# How many electrons are unpaired in the orbitals of nitrogen?

Apr 24, 2018

$3$ Unpaired electrons.

#### Explanation:

Nitrogen atom has total $7$ electrons. Two will fill up the $n = 1$ level, and then there are five electrons in the $n = 2$ level.

Nitrogen can bond three times with other electrons to fill up it's shell with 8, (8-5=3). And these are those $3$ unpaired electrons which were residing the $2 p$ sub-shell of the Nitrogen atom , before the formation of $3$ bonds.

The $2 {p}_{x}$, $2 {p}_{y}$ and $2 {p}_{z}$ orbitals of the Nitrogen atom have $1$ unpaired electron in each of them as shown below :-

Thus, the total no. of unpaired electrons in Nitrogen atom is $3$.

Hope that helps!

Apr 24, 2018

Three (3).

#### Explanation:

From the Periodic Table or other description of the electron shells of nitrogen we see that its configuration is $1 {s}^{2} 2 {s}^{2} 2 {p}^{3}$.

That means that it has only 3 electrons in the 2p orbitals. Per Hund's Rule, they will not become paired until each available orbital has one electron in it. Thus, nitrogen contains 3 unpaired electrons - one in each of the available p orbitals.