Arrange the following 6-carbon compounds in order of their...

Arrange the following 6-carbon compounds in order of their expected boiling points, and explain your ranking:
(a) Hexane
(b) Hexan-1-ol
(c) Dipropyl ether $\left(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2}-\mathrm{O}-\mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{3}\right)$

Key Concepts

Intermolecular Forces

Intermolecular forces are the attractions between molecules that determine many physical properties, including boiling points. These forces include London dispersion forces, which are weak and present in all molecules, dipole-dipole interactions which occur between polar molecules, and hydrogen bonds, which are a strong type of dipole-dipole interaction that occur when hydrogen is bonded to electronegative atoms like oxygen. The strength and type of these forces directly affect the boiling point of a substance.

Impact of Functional Groups on Boiling Points

Functional groups in organic molecules affect the polarity and the type of intermolecular forces that the molecule can participate in. For example, alkanes with nonpolar characteristics display only weak London dispersion forces, resulting in lower boiling points. In contrast, the presence of an -OH group in alcohols allows for hydrogen bonding, significantly increasing boiling point. Ethers, while containing an oxygen, are less capable of hydrogen bonding compared to alcohols, leading to intermediate boiling points.

Hydrogen Bonding and Boiling Point Elevation

Hydrogen bonding is a particularly strong form of intermolecular attraction that occurs when hydrogen is directly bonded to a highly electronegative atom such as oxygen. This effect is responsible for a substantial increase in the boiling points of molecules that can engage in hydrogen bonding, such as alcohols. Consequently, molecules capable of hydrogen bonding, despite having similar molecular weights to non-hydrogen bonding molecules, will typically exhibit higher boiling points.

Transcript

Please give Ace some feedback