In molecular orbital theory, the bond order is determined by the difference between the number of electrons in bonding and antibonding orbitals, divided by 2. For a nitrogen molecule N2 , each nitrogen atom has 7 electrons, so there are a total of 14 electrons in the molecule.To determine the bond order, we need to fill the molecular orbitals with these 14 electrons. The molecular orbitals for N2, in increasing energy levels, are:1. 1s bonding 2. *1s antibonding 3. 2s bonding 4. *2s antibonding 5. 2p bonding 6. *2p antibonding 7. 2p bonding Now, we fill the orbitals with the 14 electrons:1. 1s: 2 electrons2. *1s: 2 electrons3. 2s: 2 electrons4. *2s: 2 electrons5. 2p: 4 electrons 2 in each degenerate orbital 6. *2p: 0 electrons7. 2p: 2 electronsNow, we calculate the bond order:Bond order = Number of electrons in bonding orbitals - Number of electrons in antibonding orbitals / 2Bond order = 2 + 2 + 4 + 2 - 2 - 2 / 2Bond order = 10 - 4 / 2Bond order = 6 / 2Bond order = 3So, the bond order of the nitrogen molecule N2 is 3, which indicates a triple bond between the two nitrogen atoms.