The molecular orbital diagram of a nitrogen molecule N2 shows the combination of atomic orbitals from two nitrogen atoms to form molecular orbitals. In N2, both nitrogen atoms have the electron configuration 1s 2s 2p. When these atomic orbitals combine, they form molecular orbitals with different energy levels.Here is the molecular orbital diagram for N2:1. The two 1s orbitals from each nitrogen atom combine to form two molecular orbitals: one sigma bonding orbital lower energy and one sigma * antibonding orbital higher energy . Both and * orbitals are filled with 2 electrons each total 4 electrons .2. The two 2s orbitals from each nitrogen atom combine to form two molecular orbitals: one sigma bonding orbital lower energy and one sigma * antibonding orbital higher energy . Both and * orbitals are filled with 2 electrons each total 4 electrons .3. The six 2p orbitals from the two nitrogen atoms combine to form six molecular orbitals: one sigma bonding orbital, two pi bonding orbitals, one sigma * antibonding orbital, and two pi * antibonding orbitals. The bonding orbital is filled with 2 electrons, and the two bonding orbitals are filled with 2 electrons each total 6 electrons . The * antibonding orbital and the two * antibonding orbitals remain empty.The electronic structure of N2 can be represented as: 1 1* 2 2* 3 1 The bond order, which indicates the stability of the molecule, can be calculated as:Bond order = number of electrons in bonding orbitals - number of electrons in antibonding orbitals / 2For N2:Bond order = 10 - 4 / 2 = 3This means that N2 has a triple bond between the two nitrogen atoms, making it a very stable molecule.