# What is the ground-state electron configuration of a neutral atom of neon?

Jun 13, 2017

$1 {s}^{2} 2 {s}^{2} 2 {p}^{6}$
or
$\left[\text{Ne}\right]$
or
$\left[\text{He}\right] 2 {s}^{2} 2 {p}^{6}$

#### Explanation:

First: Determine the number of electrons the element has. Neon has a total of then electrons.

Know how many electrons each orbital can hold and their order.
(Refer to the following pictures as notes)

Third: Write out the electron configuration:

For Neon and other elements there are more the just one way to write the electron configuration. One way is to write out the entire electron configuration by going through each orbital or we can use a shorthand notation using the noble gases as a starting point.

The first way:
Neon has a total of $10$ electrons
We know that the $1 s$ orbital can hold up to a max of $2$ electrons. We continue this path until we reach a total of $10$ electrons.

We find the configuration to be $1 {s}^{2} 2 {s}^{2} 2 {p}^{6}$ which we know is correct because if you add up the superscripts, you'll get the total number of electrons; $10$

The second way (Shorthand)
The key to using this method is to identify the noble gas closest to the desired element that is not at a higher energy (Has a higher atomic number if I'm loosely speaking). In essence, the shorthand notation tells us the configuration by using a noble gas element as our starting point instead of starting all the way at $1 s$

Coincidently, Neon itself is a noble gas so we could also write the electron configuration as $\left[\text{Ne}\right]$. We could also have written used $\text{He}$ as our starting point as it is the closest noble gas to Neon and continued the configuration from there. The end result would then be $\left[\text{He}\right] 2 {s}^{2} 2 {p}^{6}$

All in all, the three given answers are correct ways of figuring out the electron configuration of Neon.