# What electron configuration represents an atom in the excited state?

Jan 14, 2016

The excited state electron configuration of an atom indicates the promotion of a valence electron to a higher energy state.

#### Explanation:

An electron configuration representing an atom in the excited state will show a valence electron promoted to a higher energy level.

Example
The ground state electron configuration of sodium is ${\text{1s"^2"2s"^2"2p"^6"3s}}^{1}$.

In its excited state, the valence electron in the $\text{3s}$ sublevel is promoted to the $\text{3p}$ sublevel, giving the electron configuration as
${\text{1s"^2"2s"^2"2p"^6"3p}}^{1}$.

This is a very unstable condition and the excited electron will drop back down to the $\text{3s}$ sublevel, releasing the same amount of energy that was absorbed, and producing a characteristic color of light, in this case yellow.

Jan 14, 2016

The first excited state is the same configuration as the ground state, except for the position of one electron.

As an example, sodium goes through a $3 s \to 3 p$ transition.

The ground state electron configuration for sodium is:

$\textcolor{b l u e}{1 {s}^{2} 2 {s}^{2} 2 {p}^{6} 3 {s}^{1}}$

And the first excited state electron configuration for sodium is:

$\textcolor{b l u e}{1 {s}^{2} 2 {s}^{2} 2 {p}^{6} 3 {p}^{1}}$

This corresponds to an excitation to a first excited state that is less stable; that then leads to a relaxation back down to the ground state. The relaxation emits yellow light ($\text{589 nm}$).

I end up going through selection rules (which help you predict whether an electronic transition is allowed or forbidden), term symbols, and predicting transitions. That overall tells you how I know that a $3 s \to 3 p$ transition is a real transition for sodium.

(If you want, you can skip the term symbols contextual section; it's optional.)

You may or may not have learned selection rules yet, but they aren't too difficult to take note of. They would help you determine how to write electron configurations for excited states.

SELECTION RULES

The selection rules govern how an electron is observed to transition (excite upwards or relax downwards) from one orbital to another.

Formally, they are written as:

$\textcolor{b l u e}{\Delta S = 0}$
$\textcolor{b l u e}{\Delta L = 0 , \pm 1}$

$\textcolor{b l u e}{L + S = J}$

$\therefore \textcolor{b l u e}{\Delta J = 0 , \pm 1}$

where $\Delta S$ is the change in intrinsic angular momentum of the electron (spin multiplicity is $2 S + 1$), $\Delta L$ is the change in orbital angular momentum, and $\Delta J$ is the change in the total angular momentum.

It is helpful to know the selection rules if you want to predict how an excited state configuration can be written just based on the atom's (correct) ground state configuration.

EXAMPLES OF ELECTRONIC EXCITATION TRANSITIONS

Allowed:

An example of an allowed electronic transition upwards of one unpaired electron to an empty orbital:

$\textcolor{g r e e n}{2 s \to 2 p}$ (color(green)(DeltaS = 0, $\textcolor{g r e e n}{\Delta L = + 1}$, $\textcolor{g r e e n}{\Delta J = 0 , \pm 1}$)

$\Delta L = + 1$ because for $s$, $l = 0$, and for $p$, $l = 1$. Thus, $\Delta L = + 1$.

$\Delta S = 0$ because the electron didn't get paired with any new electron. It started out unpaired, and it stayed unpaired (${m}_{s}^{\text{new" = m_s^"old}}$), so $\Delta S = {m}_{s}^{\text{new" - m_s^"old}} = 0$.

Forbidden:

An example of a forbidden electronic transition upwards of one unpaired electron to an empty orbital:

$\textcolor{g r e e n}{3 s \to 3 d}$ ($\textcolor{g r e e n}{\Delta S = 0}$, $\textcolor{g r e e n}{\Delta L = \textcolor{red}{+ 2}}$, $\textcolor{g r e e n}{\Delta J = 0 , \pm 1 , \textcolor{red}{\pm 2}}$)

$\Delta L = + 2$ because for $s$, $l = 0$, and for $d$, $l = 2$. Thus, $\Delta L = + 2$, which is larger than is allowed, so it is forbidden.

$\Delta S$ is still $0$ because it's the same electron transitioning as before, just towards a different orbital.

TERM SYMBOLS / CONTEXT

"I've never seen $L$, $S$, or $J$ before. Huh? What are they used for?"

DISCLAIMER: The above link explains term symbols for context. It helps to know this, but you don't have to know this like the back of your hand unless you are taking Physical Chemistry.

APPLICATION OF THE SELECTION RULES

Alright, so let's apply the selection rules themselves. I gave examples already, so let's work off of the allowed transition example and change it a little bit. The values for $L$, $S$, and $J$ are pretty similar.

Let us examine this energy level diagram for sodium: You can see lines on the diagram going from the $3 s$ orbital to two $3 p$ orbital destinations. That indicates either an excitation from the $3 s$ to the $3 p$ or a relaxation from the $3 p$ to the $3 s$.

These two lines are marked $589.6$ and $589.0$, respectively, in $\text{nm}$, so what you see happening is that sodium makes its $\text{589 nm}$ excitation transition (upwards), and then relaxes (downwards) to emit yellow light.

Therefore, a common excitation/relaxation transition sodium makes is:

Excitation Transition: $3 s \to 3 p$ ($\Delta S = 0$, $\Delta L = + 1$, $\Delta J = 0 , + 1$)

Relaxation Transition: $3 p \to 3 s$ ($\Delta S = 0$, $\Delta L = - 1$, $\Delta J = 0 , - 1$)

(Term symbol notation:

$\text{^2 S_"1/2" -> ""^2 P_"1/2", ""^2 P_"3/2}$, excitation

$\text{^2 P_"1/2", ""^2 P_"3/2" -> ""^2 S_"1/2}$, relaxation)

So the ground state electron configuration for sodium is:

$\textcolor{b l u e}{1 {s}^{2} 2 {s}^{2} 2 {p}^{6} 3 {s}^{1}}$

And the first excited state electron configuration for sodium is:

$\textcolor{b l u e}{1 {s}^{2} 2 {s}^{2} 2 {p}^{6} 3 {p}^{1}}$

Lastly, an easy way to remember what transitions are allowed is to note that electronic transitions on energy level diagrams are diagonal, and involves adjacent columns.