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**INDUSTRIAL MATERIALS Instructed by: Dr. Sajid Zaidi**

PhD in Advanced Mechanics, UTC, France MS in Advanced Mechanics, UTC, France B.Sc. in Mechanical Engineering, UET, Lahore B.TECH Mechanical Technology IQRA COLLEGE OF TECHNOLOGY (ICT) INTERNATIONAL ISLAMIC UNIVERSITY, ISLAMABAD

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Crystal Geometry (a) Inert monoatomic gases have no regular ordering of atoms (b,c) Some materials, including water vapor, nitrogen gas, amorphous silicon and silicate glass have short-range order (d) Metals, alloys, many ceramics and some polymers have regular ordering of atoms/ions that extends through the material INDUSTRIAL MATERIALS (a,b,c) non-dense, random packing, (d) dense, regular packing

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**Concept of Crystal Geometry**

Space Lattice Atomic arrangements in crystalline solids can be described by referring the atoms to the points of intersection of a network of lines in three dimensions. Such a network is called a space lattice. It can be described as an infinite three-dimensional array of points. Each space lattice can be described by specifying the atom positions in a repeating unit cell. The unit cell is the subdivision of a lattice that still retains the overall characteristics of the entire lattice. INDUSTRIAL MATERIALS Crystal Geometry

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**Concept of Crystal Geometry**

Unit Cell The basic structural unit of a crystal structure. Its geometry and atomic positions define the crystal structure. A unit cell is the smallest component of the crystal that reproduces the whole crystal when stacked together with purely translational repetition. INDUSTRIAL MATERIALS Crystal Geometry By stacking identical unit cells, the entire lattice can be constructed.

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**Concept of Crystal Geometry**

Lattice Parameters The lattice parameters include Dimensions of the sides of the unit cell Angles between the sides The length is often given in nanometers (nm) or Angstrom (Å) units, where: 1 angstrom (Å) = 0.1 nm = m = 10-8 cm INDUSTRIAL MATERIALS Crystal Geometry

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**Concept of Crystal Geometry**

Crystal System There are 7 unique arrangements of the unit cell that define the crystal system INDUSTRIAL MATERIALS Crystal Geometry Axes Angle b/w axes Volume of unit cell a = b = c α = β = γ = 90º a3 Cubic Tetragonal a = b ≠ c α = β = γ = 90º a2c Orthorhombic a ≠ b ≠ c α = β = γ = 90º abc

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**Concept of Crystal Geometry**

Crystal System Axes Angle b/w axes Volume of unit cell INDUSTRIAL MATERIALS Crystal Geometry Rhombohedral a = b = c α = β = γ ≠ 90º a3(1-3cos2α+2cos3α)1/2 Monoclinic a ≠ b ≠ c α = β = 90º, γ ≠ 90º abc sinγ Triclinic a ≠ b ≠ c α ≠ β ≠ γ ≠ 90º abc (1-cos2α-cos2β-cos2γ+2cosαcosβcosγ)1/2 Hexagonal a = b ≠ c α = β = 90º, γ = 120º 3*0.866a2c

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**Concept of Crystal Geometry**

Bravais Lattices Lattice points are located at the corners of the unit cells and, in some cases, at either faces or the center of the unit cell. 14 distinct arrangements of lattice points are possible. These unique arrangements of lattice points are known as the Bravais lattices. Concept of a lattice is mathematical and does not mention atoms, ions or molecules. One or more atoms can be associated with each lattice point INDUSTRIAL MATERIALS Crystal Geometry

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**Concept of Crystal Geometry**

Bravais Lattices INDUSTRIAL MATERIALS Crystal Geometry

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**Concept of Crystal Geometry**

Atomic Radius vs Lattice Parameters INDUSTRIAL MATERIALS Crystal Geometry a0 = 2r a0√3 = 4r a0√2 = 4r

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**Concept of Crystal Geometry**

No. of Atoms per Unit Cell The number of atoms per unit cell is the product of the number of atoms per lattice point and the number of lattice points per unit cell. In most metals, one atom is located at each lattice point. A unit cell has specific number of lattice points: at each corner of the cell at center of the cell (in case of body-centered) at each face of the cell (in case of face-centered) It must be noticed that one lattice point may be shared by more than one unit cell. INDUSTRIAL MATERIALS Crystal Geometry

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**Concept of Crystal Geometry**

No. of Atoms per Unit Cell A lattice point at a corner of one unit cell is shared by seven adjacent unit cells (thus a total of eight cells); only one-eighth of each corner lattice point belongs to one particular cell. INDUSTRIAL MATERIALS Crystal Geometry Similarly, a lattice point at the face of one unit cell is shared by one adjacent unit cells (thus a total of two cells); only one-half of each face lattice point belongs to one particular cell.

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**Concept of Crystal Geometry**

No. of Atoms per Unit Cell Number of total corner lattice points in a unit cell is (Total number of corners) x (lattice point per corner) = 8 x 1/8 = 1 Number of total body-centered lattice points in a unit cell is (Total number of centers) x (lattice point per center) = 1 x 1 = 1 Number of total face-centered lattice points in a unit cell is (Total number of faces) x (lattice point per face) = 6 x 1/2 = 3 INDUSTRIAL MATERIALS Crystal Geometry

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**Concept of Crystal Geometry**

Coordination Number The coordination number is the number of atoms touching a particular atom, or the number of nearest neighbors for that particular atom. INDUSTRIAL MATERIALS Crystal Geometry Simple Cubic

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**Concept of Crystal Geometry**

Packing Factor The packing factor is the fraction of space occupied by atoms, assuming that atoms are hard spheres sized so that they touch their closest neighbor. The general expression for the packing factor is: Packing factor = (number of atoms/cell) x (volume of each atom) / (volume of unit cell) No commonly encountered engineering metals or alloys have the SC structure, although this structure is found in ceramic materials. INDUSTRIAL MATERIALS Crystal Geometry Packing Factor of SC = 0.52

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**Principle Metallic Crystal Structures**

Most elemental metals (about 90 percent) crystallize upon solidification into three densely packed crystal structures: Body-Centered Cubic (BCC) Face-Centered Cubic (FCC) Hexagonal Close-Packed (HCP) INDUSTRIAL MATERIALS Crystal Geometry

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**Principle Metallic Crystal Structures**

Most metals crystallize in these dense-packed structures because energy is released as the atoms come closer together and bond more tightly with each other. Thus, the densely packed structures are in lower and more stable energy arrangements. INDUSTRIAL MATERIALS Crystal Geometry Simple Cubic Face-Centered Cubic Body-Centered Cubic Hexagonal Close-Packed

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**Body-Centered Cubic (BCC)**

Number of atoms in a unit cell of BCC = 2 Coordination number = 8 Packing Factor = 0.68 That is, 68 percent of the volume of the BCC unit cell is occupied by atoms and the remaining 32 percent is empty space. The BCC crystal structure is not 100% close-packed structure since the atoms could be packed closer together. a0√3 = 4r INDUSTRIAL MATERIALS Crystal Geometry Hard Sphere Unit Cell Isolated Unit Cell

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**Body-Centered Cubic (BCC)**

Many metals such as iron, chromium, tungsten, molybdenum, and vanadium have the BCC crystal structure at room temperature. Metals with mixed bonding, such as iron, may have unit cells with less than the maximum packing factor. INDUSTRIAL MATERIALS Crystal Geometry Selected metals that have the BCC Crystal Structure at room temperature (20◦C) and their Lattice Constants and Atomic Radii

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**Face-Centered Cubic (FCC)**

Number of atoms in a unit cell of FCC = 4 Coordination number = 12 Packing Factor = 0.74 That is, 74 percent of the volume of the BCC unit cell is occupied by atoms and the remaining 26 percent is empty space. INDUSTRIAL MATERIALS Crystal Geometry Hard Sphere Unit Cell Isolated Unit Cell a0√2 = 4r

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**Face-Centered Cubic (FCC)**

The PF of 0.74 is for the closest packing possible of “spherical atoms.” Many metals such as aluminum, copper, lead, nickel, and iron at elevated temperatures (912 to 1394◦C) crystallize with the FCC crystal structure. Metals with only metallic bonding are packed as efficiently as possible. INDUSTRIAL MATERIALS Crystal Geometry Selected metals that have the FCC Crystal Structure at room temperature (20◦C) and their Lattice Constants and Atomic Radii

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**Hexagonal Close-Packed (HCP)**

Metals do not crystallize into the simple hexagonal crystal structure because the PF is too low. The atoms can attain a lower energy and a more stable condition by forming the HCP structure. The PF of the HCP crystal structure is 0.74, the same as that for the FCC crystal structure since in both structures the atoms are packed as tightly as possible. INDUSTRIAL MATERIALS Crystal Geometry Hard Sphere Unit Cell Isolated Unit Cell

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**Hexagonal Close-Packed (HCP)**

The HCP has six atoms per unit cell. Three atoms form a triangle in the middle layer. There are six 1/6 atom sections on both the top and bottom layers, making an equivalent of two more atoms (2 × 6 × 1/6 = 2). Finally, there is one-half of an atom in the center of both the top and bottom layers making the equivalent of one more atom. The total number of atoms in the HCP crystal structure unit cell is thus = 6. INDUSTRIAL MATERIALS Crystal Geometry

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**Hexagonal Close-Packed (HCP)**

Coordination number is 12. The ratio of the height c of the hexagonal prism of the HCP crystal structure to its basal side a is called the c/a ratio. The c/a ratio for an ideal HCP crystal structure consisting of uniform spheres packed as tightly together as possible is INDUSTRIAL MATERIALS Crystal Geometry Selected metals that have the HCP Crystal Structure at room temperature (20◦C) and their Lattice Constants, Atomic Radii and c/a ratios

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**Hexagonal Close-Packed (HCP)**

Cadmium and zinc have c/a ratios higher than ideality, which indicates that the atoms in these structures are slightly elongated along the c axis of the HCP unit cell. The metals magnesium, cobalt, zirconium, titanium, and beryllium have c/a ratios less than the ideal ratio. Therefore, in these metals the atoms are slightly compressed in the direction along the c axis. Thus, for the HCP metals listed in the table, there is a certain amount of deviation from the ideal hard-sphere model. INDUSTRIAL MATERIALS Crystal Geometry

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**Atom Positions in Cubic Unit Cells**

To locate atom positions in cubic unit cells, rectangular x, y, and z axes are used. In crystallography the positive x axis is usually the direction coming out of the paper, the positive y axis is the direction to the right of the paper, and the positive z axis is the direction to the top. Negative directions are opposite to those just described. z (0,1,1) INDUSTRIAL MATERIALS Crystal Geometry (0,0,1) (1,0,1) (1,1,1) (0,1,0) (0,0,0) y (1,0,0) (1,1,0) x (1/2,1/2,1/2) Body – Centered Cubic (BCC)

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**Atom Positions in Cubic Unit Cells**

z INDUSTRIAL MATERIALS Crystal Geometry (0,0,0) y x Face – Centered Cubic (FCC)

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**Directions in Cubic Unit Cells**

Directions in crystal lattices are especially important for metals and alloys with properties that vary with crystallographic orientation. INDUSTRIAL MATERIALS Crystal Geometry z Direction of OS Coordinates of S - Coordinates of O (1,1,0) – (0,0,0) = (1,1,0) = [110] Position coordinates of direction vector OS O Direction indices of direction vector OS y S x

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**Directions in Cubic Unit Cells**

Some directions in cubic unit cell INDUSTRIAL MATERIALS Crystal Geometry

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**Significance of Crystallographic Directions**

Metals deform more easily, for example, in directions along which atoms are in closest contact. Another real-world example is the dependence of the magnetic properties of iron and other magnetic materials on the crystallographic directions. It is much easier to magnetize iron in the [100] direction compared to [111] or [110] directions. This is why the grains in Fe-Si steels used in magnetic applications are oriented in the [100] or equivalent directions. In the case of magnetic materials used for recording media, we have to make sure the grains are aligned in a particular crystallographic direction such that the stored information is not erased easily. Similarly, crystals used for making turbine blades are aligned along certain directions for better mechanical properties. INDUSTRIAL MATERIALS Crystal Geometry

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**Planes in Cubic Unit Cells**

Sometimes it is necessary to refer to specific lattice planes of atoms within a crystal structure, or it may be of interest to know the crystallographic orientation of a plane or group of planes in a crystal lattice. Metals deform easily along planes of atoms that are most tightly packed together. The surface energy of different faces of a crystal depends upon the particular crystallographic planes. This becomes important in crystal growth. In thin film growth of certain electronic materials (e.g., Si or GaAs), we need to be sure the substrate is oriented in such a way that the thin film can grow on a particular crystallographic plane. To identify crystal planes in cubic crystal structures, the Miller notation system is used. INDUSTRIAL MATERIALS Crystal Geometry

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Miller Indices The Miller indices of a crystal plane are defined as the reciprocals of the fractional intercepts (with fractions cleared) that the plane makes with the crystallographic x, y, and z axes of the three nonparallel edges of the cubic unit cell. The procedure for determining the Miller indices for a cubic crystal plane is as follows: Choose a plane that does not pass through the origin at (0, 0, 0). Determine the intercepts of the plane in terms of the crystallographic x, y, and z axes for a unit cube. These intercepts may be fractions. Form the reciprocals of these intercepts. Clear fractions and determine the smallest set of whole numbers that are in the same ratio as the intercepts. These whole numbers are the Miller indices of the crystallographic plane and are enclosed in parentheses INDUSTRIAL MATERIALS Crystal Geometry

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Miller Indices Some examples INDUSTRIAL MATERIALS Crystal Geometry

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Miller Indices In cubic crystal structures the interplanar spacing between two closest parallel planes with the same Miller indices is designated dhkl , where h, k, and l are the Miller indices of the planes. This spacing represents the distance from a selected origin containing one plane and another parallel plane with the same indices that is closest to it. From simple geometry, it can be shown that for cubic crystal structures dhkl = a S √h2 + k2 + l2 INDUSTRIAL MATERIALS Crystal Geometry

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**Crystallographic Planes in Hexagonal Unit Cells**

Crystal planes in HCP unit cells are commonly identified by using four indices, Miller-Bravais indices, instead of three. These are denoted by the letters h, k, i, and l and are enclosed in parentheses as (hkil). These four-digit hexagonal indices are based on a coordinate system with four axes There are three basal axes, a1, a2, and a3, which make 120◦ with each other. The fourth axis or c axis is the vertical axis located at the center of the unit cell. INDUSTRIAL MATERIALS Crystal Geometry

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**Crystallographic Planes in Hexagonal Unit Cells**

The a unit of measurement along the a1, a2, and a3 axes is the distance between the atoms along these axes. The unit of measurement along the c axis is the height of the unit cell. The reciprocals of the intercepts that a crystal plane makes with the a1, a2, and a3 axes give the h, k, and i indices, while the reciprocal of the intercept with the c axis gives the l index. INDUSTRIAL MATERIALS Crystal Geometry

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**Crystallographic Planes in Hexagonal Unit Cells**

Basal Planes As the basal plane on the top of the HCP unit cell is parallel to a1, a2, and a3, the intercepts of this plane with these axes will all be infinite. Thus, a1 = ∞, a2 = ∞, and a3 = ∞. The c axis is unity since the top basal plane intersects the c axis at unit distance. Taking the reciprocals of these intercepts gives the Miller-Bravais indices for the HCP basal plane. Thus h = 0, k = 0, = 0, and l = 1. The HCP basal plane is, therefore, a zero-zero-zero-one or (0001) plane. INDUSTRIAL MATERIALS Crystal Geometry

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**Crystallographic Planes in Hexagonal Unit Cells**

Prism Planes The intercepts of the front prism Plane (ABCD) are a1 = +1, a2 = ∞, a3 = −1, and c = ∞. Taking the reciprocals of these intercepts gives h = 1, k = 0, i = −1, and l = 0, or the (1010) plane. The ABEF prism plane has the indices (1100) and the DCGH plane the indices (0110). All HCP prism planes can be identified collectively as the {1010} family of planes. INDUSTRIAL MATERIALS Crystal Geometry

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Expected Questions Calculate the packing factor for the SC, BCC and FCC. Calculate the percent volume change as zirconia (ZrO2) transforms from a tetragonal to a monoclinic structure. The lattice constants for the monoclinic unit cells are: a =5.156Å, b=5.191Å, c=5.304Å , and the angle β is 98.9º. The lattice constants for the tetragonal unit cell are a=5.094Å and c=5.304Å. Does the zirconia expand or contract during this transformation? Draw [121] direction and (210) plane in a cubic unit cell. Iron at 20ºC is BCC with atoms of atomic radius nm. Calculate the lattice constant a for the cube edge of the iron unit cell. INDUSTRIAL MATERIALS Crystal Geometry

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Expected Questions Calculate the volume of the zinc crystal structure unit cell by using the following data: pure zinc has the HCP crystal structure with lattice constants a = nm and c = nm. Draw the following direction vectors in cubic unit cells: [100], [110], [112], [110], [321] Draw the following crystallographic planes in cubic unit cells: (101), (110), (221) Draw a (110) plane in a BCC atomic-site unit cell, and list the position coordinates of the atoms whose centers are intersected by this plane. INDUSTRIAL MATERIALS Crystal Geometry

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