To calculate the bond order and bond length of the nitrogen-oxygen bond in nitric oxide NO , we first need to determine the molecular orbital configuration of the molecule.Nitric oxide NO has an odd number of electrons 7 from nitrogen and 6 from oxygen, for a total of 13 . The molecular orbital configuration for NO can be determined using the Aufbau principle and the molecular orbital diagram for diatomic molecules. The molecular orbitals are filled in the following order: 1s, *1s, 2s, *2s, 2px, 2py, 2pz.The electron configuration for NO is:1s, *1s, 2s, *2s, 2px, 2py, 2pzNow, we can calculate the bond order using the formula:Bond order = number of electrons in bonding orbitals - number of electrons in antibonding orbitals / 2Bond order = 2 + 2 + 2 + 1 - 2 - 2 / 2Bond order = 9 - 4 / 2Bond order = 5 / 2Bond order = 2.5The bond order of the nitrogen-oxygen bond in nitric oxide is 2.5.To determine the bond length, we can refer to experimental data or use a general trend. In general, as bond order increases, bond length decreases. The bond length of a nitrogen-nitrogen triple bond NN is approximately 1.10 , while the bond length of a nitrogen-nitrogen double bond N=N is approximately 1.25 . Since the bond order of the nitrogen-oxygen bond in nitric oxide is 2.5, which is between a double and triple bond, we can estimate that the bond length will be between 1.10 and 1.25 .Experimental data shows that the bond length of the nitrogen-oxygen bond in nitric oxide is approximately 1.15 .In summary, the bond order of the nitrogen-oxygen bond in nitric oxide NO is 2.5, and the bond length is approximately 1.15 .