🤓 Based on our data, we think this question is relevant for Professor Cole & Geng & Lovander's class at IOWA.
You may want to reference(Pages 227 - 231)Section 6.5 while completing this problem.
For the table that follows, indicate which orbital corresponds to each set of quantum numbers. Ignore x, y, and z subscripts. If the
quantum numbers are not allowed (i.e., contain an illegitimate value), indicate that by using the "not allowed" label.
We are asked to determine the orbitals which correspond to the values of n, l, and m_{l} values given.
n | l | m_{l} | Orbital |
2 | 1 | -1 | 2p (example) |
1 | 0 | 0 | |
3 | 3 | 2 | |
3 | 2 | -2 | |
2 | 0 | -1 | |
0 | 0 | 0 | |
4 | 2 | 1 | |
5 | 3 | 0 |
Let’s first define the values of first three quantum numbers:
• principal quantum number (n) → energy level in orbitals and its value could be any positive integer starting from 1
• angular momentum quantum number (ℓ) → (l) has to be at least 1 less than n, range of values from 0 up to (n-1) and each number corresponds to a subshell: