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The Solid State

The Solid State. Structures of Solids Section 11.7. Solid structures can be categorized into two broad categories Amorphous solids have no recognizable structure Crystalline solids have a definite pattern (order) to their structure. Unit Cells.

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The Solid State

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  1. The Solid State

  2. Structures of SolidsSection 11.7 • Solid structures can be categorized into two broad categories • Amorphous solids have no recognizable structure • Crystalline solids have a definite pattern (order) to their structure

  3. Unit Cells • Crystalline solids form a repeating structure made up of individual units that are referred to as unit cells • Amorphous solids do not possess unit cells • We will be discussing 4 different unit cells: • Primitive (simple) cubic • Body-centered cubic (BCC) • Face-centered cubic (FCC) • Hexagonal close packed (HCP)

  4. Primitive Cubic Unit Cell • Contains 8 atoms (all located on the corners of the unit cell) • Translates to 1 atom/unit cell

  5. Body-Centered Cubic Unit Cell • Contains 8 atoms located on the corners as well as one atom located at the very center • Translates to 2 atoms/unit cell

  6. Face-Centered Cubic Unit Cell • Contains 8 atoms located on the corners of the unit cell as well as 6 atoms (one on each face of the unit cell) • Translates to 4 atoms/unit cell

  7. Hexagonal Close Packed Unit Cell Contains 6 atoms/unit cell

  8. Determine the number of Na+ and Cl- ions present in the unit cell for NaCl. A representation of this unit cell is provided See Sample Exercise 11.7 (Pg. 462) Determining the Contents of a Unit Cell

  9. Edge Length in BCC

  10. LiF crystallizes in the exact manner as NaCl. The unit cell is 4.02 Å on an edge. Based on this and the data from the NaCl unit cell, calculate the density of LiF. See Sample Exercise 11.8 (Pg. 462) Calculating Density from Unit Cell Data

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