In its ground state, the carbon monoxide CO molecule is diamagnetic, meaning it has no unpaired electrons and thus no net magnetic moment. The magnetic moment of a molecule is determined by the presence of unpaired electrons, which create a magnetic field due to their spin.In the case of CO, the electron configuration of carbon C is 1s 2s 2p, and that of oxygen O is 1s 2s 2p. When these two atoms form a CO molecule, they share electrons to create a covalent bond. The resulting molecular orbital diagram shows that all the electrons in the CO molecule are paired, with no unpaired electrons.Therefore, the magnetic moment of a carbon monoxide CO molecule in its ground state is 0.