Provide an example of the boiling and melting points of different alkenes.

The boiling and melting points of alkenes vary depending on their molecular structure and size.

Alkenes are unsaturated hydrocarbons that contain at least one carbon-carbon double bond. The boiling and melting points of alkenes are influenced by the strength of the intermolecular forces between the molecules. The larger the molecule, the stronger the intermolecular forces, and the higher the boiling and melting points.

For example, ethene (C2H4) has a boiling point of -103.7°C and a melting point of -169.4°C. This is because ethene is a small molecule with weak intermolecular forces. In contrast, propene (C3H6) has a boiling point of -47.6°C and a melting point of -185.2°C. Propene is a larger molecule than ethene, so it has stronger intermolecular forces.

Similarly, butene (C4H8) has a boiling point of -6.3°C and a melting point of -185.2°C. Butene is larger than propene, so it has even stronger intermolecular forces. The trend continues with larger alkenes having higher boiling and melting points.

In summary, the boiling and melting points of alkenes depend on their molecular size and structure. The larger the molecule, the stronger the intermolecular forces, and the higher the boiling and melting points.