# What is an intuitive explanation for Electron Configurations

I'm sort of self studying Chemistry. I'm now getting stuck wrapping my head around a concept (and I realize it was the same concept I had difficulty grasping years ago) and that is Electron Configurations.

I know that perhaps due to the nature of chemistry it is non-intuitive. However, I want an explanation that is more than "This is a bunch of numbers and letters that follow a pattern. Live with it" - which seems to just be the explanations I'm getting when I went to school.

So, my question is, what are Electron Configurations, and how would you explain them intuitively?

The intuitive answer is this: Electron configurations are a way of telling in which atomic orbitals the electrons are put in, according to the Aufbau principle and the Pauli exclusion principle. Decoding it is pretty easy, as it always follows this pattern: $n$$(s|p|d|f)^x$ where $n$ is the main quantum number (or shell number), $(s|p|d|f)$ denotes the atomic orbitals with the quantum number and $x$ is the number of electrons found in the orbitals.
The orbital "groups" ($p$, $d$, $f$) contain several "orbitals" (side note: an orbital is strictly seen a one-electron function) where two electrons with opposite spin fit in. $p$ has 3 ($p_x,\; p_y,\; p_z$), $d$ has 5 ($d_{xy},\; d_{xz},\; d_{yz},\; d_{x^2-y^2},\; d_{z^2}$) and $f$ even more. This means that the maximal number of electrons in the $p$ group is $6$, and in the $d$ group $10$. So when you fill in the electrons according to the aufbau principle, you have to go to the next orbital group when you reach this number.
Bottom line: Every electron in an atom is defined by the four quantum numbers $n$ (main or principal quantum number), $l$ (azimuthal), $m_l$ (magnetic) and $m_s$ (spin). Using the electron configuration we can derive the first three of these four numbers.