To determine the bond order and bond length of the N-O bond in the NO ion, we first need to examine its molecular orbital MO diagram. The molecular orbital diagram for NO is similar to that of the NO molecule, but with an additional electron in the * antibonding orbital due to the extra negative charge.For NO, there are 11 valence electrons 5 from nitrogen and 6 from oxygen . In NO, there is an additional electron, making a total of 12 valence electrons. We can distribute these electrons in the molecular orbitals as follows:1. 2s bonding orbital: 2 electrons2. 2s antibonding orbital: 2 electrons3. 2p bonding orbital: 2 electrons4. 2p bonding orbitals: 4 electrons 2 in each degenerate orbital 5. * 2p antibonding orbitals: 2 electrons 1 in each degenerate orbital Now, 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 + 4 - 2 / 2 = 6 / 2 = 3The bond order of the N-O bond in NO is 3.As for the bond length, it is inversely proportional to the bond order. A higher bond order generally corresponds to a shorter bond length and a stronger bond. However, the exact bond length cannot be determined without experimental data or computational methods. In general, we can say that the bond length of the N-O bond in NO will be shorter than that of a typical single bond N-O and closer to that of a triple bond NO .