We’re being asked to find **which set of quantum numbers** is **not possible**.

Recall that the ** quantum numbers** that define an electron are:

• *Principal Quantum Number* **(n)**: deals with the size and energy of the atomic orbital. The possible values for n are **1 to ∞**.

• *Angular Momentum Quantum Number ***(l)**: deals with the shape of the atomic orbital. The possible values for l are **0 to n – 1**.

• *Magnetic Quantum Number ***(m _{l})**: deals with the orientation of the atomic orbital in 3D space. The possible values for m

•

**A. n = 4, l = 3, m _{l} = –2, m_{s} = +1/2**

The given value of n is **4**. This means: n – 1 = 4 – 1 = **3**; for n = 1, the possible values for l is **0 to 3**. We’re given **l = 3**, which means it’s a valid value.

Which one of the following sets of quantum numbers is not possible?

n |
| m | m | ||||||

A. | 4 | 3 | -2 | +1/2 | |||||

B. | 3 | 0 | 1 | -1/2 | |||||

C. | 3 | 0 | 0 | +1/2 | |||||

D. | 2 | 1 | 1 | -1/2 | |||||

E. | 2 | 0 | 0 | +1/2 |

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

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