Question

Which of the following is a possible set of quantum numbers for an electron?
(1, 1, 0, +½)
(2, 1, 2, +½)
(3, 2, 0, -½)
(3, -2, 1, -½)

Answer 1

Do you know What kind of quantum numbers those 4 are?

Answer 2

._. What do you mean?

Answer 3

I mean do you know what the first, second, third and fourth number mean?

Answer 4

Yes

Answer 5

I Kind Of Forgot Like the rule of it though.

Answer 6

What's the first number?

Answer 7

-_- N, The Principal Quantum Number.

Answer 8

L, the azimuthal number, Ml the magnetic, and the last is the spin.
I Just need to know the part where it says which numbers can be in each levels...if that makes sense.

Answer 9

N ranges from 1 to infinity
L ranges from 0 to N-1
Ml ranges from -L to L
Ms is either \(-\frac{1}2\) or \(\frac{1}2\)

Answer 10

to check which one is correct, you have to look at N, then look at the possibilities for L

For example in the first one: N = 1
L ranges from 0 to N-1, N-1 = 1-1 = 0
So L can only be 0.
In the first option, L=1 so the first one is not a possible set of quantum numbers

Answer 11

I think it's the second one?

Answer 12

Second one:
N=2
L= 0 \(\to\) N-1 L=2-1=1
So L ranges from 0 to 1
That means L for the second option is possible.

Now the magnetic number
Ml = -L to +L = -1 to +1

It's 2 in the option so second one is also not possible

Answer 13

Now check if the third one is possible, can you do that? :)

Answer 14

Ohhh Yea I Got It Thank You!

Answer 15

Wait, What about the spin?

Answer 16

The spin is always correct. It can only be -1/2 or +1/2