The bond order of a nitrogen molecule N2 can be determined using molecular orbital theory by calculating the difference between the number of electrons in bonding and antibonding orbitals, divided by 2.For N2, each nitrogen atom has 7 electrons, so there are a total of 14 electrons in the molecule. The molecular orbitals are filled in the following order: 1s, *1s, 2s, *2s, 2p, 2p, and *2p.Filling the orbitals with 14 electrons, we have:- 2 electrons in 1s bonding - 2 electrons in *1s antibonding - 2 electrons in 2s bonding - 2 electrons in *2s antibonding - 4 electrons in 2p bonding - 2 electrons in 2p bonding There are no electrons in the *2p orbital.Now, we can calculate the bond order:Bond order = Number of electrons in bonding orbitals - Number of electrons in antibonding orbitals / 2Bond order = 10 - 4 / 2Bond order = 6 / 2Bond order = 3So, the bond order of a nitrogen molecule N2 is 3. This means there is a triple bond between the two nitrogen atoms.