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There are different cases when the dipole moments cancel out. You need to look at the VSEPR structure and the dipole moment of the individual bonds. If one of the individual bonds is more polar than another bond, there will be a net dipole moment, making the entire molecule polar. If all the bonds in the atom are polar and the entire molecule is non polar, it implies that each individual bond is equally polar and that the VSEPR structure causes the dipole moment to cancel out. Ex - CCl4 is non polar but Ch3Cl is polar. This is because although both have the same VSEPR structure, the dipole of the C-Cl bond is more than the C-H bond.
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