Question:
Which among the following will have the highest boiling point?
Which among the following will have the highest boiling point?
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Hydrogen bonding is the strongest intermolecular force among the given options and increases boiling point significantly.
Updated On: Jun 19, 2026
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The Correct Option is A
Solution and Explanation
Step 1: Understanding boiling point factors.
Boiling point depends mainly on intermolecular forces such as hydrogen bonding, dipole-dipole interactions, and van der Waals forces. Stronger intermolecular forces lead to higher boiling points.
Step 2: Analyzing alcohol (2-propanol).
2-propanol contains an \(-OH\) group which forms strong intermolecular hydrogen bonding between molecules. This significantly increases its boiling point.
Step 3: Comparing acetone.
Acetone has a polar carbonyl group and shows dipole-dipole interactions, but it does not form hydrogen bonds between its own molecules, so its boiling point is lower than alcohols.
Step 4: Comparing ether and propane.
Ethers show weak dipole interactions and cannot hydrogen bond with themselves. Propane is nonpolar and only exhibits weak London dispersion forces, giving the lowest boiling point.
Step 5: Final comparison.
Strength of intermolecular forces: \[ \text{Alcohol} > \text{Acetone} > \text{Ether} > \text{Alkane} \]
Step 6: Final conclusion.
Thus, 2-propanol has the highest boiling point among the given compounds.
Final Answer: \[ \boxed{\text{2-propanol}} \]
Boiling point depends mainly on intermolecular forces such as hydrogen bonding, dipole-dipole interactions, and van der Waals forces. Stronger intermolecular forces lead to higher boiling points.
Step 2: Analyzing alcohol (2-propanol).
2-propanol contains an \(-OH\) group which forms strong intermolecular hydrogen bonding between molecules. This significantly increases its boiling point.
Step 3: Comparing acetone.
Acetone has a polar carbonyl group and shows dipole-dipole interactions, but it does not form hydrogen bonds between its own molecules, so its boiling point is lower than alcohols.
Step 4: Comparing ether and propane.
Ethers show weak dipole interactions and cannot hydrogen bond with themselves. Propane is nonpolar and only exhibits weak London dispersion forces, giving the lowest boiling point.
Step 5: Final comparison.
Strength of intermolecular forces: \[ \text{Alcohol} > \text{Acetone} > \text{Ether} > \text{Alkane} \]
Step 6: Final conclusion.
Thus, 2-propanol has the highest boiling point among the given compounds.
Final Answer: \[ \boxed{\text{2-propanol}} \]
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