Quantum Mechanics Worksheet #9 [ENDORSED]

[Alysia Garcia 1B]

For this problem, why would would b and d be impossible? I thought the ml values were in range.

[Bree Perkins 1E]

B would be impossible because if n=3, then l can only go to 2 because the l maximum is (n-1). So at n=3 energy level, you can have 3 subshells (l) which are 0,1, and 2. Keep in mind that l=0 is s, l=1 is p, and l=2 is d.

D would be impossible for the same reasoning. When n=3, l can only go up to n-1, which would be 2 (0,1,2).

Hope this helps!

[Or Fisher 1I]

Hi, was just wondering where you got this worksheet from?
Thanks

[Alysia Garcia 1B]

If you search Sunday worksheet, all the worksheets should come up :)

[Daniel Cho Section 1H]

The general rule for these quantum numbers is that ml is in range for these choices but when you see n and l being the same number, just know that it is not possible. It is exactly like saying that there is a 3f orbital in the periodic table even though that orbital does not exist.

Always know that the possible values for l must be from 0 to n-1.

As for ml, ml can not be greater than the value of l since the trend contains values from the [-l,+l].

When looking at these problems, always look at the values of n and l first to see if it follows the rule and then look at ml to see if it respects the rule.

I hope this helps. Correct me if I am wrong in certain places.