prentice hall 2003chapter 11 types of solids molecular solidsex. co 2, h 2 o, ar covalent-network...
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Prentice Hall © 2003Chapter 11 Close Packing of Spheres Describes many of the types of solids Assumes molecules/atoms/ions are spheres Characterized by – lattice – unit cell – lattice pointsTRANSCRIPT
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Prentice Hall © 2003 Chapter 11
Types of Solids
• Molecular Solids ex. CO2, H2O, Ar• Covalent-Network Solids ex. Diamond,
quartz, SiO2
• Metallic Solids ex. Au, Ag• Ionic Solids ex. LiF, KCl, AgCl,
CaO
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Prentice Hall © 2003 Chapter 11
MODEL
• Close Packing of Spheres
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Prentice Hall © 2003 Chapter 11
Close Packing of Spheres
• Describes many of the types of solids
• Assumes molecules/atoms/ions are spheres
• Characterized by– lattice– unit cell– lattice points
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Prentice Hall © 2003 Chapter 11
Unit Cells
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Prentice Hall © 2003 Chapter 11
Types of Units Cells• Simple Cubic = 8 corners occupied by 1/8 of an atom Total #
atoms in simple cubic = 1 atom
• Body-Centered = 8 corners occupied by 1/8 of an atom + 1 whole atom in center Total # atoms in simple cubic = 2 atoms
• Face-Centered = 8 corners occupied by 1/8 of an atom + 6 half- atoms on the 6 faces of the cube Total # atoms in simple cubic = 4 atoms
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Prentice Hall © 2003 Chapter 11
The Crystal Structure of Sodium Chloride
Structures of Solids
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Prentice Hall © 2003 Chapter 11
Unit Cells
Structures of Solids
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Prentice Hall © 2003 Chapter 11
Most Common Types of Unit Cells based on Close Packing
of Spheres Model • Simple Cubic– 1 atom
• Body Centered Cubic (BCC)– 2 atoms
• Face Centered Cubic (FCC)– 4 atoms
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1 2 4
Number of Atoms in a Cubic Unit Cell
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Prentice Hall © 2003 Chapter 11
• Unit Cells can be used to determine the DENSITY and the SIZE of atoms
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Prentice Hall © 2003 Chapter 11
Sample Problem
• The simple cubic unit cell of a particular crystalline form of barium is 2.8664 oA on each side. Calculate the density of this form of barium in gm/cm3.
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Prentice Hall © 2003 Chapter 11
Steps to Solving the Problem
• (1.) Determine the # of atoms in the unit cell.• (2.) Convert oA (if given) to cm. (3.) Find volume
of cube using Vcube = s3 = cm3
• (4.) Convert a.m.u. to grams. [Note: 1 gm= 6.02 x 1023 a.m.u.]
• (5.) Plug in values to the formula: D = mass/volume
•
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Prentice Hall © 2003 Chapter 11
Conversions
• Useful Conversions:
• 1 nm(nanometer) = 1 x 10-7 cm• 1 oA (angstrom)= 1 x 10-8 cm• 1 pm (picometer) = 1 x 10-10 cm
• 1 gram = 6.022 x 10 23 a. m. u. (atomic mass unit)
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Prentice Hall © 2003 Chapter 11
Sample Problem• LiF has a face-centered cubic unit cell (same as NaCl). [F- ion
is on the face and corners. Li+ in between.]
• Determine:• 1. The net number of F- ions in the unit cell.• 2. The number of Li+ ions in the unit cell.• 3. The density of LiF given that the unit cell is 4.02 oA on an
edge. (oA = 1 x 10-8 cm)
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Prentice Hall © 2003 Chapter 11
Sample Problem
• The body-centered unit cell of a particular crystalline form of iron is 2.8664 oA on each side. (a.) Calculate the density of this form of iron in gm/cm3. (b.)Calculate the radius of Fe.
• Note: First determine:• A. The net number of iron in the unit cell.• B. 1 oA = 1 x 10-8 cm
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The body-centered cubic unit cell of a particular crystalline
form of an element is 0.28664 nm on each side. The density
of this element is 7.8753 g/cm3. Identify the element.