Saturday, 4 June 2016

organic chemistry - Difference of dipole moments of dichloromethane and trichloromethane?


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 CCl bond, which has a bond dipole moment of magnitude A. The contribution from CH is neglected here to simplify the calculations.


Now consider dichloromethane. The resultant of the two CCl dipoles will have a magnitude of 2Acosθ2

where θ109.5, the angle between the vectors from the ends of tetrahedron to the centre. This turns out to be 1.154A.


For tricholoromethane, the three CCl 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

which will be 1A, lesser than in the case of dichloromethane.


To visualise how can you get those angles and cosines, see this page.


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