Consider the following conversions:(i) , O_{( | vedclass

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(D) The electron gain enthalpy values for the given processes are as follows:$1$. For $(i)$,$(ii)$,and $(iii)$,the addition of an electron to a neutra

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$\Delta H_1$ and $\Delta H_3$ are negative whereas $\Delta H_2$ and $\Delta H_4$ are positive

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(D) The electron gain enthalpy values for the given processes are as follows:$1$. For $(i)$,$(ii)$,and $(iii)$,the addition of an electron to a neutral atom is an exothermic process,so $\Delta H_1, \Delta H_2, 	ext{ and } \Delta H_3$ are negative.$2$. The order of electron gain enthalpy (magnitude) is $Cl > F > O$. Thus,$\Delta H_3$ (for $Cl$) is more negative than $\Delta H_2$ (for $F$) and $\Delta H_1$ (for $O$).$3$. For $(iv)$,the addition of an electron to a negatively charged ion $(O^-)$ experiences strong inter-electronic repulsion,making the process endothermic. Thus,$\Delta H_4$ is positive.$4$. Comparing the options,statement $(D)$ is incorrect because $\Delta H_2$ is negative,not positive.

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The formation of the oxide ion $O_{(g)}^{2-}$ requires first an exothermic and then an endothermic step as shown below. This is because
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