How do the boiling points of aldehydes and ketones compare to hydrocarbons and ethers of similar molecular masses, and what interactions contribute to their higher boiling points?

The boiling points of aldehydes and ketones are generally higher than those of hydrocarbons and ethers of similar molecular masses. This is due to the presence of polar carbonyl groups in aldehydes and ketones, which allow for dipole-dipole interactions. Hydrocarbons lack such polar groups, resulting in weaker London dispersion forces. The dipole-dipole interactions in aldehydes and ketones contribute to elevated boiling points compared to hydrocarbons and ethers. Additionally, aldehydes and ketones can engage in hydrogen bonding, further increasing their boiling points, especially when compared to hydrocarbons and ethers with similar molecular masses.