12-05-08%20-%20Lecture%2026%20-%20Chapter%205%2c%20Final%20Review

12-05-08%20-%20Lecture%2026%20-%20Chapter%205%2c%20Final%20Review

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Packing in Metallic Solids Assume atoms are hard spheres and that crystals are built by PACKING of these spheres as efficiently as possible. Closed-packed structure has the least amount of wasted space.
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Layer B doesn’t lay directly on top of Layer A because there would be wasted space
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The third layer can lay directly above the first layer = hexagonal close-packed (hcp) structure Hexagonal Close-Packed
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Cubic Close-Packed The third layer can lay in the dips above the dips in the first layer = cubic close-packed (ccp) or face- centered cubic (fcc)
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Body-centered cubic One atom surrounded by 8 other atoms
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Simple Cubic Not very many examples of this type
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Units Cells for Metals
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Cubic Unit Cells of Metals Simple Simple cubic (SC) cubic (SC) Body- centered cubic (BCC) Face- centered cubic (FCC)
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Atom Sharing at Cube Faces and Corners Atom shared in corner a 1/8 inside each unit cell Atom shared in face a 1/2 inside each unit cell
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Atom Sharing in FCC
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Number of Atoms per Unit Cell Unit Cell Type Net Number Atoms SC SC BCC BCC FCC FCC 1 1 2 2 4 4
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Simple Cubic
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Body-Centered Cubic (BCC)
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Face-Centered Cubic (fcc)
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Metallic Solids Cations surrounded by a sea of valence electrons Luster (reflects light) mirror Malleability and ductility Electrons move with cation Conduct electricity Charge carried by electrons
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Alloys Substitutional Alloy Interstitial Alloy
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12-05-08%20-%20Lecture%2026%20-%20Chapter%205%2c%20Final%20Review

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