Which of the following isoelectronic series w | vedclass

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(A) The given species $S^{2-}$,$Cl^{-}$,$Ar$,and $K^{+}$ are isoelectronic,meaning they all have $18$ electrons. For isoelectronic species,the ease of

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$S^{2-}$

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(A) The given species $S^{2-}$,$Cl^{-}$,$Ar$,and $K^{+}$ are isoelectronic,meaning they all have $18$ electrons. For isoelectronic species,the ease of losing an electron (ionization energy) depends on the nuclear charge (number of protons). As the nuclear charge increases,the attraction between the nucleus and the valence electrons increases,making it harder to remove an electron. The nuclear charges are: $S^{2-} (Z=16)$,$Cl^{-} (Z=17)$,$Ar (Z=18)$,and $K^{+} (Z=19)$. Since $S^{2-}$ has the lowest nuclear charge $(Z=16)$,it has the weakest hold on its electrons,making it the easiest to lose an electron.

$I.E.$	$1^{st}$	$2^{nd}$	$3^{rd}$	$4^{th}$	$5^{th}$
Value	$577.5$	$1810$	$2750$	$11580$	$14820$

$(IP)_1$	$7.1 \ eV$
$(IP)_2$	$10.3 \ eV$
$(IP)_3$	$36.2 \ eV$
$(IP)_4$	$39.1 \ eV$

Which of the following isoelectronic series would lose an electron most easily?

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The first $I.P.$ of $Mg$ is ...... than $Al$.

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$I.E.$ $1^{st}$ $2^{nd}$ $3^{rd}$ $4^{th}$ $5^{th}$

Value $577.5$ $1810$ $2750$ $11580$ $14820$

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$(IP)_1$ $7.1 \ eV$
$(IP)_2$ $10.3 \ eV$
$(IP)_3$ $36.2 \ eV$
$(IP)_4$ $39.1 \ eV$

Which of the following processes requires the largest amount of energy?

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