Thiols have lower boiling points and are less water soluble...

Thiols have lower boiling points and are less water soluble than the corresponding alcohol (e.g., $\mathrm{CH}_3 \mathrm{CH}_2-\mathrm{OH}$ and $\mathrm{CH}_3 \mathrm{CH}_2-\mathrm{SH}$ ). Explain why.

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Key Concepts

Molecular Polarity and Intermolecular Forces

Molecular polarity arises from differences in electronegativity between atoms in a molecule, leading to permanent dipoles. This polarity enhances dipole-dipole interactions, which, along with hydrogen bonding, contributes to stronger intermolecular attractions. In the context of comparing similar functional groups, compounds with more polar bonds experience heightened intermolecular forces and consequently, higher boiling points and greater solubility in polar solvents. Conversely, molecules with less polar bonds have weaker intermolecular forces, leading to lower boiling points and reduced solubility.

Intermolecular Hydrogen Bonding

Intermolecular hydrogen bonding refers to the strong dipole-dipole interaction that occurs when a hydrogen atom is bonded to highly electronegative atoms like oxygen. This bonding allows molecules to attract each other more effectively, significantly increasing boiling points and solubility in water. In molecules capable of hydrogen bonding, such as alcohols, the presence of an -OH group leads to robust interactions between molecules, unlike in similar compounds that cannot engage in hydrogen bonding.

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