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Chapter 12: Problem 31

Predict which of these liquids has the greater surface tension: ethanol \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)\) or dimethyl ether \(\left(\mathrm{CH}_{3} \mathrm{OCH}_{3}\right)\)

Short Answer

Expert verified
Ethanol will have a greater surface tension because it has stronger intermolecular forces due to the presence of hydrogen bonding.

Step by step solution

01

Identify the Intermolecular Forces in Ethanol

Ethanol \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)\) has two types of intermolecular forces: dispersion forces and hydrogen bonding. The dispersion forces occur between all molecules, these are the weakest intermolecular forces. The hydrogen bonding, on the other hand, occurs because of the -OH group in ethanol. Hydrogen bonding is a special type of dipole-dipole attraction between molecules, where a hydrogen atom is bonded to a highly electronegative atom (Oxygen in this case). This makes the hydrogen atom to acquire a partial positive charge and the oxygen atom a partial negative charge, thus creating an attraction between these molecules.
02

Identify the Intermolecular Forces in Dimethyl Ether

Dimethyl ether \(\left(\mathrm{CH}_{3} \mathrm{OCH}_{3}\right)\) also has two types of intermolecular forces: dispersion forces and dipole-dipole interaction. Here also, dispersion forces exist between all molecules. Despite having oxygen, dimethyl ether does not form hydrogen bonds. The reason for this is that the hydrogen atoms in dimethyl ether are not bonded to oxygen directly, thus a difference in electronegativities does not exist. Therefore, no hydrogen bonding takes place.
03

Compare the Strength of Intermolecular Forces

Hydrogen bonds are significantly stronger than both dispersion forces and dipole-dipole interactions. As ethanol has hydrogen bonds, and dimethyl ether does not, ethanol has stronger intermolecular forces.
04

Relate the Strength of Intermolecular Forces to Surface Tension

The greater the intermolecular forces, the greater the surface tension of the liquid. As ethanol has stronger intermolecular forces due to hydrogen bonding, it has a greater surface tension compared to dimethyl ether.

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Most popular questions from this chapter

A student heated a beaker of cold water (on a tripod) with a Bunsen burner. When the gas is ignited, she noticed that there was water condensed on the outside of the beaker. Explain what happened.

Which of these are molecular solids and which are covalent solids: \(\mathrm{Se}_{8}, \mathrm{HBr}, \mathrm{Si}, \mathrm{CO}_{2}, \mathrm{C}, \mathrm{P}_{4} \mathrm{O}_{6}, \mathrm{~B},\) \(\mathrm{SiH}_{4} ?\)

Diethyl ether has a boiling point of \(34.5^{\circ} \mathrm{C},\) and I-butanol has a boiling point of \(117^{\circ} \mathrm{C}\) Both of these compounds have the same numbers and types of atoms. Explain the difference in their boiling points.

A beaker of water is heated to boiling by a Bunsen burner. Would adding another burner raise the boiling point of water? Explain.

Why are metals good conductors of heat and electricity? Why does the ability of a metal to conduct electricity decrease with increasing temperature?
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