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(B) The addition of the first electron to a neutral atom is generally exothermic (energy is released),as seen in options $A$,$C$,and $D$. However,when

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$O^{-}_{(g)} + e^{-} \rightarrow O^{2-}_{(g)}$

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(B) The addition of the first electron to a neutral atom is generally exothermic (energy is released),as seen in options $A$,$C$,and $D$. However,when an electron is added to a negatively charged ion,such as $O^{-}_{(g)}$,there is a strong electrostatic repulsion between the incoming electron and the existing negative charge. To overcome this repulsion,energy must be supplied to the system. Therefore,the process $O^{-}_{(g)} + e^{-} \rightarrow O^{2-}_{(g)}$ is endothermic and involves the absorption of energy.

Which of the following processes involves absorption of energy?

Similar Questions

$Na^{-} \xleftarrow{x} Na \xrightarrow{5 \ eV} Na^{+}$
Predict the value of $X$ in $eV$.

What is the value of electron gain enthalpy of $Na^{+}$ if $IE_{1}$ of $Na$ is $5.1 \ eV$? .......... $eV$

Consider the following conversions:
$(i) \ O_{(g)} + e^- \to O^{-}_{(g)} ; \Delta H_1$
$(ii) \ F_{(g)} + e^- \to F^{-}_{(g)} ; \Delta H_2$
$(iii) \ Cl_{(g)} + e^- \to Cl^{-}_{(g)} ; \Delta H_3$
$(iv) \ Na_{(g)} \to Na^{+}_{(g)} + e^- ; \Delta H_4$
Which of the following statements is incorrect?

Which elements show an anomalous trend in the negative value of electron gain enthalpy within their respective groups?

In which of the following processes is the least energy required?

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