The bond order of a molecule can be determined using its molecular orbital diagram. 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 a nitrogen molecule N2 :Nitrogen has 7 electrons, so N2 has a total of 14 electrons. In the molecular orbital diagram, the electrons fill the following orbitals: 1s, *1s, 2s, *2s, 2p^4. The bond order for N2 is calculated as follows:Bond order = number of electrons in bonding orbitals - number of electrons in antibonding orbitals / 2Bond order = 10 - 4 / 2Bond order = 6 / 2Bond order = 3For an oxygen molecule O2 :Oxygen has 8 electrons, so O2 has a total of 16 electrons. In the molecular orbital diagram, the electrons fill the following orbitals: 1s, *1s, 2s, *2s, 2p^4, *2p. The bond order for O2 is calculated as follows:Bond order = number of electrons in bonding orbitals - number of electrons in antibonding orbitals / 2Bond order = 12 - 4 / 2Bond order = 8 / 2Bond order = 4The bond order of N2 is 3, and the bond order of O2 is 2.In general, a higher bond order corresponds to a stronger bond and a shorter bond length. In this case, the triple bond in N2 bond order of 3 is stronger and shorter than the double bond in O2 bond order of 2 .