Which of the following sets of quantum numbers do not belong to 2p subshell?
(i) `n=2, l=1, m=+1, s=+1/2`
(ii) `n=2, l=0, m=0, s=-1/2`
(iii) `n=1, l=1, m=0, s=+1/2`

Answer

To determine which of the given sets of quantum numbers do not belong to the 2p subshell, we need to analyze each set based on the rules governing quantum numbers.

### Step-by-Step Solution:

1. **Identify the Principal Quantum Number (n)**:
- The principal quantum number (n) indicates the energy level of the electron. For the 2p subshell, n must be equal to 2.
- Check each option:
- (i) `n=2` → Valid for 2p subshell.
- (ii) `n=2` → Valid for 2p subshell.
- (iii) `n=1` → Not valid for 2p subshell.

2. **Identify the Azimuthal Quantum Number (l)**:
- The azimuthal quantum number (l) defines the subshell:
- For p subshell, l = 1.
- For s subshell, l = 0.
- Check each option:
- (i) `l=1` → Valid for p subshell.
- (ii) `l=0` → Valid for s subshell (not p).
- (iii) `l=1` → Valid for p subshell.

3. **Identify the Magnetic Quantum Number (m)**:
- The magnetic quantum number (m) can take values from -l to +l.
- For l = 1 (p subshell), m can be -1, 0, or +1.
- Check each option:
- (i) `m=+1` → Valid for p subshell.
- (ii) `m=0` → Valid for s subshell (but since l=0, m=0 is valid).
- (iii) `m=0` → Valid for p subshell.

4. **Identify the Spin Quantum Number (s)**:
- The spin quantum number (s) can be either +1/2 or -1/2.
- Check each option:
- (i) `s=+1/2` → Valid.
- (ii) `s=-1/2` → Valid.
- (iii) `s=+1/2` → Valid.

### Conclusion:
- From the analysis, we find:
- Option (i) `n=2, l=1, m=+1, s=+1/2` belongs to the 2p subshell.
- Option (ii) `n=2, l=0, m=0, s=-1/2` belongs to the 2s subshell.
- Option (iii) `n=1, l=1, m=0, s=+1/2` is invalid because n cannot be 1 if l is 1 (there is no 1p subshell).

Thus, the sets of quantum numbers that do not belong to the 2p subshell are:
- Option (ii) and Option (iii).