Why is the dipole moment of CHX2ClX2 (1.60 D) greater than that of CHClX3 (1.08 D)?
Based on my knowledge of vectors, I feel it should be the other way around.
Answer
Just to add some quantification to Ben Norris's answer. Consider each C−Cl bond, which has a bond dipole moment of magnitude A. The contribution from C−H is neglected here to simplify the calculations.
Now consider dichloromethane. The resultant of the two C−Cl dipoles will have a magnitude of 2Acosθ2
For tricholoromethane, the three C−Cl dipoles will be at an angle θ such that cosθ=1/3 with a straight line symmetrically passing through its centre. Thus the resultant in this case will be 3Acosθ
To visualise how can you get those angles and cosines, see this page.
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