Which of the following represents an exotherm | vedclass

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(C) An exothermic reaction is one where energy is released,meaning the electron gain enthalpy is negative.$1$. Option $A$ represents the ionization en

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$O_{(g)} + e^- 	o O_{(g)}^{-}$

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(C) An exothermic reaction is one where energy is released,meaning the electron gain enthalpy is negative.$1$. Option $A$ represents the ionization energy of $F^-$,which is endothermic.$2$. Option $B$ involves adding an electron to $Be$. Since $Be$ has a stable $2s^2$ configuration,adding an electron is endothermic.$3$. Option $C$ represents the first electron gain enthalpy of oxygen,which is exothermic ($O_{(g)} + e^- 	o O_{(g)}^{-}$,$\Delta H = -141 \ kJ/mol$).$4$. Option $D$ represents the formation of $O^{2-}$ from $O$. The addition of the second electron to $O^-$ is endothermic due to inter-electronic repulsion.

Which of the following represents an exothermic reaction?

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