the atomic radius of $Si, S, Na, Mg, Al$ is

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