Quantum Numbers Sapling Homework

[Elizabeth Kaplan 3I]

How many electrons in an atom could have these sets of quantum numbers?

n=2

n=5, l=3

n=7, l=3, ml=-1

How do you determine this?

[KatarinaReid_3H]

n=2 should have 8e- because 2e- in 2s and 6e- in 2p
n=5, l=3 is 5f orbital, so 14e- in total
n=7, l=3, ml=-1 so that would be 7f subshell with the specific -1 orbital. Since each orbital can only have 2e- (spin up/spin down) then this must have 2e- max.
Each consecutive quantum number narrows down the number of electrons that it could be specifying. By the time you get to ml, the max would be 2e-, and ms, is one specific e-.

[Leyna Tran 2D]

I agree with the above post! During on of the UA sessions, the UA said that drawing out the electron configuration/ orbital diagram can help visualize how many electrons there can be. I started using this method for problems like this, as well as other problems that asks for the amount of unpaired electrons there are. It is helpful especially if you are a visual learner!