To calculate the bond order and bond length of the CO molecule using molecular orbital theory, we first need to determine the electronic configuration of the molecule. CO has a total of 14 electrons 6 from carbon and 8 from oxygen .The molecular orbitals for CO can be represented as follows in increasing energy order :1. 1s 2. * 1s 3. 2s 4. * 2s 5. 2pz 6. 2px = 2py 7. * 2px = * 2py 8. * 2pz 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 electrons8. * 2pz - 0 electronsThe bond order can be calculated using the formula:Bond order = number of electrons in bonding orbitals - number of electrons in antibonding orbitals / 2Bond order = 2 + 2 + 2 + 4 - 2 - 2 / 2 = 6 / 2 = 3The bond order of CO is 3, which indicates a triple bond between the carbon and oxygen atoms.To determine the bond length, we can refer to experimental data. The bond length of CO is approximately 1.128 angstroms . It's important to note that molecular orbital theory doesn't provide a direct method for calculating bond lengths, so we rely on experimental data for this value.