To calculate the bond order and bond length of the nitrogen-nitrogen bond in the N2 molecule, we need to consider both the Lewis structure and molecular orbital theory.1. Lewis Structure:The Lewis structure of N2 is a triple bond between the two nitrogen atoms, with each nitrogen atom having one lone pair of electrons. The bond order in the Lewis structure is the number of bonds between the two atoms, which is 3 in this case.2. Molecular Orbital Theory:According to molecular orbital theory, atomic orbitals of the two nitrogen atoms combine to form molecular orbitals. Nitrogen has 5 valence electrons, so there are a total of 10 electrons in the N2 molecule. The molecular orbitals are filled in the following order: 1s, *1s, 2s, *2s, 2p, *2p, and 2p.The molecular orbital configuration for N2 is:1s^2, *1s^2, 2s^2, *2s^2, 2p^4, 2p^2Now, we can calculate the bond order using the molecular orbital theory: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 = 3The bond order calculated using molecular orbital theory is also 3, which matches the Lewis structure.To determine the bond length, we can refer to experimental data. The bond length of the nitrogen-nitrogen triple bond in N2 is approximately 1.10 angstroms .In conclusion, the bond order of the nitrogen-nitrogen bond in the N2 molecule is 3, and the bond length is approximately 1.10 .