The bond order of an oxygen molecule O2 can be determined using the Molecular Orbital Theory. According to this 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, the electronic configuration is:1s 2s 2pWhen the two oxygen atoms combine to form O2, the molecular orbital configuration becomes:1s *1s 2s *2s 2pHere, the bonding orbitals are 1s, 2s, and 2p, which have a total of 8 electrons. The antibonding orbitals are *1s and *2s, which have a total of 4 electrons.Using the bond order formula:Bond order = Number of electrons in bonding orbitals - Number of electrons in antibonding orbitals / 2Bond order = 8 - 4 / 2 = 4 / 2 = 2The bond order of O2 is 2, which indicates that there are two bonds between the two oxygen atoms. A bond order of 2 suggests that the oxygen molecule is stable and has a double bond between the two oxygen atoms. The higher the bond order, the stronger and more stable the bond. In this case, the bond order of 2 indicates a relatively stable oxygen molecule.