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

I was helping you yesterday with the same question, and I didn't get you back

Answer 2

I'm sorry, I got busy but I reallyy need to figure it out now!

Answer 3

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 4

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

Answer 5

3?

Answer 6

(1, 1, 0, +1/2)
n= principal level is the first number in the serie

Answer 7

Okay thanks loads:)

Answer 8

That is not the correct answer

Answer 9

So what is?

Answer 10

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