Polar and Nonpolar Molecules


Examples of Polar and Nonpolar Molecules
Bonding electrons are evenly distributed in nonpolar molecules, but unevenly distributed in polar molecules.

Polar and nonpolar molecules are the two broad classes of molecules. Polarity describes the distribution of electrical charge around a molecule. Charge is evenly distributed in a nonpolar molecule, but unevenly distributed in a polar molecule. In other words, a polar molecule has regions of partial charge.

Here are examples of polar and nonpolar molecules, a look at how polarity relates to ionic and covalent bonds, and how you can use polarity to predict which molecules will mix.

Polar Molecules

A polar molecule has a dipole, where part of the molecule has a partial positive charge and part has a partial negative charge. A polar molecule has an asymmetric shape, lone electron pair, or central atom bonded to other atoms with different electronegativity values. Usually, a polar molecule contains ionic or polar covalent bonds. Examples of polar molecules include:

  • Water – H2O
  • Ammonia – NH3
  • Sulfur dioxide – SO2
  • Hydrogen sulfide – H2S
  • Carbon monoxide – CO
  • Ozone – O3
  • Hydrofluoric acid – HF (and other molecules with a single H)
  • Ethanol – C2H6O (and other alcohols with an OH at one end)
  • Sucrose – C12H22O11 (and other sugars with OH groups)

Polar molecules are often hydrophilic and soluble in polar solvents. Polar molecules often have higher melting points than nonpolar molecules with similar molar masses. This is due to intermolecular forces between polar molecules, such as hydrogen bonding.

Nonpolar Molecules

Nonpolar molecules form either when electrons are equally shared between atoms in a molecule or when the arrangement of electrons in a molecule is symmetrical so that dipole charges cancel each other out. Examples of nonpolar molecules include:

  • Any of the noble gases: He, Ne, Ar, Kr, Xe (Although, technically these are atoms and not molecules.)
  • Any of the homonuclear diatomic elements: H2, N2, O2, Cl2 (These are truly nonpolar molecules.)
  • Carbon dioxide – CO2
  • Boron trifluoride – BF3
  • Benzene – C6H6
  • Carbon tetrachloride – CCl4
  • Methane – CH4
  • Ethylene – C2H4
  • Hydrocarbon liquids, such as gasoline and toluene
  • Most organic molecules, with exceptions (like alcohols and sugars)

Nonpolar molecules share some common properties. They tend to be water insoluble at room temperature, hydrophobic, and able to dissolve other nonpolar compounds.

Nonpolar Molecules With Polar Bonds

Polarity depends on the relative electronegativity values between two atoms forming a chemical bond. Two atoms with the same electronegativity values form a covalent bond. Electrons are shared evenly between atoms in a covalent bond, so the bond is nonpolar. Atoms with slightly different electronegativity values form polar covalent bonds. When electronegativity values between atoms are very different, ionic bonds form. Ionic bonds are highly polar.

Often, the polarity of the bonds is the same as the polarity of the molecule. However, there are nonpolar molecules with polar bonds and polar molecules with nonpolar bonds! For example, boron trifluoride is a nonpolar molecule that contains polar covalent bonds. BF3 is a trigonal planar molecule that evenly distributes electrical charge around the molecule, even though the bond between the boron and fluorine atoms is polar. Ozone is an example of a polar molecule made of nonpolar covalent bonds. The chemical bonds between oxygen molecules in O3 are purely covalent because the atoms have identical electronegativity values. However, the ozone molecule has a bent shape (like water) and its electrons don’t spend equal time with all three atoms. The middle atom has a partial positive electrical charge, while the two outer atoms each bear a partial negative charge.

Polarity and Miscibility

You can use polarity to predict whether or not two compounds are miscible (will mix to form a solution). The rule of thumb is that “like dissolves like.” What this means is that polar solvents dissolve polar solutes, while nonpolar solvents dissolve nonpolar solutes. This explains why alcohol and water are completely miscible (both polar) and why oil and water don’t mix (nonpolar with polar).

A compound with an intermediate polarity between one molecule and another can act as a go-between to dissolve a chemical into a solvent when it’s normally insoluble. For example, to mix an ionic or polar compound into an organic nonpolar solvent, you might first dissolve it in ethanol. Ethanol is only slightly polar, but often it’s enough to dissolve the solute. After the polar molecule has dissolved, mix the ethanol solution into a nonpolar organic solvent, such as xylene or benzene.

References

  • Ingold, C. K.; Ingold, E. H. (1926). “The Nature of the Alternating Effect in Carbon Chains. Part V. A Discussion of Aromatic Substitution with Special Reference to Respective Roles of Polar and Nonpolar Dissociation; and a Further Study of the Relative Directive Efficiencies of Oxygen and Nitrogen”. J. Chem. Soc.: 1310–1328. doi:10.1039/jr9262901310
  • Mack, Kenneth M.; Muenter, J. S. (1977). “Stark and Zeeman properties of ozone from molecular beam spectroscopy”. Journal of Chemical Physics. 66 (12): 5278–5283. doi:10.1063/1.433909
  • Pauling, L. (1960). The Nature of the Chemical Bond (3rd ed.). Oxford University Press. ISBN 0801403332.
  • Ziaei-Moayyed, Maryam; Goodman, Edward; Williams, Peter (November 1,2000). “Electrical Deflection of Polar Liquid Streams: A Misunderstood Demonstration”. Journal of Chemical Education. 77 (11): 1520. doi:10.1021/ed077p1520

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