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Chapter 11: Problem 69

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?

Short Answer

Expert verified
(a) The intermolecular forces between argon atoms are van der Waals forces, also known as London dispersion forces or weak inter-atomic forces, arising from temporary fluctuations in electron density. (b) Solid argon is not a covalent network solid because it does not consist of a continuous network of covalent bonds. Instead, it is held together by weak van der Waals forces, resulting in a relatively low melting temperature compared to covalent network solids.

Step by step solution

01

(a) Intermolecular Forces in Argon

Argon, being a noble gas (having a filled valence electron shell) is chemically inert and does not form molecules. Therefore, the intermolecular forces in argon gas are van der Waals forces, also known as London dispersion forces or weak inter-atomic forces. This type of force arises from temporary fluctuations in electron density around the argon atoms, which create instant dipoles that induce dipoles on neighboring atoms.
02

(b) Determine if Solid Argon is a Covalent Network Solid

A covalent network solid is a type of covalent crystal in which the atoms are joined together by a network of covalent bonds. These types of solids are generally very hard, brittle, and have high melting temperatures due to the strength of the covalent bonds in the network. Examples of covalent network solids include diamond, silica, and graphite. Solid argon, on the other hand, is composed of argon atoms held together by the weak van der Waals forces mentioned earlier. These forces are significantly weaker than the covalent bonds present in covalent network solids, resulting in solid argon having a relatively low melting temperature compared to covalent network solids. As a result, solid argon is not considered a covalent network solid because it does not consist of a continuous network of covalent bonds but instead is held together by weak van der Waals forces.

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Most popular questions from this chapter

The critical temperatures (K) and pressures (atm) of a series of halogenated methanes are as follows: $$ \begin{array}{lllll} \hline \text { Compound } & \mathrm{CCl}_{3} \mathrm{~F} & \mathrm{CCl}_{2} \mathrm{~F}_{2} & \mathrm{CClF}_{3} & \mathrm{CF}_{4} \\ \hline \text { Critical Temperature } & 471 & 385 & 302 & 227 \\ \text { Critical Pressure } & 43.5 & 40.6 & 38.2 & 37.0 \\ \hline \end{array} $$ (a) List the intermolecular forces that occur for each compound. (b) Predict the order of increasing intermolecular attraction, from least to most, for this series of compounds. (c) Predict the critical temperature and pressure for \(\mathrm{CCl}_{4}\) based on the trends in this table. Look up the experimentally determined critical temperatures and pressures for \(\mathrm{CCl}_{4}\), using a source such as the \(\mathrm{CRC}\) Handbook of Chemistry and Physics, and suggest a reason for any discrepancies.

In dichloromethane, \(\mathrm{CH}_{2} \mathrm{Cl}_{2}(\mu=1.60 \mathrm{D})\), the disper sion force contribution to the intermolecular attractive forces is about five times larger than the dipole-dipole contribution. Would you expect the relative importance of the two kinds of intermolecular attractive forces to differ (a) in dibromomethane \((\mu=1.43 \mathrm{D}),(\mathrm{b})\) in difluo romethane \((\mu=1.93 \mathrm{D}) ?\) Explain.

When an atom or group of atoms is substituted for an atom in benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\), the boiling pointchanges. Explair the order of the following boiling points: \(\mathrm{C}_{6} \mathrm{H}_{6}\left(80^{\circ} \mathrm{C}\right)\) \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{Cl}\left(132{ }^{\circ} \mathrm{C}\right), \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{Br}\left(156^{\circ} \mathrm{C}\right), \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{OH}\left(182{ }^{\circ} \mathrm{C}\right) .\)

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

(a) What is meant by the term polarizability? (b) Which of the following atoms would you expect to be most polarizable: \(\mathrm{N}, \mathrm{P}, \mathrm{As}, \mathrm{Sb}\) ? Explain. (c) Put the following molecules in order of increasing polarizability: \(\mathrm{GeCl}_{4}, \mathrm{CH}_{4}\) \(\mathrm{SiCl}_{4}, \mathrm{SiH}_{4}\), and \(\mathrm{GeBr}_{4}\). (d) Predict the order of boiling points of the substances in part (c).
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