Which of the following is not possible for 4p or 3d electrons?

Options

A. `n = 3, l = 2, m = +1, s = +(1)/(2)`
B. `n = 4, l = 1, m = 0, s = +(1)/(2)`
C. `n = 3, l = 3, m = +3, s = +(1)/(2)`
D. `n = 4, l = 2, m = -1, s = +(1)/(2)`

Explanation

To determine which of the given quantum numbers is not possible for 4p or 3d electrons, we need to analyze the quantum numbers associated with these orbitals. The quantum numbers are:

1. Principal quantum number (n)
2. Azimuthal quantum number (l)
3. Magnetic quantum number (m)
4. Spin quantum number (s)

### Step-by-Step Solution:

**Step 1: Analyze the 4p Electrons**
- For 4p electrons:
- Principal quantum number (n) = 4
- Azimuthal quantum number (l) for p orbitals = 1
- The magnetic quantum number (m) can take values from -l to +l, which means:
- m = -1, 0, +1
- The spin quantum number (s) can be either +1/2 or -1/2.

**Step 2: Analyze the 3d Electrons**
- For 3d electrons:
- Principal quantum number (n) = 3
- Azimuthal quantum number (l) for d orbitals = 2
- The magnetic quantum number (m) can take values from -l to +l, which means:
- m = -2, -1, 0, +1, +2
- The spin quantum number (s) can also be either +1/2 or -1/2.

**Step 3: Evaluate the Given Options**
- We need to check the validity of each set of quantum numbers provided in the options:
1. **n = 3, l = 2, m = +1, s = +1/2**: This is possible (3d).
2. **n = 4, l = 1, m = 0, s = +1/2**: This is possible (4p).
3. **n = 3, l = 3**: This is **not possible** because for n = 3, l can only be 0, 1, or 2 (s, p, or d orbitals).
4. **n = 4, l = 2, m = -1, s = +1/2**: This is possible (4d).

**Conclusion:**
The only set of quantum numbers that is not possible is **n = 3, l = 3**.

### Final Answer:
**The quantum numbers that are not possible for 4p or 3d electrons are: n = 3, l = 3.**

---