The boiling point of propanol is 97^∘ C(370 K), much higher than that of either ethanethiol (37

step 1 explanation for the given question the boiling point of propanol boiling point of propanol and p

The boiling point of propanol is 97^∘ C(370 K), much higher...

The boiling point of propanol is $97^{\circ} \mathrm{C}(370 \mathrm{~K})$, much higher than that of either ethanethiol $\left(37^{\circ} \mathrm{C} / 310 \mathrm{~K}\right)$ or chloroethane $\left(13^{\circ} \mathrm{C} / 286 \mathrm{~K}\right)$, even though all three compounds have similar molecular masses. Explain.

Key Concepts

Intermolecular Forces

Intermolecular forces include all the attractions between molecules, such as dispersion forces, dipole-dipole interactions, and hydrogen bonding. Although compounds with similar molecular masses may exhibit similar dispersion forces, the presence or absence of additional intermolecular interactions, such as hydrogen bonding, can lead to significant differences in boiling points.

Molecular Structure and Functional Groups

The molecular structure, particularly the presence of specific functional groups, influences the type and strength of intermolecular forces a molecule can participate in. In the case of propanol, the hydroxyl functionality enables hydrogen bonding, whereas ethanethiol features a thiol group and chloroethane contains a halogen substituent. These differences lead to variations in polarity and the ability to form strong interactions, ultimately affecting the compound’s boiling point.

Hydrogen Bonding

Hydrogen bonding is a strong type of dipole-dipole interaction that occurs when hydrogen is bonded to a highly electronegative atom like oxygen. In molecules such as propanol, the presence of a hydroxyl (-OH) group allows for the formation of hydrogen bonds between molecules, significantly increasing the energy required to separate them in the liquid phase. This contributes to a higher boiling point compared to compounds that lack groups capable of hydrogen bonding.

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