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

Vedclass · Accepted Answer

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

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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?

Similar Questions

Given below are two statements:
Statement $I$: Fluorine has most negative electron gain enthalpy in its group.
Statement $II$: Oxygen has least negative electron gain enthalpy in its group.
In the light of the above statements,choose the most appropriate from the options given below.

Which of the following arrangements represents the correct order of electron gain enthalpy (with negative sign) for the given elements?

For the process
$A_{(g)} + e^- \to A^{-}_{(g)};$ $\Delta H = x$
and $A^{-}_{(g)} \to A_{(g)} + e^-;$ $\Delta H = y$
Select the correct statement:

In which of the following is the electron gain enthalpy of elements correctly arranged?

Fluorine has lower electron affinity than chlorine because of

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