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(A) All the given ions $(O^{2-}, F^{-}, Na^{+}, Mg^{2+})$ are isoelectronic,having $10$ electrons each.Ionisation potential is the energy required to

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$O^{2-}$

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(A) All the given ions $(O^{2-}, F^{-}, Na^{+}, Mg^{2+})$ are isoelectronic,having $10$ electrons each.Ionisation potential is the energy required to remove an electron from an atom or ion.For isoelectronic species,the ionisation potential increases as the nuclear charge (number of protons) increases.$O^{2-}$ has the lowest nuclear charge $(Z = 8)$ among the given ions.Therefore,it is easiest to remove an electron from $O^{2-}$,making it the species with the lowest ionisation potential.

List-$I$ ($IE_1, IE_2, IE_3$ in $kJ \ mol^{-1}$)	List-$II$ (Element)
$A$. $1510$	$1$. $H$
$B$. $495, 6500, 10200$	$2$. $Li$
$C$. $840, 1630, 13100$	$3$. $Be$
$D$. $600, 2050, 3100$	$4$. $B$

Of the following isoelectronic ions,the one which has the lowest ionisation potential is

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List-$I$ ($IE_1, IE_2, IE_3$ in $kJ \ mol^{-1}$) List-$II$ (Element)

$A$. $1510$ $1$. $H$

$B$. $495, 6500, 10200$ $2$. $Li$

$C$. $840, 1630, 13100$ $3$. $Be$

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