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Chapter 11: Problem 14

Based on what you have learned about intermolecular forces, would you say that matter is fundamentally attracted or repulsed by other matter?

Short Answer

Expert verified
From our analysis of intermolecular forces such as London dispersion forces, dipole-dipole interactions, and hydrogen bonding, we can conclude that matter is fundamentally attracted to other matter. Although repulsive forces may exist in certain circumstances, the overall impact of intermolecular forces is attractive, which allows molecules to come together and form substances with specific physical properties.

Step by step solution

01

Definition of Intermolecular Forces

Intermolecular forces are the forces that exist between molecules in a substance, which determine its physical properties like melting and boiling points, viscosity, and surface tension. These forces can be attractive or repulsive, and they include van der Waals forces (London dispersion forces, dipole-dipole, and dipole-induced dipole interactions) and hydrogen bonding.
02

Types of Intermolecular Forces

There are mainly three types of intermolecular forces: 1. London Dispersion Forces: These are weak attractions between temporary dipoles of non-polar molecules due to the random movements of electrons. 2. Dipole-Dipole Interactions: These are the attractive forces between the positive end of one polar molecule and the negative end of another polar molecule. 3. Hydrogen Bonding: This is a special kind of dipole-dipole interaction where the hydrogen atom is bonded to a highly electronegative element like nitrogen, oxygen, or fluorine; it forms a comparatively strong attraction with another electronegative atom in a different molecule.
03

The role of Intermolecular Forces

Overall, intermolecular forces are responsible for holding the matter together in the form of solids, liquids, or gases, and thus dictate its physical and chemical properties. The stronger the forces, the higher the boiling and melting points, and the more viscous and denser the substance becomes.
04

Conclusion

From our analysis of intermolecular forces, we can conclude that matter is fundamentally attracted to other matter. The reason being that most of these forces, like London dispersion forces, dipole-dipole interactions, and hydrogen bonding, are attractive in nature, allowing molecules to come together and form substances with specific physical properties. While there may be repulsive forces in certain circumstances, the overall impact of intermolecular forces is attractive, and thus, matter is fundamentally attracted to other matter.

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Most popular questions from this chapter

Look up and compare the normal boiling points and normal melting points of \(\mathrm{H}_{2} \mathrm{O}\) and \(\mathrm{H}_{2} \mathrm{~S}\). (a) Based on these physical properties, which substance has stronger intermolecular forces? What kind of intermolecular forces exist for each molecule? (b) Predict whether solid \(\mathrm{H}_{2} \mathrm{~S}\) is more or less dense than liquid \(\mathrm{H}_{2} \mathrm{~S}\). How does this compare to \(\mathrm{H}_{2} \mathrm{O} ?\) Explain. (c) Water has an unusually high specific heat. Is this related to its intermolecular forces? Explain.

(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 one atmosphere of air? Explain.

It is possible to change the temperature and pressure of a vessel containing argon gas so that the gas solidifies. (a) What intermolecular forces exist between argon atoms? (b) Is the solid argon a "covalent network solid"? Why or why not?

The elements xenon and gold both have solid-state structures with face- centered cubic unit cells, yet Xe melts at \(-112^{\circ} \mathrm{C}\) and gold melts at \(1064^{\circ} \mathrm{C}\). Account for these greatly different melting points.

(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?
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