Comparing two FCC metals, one with melting temperature of 857 ºC and one with melting temperature = 1284 ºC, which would you expect to have a larger fraction of vacant sites (Nv/N) at a temperature one degree below their respective melting points? Write down answer in about 4 sentences, and include all relevant quantities to make your point.

Comparing two FCC metals, one with melting temperature of 857 ºC and one with melting temperature = 1284 ºC, which would you expect to have a larger fraction of vacant sites (Nv/N) at a temperature one degree below their respective melting points? Write down answer in about 4 sentences, and include all relevant quantities to make your point.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter22: Inorganic Materials

Section: Chapter Questions

Problem 7P

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1. Show that the atomic packing factor for FCC is 0.74.2. Show that the atomic packing factor for BCC is 0.68.3. Iron has a BCC crystal structure, an atomic radius of 0.124 nm, and an atomic weight of 55.85 g/mol. Compute and compare its theoretical density with the experimental value, 7.87 g/cm3.4. Rhodium has an atomic radius of 0.1345 nm and density of 12.41 g/cm3. Determine whether it has an FCC or BCC crystal structure.5. The unit cell for tin has tetragonal symmetry, with a and b lattice parameters of 0.583 and 0.318 nm, respectively. If the density, atomic weight, and atomic radius are 7.30 g/cm3, 118.69 g/mol, and 0.151 nm, respectively, compute the atomic packing factor.
1. Show that the atomic packing factor for FCC is 0.74. 2. Show that the atomic packing factor for BCC is 0.68. 3. Iron has a BCC crystal structure, an atomic radius of 0.124 nm, and an atomic weight of 55.85 g/mol. Compute and compare its theoretical density with the experimental value, 7.87 g/cm. 4. Rhodium has an atomic radius of 0.1345 nm and density of 12.41 g/cm. Determine whether it has an FCC or BCC crystal structure. 5. The unit cell for tin has tetragonal symmetry, with a and b lattice parameters of 0.583 and 0.318 nm, respectively. If the density, atomic weight, and atomic radius are 7.30 g/cm3, 118.69 g/mol, and 0.151 nm, respectively, compute the atomic packing factor. To be submitted in Google classroom on:
3. a) Calculate the atomic packing factor for the face-centered cubic (FCC) crystal structure.
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value, 7.87 g/cm'. 4. Rhodium has an atomic radius of 0.1345 nm and density of 12.41 g/cm'. Determine whether it has an FCC or BCC crystal structure. The unit cell for tin has tetragonal symmetry, with a and b lattice parameters of 0.583 and 0.318 nm, respectively. If the density, atomic weight, and atomic radius are 7.30 g/cm3, 118.69 g/mol, and 0.151 nm, respectively, compute the atomic packing factor. 5.
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