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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) Intermolecular interactions are broken when a liquid is converted to a gas during the process of vaporization.

Step by step solution

01

Part (a): Understanding intermolecular and intramolecular interactions

Intermolecular interactions are the forces of attraction or repulsion between particles (atoms, molecules, or ions) in a substance. Some examples of intermolecular forces include hydrogen bonding, dipole-dipole interactions, and van der Waals forces. Intramolecular interactions, on the other hand, are the forces that hold atoms together within a molecule. These forces are chemical bonds, such as covalent bonds, ionic bonds, and metallic bonds.
02

Part (a): Identifying the stronger type of interaction

Generally, intramolecular interactions are stronger than intermolecular interactions. This is because chemical bonds, which are within molecules, have more energy and are more difficult to break than the forces of attraction or repulsion between particles in a substance.
03

Part (b): Understanding the process of liquid to gas conversion

When a liquid is converted to a gas, a substance undergoes a change of state called vaporization. During vaporization, particles in the liquid phase gain enough energy to overcome the forces of attraction between them, allowing them to move freely and become part of the gas phase.
04

Part (b): Identifying the type of interactions broken during vaporization

Vaporization involves breaking the intermolecular interactions between particles in a substance, as these are the forces that hold them together in the liquid phase. The intramolecular interactions within molecules usually remain intact during this process, as they are stronger and involve more energy.

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Most popular questions from this chapter

Ethylene glycol \(\left(\mathrm{HOCH}_{2} \mathrm{CH}_{2} \mathrm{OH}\right)\) and pentane \(\left(\mathrm{C}_{5} \mathrm{H}_{12}\right)\) are both liquids at room temperature and room pressure, and have about the same molecular weight. (a) One of these liquids is much more viscous than the other. Which one do you predict is more viscous? (b) One of these liquids has a much lower normal boiling point \(\left(36.1^{\circ} \mathrm{C}\right)\) compared to the other one \(\left(198^{\circ} \mathrm{C}\right)\). Which liquid has the lower normal boiling point? (c) One of these liquids is the major component in antifreeze in automobile engines. Which liquid would you expect to be used as antifreeze? (d) One of these liquids is used as a "blowing agent" in the manufacture of polystyrene foam because it is so volatile. Which liquid would you expect to be used as a blowing agent?

The following data present the temperatures at which certain vapor pressures are achieved for dichloromethane $\left(\mathrm{CH}_{2} \mathrm{Cl}_{2}\right)\( and methyl iodide \)\left(\mathrm{CH}_{3} \mathrm{I}\right):$ (a) Which of the two substances is expected to have the greater dipole-dipole forces? Which is expected to have the greater dispersion forces? Based on your answers, explain why it is difficult to predict which compound would be more volatile. (b) Which compound would you expect to have the higher boiling point? Check your answer in a reference book such as the CRC Handbook of Chemistry and Physics. (c) The order of volatility of these two substances changes as the temperature is increased. What quantity must be different for the two substances for this phenomenon to occur? (d) Substantiate your answer for part (c) by drawing an appropriate graph.

(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?

(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 $101.32 \mathrm{kPa}$ of air? Explain.

(a) Do you expect the viscosity of glycerol, $\mathrm{C}_{3} \mathrm{H}_{5}(\mathrm{OH})_{3}$, to be larger or smaller than that of 1 -propanol, \(\mathrm{C}_{3} \mathrm{H}_{7} \mathrm{OH} ?\) (b) Explain. [Section 11.3\(]\)
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