Describe the differences between the boiling and melting points of different alkanes.

The boiling and melting points of alkanes increase with increasing carbon chain length.

Alkanes are a group of hydrocarbons that have only single bonds between carbon atoms. The boiling and melting points of alkanes depend on their molecular size and shape. As the number of carbon atoms in the molecule increases, the boiling and melting points also increase. This is because larger molecules have stronger intermolecular forces of attraction, which require more energy to break.

For example, methane (CH4) has a boiling point of -161.5°C and a melting point of -182.5°C, while butane (C4H10) has a boiling point of -0.5°C and a melting point of -138.4°C. As the number of carbon atoms increases, the boiling and melting points increase due to the increased size and complexity of the molecule.

Branched alkanes have lower boiling and melting points than their straight-chain counterparts. This is because the branching reduces the surface area of the molecule, which reduces the strength of the intermolecular forces of attraction.

In summary, the boiling and melting points of alkanes increase with increasing carbon chain length. Branched alkanes have lower boiling and melting points than their straight-chain counterparts. These properties are important in determining the physical and chemical properties of alkanes, which have many practical applications in industry and everyday life.