What is a characteristic of larger hydrocarbons compared to smaller ones?

Larger hydrocarbons are characterized by having higher boiling points compared to smaller hydrocarbons. This is primarily due to their increased molecular size and mass, which lead to stronger van der Waals forces (intermolecular forces) acting between the molecules. As the size of a hydrocarbon increases, the number of electrons also increases, resulting in greater polarization and stronger interactions between individual molecules. This means that more energy is required to separate the molecules and convert the liquid into a gas, leading to a higher boiling point.

In contrast, smaller hydrocarbons are lighter, have fewer atoms, and exhibit weaker van der Waals forces, resulting in lower boiling points. This fundamental concept about the relationship between molecular size and boiling point is crucial when understanding the physical properties of hydrocarbons in chemistry.