Provide an example of the boiling point of different molecules and their intermolecular forces.

Different molecules have different boiling points due to their intermolecular forces.

The boiling point of a molecule is determined by the strength of its intermolecular forces. These forces include hydrogen bonding, dipole-dipole interactions, and London dispersion forces. Molecules with stronger intermolecular forces require more energy to break apart their bonds and reach their boiling point.

For example, water has a boiling point of 100°C due to its strong hydrogen bonding. The hydrogen bonds between water molecules require a lot of energy to break apart, which is why water boils at a high temperature. In contrast, methane has a boiling point of -161°C because it only has weak London dispersion forces between its molecules.

Another example is ethanol, which has a boiling point of 78°C due to its hydrogen bonding and dipole-dipole interactions. These intermolecular forces are stronger than the London dispersion forces in methane, which is why ethanol has a higher boiling point.

In summary, the boiling point of a molecule is determined by the strength of its intermolecular forces. Molecules with stronger intermolecular forces require more energy to break apart their bonds and reach their boiling point.