To calculate the bond order and bond length of the nitrogen-oxygen bond in nitric oxide NO , we will follow these steps:Step 1: Determine the molecular orbital configuration of NONitrogen N has an atomic number of 7, so it has 7 electrons. Oxygen O has an atomic number of 8, so it has 8 electrons. Therefore, NO has a total of 15 electrons. The molecular orbital configuration of NO can be represented as follows:1s, *1s, 2s, *2s, 2p^4, 2pStep 2: Calculate the bond orderBond order is calculated using the formula:Bond order = Number of electrons in bonding orbitals - Number of electrons in antibonding orbitals / 2In the molecular orbital configuration of NO, there are 10 electrons in bonding orbitals 2 in 1s, 2 in 2s, 4 in 2p, and 2 in 2p and 4 electrons in antibonding orbitals 2 in *1s and 2 in *2s . Using the formula:Bond order = 10 - 4 / 2 = 6 / 2 = 3The bond order of the nitrogen-oxygen bond in nitric oxide NO is 3.Step 3: Determine the bond lengthThe bond length of a molecule can be determined using experimental data or by comparing it to similar molecules. In the case of NO, the bond length has been experimentally determined to be approximately 1.15 angstroms .In conclusion, the nitrogen-oxygen bond in nitric oxide NO has a bond order of 3 and a bond length of approximately 1.15 .