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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.

Which electron affinity process would liberate the most energy?

Similar Questions

Among the following options, the correct trend in the electron gain enthalpy is

Arrange the three halogens $Cl$,$Br$,and $I$ in the increasing order of their electron affinity. Which of the following arrangements is correct?

Identify the element having positive electron gain enthalpy.

Which of the following represents the correct order of increasing electron gain enthalpy (with negative sign) for the elements?
$a.$ Nitrogen
$b.$ Phosphorus
$c.$ Chlorine
$d.$ Fluorine

Halogens have maximum negative electron gain enthalpy in the respective periods of the periodic table. Why?

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