Chapter 3: Problem 51
Sketch the (1\overline{1101) and (1120) planes in a hexag- } onal unit cell.
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Chapter 3: Problem 51
Sketch the (1\overline{1101) and (1120) planes in a hexag- } onal unit cell.
These are the key concepts you need to understand to accurately answer the question.
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The unit cell for tin has tetragonal symmetry, with \(a\) and \(b\) lattice parameters of \(0.583\) and \(0.318 \mathrm{~nm}\), respectively. If its density, atomic weight, and atomic radius are \(7.27 \mathrm{~g} / \mathrm{cm}^{3}\), \(118.71 \mathrm{~g} / \mathrm{mol}\), and \(0.151 \mathrm{~nm}\), respectively, compute the atomic packing factor.
(a) Derive planar density expressions for BCC (100) and (110) planes in terms of the atomic radius \(R\). (b) Compute and compare planar density values for these same two planes for vanadium.
Would you expect a material in which the atomic bonding is predominantly ionic in nature to be more or less likely to form a noncrystalline solid upon solidification than a covalent material? Why? (See Section 2.6.)
Determine the expected diffraction angle for the first-order reflection from the (113) set of planes for FCC platinum when monochromatic radiation of wavelength \(0.1542 \mathrm{~nm}\) is used.
Using atomic weight, crystal structure, and atomic radius data tabulated inside the front cover, compute the theoretical densities of lead, chromium, copper, and cobalt, and then compare these values with the measured densities listed in this same table. The \(c / a\) ratio for cobalt is \(1.623\).
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