How do boiling points relate to polar bonds?

1 Answer
Jun 14, 2015

Answer:

Boiling point increases with increasing strength of polar bonds, because more energy is required to break the stronger bonds.

Explanation:

There are 4 main types of polar intermolecular bonds:

Hydrogen bonds

The strongest polar bonds, these form between a hydrogen atom, and an electronegative acceptor atom.

The most common example of hydrogen bonds are those found in water, between hydrogen and the electronegative oxygen atom:http://commons.wikimedia.org/wiki/File:Hydrogen-bonding-in-water-2D

Permanent dipole - Permanent dipole bonds

These bonds form between two molecules possessing permanent dipoles a.k.a polar molecules. Usually the bond forms between an electronegative (𝛿-) atom, and a more electropositive (𝛿+) atom on a neighbouring molecule.

For example, in hydrochloric acid there is a permanent dipole-permanent dipole bond between the 𝛿- chlorine, and 𝛿+ hydrogen on a neighbouring molecule:
https://www.boundless.com/chemistry/textbooks/boundless-chemistry-textbook/liquids-and-solids-11/intermolecular-forces-84/dipole-dipole-force-372-572/

Permanent dipole - Induced dipole bonds

These bonds form between a polar molecule, and non-polar molecule.

When a polar molecule moves close to a non-polar molecule, the high electron density present at the 𝛿- end repels electrons in the neighbouring molecule. This causes an uneven distribution of electrons in the neighbouring molecule, leading to a 𝛿- and 𝛿+ end.

The, now polar, molecule, can now form an intermolecular bond with the original polar molecule.

Instantaneous dipole - Induced dipole bonds

Also known as London Dispersion forces, these bonds are formed in every species, regardless of polarity. They are the weakest polar bond.

They occur when there is a random uneven distribution of electrons in a molecule, leading to 𝛿+ and 𝛿- ends. When this polar molecule moves close to another molecule, it induces a dipole, and the polar bond is formed.

How are these different bonds related to boiling point?

When a liquid boils, the intermolecular bonds are broken, and the molecules are dispersed in the gas phase. Breaking these bonds requires energy, provided by heat.

A stronger intermolecular bond requires more energy to break, and a higher temperature is required to provide this energy. Thus, molecules with stronger intermolecular bonds have higher boiling points.

Boiling point decreases in the order:

Hydrogen bonds > Permanent dipole - Permanent dipole > Permanent dipole - Induced dipole > Instantaneous Dipole - Induced Dipole