GTBL042-03 GTBL042-Callister-v2 September 6, 2007 15:33
92 • Chapter 3 / Structures of Metals and CeramicsREFERENCES
Azaroff, L. F.,Elements of X-Ray Crystallography,
McGraw-Hill, New York, 1968. Reprinted by
TechBooks, Marietta, OH, 1990.
Buerger, M. J.,Elementary Crystallography, Wiley,
New York, 1956.
Chiang, Y. M., D. P. Birnie, III, and W. D. Kingery,
Physical Ceramics: Principles for Ceramic Sci-
ence and Engineering,Wiley, New York, 1997.
Cullity, B. D., and S. R. Stock,Elements of X-Ray
Diffraction, 3rd edition, Prentice Hall, Upper
Saddle River, NJ, 2001.
Curl, R. F. and R. E. Smalley, “Fullerenes,”Scien-
tific American, Vol. 265, No. 4, October 1991,
pp. 54–63.Hauth, W. E., “Crystal Chemistry in Ceramics,”
American Ceramic Society Bulletin,Vol. 30,
1951: No. 1, pp. 5–7; No. 2, pp. 47–49; No. 3, pp.
76–77; No. 4, pp. 137–142; No. 5, pp. 165–167;
No. 6, pp. 203–205. A good overview of silicate
structures.
Kingery, W. D., H. K. Bowen, and D. R. Uhlmann,
Introduction to Ceramics,2nd edition, Wiley,
New York, 1976. Chapters 1–4.
Richerson, D. W.,The Magic of Ceramics,American
Ceramic Society, Westerville, OH, 2000.
Richerson, D. W.,Modern Ceramic Engineering,3rd
edition, CRC Press, Boca Raton, FL, 2006.QUESTIONS AND PROBLEMS
Additional problems and questions for this chapter may be found on both Student and
Instructor Companion Sites atwww.wiley.com/college/callister.Unit Cells
Metallic Crystal Structures
3.1If the atomic radius of lead is 0.175 nm, calcu-
late the volume of its unit cell in cubic meters.
3.2Show that the atomic packing factor for BCC
is 0.68.
Density Computations—Metals
3.3Molybdenum has a BCC crystal structure, an
atomic radius of 0.1363 nm, and an atomic
weight of 95.94 g/mol. Compute its theoretical
density and compare it with the experimental
value found inside the front cover.
3.4Calculate the radius of a palladium atom,
given that Pd has an FCC crystal structure, a
density of 12.0 g/cm^3 , and an atomic weight of
106.4 g/mol.
3.5Some hypothetical metal has the simple cu-
bic crystal structure shown in Figure 3.42. If
its atomic weight is 74.5 g/mol and the atomic
radius is 0.145 nm, compute its density.
Figure 3.42 Hard-sphere unit cell
representation of the simple cubic
crystal structure.3.6Using atomic weight, crystal structure, and
atomic radius data tabulated inside the front
cover, compute the theoretical densities of alu-
minum, nickel, magnesium, and tungsten, and
then compare these values with the measured
densities listed in this same table. Thec/aratio
for magnesium is 1.624.
3.7Below are listed the atomic weight, density,
and atomic radius for three hypothetical al-
loys. For each determine whether its crystal
structure is FCC, BCC, or simple cubic and
then justify your determination. A simple cu-
bic unit cell is shown in Figure 3.42.Atomic Atomic
Weight Density Radius
Alloy (g/mol) (g/cm^3 ) (nm)
A 43.1 6.40 0.122
B 184.4 12.30 0.146
C 91.6 9.60 0.137