Which of the following electronic configurati | vedclass

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(C) Electron affinity is the energy released when an electron is added to a neutral gaseous atom. Elements with stable electronic configurations,such

Vedclass · Accepted Answer

$ns^2 np^3$

Vedclass · Answer

(C) Electron affinity is the energy released when an electron is added to a neutral gaseous atom. Elements with stable electronic configurations,such as half-filled or fully-filled orbitals,have very low or negative electron affinity because they are already stable and do not readily accept an additional electron. Comparing the given configurations: $ns^2 np^5$ (Halogen) has a high electron affinity as it needs only one electron to complete its octet. $ns^2 np^2$ and $ns^2 np^4$ have intermediate electron affinities. $ns^2 np^3$ represents a half-filled $p$-orbital $(p^3)$,which is exceptionally stable due to exchange energy and symmetry. Therefore,the configuration $ns^2 np^3$ has the lowest electron affinity.

Which of the following electronic configurations will have the lowest electron affinity?

Similar Questions

Which of the following has the highest electron affinity?

The correct order of electron affinity is:

In which of the following,elements are arranged in the correct order of their electron gain enthalpies?

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

In which of the following options are the elements correctly arranged with respect to their negative electron gain enthalpies?

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