Step 1: Factors influencing boiling point. Boiling point elevation correlates with the strength of intermolecular attractions: hydrogen bonding>dipole-dipole>van der Waals forces. Step 2: Analyzing 2-propanol. The –OH group enables robust intermolecular hydrogen bonding, substantially raising its boiling point. Step 3: Analyzing acetone. Acetone's polar carbonyl engages in dipole-dipole interactions but lacks the capacity for self-hydrogen-bonding, so it boils lower than alcohols. Step 4: Analyzing ether and propane. Ethers have weaker dipole interactions without hydrogen bonding; propane, being nonpolar, relies solely on weak London forces, giving the lowest boiling point. Step 5: Overall ranking. Intermolecular force strength: alcohol>ketone>ether>alkane. Step 6: Conclusion. 2-propanol possesses the highest boiling point among these compounds.
