How are the chlorines facing opposite directions? In the case of dichloromethane, the central carbon is sp3 hybridized. The chlorines definitely are not facing opposite directions, hence their bond dipoles do not cancel out. There is not a particularly strong dipole, because the electronegativity difference between C-H is not that far from C-Cl, but there is some net polarity to the compound.A solvent is polar if it has a total dipole movement, that is if the molecule as a whole has a charge concentrated in one area. In the case of CH2Cl2, since it has 2 Cl groups (ewg) facing two opposite directions, the charge pull cancels out and it a nonpolar solvent.
Your book is wrong. Molecular dipoles come about because of two factors:I think the chlorines must be opposite and cancel the dipole because the book says that its a non-polar solvent. So just to clear something up, if there is a large dipole meaning a large difference between electronegativity than the solvent will be polar? Can you guys give me some examples of common solvents polar and non polar it would really help clear things up, thanks.
You might want to use a different book for your review. Fundamental errors are some of the most deadly on the MCAT. because many questions require that you reason your way through the information using fundamental information.I think the chlorines must be opposite and cancel the dipole because the book says that its a non-polar solvent.