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Chapter 12: Problem 18

You are given a white substance that melts at \(100^{\circ} \mathrm{C}\) . The substance is soluble in water. Neither the solid nor the solution is a conductor of electricity. Which type of solid (molecular, metallic, covalent- network, or ionic) might this substance be?

Short Answer

Expert verified
The given substance might be a molecular solid, as it has a relatively low melting point (100°C), is soluble in water, and does not conduct electricity in either solid or solution forms.

Step by step solution

01

Analyze Molecular Solids

Molecular solids are composed of molecules held together by weak van der Waals forces or hydrogen bonds. They tend to have relatively low melting points, and they do not conduct electricity. When dissolved in water, they form non-conductive solutions. Considering all these properties, the substance could be a molecular solid.
02

Analyze Metallic Solids

Metallic solids are composed of metal atoms held together by metallic bonds. These solids have high melting points and are good conductors of electricity, both in solid form and when dissolved (forming ions in a solution). Considering the given properties, the substance cannot be a metallic solid because it does not conduct electricity.
03

Analyze Covalent-Network Solids

Covalent-network solids are composed of atoms connected by strong covalent bonds in a large network. They usually have high melting points and are not soluble in water. Also, they do not conduct electricity. Given these properties, our substance cannot be a covalent-network solid because it is soluble in water.
04

Analyze Ionic Solids

Ionic solids are composed of oppositely charged ions held together by strong ionic bonds. They have high melting points and can conduct electricity when dissolved in water (forming ions in a solution). However, they do not conduct electricity in their solid form. In this case, our substance cannot be an ionic solid because neither the solid nor the solution conducts electricity.
05

Determine the Type of Solid

Comparing the properties of the given substance with those of the various types of solids, we can conclude that the substance might be a molecular solid, as it fits the properties of having a relatively low melting point, being soluble in water, and not conducting electricity in either solid or solution forms.

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Most popular questions from this chapter

Indicate whether each statement is true or false: $$ \begin{array}{l}{\text { (a) The band gap of a semiconductor decreases as the parti- }} \\ {\text { cle size decreases in the } 1-10 \text { -nm range. }} \\\ {\text { (b) The light that is emitted from a semiconductor, upon }} \\\ {\text { external stimulation, becomes longer in wavelength as }} \\ {\text { the particle size of the semiconductor decreases. }}\end{array} $$

Clausthalite is a mineral composed of lead selenide (PbSe). The mineral adopts the rock salt structure. The density of PbSe at \(25^{\circ} \mathrm{C}\) is 8.27 \(\mathrm{g} / \mathrm{cm}^{3} .\) Calculate the length of an edge of the PbSe unit cell.

Both covalent-network solids and ionic solids can have melting points well in excess of room temperature, and both can be poor conductors of electricity in their pure form. However, in other ways their properties are quite different. $$ \begin{array}{l}{\text { (a) Which type of solid is more likely to dissolve in water? }} \\ {\text { (b) Which type of solid can become a considerably better }} \\ {\text { conductor of electricity via chemical substitution? }}\end{array} $$

For each of the following alloy compositions, indicate whether you would expect it to be a substitutional alloy, an interstitial alloy, or an intermetallic compound: $$ (a)\mathrm{Fe}_{0.97} \mathrm{Si}_{0.03}, \quad(\mathbf{b})\mathrm{Fe}_{0.60} \mathrm{Ni}_{0.40}, \quad(\mathbf{c}) \mathrm{Sm} \mathrm{Co}_{5} $$

Sodium metal (atomic weight 22.99 \(\mathrm{g} / \mathrm{mol}\) ) adopts a body- centered cubic structure with a density of 0.97 \(\mathrm{g} / \mathrm{cm}^{3}\) . (a) Use this information and Avogadro's number \(\left(N_{\mathrm{A}}=6.022 \times 10^{23} / \mathrm{mol}\right)\) to estimate the atomic radius of sodium. \((\mathbf{b})\) If sodium didn't react so vigorously, it could float on water. Use the answer from part (a) to estimate the density of Na if its structure were that of a cubic close packed metal. Would it still float on water?
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