Provide an example of the dipole moment of different molecules and their polarity.

The dipole moment of a molecule determines its polarity.

The dipole moment is the measure of the separation of positive and negative charges in a molecule. It is a vector quantity, which means it has both magnitude and direction. The unit of dipole moment is Debye (D).

Polar molecules have a dipole moment greater than zero, while nonpolar molecules have a dipole moment of zero. For example, water (H2O) is a polar molecule with a dipole moment of 1.85 D. This is because the oxygen atom is more electronegative than the hydrogen atoms, creating a partial negative charge on the oxygen and a partial positive charge on the hydrogens.

Carbon dioxide (CO2), on the other hand, is a nonpolar molecule with a dipole moment of zero. This is because the two oxygen atoms are equally electronegative, resulting in no separation of charges.

Another example of a polar molecule is ammonia (NH3), which has a dipole moment of 1.47 D. This is because the nitrogen atom is more electronegative than the hydrogen atoms, creating a partial negative charge on the nitrogen and partial positive charges on the hydrogens.

In summary, the dipole moment of a molecule determines its polarity. Polar molecules have a dipole moment greater than zero, while nonpolar molecules have a dipole moment of zero. Examples of polar molecules include water and ammonia, while carbon dioxide is an example of a nonpolar molecule.