To solve the question of selecting the correct set(s) of quantum numbers, we will follow a systematic approach based on the rules governing quantum numbers.
### Step-by-Step Solution:
1. **Understand the Quantum Numbers**:
- There are four types of quantum numbers:
- **Principal Quantum Number (n)**: Indicates the shell and size of the orbital. It can take positive integer values (1, 2, 3,...).
- **Azimuthal Quantum Number (l)**: Indicates the shape of the orbital. It can take values from 0 to n-1.
- **Magnetic Quantum Number (ml)**: Indicates the orientation of the orbital. It can take values from -l to +l.
- **Spin Quantum Number (s)**: Indicates the spin of the electron, which can be +1/2 or -1/2.
2. **Evaluate Each Option**:
- **Option A**: n = 3, l = 0, ml = -1
- Here, l = 0 corresponds to an s orbital (3s).
- The value of ml for l = 0 can only be 0. Therefore, ml = -1 is incorrect.
- **Option B**: n = 3, l = 3
- The maximum value of l can be n-1. For n = 3, l can only be 0, 1, or 2. Hence, l = 3 is incorrect.
- **Option C**: n = 3, l = 2, ml = -2
- Here, l = 2 corresponds to a d orbital.
- The values of ml can range from -2 to +2 (i.e., -2, -1, 0, +1, +2). Therefore, ml = -2 is correct.
- **Option D**: n = 3, l = 1, ml = 0
- Here, l = 1 corresponds to a p orbital.
- The values of ml can range from -1 to +1 (i.e., -1, 0, +1). Therefore, ml = 0 is correct.
3. **Conclusion**:
- The correct sets of quantum numbers are found in options C and D.
### Final Answer:
The correct sets of quantum numbers are **Option C** (n = 3, l = 2, ml = -2) and **Option D** (n = 3, l = 1, ml = 0).
---
