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(B) The energy liberated during an electron affinity process is related to the stability of the resulting anion. Option $B$ involves adding an electro

Vedclass · Accepted Answer

$[He] \ 2s^2 \ 2p^2 + e^- 	o [He] \ 2s^2 \ 2p^3$

Vedclass · Answer

(B) The energy liberated during an electron affinity process is related to the stability of the resulting anion. Option $B$ involves adding an electron to a $2p^2$ configuration to form a $2p^3$ configuration. The $2p^3$ configuration is a half-filled $p$-orbital,which is exceptionally stable due to exchange energy and symmetry. Therefore,the process $[He] \ 2s^2 \ 2p^2 + e^- 	o [He] \ 2s^2 \ 2p^3$ (forming the $N^-$ ion) is highly exothermic compared to the others,as it achieves a stable half-filled subshell.

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

Which electron affinity process would liberate the most energy?

Similar Questions

The electron gain enthalpy values (in $kJ \ mol^{-1}$) of three halogens $X$,$Y$ and $Z$ are respectively $-349$,$-333$ and $-325$. Then $X$,$Y$ and $Z$ are respectively

Explain the trends in electron gain enthalpy across periods and down groups.

Would you expect the second electron gain enthalpy of $O$ to be positive,more negative,or less negative than the first? Justify your answer.

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

Explain the periodicity of electron gain enthalpy of elements in the periodic table.

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