Question

Which of the following represents the outermost shell electronic configuration of halogens?
A. $n{{s}^{2}}n{{p}^{3}}$
B. $n{{s}^{2}}n{{p}^{6}}$
C. $n{{s}^{2}}n{{p}^{4}}$
D. $n{{s}^{2}}n{{p}^{5}}$

Answer 1

Hint: The halogens have $7$ valence electrons. Among the $7$ valence electrons, $ns$ orbital has two electrons and $np$ orbital has five electrons.

Complete Step by Step Answer:
Halogens are group $17$ elements of the modern periodic table. The halogen elements are fluorine, chlorine, bromine, iodine, astatine. These elements have $7$ valence electrons so their general electronic configuration is given as $n{{s}^{2}}n{{p}^{5}}$. So, the $ns$ orbital have two electrons and $np$ orbital has five electrons.
Thus the correct option is D.

Additional information: The halogen elements are colored elements. The electron releasing tendency increases and electronegativity decreases down the halogen group. Thus fluorine is the most electronegative element among halogens. Electron affinity is defined as the energy released to accept an electron. Among halogens chlorine has the highest electron affinity.

Note: Halogens have one electron less from the electronic configuration of inert gas. Thus halogens easily gain one electron and get stability. The halogens have high electronegativity and high electron affinity.