Intermolecular forces significantly affect boiling points. - Hydrogen bonding is a strong type of intermolecular force present in alcohols. - Van der Waals forces (London dispersion forces and dipole-dipole interactions) also contribute to intermolecular attraction. - For homologous series of alcohols, boiling point generally increases with increasing molecular size and chain length due to increased van der Waals forces and more extensive hydrogen bonding.
Arrange the following set of compounds in order of their increasing boiling points - Pentan-1-ol, Butan-1-ol, Propan-1-ol, Methanol (1) Methanol < Propan-1-ol < Butan-1-ol < Pentan-1-ol (2) Methanol < Butan-1-ol < Pentan-1-ol < Propan-1-ol (3) Methanol < Pentan-1-ol < Butan-1-ol < Propan-1-ol (4) Methanol > Propan-1-ol > Butan-1-ol > Pentan-1-ol (5) Question not attempted
Asked in Department Recruitment 2024 (Chemist) 2024 · Topic: Alcohol (Physical Properties of Alcohols (boiling points, solubility, acidity, density))
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