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Chapter 12: Problem 46

Cite one reason why ceramic materials are, in general, harder yet more brittle than metals.

Short Answer

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Question: Explain one reason why ceramic materials tend to be harder yet more brittle than metals, considering their atomic structure and bonding. Answer: One reason why ceramic materials are harder yet more brittle than metals is due to their strong and directional ionic or covalent bonds. These bonds form a rigid and strongly bonded structure, which results in higher resistance to deformation as the individual atoms or ions find it more difficult to slide past each other, contributing to higher hardness. However, the same strong and rigid bonding structure also makes ceramics more brittle, as their bonds are less flexible and more prone to breaking under stress, limiting their ability to deform plastically before fracturing. In contrast, metals have non-directional and more flexible metallic bonds, allowing them to deform plastically, making them less brittle and more ductile compared to ceramic materials.

Step by step solution

01

Understand the properties of ceramic materials and metals

In general, ceramic materials are known for their hardness, wear resistance, and brittleness, while metals are known for their malleability, ductility, and toughness.
02

Explore the atomic structure and bonding in ceramic materials and metals

Ceramic materials are composed of ionic or covalent bonds, while metals primarily consist of metallic bonds. Ionic and covalent bonds are much stronger and more directional than metallic bonds, which leads to the differences in properties between ceramic materials and metals.
03

Explain one reason why ceramic materials are harder than metals

One reason why ceramic materials are generally harder than metals is their strong and directional bonding. The strong ionic or covalent bonds in ceramic materials result in a rigid and strongly bonded structure. This structure makes it more difficult for the individual atoms or ions to slide past each other, which contributes to a higher resistance to deformation and higher hardness compared to metals with non-directional metallic bonds.
04

Explain one reason why ceramic materials are more brittle than metals

The same strong and rigid bonding structure that gives ceramic materials their hardness also contributes to their brittleness. Since the ionic or covalent bonds are less flexible and more prone to breaking under stress, ceramic materials have limited ability to deform plastically before fracturing. On the other hand, the non-directional and more flexible metallic bonds allow metals to deform plastically, which makes them less brittle and more ductile compared to ceramic materials.

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Most popular questions from this chapter

In terms of bonding, explain why silicate materials have relatively low densities.

Using the Molecule Definition Utility found in both "Metallic Crystal Structures and Crystallography" and "Ceramic Crystal Structures" modules of \(V M S E\), located on the book's web site [www.wiley.com/ college/callister (Student Companion Site)], generate (and print out) a three-dimensional unit cell for titanium dioxide, \(\mathrm{TiO}_{2}\), given the following: (1) The unit cell is tetragonal with \(a=0.459 \mathrm{~nm}\) and \(c=0.296 \mathrm{~nm},(2)\) oxygen atoms are located at the following point coordinates: \(\begin{array}{llllll}0.356 & 0.356 & 0 & 0.856 & 0.144 & \frac{1}{2} \\\ 0.664 & 0.664 & 0 & 0.144 & 0.856 & \frac{1}{2}\end{array}\) and (3) Ti atoms are located at the following point coordinates: \(\begin{array}{llllll}0 & 0 & 0 & & 1 & 0 & 1 \\ 1 & 0 & 0 & & 0 & 1 & 1 \\\ 0 & 1 & 0 & & 1 & 1 & 1 \\ 0 & 0 & 1 & & \frac{1}{2} & \frac{1}{2} & \frac{1}{2} \\ 1 & 1 & 0 & & & & \end{array}\)

(a) Suppose that \(\mathrm{Li}_{2} \mathrm{O}\) is added as an impurity to \(\mathrm{CaO}\). If the \(\mathrm{Li}^{+}\)substitutes for \(\mathrm{Ca}^{2+}\), what kind of vacancies would you expect to form? How many of these vacancies are created for every \(\mathrm{Li}^{+}\)added? (b) Suppose that \(\mathrm{CaCl}_{2}\) is added as an impurity to \(\mathrm{CaO}\). If the \(\mathrm{Cl}^{-}\)substitutes for \(\mathrm{O}^{2-}\), what kind of vacancies would you expect to form? How many of the vacancies are created for every \(\mathrm{Cl}^{-}\)added?

Calculate the fraction of lattice sites that are Schottky defects for sodium chloride at its melting temperature \(\left(801^{\circ} \mathrm{C}\right)\). Assume an energy for defect formation of \(2.3 \mathrm{eV}\).

Compute the theoretical density of diamond given that the \(\mathrm{C}-\mathrm{C}\) distance and bond angle are \(0.154 \mathrm{~nm}\) and \(109.5^{\circ}\), respectively. How does this value compare with the measured density?
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