Question

Which of the following outer electronic configuration represent argon?

• A. ${\mathrm{ns}}^2$
• B. ${\mathrm{ns}}^2{\mathrm{np}}^6$
• C. ${\mathrm{ns}}^2{\mathrm{np}}^5$
• D. ${\mathrm{ns}}^2{\mathrm{np}}^4$

Answer 1

The correct option is B

${\mathrm{ns}}^2{\mathrm{np}}^6$

Explanation for correct option:

B. ${\mathrm{ns}}^2{\mathrm{np}}^6$

Noble gas:

• Noble gases belong to Group-$18$.
• The stability of noble gases is very high.
• Noble gases exhibit stable electronic configuration due to the completely filled orbitals.
• They are fairly non-reactive gases.
• The general electronic configuration of Noble gas is ${\mathrm{ns}}^2{\mathrm{np}}^6$.

Argon is a noble gas with an atomic number$18$ and it has an electronic configuration $1{\mathrm{s}}^{2}2{\mathrm{s}}^{2}2{\mathrm{p}}^{6}3{\mathrm{s}}^{2}3{\mathrm{p}}^6$.

Explanation for incorrect options:

A. ${\mathrm{ns}}^2$represents the outer electronic configuration for Helium.

C. ${\mathrm{ns}}^2{\mathrm{np}}^5$ represents the outer electronic configuration for Halogens.

D. ${\mathrm{ns}}^2{\mathrm{np}}^4$ represents the outer electronic configuration for Group-$16$.

Hence, the correct option is B i.e. ${\mathrm{ns}}^2{\mathrm{np}}^6$.