The Solid State.

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Presentation transcript:

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 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)

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

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

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

Hexagonal Close Packed Unit Cell Contains 6 atoms/unit cell

Determining the Contents of a Unit Cell 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)

Edge Length in BCC

Calculating Density from Unit Cell Data 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)