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Chapter 11: Problem 17

Describe the intermolecular forces that must be overcome to convert these substances from a liquid to a gas: (a) SO \(_{2}\) (b) \(\mathrm{CH}_{3} \mathrm{COOH},(\mathbf{c}) \mathrm{H}_{2} \mathrm{S}\) .

Short Answer

Expert verified
To convert (a) SO\(_{2}\) from a liquid to a gas, we must overcome London dispersion forces and dipole-dipole interactions. For (b) CH\(_{3}\)COOH, we must overcome London dispersion forces, dipole-dipole interactions, and hydrogen bonding. And for (c) H\(_{2}\)S, we must overcome London dispersion forces and dipole-dipole interactions. Increasing the temperature provides the kinetic energy needed for the molecules to overcome these intermolecular forces and enter the gaseous phase.

Step by step solution

01

(a) Intermolecular forces in SO\(_{2}\)

(Sulfur dioxide, or SO\(_{2}\), is a polar molecule due to the differences in electronegativity between sulfur and oxygen atoms. This results in two types of intermolecular forces: London dispersion forces, which are present in all molecules, and dipole-dipole interactions, which are specific to polar molecules.)
02

(a) Overcoming these forces

(To convert SO\(_{2}\) from a liquid to a gas, we must provide energy to overcome both the London dispersion forces and the dipole-dipole interactions. As the temperature increases, the kinetic energy of SO\(_{2}\) molecules increases, allowing them to overcome these forces and enter the gaseous phase.)
03

(b) Intermolecular forces in CH\(_{3}\)COOH

(Acetic acid, or CH\(_{3}\)COOH, is a polar molecule with an additional feature, an -OH group. This results in three types of intermolecular forces being present: London dispersion forces, dipole-dipole interactions, and hydrogen bonding, the latter of which occurs due to the presence of hydrogen atoms bonded to highly electronegative oxygen atoms.)
04

(b) Overcoming these forces

(To convert CH\(_{3}\)COOH from a liquid to a gas, we must provide energy to overcome all three intermolecular forces: London dispersion forces, dipole-dipole interactions, and hydrogen bonding. As the temperature increases, the kinetic energy of CH\(_{3}\)COOH molecules increases, allowing them to overcome these forces and enter the gaseous phase.)
05

(c) Intermolecular forces in H\(_{2}\)S

(Hydrogen sulfide, or H\(_{2}\)S, is also a polar molecule due to the difference in electronegativity between hydrogen and sulfur atoms. This results in two types of intermolecular forces being present: London dispersion forces and dipole-dipole interactions.)
06

(c) Overcoming these forces

(To convert H\(_{2}\)S from a liquid to a gas, we must provide energy to overcome both the London dispersion forces and the dipole-dipole interactions. As the temperature increases, the kinetic energy of H\(_{2}\)S molecules increases, allowing them to overcome these forces and enter the gaseous phase.)

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Most popular questions from this chapter

List the three states of matter in order of (a) increasing molecular disorder and (b) increasing intermolecular attraction. (c) Which state of matter is most easily compressed?

Indicate whether each statement is true or false: (a) The critical pressure of a substance is the pressure at which it turns into a solid at room temperature. (b) The critical temperature of a substance is the highest temperature at which the liquid phase can form. (c) Generally speaking, the higher the critical temperature of a substance, the lower its critical pressure. (\boldsymbol{d} ) In general the more intermolecular forces there are in a substance, the higher its critical temperature and pressure.

Acetone \(\left[\left(\mathrm{CH}_{3}\right)_{2} \mathrm{CO}\right]\) is widely used as an industrial solvent. (a) Draw the Lewis structure for the acetone molecule and predict the geometry around each carbon atom. (b) Is the acetone molecule polar or nonpolar? (c) What kinds of intermolecular attractive forces exist between acetone mol-ecules? (\boldsymbol{d} 1 Propanol ~ ( C H ~ \(_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{OH}\) ) has a molecular weight that is very similar to that of acetone, yet acetone boils at \(56.5^{\circ} \mathrm{C}\) and 1 -propanol boils at \(97.2^{\circ} \mathrm{C}\) . Explain the difference.

Butane and 2 -methylpropane, whose space-filling models are shown here, are both nonpolar and have the same molecular formula, \(\mathrm{C}_{4} \mathrm{H}_{10},\) yet butane has the higher boiling point \(\left(-0.5^{\circ} \mathrm{C}\) compared to \(-11.7^{\circ} \mathrm{C}\right) .\) Explain.

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.
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