To calculate the bond order of the nitrogen molecule N2 using molecular orbital theory, we need to determine the number of electrons in bonding and antibonding molecular orbitals.Nitrogen has 7 electrons in its valence shell, and since there are two nitrogen atoms in N2, there are a total of 14 valence electrons.According to molecular orbital theory, the order of filling molecular orbitals for diatomic molecules is as follows:1. 1s2. *1s3. 2s4. *2s5. 2p_x and 2p_y degenerate orbitals 6. *2p_x and *2p_y degenerate orbitals 7. 2p_z8. *2p_zNow, let's fill the molecular orbitals with the 14 valence electrons:1. 1s: 2 electrons2. *1s: 2 electrons3. 2s: 2 electrons4. *2s: 2 electrons5. 2p_x and 2p_y: 4 electrons 2 in each 6. *2p_x and *2p_y: 0 electrons7. 2p_z: 2 electrons8. *2p_z: 0 electronsNow, 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 = 10 - 4 / 2 = 6 / 2 = 3So, the bond order of the nitrogen molecule N2 is 3, which indicates a strong triple bond between the two nitrogen atoms.