# What electron pattern can be observed with the Noble Gases?

Sep 7, 2017

The electronic configuration is that noble gases have fully filled subshells.

#### Explanation:

The noble gases are present in the last group of the periodic table having the maximum possible number of electrons allowed for that period in which they are. This can also be restated as: They have fully filled electronic shells having Electron configuration $n {s}^{2} n {p}^{6}$.

There are six noble gases and have the following electronic configuration.

He = $1 {s}^{2}$
Ne =$\left[H e\right] 2 {s}^{2} 2 {p}^{6}$
Ar = $\left[N e\right] 3 {s}^{2} 3 {p}^{6}$
Kr = $\left[A r\right] 4 {s}^{2} 3 {d}^{10} 4 {p}^{6}$
Xe =$\left[K r\right] 5 {s}^{2} 4 {d}^{10} 5 {p}^{6}$
Rn =$\left[X e\right] 6 {s}^{2} 4 {f}^{14} 5 {d}^{10} 6 {p}^{6}$

The electron pattern is that all of them have fully filled subshells. This makes them reluctant to react with other molecules an d hence earns them the name " Noble gases ". However, there is an exception about Xenon compounds which is out of the scope of this question.