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Chapter 11: Problem 82

One of the attractive features of ionic liquids is their low vapor pressure, which in turn tends to make them nonflammable. Why do you think ionic liquids have lower vapor pressures than most room-temperature molecular liquids?

Short Answer

Expert verified
Ionic liquids have lower vapor pressures than most room-temperature molecular liquids because they have stronger intermolecular forces, primarily due to the significant Coulombic forces between their cations and anions. In contrast, room-temperature molecular liquids have weaker forces, such as dipole-dipole, hydrogen bonding, and van der Waals forces. Stronger intermolecular forces require more energy for evaporation, resulting in lower vapor pressures and making ionic liquids nonflammable.

Step by step solution

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1. Understanding the composition of ionic liquids

Ionic liquids are composed of ions, specifically cations and anions. These ions are not well-coordinated, meaning that they are not highly ordered in their structure. In ionic liquids, the electrostatic forces between cations and anions, called Coulombic forces, are a significant contributor to the overall intermolecular forces present in the liquid.
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2. Understanding the composition of room-temperature molecular liquids

Room-temperature molecular liquids consist of neutral molecules which interact through various types of intermolecular forces including dipole-dipole, hydrogen bonding, and van der Waals forces. These forces tend to be weaker than the forces present in ionic liquids.
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3. The relationship between intermolecular forces and vapor pressure

Vapor pressure is influenced by the strength of the intermolecular forces present in a substance. A substance with stronger intermolecular forces requires more energy to evaporate, leading to a lower vapor pressure. Conversely, a substance with weaker intermolecular forces requires less energy to evaporate, resulting in a higher vapor pressure.
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4. Comparing intermolecular forces in ionic and molecular liquids

As discussed earlier, ionic liquids have significant Coulombic forces acting between the ions that contribute to the overall intermolecular forces present in the liquid, making them stronger compared to the forces in room-temperature molecular liquids. Room-temperature molecular liquids have weaker intermolecular forces such as dipole-dipole, hydrogen bonding, and van der Waals forces, which are not as strong as the ionic forces in ionic liquids.
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5. Connecting the strength of intermolecular forces to the vapor pressure of ionic liquids

The stronger intermolecular forces in ionic liquids mean that more energy is required for these substances to evaporate, or transition to their gas phase. As a result, ionic liquids have lower vapor pressures compared to room-temperature molecular liquids, which have weaker intermolecular forces and, therefore, higher vapor pressures. This explains why ionic liquids have lower vapor pressures and tend to be nonflammable compared to most room-temperature molecular liquids.

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Most popular questions from this chapter

Propyl alcohol \(\left(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{OH}\right)\) and isopropyl alcohol \(\left[\left(\mathrm{CH}_{3}\right)_{2} \mathrm{CHOH}\right],\) whose space- filling models are shown, have boiling points of 97.2 and \(82.5^{\circ} \mathrm{C}\) , respectively. Explain why the boiling point of propyl alcohol is higher, even though both have the molecular formula, \(\mathrm{C}_{3} \mathrm{H}_{8} \mathrm{O}\) .

At \(25^{\circ} \mathrm{C}\) gallium is a solid with a density of 5.91 \(\mathrm{g} / \mathrm{cm}^{3} .\) Its melting point, \(29.8^{\circ} \mathrm{C},\) is low enough that you can melt it by holding it in your hand. The density of liquid gallium just above the melting point is 6.1 \(\mathrm{g} / \mathrm{cm}^{3} .\) Based on this information, what unusual feature would you expect to find in the phase diagram of gallium?

(a) What is the significance of the triple point in a phase diagram? (b) Could you measure the triple point of water by measuring the temperature in a vessel in which water vapor, liquid water, and ice are in equilibrium under 1 atm of air? Explain.

(a) What is the relationship between surface tension and temperature? (b) What is the relationship between viscosity and temperature? (c) Why do substances with high surface tension also tend to have high viscosities?

Look up and compare the normal boiling points and normal melting points of \(\mathrm{H}_{2} \mathrm{O}\) and \(\mathrm{H}_{2} \mathrm{S}\) . Based on these physical properties, which substance has stronger intermolecular forces? What kinds of intermolecular forces exist for each molecule?
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