To calculate the bond order and predict the magnetic behavior of carbon monoxide CO using molecular orbital theory, we first need to determine the electronic configuration of CO.Carbon C has an atomic number of 6, so it has 6 electrons. Oxygen O has an atomic number of 8, so it has 8 electrons. Therefore, CO has a total of 14 electrons.Now, let's fill the molecular orbitals according to the energy levels and the aufbau principle. The order of energy levels for CO is as follows:1. 2s 2. * 2s 3. 2pz 4. 2px = 2py 5. * 2px = * 2py 6. * 2pz Now we fill the orbitals with the 14 electrons:1. 2s - 2 electrons2. * 2s - 2 electrons3. 2pz - 2 electrons4. 2px = 2py - 4 electrons 2 in each 5. * 2px = * 2py - 4 electrons 2 in each 6. * 2pz - 0 electronsNext, we calculate the bond order using the formula:Bond order = number of electrons in bonding orbitals - number of electrons in antibonding orbitals / 2Bond order = 8 - 6 / 2 = 2 / 2 = 1The bond order of CO is 1, which indicates a single bond between the carbon and oxygen atoms.To predict the magnetic behavior, we need to check for unpaired electrons in the molecular orbitals. In CO, all the electrons are paired, so it is diamagnetic.In conclusion, according to molecular orbital theory, carbon monoxide CO has a bond order of 1 and is diamagnetic.