To calculate the bond order and bond length of the nitrogen-oxygen bond in nitrous oxide N2O , we need to consider its molecular orbital diagram and the Lewis structure.1. Molecular orbital diagram:N2O has a total of 16 valence electrons. The molecular orbital diagram for N2O is similar to that of N2 and O2. The molecular orbitals are filled in the following order: 1s, *1s, 2s, *2s, 2px, 2py, 2pz, *2px, *2py, and *2pz.2. Lewis structure:The Lewis structure of N2O can be represented as NNO, where the nitrogen-nitrogen bond is a triple bond and the nitrogen-oxygen bond is a single bond.3. Bond order:Bond order is calculated as the difference between the number of bonding electrons and the number of antibonding electrons, divided by 2.For the nitrogen-oxygen bond in N2O, there are 2 electrons in the 2pz bonding orbital and 0 electrons in the *2pz antibonding orbital.Bond order = 2 - 0 / 2 = 1The bond order of the nitrogen-oxygen bond in N2O is 1, which indicates a single bond.4. Bond length:The bond length of a nitrogen-oxygen single bond can be found in a reference table or calculated using experimental data. The average bond length for a nitrogen-oxygen single bond is approximately 1.47 angstroms .In conclusion, the nitrogen-oxygen bond in nitrous oxide N2O has a bond order of 1 and a bond length of approximately 1.47 .