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

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

Ethers are organic compounds that contain an oxygen atom bonded to two alkyl or aryl groups. The boiling and melting points of ethers depend on their molecular structure, specifically the size and shape of the alkyl or aryl groups attached to the oxygen atom.

For example, diethyl ether (C4H10O) has a boiling point of 34.6°C and a melting point of -116.3°C. This is because the two ethyl groups attached to the oxygen atom are relatively small and nonpolar, which allows for weak intermolecular forces between molecules. As a result, diethyl ether has a low boiling and melting point.

On the other hand, diphenyl ether (C12H10O) has a boiling point of 258°C and a melting point of 26°C. This is because the two phenyl groups attached to the oxygen atom are much larger and more polar than ethyl groups, which results in stronger intermolecular forces between molecules. As a result, diphenyl ether has a higher boiling and melting point.

Overall, the boiling and melting points of ethers can be used to predict their physical properties and behaviour in different chemical reactions.