Diagram showing the net effect of symmetrical polar bonds within boron trifluoride cancelling out to give a net polarity of zero. δ- shows an increase in negative charge and δ+ shows an increase in positive charge. There are two possibilities a molecule may be nonpolar:
● there is almost no polarity in the bonds ( happens when there’s an equal sharing of electrons
between two different atoms);
● the symmetrical arrangement of polar bonds.
Household nonpolar compounds examples include oil, fats and gasoline. (CARBURANT) Thus, most nonpolar molecules are water-insoluble (hydrophobic) at room temperature. However, many nonpolar organic solvents, such as turpentine, are able to dissolve polar substances. If a polar and nonpolar molecule with similar molar masses are compared, in most of the cases, the polar molecule has a higher boiling point, because of the dipoles interaction between their molecules.
The most common form of such an interaction is the hydrogen bond, which is also known as the H-bond. There are a few examples such as:
● In the methane molecule (CH4) the four C–H bonds are arranged tetrahedrally around the
carbon atom. Each bond has polarity (though not very strong).
● The oxygen molecule (O2) does not have polarity in the covalent bond because of equal
electronegativity, hence there is no polarity in the molecule.