Question

Which of the following will exhibit the highest boiling point?
(A) $C{H_3}C{H_2}OC{H_2}C{H_3}$
(B) $C{H_3}C{H_2}C{H_2}C{H_2}C{H_2}OH$
(C) $C{H_3}C{H_2}C{H_2}C{H_2}\left( {C{H_3}} \right)OH$
(D) $C{H_3}C{H_2}C{\left( {C{H_3}} \right)_2}OH$

Answer 1

Ethers are chemical compounds with the general molecular formula of $ROR$ . Alcohols exhibit hydrogen bonding. When the molecule has hydrogen bonding it has a high boiling point. The compounds with high molar mass have a high boiling point. Branching molecules will have a lower boiling point than unbranched molecules.

Complete Step By Step Answer:
Boiling point is defined as the temperature at which the substance in a liquid state converts into a vapor state.
The molecules with the same molecular formula but differ in branching have different boiling points. The unbranched structure has a high boiling point than the
In option A, the given molecule is $C{H_3}C{H_2}OC{H_2}C{H_3}$ which means it is ether, it does not involve in hydrogen bonding which means it has a low boiling point.
In the given option B, the molecule is $C{H_3}C{H_2}C{H_2}C{H_2}C{H_2}OH$ , this molecule involved in hydrogen bonding and does not have a branched structure, which leads to having a high boiling point.
In the given option C, the molecule is $C{H_3}C{H_2}C{H_2}C{H_2}\left( {C{H_3}} \right)OH$ , this molecule involved in hydrogen bonding and has branched structure, leads to have a low boiling point.
In the given option D, the molecule is $C{H_3}C{H_2}C{\left( {C{H_3}} \right)_2}OH$ , this molecule involved in hydrogen bonding and has a branched structure, leads to having a low boiling point.
Thus, $C{H_3}C{H_2}C{H_2}C{H_2}C{H_2}OH$ has a high boiling point.
Option A is the correct one.

Note:
The molecules with the same molecular formula, but with different structures like one is branched and the other is unbranched. The molecule which is unbranched has a high boiling point. This is due to the fact that the branching is inversely proportional to the boiling point.