In molecular orbital theory, the bond order is calculated as the difference between the number of electrons in bonding orbitals and the number of electrons in antibonding orbitals, divided by 2.For O2 molecule:Oxygen has 8 electrons, so O2 has a total of 16 electrons. The molecular orbital configuration for O2 is:1s 1s * 2s 2s * 2p 2p 2p 2p * Bonding electrons: 2 in 2p + 2 in 2p Antibonding electrons: 2 in 2p * Bond order of O2 = Bonding electrons - Antibonding electrons / 2Bond order of O2 = 4 - 2 / 2 = 2 / 2 = 1For N2 molecule:Nitrogen has 7 electrons, so N2 has a total of 14 electrons. The molecular orbital configuration for N2 is:1s 1s * 2s 2s * 2p 2p 2p Bonding electrons: 2 in 2p + 2 in 2p Antibonding electrons: 0Bond order of N2 = Bonding electrons - Antibonding electrons / 2Bond order of N2 = 4 - 0 / 2 = 4 / 2 = 2Comparing the bond orders:The bond order of O2 is 1, while the bond order of N2 is 2. This means that the N2 molecule has a stronger and more stable bond compared to the O2 molecule.