Arrange the following compounds in increasing order of their boiling point:
\[
\text{(CH}_3\text{)}_2\text{NH, CH}_3\text{CH}_2\text{NH}_2, \text{CH}_3\text{CH}_2\text{OH}
\]
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Boiling points increase with the strength of intermolecular forces. Alcohols have stronger hydrogen bonding than amines, which leads to higher boiling points.
To solve the problem, we need to arrange the given compounds in increasing order of their boiling points.
1. Understanding the Boiling Points: Boiling points of compounds are influenced by intermolecular forces such as hydrogen bonding, dipole-dipole interactions, and London dispersion forces. Stronger intermolecular forces usually result in higher boiling points.
2. Analyzing the Compounds: The given compounds are: - (CH₃)₂NH (Dimethylamine) - CH₃CH₂NH₂ (Ethylamine) - CH₃CH₂OH (Ethanol)
3. Boiling Points of Compounds: - (CH₃)₂NH (Dimethylamine): This compound is a simple amine. It exhibits hydrogen bonding, but it is weaker compared to alcohols. - CH₃CH₂NH₂ (Ethylamine): This is another amine, but it has a slightly higher boiling point than dimethylamine due to its larger molecular size and stronger dipole-dipole interactions. - CH₃CH₂OH (Ethanol): This compound has a hydroxyl group (-OH), which allows for strong hydrogen bonding, leading to a higher boiling point compared to the amines.
4. Order of Boiling Points: We can now arrange the compounds in increasing order of their boiling points based on the strength of the intermolecular forces:
Increasing Order of Boiling Points: (CH₃)₂NH < CH₃CH₂NH₂ < CH₃CH₂OH
Final Answer: The compounds in increasing order of their boiling points are: (CH₃)₂NH < CH₃CH₂NH₂ < CH₃CH₂OH.
