Nothing is more confusing to students than the difference in a shell, subshell, and an orbital. Except for maybe how the brain of the opposite sex works.

But that is a topic for another blogger!

However, I can help you explain the difference in a shell, subshell, and an orbital without breaking a sweat.

Yeah, sure. You can teach quantum chemistry like you always have. I did.

You can stand at the front of the classroom and explain about the location of an electron, how it is oriented in space, and the probability of finding it at a given time.

You can explain with no diagrams or some of the traditional, hard to understand diagrams.

You can say, "If you are in the s orbital there is only one option for l and also for ml. That should be obvious based on it being in the s orbital."

Huh?

Exactly.

Or you could really break the topic down into tangible, bite size pieces for your students. You could make students SEE quantum chemistry easily. (#DoodleNotes are awesome for this)

Imagine quantum chemistry with bright colors, simplified instructions, and specific illustrations that inspire understanding.

​ Now, that sounds amazing!