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Question

(D) The process of adding an electron to a neutral atom is usually exothermic,releasing energy. However,adding an electron to an already negatively ch

Vedclass · Accepted Answer

$O^{-} + e^- 	o O^{2-}$

Vedclass · Answer

(D) The process of adding an electron to a neutral atom is usually exothermic,releasing energy. However,adding an electron to an already negatively charged ion,such as $O^{-}$,is endothermic. This is due to the strong electrostatic repulsion between the incoming electron and the existing negative charge on the ion. Therefore,the second electron gain enthalpy is positive,meaning the process $O^{-} + e^- 	o O^{2-}$ requires the absorption of energy.

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

The process requiring the absorption of energy is

Similar Questions

For electron gain enthalpies of the elements denoted as $\Delta_{eg} H$,the incorrect option is :

When an electron is added to elements of group $16$ and $17$ in $n = 2$ and $n = 3$ shells,which case experiences less electron-electron repulsion and why?

Which of the following pairs of elements would have a more negative electron gain enthalpy?
$(i)$ $O$ or $F$
$(ii)$ $F$ or $Cl$

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

What is the correct order of electron affinity for the elements of the oxygen group in the periodic table?

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