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Chapter 12: Problem 14

Which type (or types) of crystalline solid is characterized by each of the following? (a) High mobility of electrons throughout the solid; (b) softness, relatively low melting point; (c) high melting point and poor electrical conductivity; \((\mathbf{d})\) network of covalent bonds.

Short Answer

Expert verified
(a) Metallic solid; (b) Molecular solid; (c) Ionic solid; (d) Covalent network solid.

Step by step solution

01

(a) High mobility of electrons throughout the solid

A solid with high mobility of electrons throughout it is characterized as a metallic solid. In metallic solids, the valence electrons are shared among all the atoms, and this allows for high conductivity, ductility, and favorable electrical properties.
02

(b) Softness, relatively low melting point

Softness and a low melting point are characteristics of molecular solids. In molecular solids, the atoms are held together by weak van der Waals forces, hydrogen bonds, or dipole-dipole interactions, which facilitate a relatively easier separation of the particles compared to other types of crystalline solids.
03

(c) High melting point and poor electrical conductivity

A solid with a high melting point and poor electrical conductivity is an ionic solid. Ionic solids are composed of positive and negative ions arranged in an ordered fashion and held together by strong ionic bonds. The high melting point is due to the strong electrostatic forces between the ions, but the poor electrical conductivity is a result of immobile ions in the solid state.
04

(d) Network of covalent bonds

A solid that has a network of covalent bonds is a covalent network solid. In covalent network solids, the atoms are interconnected by a continuous network of covalent bonds, making them very strong and rigid. Some examples include diamond (carbon atoms connected by covalent bonds) and quartz (silicon dioxide).

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Most popular questions from this chapter

Potassium metal (atomic weight \(39.10 \mathrm{~g} / \mathrm{mol}\) ) adopts a body-centered cubic structure with a density of $0.856 \mathrm{~g} / \mathrm{cm}^{3}\(. (a) Use this information and Avogadro's number \)(6.022 \times\( \)10^{23}$ ) to estimate the atomic radius of potassium. (b) If potassium didn't react so vigorously, it could float on water. Use the answer from part (a) to estimate the density of \(\mathrm{K}\) if its structure were that of a cubic close-packed metal. Would it still float on water?

The densities of the elements Cr, Mn, Fe, and Cu are 7.15 , \(7.30,7.87,\) and \(8.96 \mathrm{~g} / \mathrm{cm}^{3}\), respectively. One of these elements crystallizes in a face-centered cubic structure; the other three crystallize in a body-centered cubic structure. Which one crystallizes in the face- centered cubic structure? Justify your answer.

Amorphous silica, \(\mathrm{SiO}_{2}\), has a density of about $2.2 \mathrm{~g} / \mathrm{cm}^{3}$, whereas the density of crystalline quartz, another form of \(\mathrm{SiO}_{2}\), is \(2.65 \mathrm{~g} / \mathrm{cm}^{3}\). Which of the following statements is the best explanation for the difference in density? (a) Amorphous silica is a network-covalent solid, but quartz is metallic. (b) Amorphous silica crystallizes in a primitive cubic lattice. (c) Quartz is harder than amorphous silica. (d) Quartz must have a larger unit cell than amorphous silica. (e) The atoms in amorphous silica do not pack as efficiently in three dimensions as compared to the atoms in quartz.

(a) Draw a picture that represents a crystalline solid at the atomic level. (b) Now draw a picture that represents an amorphous solid at the atomic level.

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) \(\mathrm{Fe}_{0.97} \mathrm{Si}_{0.03},\) (b) \(\mathrm{Fe}_{0.60} \mathrm{Ni}_{0.40}\) (c) \(\mathrm{SmCo}_{5}\)
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