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.

$\therefore$ 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.

$$\begin{gathered} {\mathrm{CH}}_3{\mathrm{CH}}_2\mathrm{OH}>{\mathrm{CH}}_3\mathrm{CHO}>{\mathrm{CH}}_3-\mathrm{O}-{\mathrm{CH}}_3>{\mathrm{CH}}_3{\mathrm{CH}}_2{\mathrm{CH}}_3 \\ {\mathrm{CH}}_3{\mathrm{CH}}_2{\mathrm{CH}}_2\mathrm{OH}>{\mathrm{CH}}_3\mathrm{CHOH}>{\mathrm{CH}}_3>{\mathrm{CH}}_3{\mathrm{COCH}}_3>{\mathrm{CH}}_3{\mathrm{CH}}_2\mathrm{CHO}>{\mathrm{CH}}_3-\mathrm{O}-{\mathrm{C}}_2{\mathrm{H}}_5>{\mathrm{CH}}_3{\mathrm{CH}}_2{\mathrm{CH}}_2{\mathrm{CH}}_3 \end{gathered}$$

but ${\mathrm{CH}}_3{\mathrm{CH}}_2{\mathrm{CH}}_2{\mathrm{CH}}_2\mathrm{OH}>{\mathrm{CH}}_3{\mathrm{COCH}}_2{\mathrm{CH}}_3>{\mathrm{CH}}_3{\mathrm{CH}}_2{\mathrm{CH}}_2\mathrm{CHO}>{\mathrm{CH}}_3{\mathrm{CH}}_2{\mathrm{CH}}_2{\mathrm{CH}}_2{\mathrm{CH}}_3>{\mathrm{C}}_2{\mathrm{H}}_5-\mathrm{O}-{\mathrm{C}}_2{\mathrm{H}}_5$

It is intereseting to note that boiling point of ethoxyethane (307K) < n-pentane(309K)