Chapter 3: Problem 25
Sketch a tetragonal unit cell, and within that cell indicate locations of the \(\frac{1}{2} 1 \frac{1}{2}\) and \(\frac{1}{4} \frac{1}{2} \frac{3}{4}\) point coordinates.
Chapter 3: Problem 25
Sketch a tetragonal unit cell, and within that cell indicate locations of the \(\frac{1}{2} 1 \frac{1}{2}\) and \(\frac{1}{4} \frac{1}{2} \frac{3}{4}\) point coordinates.
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Get started for freeThe 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.
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.)
Rhenium has an HCP crystal structure, an atomic radius of \(0.137 \mathrm{~nm}\), and a \(c / a\) ratio of 1.615. Compute the volume of the unit cell for Re.
Convert the \((010)\) and (101) planes into the four-index Miller-Bravais scheme for hexagonal unit cells.
Calculate the radius of a vanadium atom, given that \(\mathrm{V}\) has a BCC crystal structure, a density of \(5.96 \mathrm{~g} / \mathrm{cm}^{3}\), and an atomic weight of \(50.9 \mathrm{~g} / \mathrm{mol}\).
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