CHEMISTRY COMMUNITY

I am having trouble on how to get started on this question as I am not sure if we have gone over this in class yet, but since is part of the first 19 questions I guess we have gone over it. Hopefully someone can guide me somewhat on what to do.

Question: How many electrons in an atom could have these sets of quantum numbers?
-n=3
-n=4, ℓ=1
-n=7, ℓ=3, mℓ=−1

We have not learned this in lecture, and it will not be covered on the first midterm. Dr. Lavelle did say that the first 19 Sapling homework problems are content that we will be tested on; however, the system shuffled the questions in Sapling. I would suggest taking a look at section 1D in the textbook for guidance on quantum numbers and orbitals.

Hey! So I don't think you need to worry about this for the midterm because Dr. Lavelle said the sapling questions were randomized for some reason so they're kinda out of order (he's trying to get that fixed). But this refers to the electron orbitals that we will go over soon. n is the energy level itself, l represents the subshell (s,p,d,f), and ml is the orbital.

As others have already stated, this will not be on the first midterm. However, if you still want some guidance:

n=3: n represents the principal quantum number or shell. n=3 means that this is the 3rd shell, and there are 18 electrons in the 3rd shell (from 3s, 3p, 3d for a total of 9 orbitals * 2 electrons per orbital)

n=4, l=1: n represents 4th shell, while l represents the type of subshell you need to consider. l=1 would be the p subshell, which has 3 orbitals for a total of 6 electrons.

n=7, l=3, ml=-1: 7th shell, l=3 subshell which is the f subshell. the ml is the magnetic quantum number. When all of n, l, and ml are specified, a particular orbital is indicated. Regardless of the actual values of the quantum numbers, an orbital and hold a maximum of 2 electrons.

Hi! I was confused as well but thankfully this material will not be on the upcoming midterm. I would still complete the entire 1D section to understand the concept of electron orbitals.