Arrange the elements with the following electronic configurations… - Vidyadip

Question

Arrange the elements with the following electronic configurations in order of increasing electron gain enthalpy.
i. $1 s^2 2 s^2 2 p^5$
ii. $1 s^2 2 s^2 2 p^4$
iii. $1 s^2 2 s^2 2 p^3$
iv. $1 s^2 2 s^2 2 p^6 3 s^2 3 p^4$

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Answer

Out of $F\left(1 s^2 2 s^2 2 p^5\right), O\left(1 s^2 2 s^2 2 p^4\right), N\left(1 s^2 2 s^2 2 p^3\right)$ and $S\left(1 s^2 2 s^2 2 p^6 3 s^2 3 p^4\right)$, only $N$ has positive electron gain enthalpy because of its stable exactly half-filled electronic configuration while all others have negative electron gain enthalpies. Since, F needs only one more electron to acquire the nearest inert gas configuration, therefore, it has the most negative electron gain enthalpy. Out of O and $\mathrm{S}, \mathrm{O}$ has less negative electron gain enthalpy than S because of electron-electron repulsions present in its small compact $2 p$-orbital. Thus, overall order of increasing electron gain enthalpy is: i $<$ (iv) $<$ (ii) $<$ (iii).

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