Electron Configuration of Every Element in the Periodic Table. (scroll down to see that)
The electron configuration of an atom is just what it says it is. It is the order and arrangement of electrons into shells, subshells and orbitals in order to get the lowest energy configuration possible, which is the most stable configuration for that atom. Before we get started with this, there are a couple of "rule and regulations" you should be familiar with:
1) Occupation of orbitials: Orbitals are occupied in order to minimize the energy of the atom. Therefore, the lowest energy orbitals are filled first. Here is a great little picture to help you remember that order.
2) Pauli Exclusion Principle: This rules states that no two electrons can have the same four quantum numbers. That means that in each each suborbital (s, p, d, or f) can hold 0, 1, or 2 electrons, BUT if it holds two they have to have different spin quantum numbers.
3) Hund's rule: When filling sublevels, put one electron in each sublevel before placing electrons together. We call this the "diner rule". If there are empty tables in a diner, you sit by yourself until they are all full....Once all of the tables are full, then you politely ask someone if you can join them and sit at their table.
This is a decent YouTube video describing the process.
4) Aufbau process: Fill the lowest energy orbitals before filling the higher level ones. For example, you fill the 1s shell before the 2s shell.
Want to see a demonstration of determining electron configuration, click on the picture to advance it?
Here is one more quick video of the process. What do you think? Pretty easy, right ?