Awesome! I'm an exception!
Btw... most people don't know .0000000001% of science (some even less), so don't sell yourself short. And for someone who is only a freshman, you are pretty knowledgeable.
It is called Quantum physics, not atomic btw. That is the name for physics at the atomic and subatomic level. That said, I'm not even entirely sure that Quantum physicists know what the hell they are talking about at times. Quantum mechanics is an insane subject and it is deep and expansive, mainly because it can be applied to the entire universe, and not just larger objects like physics. In fact, quantum physics effects regular physics, because when something is discovered or theorized that proves to be true (ie Einstein's theory of relativity) it can effect everything, which is why Einstein's theory is more generally accepted than say Newton's laws. Newton's laws are more generally taught in non-science fields because chances are, if you aren't going into science, you aren't going to need quantum physics to quantify gravitational pull or the velocity of a subatomic particle. Hell, I had to learn it too, and I doubt I'm going to use much of it going into Molecular Biology...
As for the models thing... I think the Bohr model has persisted as long as it has is because it is easier to conceptualize and understand without an in depth level of understanding. HOWEVER! You gave misinformation... I assume when he said "2,8,8,8" he was referring to the numbers on the periodic table. If that is so, then that has NOTHING to do with the shell model, but everything to do with the orbital model, because those are the number of electrons in a given orbital. And that is important to know because knowing those dictates how electrons move and how electrons transfer energy between excited and ground states.
I do not like that analogy...Mainly because the energy dissipates in your room and never moves back to a ground state.
To explain it best, you have to understand that electrons don't move completely random, nor in a set path. This is important because electrons tend to like to travel in pairs in their orbitals, but prefer to have at least one electron in each space in that set orbital.
The orbitals are s, p, d, f. (there are more, but those 4 cover most of the possibilities) Before the p orbital can be used, there need to be 2 electrons in the s1 orbital, and 2 in the s2 orbital... before d can be used there need to be 2 electrons in the s1 orbital, 2 electrons in the s2 orbital, and 6 electrons in the p1 orbital... And so on. As you continue on it gets a bit more complicated.
Now why the room scenario doesn't work... The room scenario doesn't account for excited state... The natural orbital of an electron is considered the ground state. When energy is applied it moves up to a higher orbital position. THAT is the particular reason why the Bohr model has remained relevant, and is continued to be taught is because it easily and effectively shows the transition between ground and excited states. I won't get into it much further because then it starts delving into Quantum Chemistry, which I don't want to do...