Crystalline solids represent structures with well-organized patterns and shapes.
Concept: Crystalline Solids13m
Unlike crystalline solids, amorphous solids represent structures that lack an organized patterns or shapes.
When examining the particles within a crystal you may observe them tightly packed in an organized pattern. The smallest portion of which is termed the unit cell.
There are 7 crystal systems and 14 types of unit cells that naturally occur. The simple cubic unit cell represents one of the simplest types.
Concept: Simple Cubic Unit Cell10m
The Simple Cubic Unit Cell is composed of a cube with atom at each corner. In the Lattice Diagram each of the unit cells are combined to form a crystal lattice. In the Space Filling Unit Cell Diagram we are shown that the unit cell uses only 1/8 of each of the 8 corner atoms.
The body-centered cubic unit cell is composed of a cube with one atom at each of its corners and one atom at the center of the cube.
Concept: Body Centered Cubic Unit Cell9m
The face-centered cubic unit cell is composed of a cube with one atom at each of its corners and one atom in the center of each cube face.
Concept: Face Centered Cubic Unit Cell8m
Concept: Unit Cell Calculations 1 Example 13m
Concept: Unit Cell Calculations 1 Example 22m
Concept: Unit Cell Calculations 1 Example 32m
Concept: Unit Cell Calculations 1 Example 43m
Concept: Unit Cell Calculations 2 Example 18m
Concept: Unit Cell Calculations 2 Example 23m
Concept: Unit Cell Calculations 2 Example 33m
Concept: Unit Cell Calculations 3 Example 12m
Concept: Unit Cell Calculations 3 Example 23m
Concept: Unit Cell Calculations 3 Example 39m
Consider a simple cubic (a.k.a, primitive cubic) unit cell as shown here.
(i) How many atoms are shown in this image?
(ii) What fraction of each atom is inside the boundaries of the cube?
(iii) If you sum all (the fractions of atoms, how many atoms are actually inside a simple cubic unit cell?
What is the number of nearest neighbors in a body-centered-cubic lattice?
The edge of a body-centered-cubic unit cell (which contains two atoms per unit cell) of an element Y was found to be 3.16 x 10 –8 cm. The density of the metal is 19.35 g•cm –3. What is the approximate molar mass of Y?
a) 65.4 g•mol –1
b) 92.0 g•mol –1
c) 184 g•mol –1
d) 238 g•mol –1
Sodium chloride, NaCl, crystallizes in a face-centered cubic lattice of chloride ions, with the smaller sodium ions occupying holes between the chloride ions. How many Cl – ions are in contact with any single Na+ ions?
How many atoms are in one body-centered cubic unit cell of a metal?
Which term describes the number of atoms surrounding an atom in a crystal lattice
a) Unit cell
b) Coordination number
c) Crystalline solid
d) Packing efficiency
Which of the following statements about crystalline and amorphous solids is TRUE?
A) A crystalline solid is composed of atoms or molecules arranged with long-range repeating order.
B) An example of a crystalline solid is glass.
C) An example of an amorphous solid is table salt (NaCl).
D) An amorphous solid is composed of atoms or molecules with a majority of its volume empty.
E) All of the above statements are TRUE.
Gold crystallizes in a face-centered cubic structure. What is the edge length of the unit cell if the atomic radius of gold is 144 pm?
a) 204 pm
b) 288 pm
c) 333 pm
d) 407 pm
Determine the radius of an Al atom (in pm) if the density of aluminum is 2.71 g/cm 3. Aluminum crystallizes in a face centered cubic structure with an edge length of 2√2 r.
a) 143 pm
b) 227 pm
c) 96 pm
d) 172 pm
e) 193 pm
Rank the three cubic crystalline structures in order of increasing space between the particles of the crystal.
Note: FCC = face-centered cubic, BCC = Body-centered cubic, and SC = simple cubic.
a) SC < BCC = FCC
b) FCC < BCC < SC
c) BCC < FCC < SC
d) FCC < SC < BCC
e) SC = BCC < FCC
Potassium metal crystallizes in a body-centered cubic structure with a unit cell edge length of 5.31 angstroms. The radius of a potassium atom is __________ angstroms.
Which one of the following cannot form a solid with a lattice based on the sodium chloride structure?
Which of the following statements a through d is incorrect?
a) Ionic solids are insulators
b) The binding forces in a molecular solid include London dispersion forces.
c) Ionic solids have high melting points.
d) Molecular solids have high melting points.
e) All of the statements a through d are correct.
Aluminum has a face-centered cubic unit structure and a density of 2.716 g/cm3. Calculate the edge length of the unit cell.
a) 4.041 x 10 -8 cm
b) 3.992 x 10 -8 cm
c) 3.615 x 10 -8 cm
d) 3.247 x 10 -8 cm
e) 2.836 x 10 -8 cm
Vanadium crystallizes in a body centered cubic structure and has an atomic radius of 131 pm. Determine the density of vanadium, if the edge length of a bcc structure is 4r/√3.
A) 3.06 g/cm3
B) 12.2 g/cm3
C) 6.11 g/cm3
D) 2.77 g/cm3
E) 8.46 g/cm3
What is the edge length of a face-centered cubic unit cell made up of atoms having a radius of 128 pm?
A) 181 pm
B) 362 pm
C) 512 pm
D) 1020 pm
E) 81 pm
Which one of the following elements is considered an insulator?