Which of the following has the least electron | vedclass

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(B) Electron gain enthalpy becomes less negative (or smaller in magnitude) as we move down a group due to an increase in atomic size.Among the given e

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Iodine

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(B) Electron gain enthalpy becomes less negative (or smaller in magnitude) as we move down a group due to an increase in atomic size.Among the given elements,$Cl$ and $S$ are in the $3^{rd}$ period,while $O$ and $I$ are in the $2^{nd}$ and $5^{th}$ periods respectively.$Cl$ has the most negative electron gain enthalpy.$Iodine$ $(I)$ has the least negative electron gain enthalpy among the halogens listed due to its large atomic size,which reduces the attraction for an incoming electron.Comparing $O$ and $S$,$O$ has a smaller electron gain enthalpy than $S$ due to inter-electronic repulsion in its small $2p$ orbital.However,comparing all four,$Iodine$ $(I)$ has the least electron gain enthalpy.

Which of the following has the least electron gain enthalpy?

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The formation of the $O^{2-}$ ion is first exothermic and then endothermic,as shown by the following reaction steps:
$O_{(g)} + e^- \to O^-_{(g)}; \Delta H^o = -142 \ kJ \ mol^{-1}$
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This is due to:

The set containing the elements with positive electron gain enthalpies is

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