1 / 39

CHAPTER 3: STRUCTURE OF CRYSTALLINE SOLIDS

CHAPTER 3: STRUCTURE OF CRYSTALLINE SOLIDS. • Crystalline – repetitive 3-D structure - all metals, many ceramics and some polymers. • Atomic Hard Sphere Model represent atoms as solid spheres touching each other. • Lattice 3-D array of points coinciding with atom

patrickbrown
Download Presentation

CHAPTER 3: STRUCTURE OF CRYSTALLINE SOLIDS

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. CHAPTER 3: STRUCTURE OF CRYSTALLINE SOLIDS • Crystalline – repetitive 3-D structure - all metals, many ceramics and some polymers • Atomic Hard Sphere Model represent atoms as solid spheres touching each other. • Lattice 3-D array of points coinciding with atom positions

  2. METALLIC CRYSTAL STRUCTURE • Tend to be densely packed. -Typically, only one element is present, so all atomic radii are the same. -Metallic bonding is not directional. -Nearest neighbor distances tend to be small in order to lower bond energy. • Have the simplest crystal structures. • Types: 1) FCC 2) BCC 3) HCP • Focus on the unit cell: smallest repetitive entity • Properties : • Coordination number – number of nearest neighbor or touching atoms • Atomic Packing Factor (APF) – ratio of volume of atoms in unit cell to the total unit cell volume

  3. FACE CENTERED CUBIC STRUCTURE (FCC) • Atom at each corner, and at center of each face. --Note: All atoms are identical; the face-centered atoms are shaded differently only for ease of viewing. • Coordination # = 12

  4. ATOMIC PACKING FACTOR: FCC • APF for a face-centered cubic structure = 0.74

  5. BODY CENTERED CUBIC STRUCTURE (BCC) • Atom at each corner, and at the center of cube. --Note: All atoms are identical; the center atom is shaded differently only for ease of viewing. • Coordination # = 8

  6. ATOMIC PACKING FACTOR: BCC • APF for a body-centered cubic structure = 0.68

  7. HEXAGONAL CLOSE-PACKED STRUCTURE (HCP) • ABAB... Stacking Sequence • 3D Projection • 2D Projection • Coordination # = 12 • APF = 0.74

  8. FCC STACKING SEQUENCE • ABCABC... Stacking Sequence • 2D Projection • FCC Unit Cell

  9. HCP APF • APF = 0.74

  10. THEORETICAL DENSITY, r

  11. Example: Density Computation Example: Compute the theoretical density of Copper Data from Table inside front cover of Callister (see next slide): • crystal structure = FCC: 4 atoms/unit cell • atomic weight = 63.55 g/mol (1 amu = 1 g/mol) • atomic radius R = 0.128 nm (1 nm = 10 cm) -7

  12. Characteristics of Selected Elements at 20C Adapted from Table, "Charac- teristics of Selected Elements", inside front cover, Callister 6e.

  13. Polymorphism and Allotropy • Polymorphism • Having more than one crystal structure (change with T & P) • Ex. Low-Carbon Steel can exist as BCC or FCC • Allotropy • Polymorphism in elemental solid • Ex. Carbon can exist as graphite or diamond

  14. SUMMARY • Atoms may have crystalline or amorphous structures. • We can predict the density of a material from the atomic weight, atomic radius, and crystal structure (e.g., FCC, BCC, HCP). • • Anisotropicmaterial - properties vary with • direction – true for a for a single crystal • orientation. • Isotropicmaterial- properties are non- • directional – true for polycrystals with randomly • oriented grains.

  15. Crystal Systems Unit Cell: Parameters: • 7 Crystal Systems: • -Cubic • Hexagonal • Tetragonal • Orthorhombic • Rhombohedral • Monoclinic • Triclini

  16. Crystallographic Positions (Coordinates) - Coordinates of points expressed as fractions of unit cell dimensions

  17. Crystallographic Directions -defined by line between two points • Steps: • Translate vector to pass at origin. • Determine lengths of components (projections) in terms of unit cell dimensions. • Multiply or divide by a common factor to reduce to smallest possible integer values, uvw. • Direction: [uvw] Family of Directions – nonparallel directions which are equivalent (same atom spacing). Ex. Cubic: <100> family – [100], [010], [001] Tetragonal <100> - [100], [010]

  18. Crystallographic Planes (Miller Indices) • Steps: • If the plane passes through origin, translate origin. • Determine lengths of planar intercepts in terms of unit cell dimensions. • Take reciprocals of the numbers in Step 2. • Multiply or divide by a common factor to reduce to integers: hkl • Enclose: (hkl) Example:

  19. Planes for Hexagonal Crystals Four axes: Example:

  20. Linear Density – fraction of the length of the line intersected by atoms. Planar Density - Fraction of the area occupied by atoms (count atoms only if plane intersect its center. • Example: For simple cubic crystal, find: • Linear density for [111] direction, • Planar density for (100) plane.

  21. Textbook Definitions: LD = PD =

  22. X-RAYS TO CONFIRM CRYSTAL STRUCTURE • Incoming X-rays diffract from crystal planes. Adapted from Fig. 3.2W, Callister 6e. • Measurement of: Critical angles, qc, for X-rays provide atomic spacing, d.

  23. For cubic crystal:

  24. Quiz Review 1. At the position equal to the equilibrium spacing of two atoms, which of the following is/are true? • The net force is equal to zero. • The net energy is maximum. • The net energy is zero. • A and B above.

  25. 2. Two atoms are at an interatomic spacing less than the equilibrium spacing.  Which of the following is true regarding the atoms? • The net energy is minimum. • The new force is zero. • The attractive force is greater than the repulsive force. • The attractive force is less than the repulsive force.

  26. 3. The interatomic bond that is formed by the transfer of one or more electrons from one atom to the other is called • Covalent bond. • Ionic bond. • Metallic bond. • Secondary bond.

  27. 4. An element with an atomic number of 9 is • Inert • Electronegative • Electropositive • Transition metal

  28. 5. Two atoms of different metals have the same crystal structure. If Atom A has a bigger atomic radius than atom B, which has the higher atomic packing factor? • Atom A • Atom B • Depends on atomic weights • None of the above.

  29. 6. What is the coordination number for a simple cubic crystal structure? • 12 • 8 • 6 • 4

  30. 7. For which crystal system is are the angles between the three axes equal to 90o and two of the unit cell dimensions are equal to each other? • Cubic • Tetragonal • Orthorhombic • Triclinic

  31. 8. Identify the crystallographic direction of the vector: • [-1 1 1] • [1 1 -1] • [1 -1 1] • [1 1 1]

  32. 9. Identify the crystallographic direction of the vector: • [-2 1 2] • [-2 1 1] • [1 -2 2] • [-1 2 1]

  33. 10. Identify the crystallographic plane. • (-201) • (321) • (320) • (231)

  34. 11. Identify the crystallographic plane. • (-3 1 -4) • (3 -1 2) • (2 1 2) • (3 0 2)

  35. 12. For an FCC crystal, along with direction is the linear density maximum? • [111] • [100] • [110] • [11-1]

More Related