# Electron Configuration

### Breana Yacoob: Page 6

## How to write electron configuration

There are many steps as far as how you write electron configuration. The number one thing you must establish is how many electrons you have. Once you figure out how many electrons you have then you have to use as many orbital sublevels as it takes to fill in your missing electrons. Remember to fill in the lowest energy first then work your way up.

## Examples:

1s^2 2s^2 2p^6 3s^2

## Instruction In order to do the orbital notation first you have to find your element. Next, you have to find the electron configuartion of the element. Lastly you figure out the orbital notation. To figure out the orbital notation you simply just draw lines to represent 1s, 2s,3s etc. Using the exponents you have from the electron configuration you will have to put as many on each line.(Draw arrows first moving upward then once you run out of spaces draw it downward.) | ## Description First, n = 3, since the valence electron is a 3p electron. We know that p sublevels have an l value of 1. We also know that ml can have a value between l and -l, and to get the ml quantum number, we go back to the orbital notation for the valence electron and focus on the 3p sublevel alone. | ## Examples 1s^2+2s^2= _^ _^ |

## Instruction

In order to do the orbital notation first you have to find your element. Next, you have to find the electron configuartion of the element. Lastly you figure out the orbital notation. To figure out the orbital notation you simply just draw lines to represent 1s, 2s,3s etc. Using the exponents you have from the electron configuration you will have to put as many on each line.(Draw arrows first moving upward then once you run out of spaces draw it downward.)

## Description

First, n = 3, since the valence electron is a 3p electron. We know that p sublevels have an l value of 1. We also know that ml can have a value between l and -l, and to get the ml quantum number, we go back to the orbital notation for the valence electron and focus on the 3p sublevel alone.

## Scientists

Aufbau Principle-lowest energy level fills first.

Pauli Exclusion Principle-No two electrons can have the same 4 quantum numbers.

Heisenburg Uncertainty Principle- One cannot determine both the position and momentum of an electron.

Hunds Rule- Also known as the "school bus rule"