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8/11/2019 MSE 101 - Lecture 4 - Crystal Structure
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Crystal structure of SolidsCrystal structure of Solids
Crystalline Solid
– a solid that contains a re ular and
repeating atomic or molecular arrangementover lar e atomic distances lon -ran e
order)
–
Non-crystalline Solid
– a so w ou ong-range or er ng a omsor molecules
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– also termed “amorphous”
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DefinitionsDefinitions
n t ce r m t ve e
– the smallest group of atoms possessing thesymme ry o e crys a w c , w en repea ein all directions, will develop the crystal lattice
• lattice constants/parameter : edge lengths, ,
•interaxial angles : angles between axesα
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Types of unit cells:Types of unit cells:
mp e – a oms are on y pos one a e
corners
2) Body-centered – an additional atom ispositioned at the center of the unit cell
3) Face-centered – atoms are positioned at
the corners, as well at the faces of the unitcell
- –
the corners, as well at two opposite faces of
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faces)
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Crystal systemsCrystal systems
→ a sc eme y w c crys a s ruc ures are
classified according to unit cell geometry;
.e., c ass e accor ng o re a ons ps
between edge lengths and interaxial angles
→ there is a total of seven crystal systems:
cubic, hexagonal, tetragonal, rhombohedral,orthorhombic, monoclinic, triclinic
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1) Cubic1) Cubic
Axial relationships: a = b = c
Interaxial an les: α = = = 90°
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2) Hexagonal2) Hexagonal
x a re a ons ps: a = ≠ c
Interaxial angles: α = β = 90° ; γ = 120°
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3) Tetragonal3) Tetragonal
x a re a ons ps: a = ≠ c
Interaxial angles: α = β = γ = 90°
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4) Rhombohedral/Trigonal4) Rhombohedral/Trigonal
x a re a ons ps: a = = c
Interaxial angles: α = β = γ ≠ 90°
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5) Orthorhombic5) Orthorhombic
x a re a ons ps: a ≠ ≠ c
Interaxial angles: α = β = γ = 90°
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6) Monoclinic6) Monoclinic
x a re a ons ps: a ≠ ≠ c
Interaxial angles: α = γ = 90° ≠ β
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7) Triclinic7) Triclinic
x a re a ons ps: a ≠ ≠ c
Interaxial angles: α ≠ β ≠ γ ≠ 90°
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Bravais latticeBravais lattice
→ ma ema ca er va on o e poss enumber of ways of arranging atoms in
space
→ arrived at by combining one of the seven
crystal systems with the basic types of unit
cells
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Bravais latticesBravais lattices
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Bravais latticesBravais lattices
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Principal Metallic StructuresPrincipal Metallic Structures
1. Face-centered cubic (FCC)
– atoms are situated at the corners of the unit cell,
as well as at the centers of each face; each
face atom touches its nearest corner atoms
16(Hard sphere model) (Point model)
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FCC structureFCC structure
x. u, ,
Ag, Au
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Principal Metallic StructuresPrincipal Metallic Structures
2. Body-centered cubic (BCC)
– atoms are situated at the corners, as well as at
the (body) center of the cube
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(Hard sphere model) (Point model)
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Principal Metallic StructuresPrincipal Metallic Structures
3.Hexagonal close-packed (HCP) – has two basal planes in the form of regular hexagons with
center. In addition, there are three atoms in the form of atriangle midway between the two basal planes
20(Hard sphere model) (Point model)
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HCP structureHCP structure
Ex. Cd, Co, Ti, Zn
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Characteristics of a crystal structureCharacteristics of a crystal structure
1. Coordination number
2. Number of atoms per unit cell
→ equivalent number of atoms enclosed
by the unit cell3. Relationship of the cube side, ao and
the atomic radius, r
→ expression relating the lattice constant,
a with the atomic radius r
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Characteristics of a crystal structureCharacteristics of a crystal structure
4. Atomic Packing Factor (APF)
→ ratio of the volume occupied by atoms to the
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Summary of crystal structure characteristicsSummary of crystal structure characteristics
Structure CN Atoms/ Equivalent APF
o
BCC 8 2 0.684 R
2
4 RFCC 12 4 0.74
HCP 12 6 2R 0.74
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Polymorphism and allotropyPolymorphism and allotropy
Polymorphism
→ henomenon wherein solids can ossess
more than one crystal structure
→ polymorphism in elemental solids
x. ure e
- BCC at room temperature
- FCC at 912°C
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Density computationsDensity computations
→ knowledge of the crystal structure permits
computation of theoretical density, ρ :
where,
n = number of atoms er unit cell A = atomic weight
VC = volume of unit cell
N A = Avogadro’s number (6.023x10 atoms/mol)
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Sample problemSample problem
Copper has an atomic radius of 0.128 nm, an
FCC crystal structure, and an atomic weight
of 63.5 g/mol. Compute its theoretical densityand compare the answer with its measured
density.
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