The melting temperatures of the two isomers of molecular formula C2H6O are-139 °c and-115 °c. Knowing that one of the isomers is an alcohol and the other a ether, indicate the melting temperature corresponding to each of them
The alcohol has intermolecular forces that the ether doesn't have; therefore, it it more difficult to break the crystal bonds for the alcohol. and it will have the higher melting point.
To determine the melting temperature corresponding to each isomer, we need to understand the structural differences between alcohols and ethers.
Alcohols have a hydroxyl (-OH) functional group attached to one of the carbon atoms in the molecule, while ethers have an oxygen atom (-O-) bonded to two carbon atoms.
It is known that alcohols generally have higher melting points compared to ethers due to the presence of intermolecular hydrogen bonding between the hydroxyl groups. Hydrogen bonding is a strong type of intermolecular force that results in a higher amount of energy required to break the bond and transition from a solid to a liquid state (melting).
Given the molecular formula C2H6O, let's consider the possible isomers:
1. If we have an alcohol, it would be ethanol (CH3CH2OH).
2. If we have an ether, it would be dimethyl ether (CH3OCH3).
Now, looking at the given melting temperatures (-139 °C and -115 °C), we can conclude that the lower melting temperature (-139 °C) corresponds to the ether, dimethyl ether (CH3OCH3) since ethers generally have lower melting points compared to alcohols.
Therefore, the higher melting temperature (-115 °C) belongs to the alcohol, ethanol (CH3CH2OH), as alcohols have generally higher melting points due to intermolecular hydrogen bonding.
In summary:
- (-139 °C) corresponds to the ether, dimethyl ether (CH3OCH3).
- (-115 °C) corresponds to the alcohol, ethanol (CH3CH2OH).