The dipole moment of a carbon monoxide CO molecule is a measure of the separation of positive and negative charges within the molecule. It is a vector quantity, which means it has both magnitude and direction. The dipole moment is calculated using the formula: = Q dwhere is the dipole moment, Q is the charge difference between the two atoms, and d is the distance between the two atoms.In the case of carbon monoxide, the electronegativity difference between carbon C and oxygen O causes a partial positive charge on the carbon atom and a partial negative charge on the oxygen atom. The electronegativity values for carbon and oxygen are 2.55 and 3.44, respectively. The difference in electronegativity is 0.89, which indicates a polar covalent bond.The bond length between carbon and oxygen in CO is approximately 1.128 angstroms , or 1.128 10^-10 meters.To calculate the dipole moment, we need to determine the charge difference Q between the two atoms. This can be done using the equation:Q = e EN / EN_total where e is the elementary charge 1.602 10^-19 C , EN is the difference in electronegativity between the two atoms, and EN_total is the sum of the electronegativities of the two atoms.Q = 1.602 10^-19 C 0.89 / 2.55 + 3.44 Q 2.7 10^-20 CNow, we can calculate the dipole moment: = Q d = 2.7 10^-20 C 1.128 10^-10 m 3.0 10^-30 CmThe dipole moment of a carbon monoxide molecule is approximately 3.0 10^-30 Cm.