Today, I had an argument with my physics teacher about the movement of electrons around the nucleus. I have read way more quantum mechanics than any normal high school student and my teacher is trained as an engineer, not a physicist, but I am not sure if I'm right. His argument was something like the following: Electrons move around the nucleus much like planets around the sun. They move in an elliptical orbit. The centrifugal force is what keeps them from crashing into the nucleus. My response was: We cannot know the precise position of an electron around the nucleus because of the uncertainty principle (note my name). It is therefore impossible to establish the electron as orbiting (elliptically) the nucleus. Other thoughts: If we approach the electron as a wave, I doubt any of his classical stuff makes sense. The centrifugal force thing even seems to be in conflict with the erroneous Rutherford and Bohr models. I am not too familiar with the following concepts but I believe they also have a role: The electron cannot fall into the nucleus because of the exclusion principle. If the electron glued itself to the nucleus, its position would be more or less certain, giving it an enormous momentum. These classical concepts where an issue after the discovery of the Rutherford model and the only way that an electron would stay out of the nucleus was if it accelerated because it would radiate energy. Anyways, those are some arguments that come to mind. Could someone please sort this out for me?