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(B) The correct order is $O^{2-} > F^{-} > Na^{+} > Mg^{2+} > Al^{3+}$.All these ions are isoelectronic species,meaning they have the same number of e

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$O^{2-} > F^{-} > Na^{+} > Mg^{2+} > Al^{3+}$

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(B) The correct order is $O^{2-} > F^{-} > Na^{+} > Mg^{2+} > Al^{3+}$.All these ions are isoelectronic species,meaning they have the same number of electrons ($10$ electrons) and the same electronic configuration $(1s^2, 2s^2, 2p^6)$.For isoelectronic species,the ionic radius decreases as the nuclear charge (atomic number) increases.The nuclear charges for these ions are: $O^{2-} (+8)$,$F^{-} (+9)$,$Na^{+} (+11)$,$Mg^{2+} (+12)$,and $Al^{3+} (+13)$.Since the nuclear charge increases from $O^{2-}$ to $Al^{3+}$,the attraction between the nucleus and the electrons increases,leading to a decrease in the ionic radius.

$Column\, A$ (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 represents the correct order of ionic radii?

Similar Questions

The correct order of atomic radii of $C$,$Al$,and $S$ is

Identify the element having the smallest atomic radius from the following:

Arrange $Na, Na^+, F, F^-$ in the decreasing order of their radii (size).

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

Identify the correct orders regarding atomic radii:
$i$. $Cl > F > Li$
$ii$. $P > C > N$
$iii$. $Tm > Sm > Eu$
$iv$. $Sr > Ca > Mg$

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