The CH3Cl molecule has a dipole moment of 1.59D. Estimate the dipole moment for the molecule CH2Cl2?

please don't google that "what is the dipole moment of ch2cl2", we need to rely on 1.59D data to calculate the bonding moment of C-Cl

The CH3Cl molecule has a dipole moment of 1.59D. Estimate the dipole moment for the molecule CH2Cl2?

(a) Using the electronegativities of Br and Cl, estimate the partial charges on the atoms in the Br – Cl molecule. (b) Using these partial charges and the atomic radii given in Figure 7.8, estimate the dipole moment of the molecule. (c) The measured dipole moment of BrCl is 0.57 D. If you assume the bond length in BrCl is the sum of the atomic radii, what are the partial charges on the atoms in BrCl using the experimental dipole moment?

The O–H bond lengths in the water molecule (H₂O) are 0.96 Å, and the H–O–H angle is 104.5°. The dipole moment of the water molecule is 1.85 D. (a) In what directions do the bond dipoles of the O–H bonds point? In what direction does the dipole moment vector of the water molecule point? (b) Calculate the magnitude of the bond dipole of the O–H bonds. (Note: You will need to use vector addition to do this.) (c) Compare your answer from part (b) to the dipole moments of the hydrogen halides (Table 8.3). Is your answer in accord with the relative electronegativity of oxygen?