chem help please!?

Question

How many electrons in an atom can have each of the following quantum numbers or sublevel designations? If a given set of quantum numbers or sublevel is not possible, enter 0 for that answer.

(a) n=2, l=1
(b) n=2, l=1, ml=0
(c) 4s

Answer 1

Its been a while but let me see.

If n is 2, obviously the most elections that could fit that number is 8.

If l = 1 then you are looking at a p orbital which can hold up to (a) six electrons.

If you designate a magnetic quatum number ml then you have to pic one of the three p sub-orbitals in with cas you have (b) 2 electrons.

as for the last question, it doesnt matter what number is in front of the s, if it is an s orbital it can only hold (c) 2 electrons.

I may have over looked something but as I remember, this should get you in the right direction.

Answer 2

(a) n=2, l=1
This is a 2p orbital and has 3 possibe magnetic number orbitals each of which can hold 2 electrons (of opposite spin). Six electrons total.

(b) n=2, l=1, m=0
This is the 2p orbital (one of three) and can hold 2 electrons (of opposite spin).

(c) 4s ?
Two if this is the 4th principal, spherical orbital.

Rules governing the combinations of quantum numbers:

Three quantum numbers n, l, and m are integers.
The principal quantum number (n) cannot be zero. [n must be 1, 2, 3, etc.]
The angular quantum number (l) can be any integer between 0 and n - 1. [For n = 3, l can be either 0, 1, or 2.]
The magnetic quantum number (m) can be any integer between -l and +l. [For l = 2, m can be either -2, -1, 0, +1, or +2.]
The spin quantum number (s) is arbitrarily assigned the numbers +1/2 and -1/2.