Question

Which of the following is a possible set of quantum numbers for an electron (n, l, m0, ms)?

(1, 1, 0, +1/2)
(2, 1, 2, +1/2)
(3, 2, 0, -1/2)
(3, -2, 1, -1/2)

Answer 1

do you know the rules for the quantum numbers?

Answer 2

Nope

Answer 3

Just need the answer haha!

Answer 4

you already has 4 answers there, how you will know if the answer is correct?

Answer 5

Alright, so then can you help me?

Answer 6

I can try

Answer 7

Thank you

Answer 8

Rules Governing the Allowed Combinations of Quantum Numbers

The three quantum numbers (n, l, and m) that describe an orbital are integers: 0, 1, 2, 3, and so on.
The principal quantum number (n) cannot be zero. The allowed values of n are therefore 1, 2, 3, 4, and so on.
The angular quantum number (l) can be any integer between 0 and n - 1. If n = 3, for example, l can be either 0, 1, or 2.
The magnetic quantum number (m) can be any integer between -l and +l. If l = 2, m can be either -2, -1, 0, +1, or +2.

Answer 9

So, what do I have to do now?

Answer 10

just check each of your answers if they follow the rules, your answers indicate in the order n,l,mo,ms
start with the first one and let me know what do you think

Answer 11

What is the "n" value of the electron for the first answer?