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:
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.
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