In which of the following processes is energy | vedclass

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(C) The process $Cl + e^{-} \rightarrow Cl^{-}$ represents the addition of an electron to a neutral chlorine atom to form a chloride ion.This process

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$Cl + e^{-} \rightarrow Cl^{-}$

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(C) The process $Cl + e^{-} \rightarrow Cl^{-}$ represents the addition of an electron to a neutral chlorine atom to form a chloride ion.This process completes the octet of the chlorine atom,which is a stable configuration.Energy is released during this process,which is known as the electron gain enthalpy (or electron affinity).In contrast,$Cl \rightarrow Cl^{+} + e^{-}$ is an ionization process requiring energy,$HCl \rightarrow H^{+} + Cl^{-}$ is a bond dissociation process requiring energy,and $O^{-} + e^{-} \rightarrow O^{2-}$ is an endothermic process due to inter-electronic repulsion.

List-$I$ (Element)	List-$II$ (Electron gain enthalpy in $kJ \ mol^{-1}$)
$(A)$ $F$	$(I)$ $-141$
$(B)$ $Cl$	$(II)$ $-328$
$(C)$ $O$	$(III)$ $-200$
$(D)$ $S$	$(IV)$ $-349$

In which of the following processes is energy liberated?

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The absolute value of the electron gain enthalpy of halogens satisfies which of the following orders?

Among the following options, the correct trend in the electron gain enthalpy is

The correct electron affinity order is $(EA = -\Delta H_{EG})$

Match the following elements in List-$I$ with their respective electron gain enthalpy values in List-$II$:
List-$I$ (Element) List-$II$ (Electron gain enthalpy in $kJ \ mol^{-1}$)
$(A)$ $F$ $(I)$ $-141$
$(B)$ $Cl$ $(II)$ $-328$
$(C)$ $O$ $(III)$ $-200$
$(D)$ $S$ $(IV)$ $-349$

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