# What is the shorthand electron configuration of Xe?

Jul 31, 2017

[Kr] $4 {d}^{10} 5 {s}^{2} 5 {p}^{6}$

#### Explanation:

Let's look at the periodic table to find where Xenon is. Xenon is element 54, in the noble gases (last) column. To get the short-handed electron configuration, look at the noble gas in the row above xenon. This would be krypton. This is the base that we use to form the configuration. So far, we have [Kr].

Now, let's look at the row for Xenon. Since it is in row 5, we will be filling the 5s and 5p orbitals. Remember that the d orbitals start at 3d in row 4, so we will be filling the 4d orbitals.

Starting from left to right, we fill in 2 electrons for the s orbitals. Since we haven't gotten to xenon yet, we need to fill in the d orbitals. This will be 10 electrons. Did we get there yet? Almost. We need to fill in the p orbitals to complete the configuration. We will fill all 6 electrons in. Now we got the electron configuration for xenon.

[Kr] $4 {d}^{10} 5 {s}^{2} 5 {p}^{6}$

Note that 4d orbitals are lower in energy than 5s, so 4d electrons are typically listed before 5s electrons.

Jul 31, 2017

Well you gots a full valence shell.........so

#### Explanation:

The complete electronic configuration for $X e , Z = 54$ is.......

$1 {s}^{2} 2 {s}^{2} 2 {p}^{6} 3 {s}^{2} 3 {p}^{6} 4 {s}^{2} 3 {d}^{10} 4 {p}^{6} 5 {s}^{2} 4 {d}^{10} 5 {p}^{6}$

I suppose we go back to the last Noble Gas, and fill the valence orbitals of the next valence shell: $\left[K r\right] , Z = 36$..........

$\left[K r\right] 5 {s}^{2} 4 {d}^{10} 5 {p}^{6}$