To calculate the bond order of the carbon monoxide CO molecule using molecular orbital theory, we first need to determine the electronic configuration of the molecule.Carbon has 6 electrons and oxygen has 8 electrons, so CO has a total of 14 electrons. The molecular orbitals of CO are filled in the following order: 1s , * 1s , 2s , * 2s , 2pz , 2px = 2py , * 2px = * 2py .Now, let's fill the molecular orbitals with the 14 electrons:1. 1s - 2 electrons2. * 1s - 2 electrons3. 2s - 2 electrons4. * 2s - 2 electrons5. 2pz - 2 electrons6. 2px = 2py - 4 electrons 2 in each orbital 7. * 2px = * 2py - 0 electrons none left Now 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 = 3The bond order of the carbon monoxide molecule CO is 3.A higher bond order indicates a stronger and more stable bond. In the case of CO, the bond order of 3 suggests a strong triple bond between the carbon and oxygen atoms, making the molecule quite stable.