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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 solids are characterized by high mobility of electrons throughout the solid. b) Molecular solids are characterized by softness and relatively low melting points. c) Ionic solids are characterized by high melting points and poor electrical conductivity. d) Covalent network solids are characterized by a network of covalent bonds.

Step by step solution

01

a) High mobility of electrons throughout the solid

High mobility of electrons throughout the solid is a characteristic of metallic solids. In metallic solids, the metal atoms are packed closely together, and their valence electrons are delocalized, meaning they are free to move throughout the material. This delocalization of electrons is responsible for the high electrical conductivity and malleability of metallic solids.
02

b) Softness, relatively low melting point

Softness and relatively low melting points are characteristics of molecular solids. Molecular solids are made up of individual molecules held together by relatively weak intermolecular forces, such as van der Waals forces, hydrogen bonds, or dipole-dipole interactions. Due to these weak intermolecular forces, molecular solids tend to have relatively low melting points and a soft, sometimes waxy texture.
03

c) High melting point and poor electrical conductivity

High melting point and poor electrical conductivity are characteristics of ionic solids. Ionic solids consist of positively and negatively charged ions arranged in a crystalline lattice structure and are held together by strong electrostatic forces. These strong interactions between different ions mean that ionic solids have high melting points. However, they do not have free-moving electrons, resulting in poor electrical conductivity in the solid state.
04

d) Network of covalent bonds

Materials with a network of covalent bonds are called covalent network solids, such as diamonds and quartz. In covalent network solids, individual atoms are bonded together by strong covalent bonds, which extend throughout the entire crystal structure. These strong covalent bonds give covalent network solids a very high melting point and hardness. However, electrons are localized in covalent bonds, so covalent network solids generally have poor electrical conductivity.

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