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Chapter 11: Problem 12

At room temperature, \(\mathrm{CO}_{2}\) is a gas, \(\mathrm{CCl}_{4}\) is a liquid, and \(\mathrm{C}_{60}\) (fullerene) is a solid. List these substances in order of (a) increasing intermolecular energy of attraction and (b) increasing boiling point.

Short Answer

Expert verified
In terms of (a) increasing intermolecular energy of attraction and (b) increasing boiling point, the order is 颁翱鈧� < CCl鈧� < C鈧嗏個. 颁翱鈧� has the weakest London dispersion forces, followed by CCl鈧�, and C鈧嗏個 with the strongest London dispersion forces. Consequently, 颁翱鈧� has the lowest boiling point, followed by CCl鈧�, and C鈧嗏個 with the highest boiling point.

Step by step solution

01

颁翱鈧� < CCl鈧� < C鈧嗏個

In terms of increasing intermolecular energy of attraction, it will be 颁翱鈧� (with the weakest London dispersion forces), followed by CCl鈧�, and finally C鈧嗏個 (with the strongest London dispersion forces). #b. Increasing Boiling Point # The boiling point of a substance is directly related to its intermolecular forces. Stronger intermolecular forces lead to higher boiling points because more energy is needed to break the bonds between the molecules.
02

颁翱鈧� < CCl鈧� < C鈧嗏個

As 颁翱鈧� has the weakest intermolecular forces, it will have the lowest boiling point, followed by CCl鈧�, and then C鈧嗏個 (with the strongest intermolecular forces) will have the highest boiling point.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Boiling Point
The boiling point of a substance is the temperature at which its vapor pressure equals the external pressure surrounding the liquid, causing the liquid to turn into a gas.
This conversion requires energy to overcome the intermolecular forces holding the molecules together in the liquid state.
  • Substances with stronger intermolecular forces will have higher boiling points because more energy is needed to separate the molecules.
  • For example, in the original problem, \( ext{C}_{60} \) (fullerene), with the strongest intermolecular forces, has the highest boiling point.
  • The sequence then is: \( ext{CO}_{2} \) < \( ext{CCl}_{4} \) < \( ext{C}_{60} \).
Understanding boiling points helps in predicting the physical state of a substance at a given temperature. It's a crucial factor in processes such as distillation and in explaining phenomena like why water boils faster at high altitudes.
London Dispersion Forces
London Dispersion Forces are the weakest type of intermolecular forces, also known as Van der Waals forces.
These forces occur between all atoms and molecules due to fluctuations in the electron cloud that create temporary dipoles.
  • They are significant in nonpolar molecules where no permanent dipole exists.
  • The strength of London Dispersion Forces increases with the size and mass of the molecule.
  • In the original exercise, \( ext{CO}_{2} \) has the weakest London Dispersion Forces, whereas \( ext{C}_{60} \) has the strongest due to its larger size.
These forces are essential in understanding the relative volatility, boiling points, and solubility of nonpolar substances. While weak individually, London dispersion forces can be substantial when a molecule has a large surface area. They often determine the physical properties of substances, especially those that are nonpolar.
States of Matter
The states of matter 鈥� solid, liquid, and gas 鈥� are fundamentally determined by the strength of the intermolecular forces between their molecules.
Each state represents a different arrangement and motion of molecules.
  • In solids, molecules are closely packed with strong intermolecular forces, keeping them in fixed positions.
  • Liquids have intermediate intermolecular attractions, allowing their molecules to flow while still being relatively close.
  • Gases have very weak intermolecular forces, with molecules far apart and moving freely.
In the exercise provided:
\( ext{CO}_{2} \) is a gas, indicating it has weak intermolecular forces;
\( ext{CCl}_{4} \) is a liquid with moderate forces; and \( ext{C}_{60} \) is a solid with strong intermolecular forces.
Understanding the states of matter is key to grasping how substances behave under different conditions, from everyday experiences to industrial applications.

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Most popular questions from this chapter

True or false: (a) Molecules containing polar bonds must be polar molecules and have dipole-dipole forces. (b) For the halogen gases, the dispersion forces decrease while the boiling points increase as you go down the column in the periodic table. (c) In terms of the total attractive forces for a given substance, the more polar bonds there are in a molecule, the stronger the dipole-dipole interaction. \(\mathbf{d}\) ) All other factors being the same, total attractive forces between linear molecules are greater than those between molecules whose shapes are nearly spherical. (e) The more electronegative the atom, the more polarizable it is.

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

Based on the type or types of intermolecular forces, predict the substance in each pair that has the higher boiling point: (a) propane \(\left(\mathrm{C}_{3} \mathrm{H}_{8}\right)\) or \(n\) -butane \(\left(\mathrm{C}_{4} \mathrm{H}_{10}\right),(\mathbf{b})\) diethyl ether \(\left(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OCH}_{2} \mathrm{CH}_{3}\right)\) or 1 -butanol \(\left(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{OH}\right)\) (c) sulfur dioxide \(\left(\mathrm{SO}_{2}\right)\) or sulfur trioxide \(\left(\mathrm{SO}_{3}\right)\), (d) phosgene \(\left(\mathrm{Cl}_{2} \mathrm{CO}\right)\) or formaldehyde \(\left(\mathrm{H}_{2} \mathrm{CO}\right)\). Look up and compare the normal boiling points and nor-

Indicate whether each statement is true or false: (a) The liquid crystal state is another phase of matter, just like solid, liquid, and gas. (b) Liquid crystalline molecules are generally spherical in shape. (c) Molecules that exhibit a liquid crystalline phase do so at well-defined temperatures and pressures. (d) Molecules that exhibit a liquid crystalline phase show weaker-than- expected intermolecular forces. (e) Molecules containing only carbon and hydrogen are likely to form liquid crystalline phases. (f) Molecules can exhibit more than one liquid crystalline phase.

Appendix \(\mathrm{B}\) lists the vapor pressure of water at various external pressures. (a) Plot the data in Appendix B,vapor pressure versus temperature \(\left({ }^{\circ} \mathrm{C}\right) .\) From your plot, estimate the vapor pressure of water at body temperature, \(37^{\circ} \mathrm{C}\). (b) Explain the significance of the data point at \(101.3 \mathrm{kPa}, 100^{\circ} \mathrm{C} .(\mathbf{c}) \mathrm{A}\) city at an altitude of \(1525 \mathrm{~m}\) above sea level has a barometric pressure of \(84.3 \mathrm{kPa}\). To what temperature would you have to heat water to boil it in this city? (d) A city at an altitude of \(150 \mathrm{~m}\) below sea level would have a barometric pressure of \(103.14 \mathrm{kPa}\). To what temperature would you have to heat water to boil it in this city?
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