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Chapter 11: Problem 16

(a) Which is generally stronger, intermolecular interactions or intramolecular interactions? (b) Which of these kinds of interactions are broken when a liquid is converted to a gas?

Short Answer

Expert verified
(a) Intramolecular interactions are generally stronger than intermolecular interactions. (b) When a liquid is converted to a gas, it is the intermolecular interactions that are broken.

Step by step solution

01

Understand Intramolecular and Intermolecular Interactions

Intramolecular interactions are forces that hold atoms together within a molecule. These forces include ionic, covalent, and metallic bonds. Intermolecular interactions, on the other hand, are forces that occur between separate molecules, such as hydrogen bonding, dipole-dipole interactions, and London dispersion forces.
02

Comparison of Interaction Strengths

Intramolecular interactions, namely ionic, covalent, and metallic bonds, are generally stronger than intermolecular interactions. This is because intramolecular forces involve the sharing or transfer of electrons between atoms, resulting in strong bonding forces. Intermolecular forces, however, are the result of weaker electrical forces that occur between molecules, such as induced dipole-dipole interactions and van der Waals forces.
03

Part (a) Answer

So, intramolecular interactions are generally stronger than intermolecular interactions.
04

Breaking Interactions in Phase Change

When a liquid is converted to a gas, the substance undergoes a phase change. This phase change requires energy, which serves to break the intermolecular interactions that hold the molecules together in the liquid state. As these interactions are broken, the molecules gain enough energy to escape the liquid phase and become a gas.
05

Part (b) Answer

When a liquid is converted to a gas, it is the intermolecular interactions that are broken.

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Most popular questions from this chapter

As the intermolecular attractive forces between molecules increase in magnitude, do you expect each of the following to increase or decrease in magnitude? (a) Vapor pressure, (b) heat of vaporization, (c) boiling point, (d) freezing point, (e) viscosity, (f) surface tension, ( g) critical temperature.

(a) How does the average kinetic energy of molecules compare with the average energy of attraction between molecules in solids, liquids, and gases? (b) Why does increasing the temperature cause a solid substance to change in succession from a solid to a liquid to a gas? (c) What happens to a gas if you put it under extremely high pressure?

The smectic liquid crystalline phase can be said to be more highly ordered than the nematic phase. In what sense is this true?

Liquid butane \(\left(\mathrm{C}_{4} \mathrm{H}_{10}\right)\) is stored in cylinders to be used as a fuel. The normal boiling point of butane is listed as \(-0.5^{\circ} \mathrm{C}\) . (a) Suppose the tank is standing in the sun and reaches a temperature of \(35^{\circ} \mathrm{C}\) . Would you expect the pressure in the tank to be greater or less than atmospheric pressure? How does the pressure within the tank depend on how much liquid butane is in it? (b) Suppose the valve to the tank is opened and a few liters of butane are allowed to escape rapidly. What do you expect would happen to the temperature of the remaining liquid butane in the tank? Explain. (c) How much heat must be added to vaporize 250 \(\mathrm{g}\) of butane if its heat of vaporization is 21.3 \(\mathrm{kJ} / \mathrm{mol}\) ? What volume does this much butane occupy at 755 torr and \(35^{\circ} \mathrm{C} ?\)

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?
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