Compare the Lewis structures with the molecular orbital view of the bonding in \(\mathrm{NO}, \mathrm{NO}^{+}\), and \(\mathrm{NO}^{-}\). Account for any discrepancies between the models.

The Lewis structure for NO can be drawn by counting the total number of valence electrons, which equals 5 from nitrogen and 6 from oxygen, giving us 11 total valence electrons. These electrons are distributed to complete the octet rule. The Lewis structure for NO can be represented as: N = O: For NO+, we have a positive charge, meaning that we remove one electron from the system. Therefore, we'll have 10 valence electrons. The Lewis structure for NO+ can be represented as: N = O^+ For NO-, we have a negative charge, meaning we add one electron to the system. Therefore, we have 12 valence electrons. The Lewis structure for NO- can be represented as: N = O:

Now, let's draw the MO diagrams for NO, NO+, and NO-, keeping in mind that we need to fill the orbitals from the lowest to the highest energy level. To simplify, we consider the most important orbitals for the problem; primarily the 2s and 2p orbitals of the atoms. For NO, we have all three bonding orbitals from the mixing of the 2p orbitals (sigma, pi_x, and pi_y) filled, three non-bonding orbitals, and one antibonding orbital filled. This gives it a bond order of 2.5. For NO+, we remove an electron from one of the antibonding orbitals, giving it a bond order of 3. For NO-, we add an electron to one of the non-bonding orbitals, resulting in a bond order that is identical to NO, equaling 2.5.

Comparing the Lewis structures with the MO diagrams, we can see the following discrepancies: 1. In the Lewis structures, NO and NO- have the same bond order (from a double bond) while, in the MO diagram, NO and NO- have bond orders of 2.5. This means that from an MO perspective, NO and NO- have intermediate bond strength between a double and triple bond, which is not depicted in the Lewis structures. 2. In the Lewis structures, it shows that NO+ has a double bond, while the MO diagrams show NO+ having a bond order of 3 (a triple bond). Again, this discrepancy indicates that MO diagrams provide a more accurate representation of the bond strength than Lewis structures. In conclusion, the molecular orbital view of the bonding in NO, NO+, and NO- provides a more accurate representation of bond order and bond strength, and thus should be preferred over the Lewis structure representation for these species.