Statement-I : Boiling points of carbonyl compounds > B.P of corresponding ethers and hydrocarbons.Statement-II: Dipole attractions stronger than London dispersion forces

Intermolecular attractions in  alcohols is intermolecular hydrogen bonding.Intermolecular attactions in carbonyl compounds are dipole-dipole attractions.Ketones are more polar than aldehydes. Inter molecular attractions in ethers are weak dipole -dipole attraction.intermolecular attractions in hydrocarbonds are very weak London dispersion forces.∴ Boiling point of (nearly same molecular weight) alcohols > ketones > aldehydes > ethers > alkane. But as molecular weight ethers increases they become more unsymmetrical. In such cases the dipole -dipole attractions are very weak. They are weaker than dispersion forces in alkanes.CH3CH2OH>CH3CHO>CH3-O-CH3>CH3CH2CH3 CH3CH2CH2OH>CH3CHOH>CH3>CH3COCH3>CH3CH2CHO>CH3-O-C2H5>CH3CH2CH2CH3but CH3CH2CH2CH2OH>CH3COCH2CH3>CH3CH2CH2CHO>CH3CH2CH2CH2CH3>C2H5-O-C2H5It is intereseting to note that boiling point of ethoxyethane (307K) < n-pentane(309K)