To solve the question, we need to analyze the statements regarding the stability and magnetic properties of the nitrogen-oxygen species: NO, NO+, and NO-. We will determine the bond order and magnetic properties of each species using Molecular Orbital Theory (MOT).
### Step-by-Step Solution:
1. **Determine the total number of electrons for each species:**
- NO has 15 electrons (7 from N and 8 from O).
- NO+ has 14 electrons (1 electron removed from NO).
- NO- has 16 electrons (1 additional electron added to NO).
2. **Construct the molecular orbital diagram:**
- For NO (15 electrons):
- Fill the molecular orbitals in the order: σ1s, σ1s*, σ2s, σ2s*, σ2p_z, π2p_x, π2p_y, π2p_x*, π2p_y*, σ2p_z*.
- The filling gives us:
- Bonding: 10 electrons (σ1s: 2, σ2s: 2, σ2p_z: 2, π2p_x: 2, π2p_y: 2)
- Antibonding: 5 electrons (σ1s*: 2, σ2s*: 2, π2p_x*: 1)
- Bond Order = (Number of bonding electrons - Number of antibonding electrons) / 2 = (10 - 5) / 2 = 2.5.
3. **Calculate the bond order for NO+:**
- For NO+ (14 electrons):
- The filling will be similar to NO but with one less electron in the antibonding orbitals.
- Bonding: 10 electrons (same as NO).
- Antibonding: 4 electrons (σ1s*: 2, σ2s*: 2).
- Bond Order = (10 - 4) / 2 = 3.
4. **Calculate the bond order for NO-:**
- For NO- (16 electrons):
- The filling will include one more electron in the bonding orbitals.
- Bonding: 11 electrons (σ1s: 2, σ2s: 2, σ2p_z: 2, π2p_x: 2, π2p_y: 3).
- Antibonding: 5 electrons.
- Bond Order = (11 - 5) / 2 = 3.
5. **Determine the magnetic properties:**
- NO has one unpaired electron, making it paramagnetic.
- NO+ has no unpaired electrons, making it diamagnetic.
- NO- has one unpaired electron, making it paramagnetic.
6. **Evaluate the stability based on bond order:**
- Higher bond order indicates greater stability.
- NO+ (bond order 3) is more stable than NO (bond order 2.5).
- NO- (bond order 3) is also stable but less than NO+.
### Conclusion:
The correct statement among the given options is:
- NO+ is diamagnetic, NO- is paramagnetic, and NO+ is more stable than NO-.
