To calculate the bond order and bond length of the nitrogen-oxygen bond in the NO molecule using molecular orbital theory, we first need to determine the electronic configuration of the molecule.Nitrogen N has 7 electrons, and Oxygen O has 8 electrons. So, the NO molecule has a total of 15 electrons. The molecular orbitals are filled in the following order: 1s, *1s, 2s, *2s, 2px, 2py, 2pz, *2px, *2py, *2pz.Now, let's fill the molecular orbitals with the 15 electrons:1. 1s: 2 electrons2. *1s: 2 electrons3. 2s: 2 electrons4. *2s: 2 electrons5. 2px: 2 electrons6. 2py: 2 electrons7. 2pz: 2 electrons8. *2px: 1 electronThe bond order can be calculated using the formula:Bond order = Number of electrons in bonding orbitals - Number of electrons in antibonding orbitals / 2Bond order = 10 - 5 / 2 = 5 / 2 = 2.5The bond order of the nitrogen-oxygen bond in the NO molecule is 2.5. This indicates that the bond is between a double bond and a triple bond, making it a strong bond.To calculate the bond length, we can use the empirical formula:Bond length = R / 1 - exp - BO - 1 Here, R and are constants that depend on the specific atoms involved in the bond. For nitrogen and oxygen, R = 1.10 and = 0.4 ^-1 .Bond length = 1.10 / 1 - exp -0.4 2.5 - 1 Bond length 1.10 / 1 - exp -0.6 Bond length 1.10 / 1 - 0.5488 Bond length 1.10 / 0.4512Bond length 2.44 The bond length of the nitrogen-oxygen bond in the NO molecule is approximately 2.44 .In conclusion, the nitrogen-oxygen bond in the NO molecule has a bond order of 2.5 and a bond length of approximately 2.44 . The bond is strong and lies between a double bond and a triple bond, indicating a high degree of electron sharing between the nitrogen and oxygen atoms.