The ground state electronic configuration of the oxygen molecule O2 using Molecular Orbital Theory can be determined by filling the molecular orbitals with the available electrons. Oxygen has 8 electrons, so O2 has a total of 16 electrons.The order of molecular orbitals in O2 is as follows:1. 1s2. *1s3. 2s4. *2s5. 2pz6. 2px = 2py7. *2px = *2py8. *2pzNow, we fill the molecular orbitals with the 16 electrons:1. 1s: 2 electrons2. *1s: 2 electrons3. 2s: 2 electrons4. *2s: 2 electrons5. 2pz: 2 electrons6. 2px = 2py: 4 electrons 2 in each 7. *2px = *2py: 2 electrons 1 in each 8. *2pz: 0 electronsSo, the ground state electronic configuration of O2 is: 1s ^2 *1s ^2 2s ^2 *2s ^2 2pz ^2 2px ^2 2py ^2 *2px ^1 *2py ^1To calculate the bond order, we use the formula:Bond order = number of electrons in bonding orbitals - number of electrons in antibonding orbitals / 2In O2, there are 10 electrons in bonding orbitals 1s, 2s, 2pz, 2px, and 2py and 6 electrons in antibonding orbitals *1s, *2s, *2px, and *2py .Bond order = 10 - 6 / 2 = 4 / 2 = 2Therefore, the bond order of the oxygen molecule O2 is 2.