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Crystalline Solids

Crystalline Solids. BLB 11 th Chapter 11 Sections 7-8. p. 464. p. 459. Macroscopic structure depends upon microscopic structure. Pyrite (FeS 2 , fool’s gold). Fluorite (CaF 2 ). Amethyst (SiO 2 ) – quartz + Fe & Mn. Crystal terms. Crystal – Lattice – Unit cell –

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Crystalline Solids

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  1. Crystalline Solids BLB 11th Chapter 11 Sections 7-8

  2. p. 464

  3. p. 459

  4. Macroscopic structure depends upon microscopic structure.

  5. Pyrite (FeS2, fool’s gold) Fluorite (CaF2) Amethyst (SiO2) – quartz + Fe & Mn

  6. Crystal terms • Crystal – • Lattice – • Unit cell – • Edge length (do) – face edge corner

  7. Lattice – unit cell relationship

  8. Packing in Crystals • Atoms and ions are represented by spheres. • The spheres stack in different patterns. • The close packing of spheres maximizes intermolecular force. • The patterns of stacking result in different types of unit cells and lattices.

  9. p. 465

  10. Types of Unit Cells

  11. Types of cubic unit cells

  12. Types of cubic unit cells • 3 questions: • How many atoms are there per unit cell? • How many nearest neighbors are there for each atom? • What is the relationship between atomic radius and the edge length?

  13. Primitive (simple) Cubic _______ atoms per unit cell _______ nearest neighbors

  14. Body-centered Cubic _______ atoms per unit cell _______ nearest neighbors

  15. Face-centered Cubic(result of close packing) _______ atoms per unit cell _______ nearest neighbors

  16. Close Packing Cubic close-packed (ccp) ABCABC layers Hexagonal close-packed (hcp) ABAB layers

  17. What about the space left over?

  18. NaCl

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