Question

08:19 hide compound 1 compound 2 the structural formulas of two compounds that are liquids at room temperature are shown above. which of the following statements best explains the observation that compound 1 boils at 35°c, whereas its structural isomer, compound 2, boils at 118°c? a molecules of compound 1 have a linear shape and no net dipole, whereas molecules of compound 2 have a bent shape and are polar. b molecules of compound 1 are bent less than molecules of compound 2; thus they have weaker dipole - dipole attractions. c there are dipole - dipole attractions among molecules of compound 1, whereas there are only dispersion forces among molecules of compound 2. d although there are dipole - dipole attractions among molecules of both compound 1 and compound 2, the - oh group in compound 2 allows strong

Explanation:

Hydrogen bonding occurs when a hydrogen atom is bonded to a highly electronegative atom like oxygen. Compound 2 has an -OH group which allows for hydrogen - bonding, a stronger intermolecular force compared to dipole - dipole forces present in compound 1. Stronger intermolecular forces lead to higher boiling points.

Answer:

D. Although there are dipole - dipole attractions among molecules of both compound 1 and compound 2, the -OH group in compound 2 allows strong hydrogen bonding.