Orbital Diagram - How To Draw, Examples, Rules, Filling Order

1. What is an Orbital diagram?
2. How to Draw Orbital Diagrams - rules?
3. How to draw an Orbital diagram/notation?
4. What is the difference between an Electron configuration or an Orbital diagram?
5. FAQ
6. Summary

All of us chemistry enthusiasts know that electrons revolve around the positively charged nucleus of an atom in specific energy levels. These energy levels are known as shells. But do you know that these shells are further divided into subshells, each with a specific number of atomic orbitals?  

In this article, we will discuss all the different rules and principles of filling electrons in an atomic orbital diagram, followed by plenty of examples for drawing an orbital diagram or orbital notation configuration. 

What is an Orbital diagram?

An atomic orbital is a three-dimensional description of the location of an electron around the nucleus of an atom. In other words, there is a maximum probability of finding an electron in an atomic orbital.

There are 4 main types of subshells, namely s, p, d, and f. Each subshell is divided into a specific number of orbitals. The atomic orbitals lying in the same subshell are degenerate, i.e., situated at an equal energy level. However, the energy of the atomic orbitals belonging to different subshells varies significantly.

“We use orbital diagrams as a pictorial representation of the electrons present in an atom’’.

The s-subshell has only a single spherical-shaped atomic orbital. The p -subshell has 3 dumbbell-shaped degenerate atomic orbitals known as px, py, and pz. In contrast, the d and f-subshells are comprised of 5 and 7 degenerate atomic orbitals, respectively.

The electrons are not randomly filled in the different atomic orbitals of an atom. Rather, special rules are followed for assigning the location of an electron in an atomic orbital.