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Lec . 1 THE NATURE OF MATERIALS

Lec . 1 THE NATURE OF MATERIALS

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Lec . 1 THE NATURE OF MATERIALS

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  1. Lec. 1 THE NATURE OF MATERIALS Industrial Material Applications, IE251 Dr M. A. Eissa King Saud University College of Engineering Department of Industrial Engineering

  2. THE NATURE OF MATERIALS • Atomic Structure and the Elements • Bonding between Atoms and Molecules • Crystalline Structures • Noncrystalline (Amorphous) Structures

  3. Importance of Materials in Manufacturing • Manufacturing is a transformation process • It is the material that is transformed • And it is the behavior of the material when subjected to the forces, temperatures, and other parameters of the process that determines the success of the operation

  4. Atomic Structure and the Elements

  5. Atomic Structure and the Elements • The basic structural unit of matter is the atom • Each atom is composed of a positively charged nucleus, surrounded by a sufficient number of negatively charged electrons so the charges are balanced • More than 100 elements, and they are the chemical building blocks of all matter

  6. Element Groupings The elements can be grouped into families and relationships established between and within the families by means of the Periodic Table • Metals occupy the left and center portions of the table • Nonmetals are on right • Between them is a transition zone containing metalloids or semi‑metals

  7. Periodic Table Figure 2.1 Periodic Table of Elements. Atomic number and symbol are listed for the 103 elements.

  8. Copper Silver Gold Platinum (Pt), Palladium (Pd) Noble metals (precious metals) are metals that are resistant to corrosion or oxidation, unlike most base metals. Question? What are the noble metals?

  9. Bonding between Atoms and Molecules

  10. Bonding between Atoms and Molecules Atoms are held together in molecules by various types of bonds • Primary bonds - generally associated with formation of molecules • Secondary bonds - generally associated with attraction between molecules • Primary bonds are much stronger than secondary bonds

  11. Bonding between Atoms and Molecules Primary Bonding Secondary Bonding Ionic Covalent Metallic Dipole forces London forces Hydrogen bonding

  12. The ones on the outer shell Primary Bonds Characterized by strong atom‑to‑atom attractions that involve exchange of valence electrons • Following forms: • Ionic • Covalent • Metallic

  13. Ionic Bonding Figure 2.4 First form of primary bonding: (a) Ionic Atoms of one element give up their outer electron(s),which are in turn attracted to atoms of some other element to increase electron count in the outermost shell. • Properties: • Poor Ductility • Low Electrical Conductivity • Example: Sodium Chloride (NaCl)

  14. Covalent Bonding Figure 2.4 Second form of primary bonding: (b) covalent Outer electrons are shared between two local atoms of different elements. • Properties: • High Hardness • Low Electrical Conductivity • Examples: Diamond, Graphite

  15. Metallic Bonding Figure 2.4 Third form of primary bonding: (c) metallic Outer shell electrons are shared by all atoms to form an electron cloud. • Properties: • - Good Conductor (Heat and Electricity) • - Good Ductility

  16. Secondary Bonds Secondary bonds involve attraction forces between molecules(whereas primary bonds involve atom‑to‑atom attractive forces), • No transfer or sharing of electrons in secondary bonding • Bonds are weaker than primary bonds • Three forms: • Dipole forces • London forces • Hydrogen bonding

  17. Macroscopic Structures of Matter • Atoms and molecules are the building blocks of more macroscopic structure of matter • When materials solidify from the molten state, they tend to close ranks and pack tightly, arranging themselves into one of two structures: • Crystalline • Noncrystalline

  18. Crystalline Structures

  19. Crystalline Structure Structure in which atoms are located at regular and recurring positions in three dimensions • Unit cell - basic geometric grouping of atoms that is repeated • The pattern may be replicated millions of times within a given crystal • Characteristic structure of virtually all metals, as well as many ceramics and somepolymers

  20. Crystallinity When the monomers are arranged in a neat orderly manner, the polymer is crystalline.Polymers are just like socks. Sometimes they are arranged in a neat orderly manner. An amorphous solid is a solid in which the molecules have no order or arrangement.Some people will just throw their socks in the drawer in one big tangled mess. Their sock drawers look like this:

  21. Question? What about glass?! Does glass have a crystalline structure?! "What is glass... is it a liquid or a solid?" • Antique windowpanes are thicker at the bottom, because glass has flowed to the bottom over time! • Glass has no crystalline structure, hence it is NOT a solid. • Glass is a supercooled liquid. • Glass is a liquid that flows very slowly. • Glass is a highly viscous liquid!!

  22. # of atoms: 14 # of atoms: 17 # of atoms in unit cell: 9 Three Crystal Structures in Metals • Body-centered cubic (BCC) • Face centered cubic (FCC) • Hexagonal close-packed (HCP) Figure 2.8 Three types of crystal structure in metals.

  23. Crystal Structures for Common Metals Room temperature crystal structures for some of the common metals: • Body‑centered cubic (BCC) • Chromium, Iron, Molybdenum, Tungsten • Face‑centered cubic (FCC) • Aluminum, Copper, Gold, Lead, Silver, Nickel, (Iron at 1670oF) • Hexagonal close‑packed (HCP) • Magnesium, Titanium, Zinc

  24. Body-Centered Cubic Crystal Structure Figure 1.2 The body-centered cubic (bcc) crystal structure: (a) hard-ball model; (b) unit cell; and (c) single crystal with many unit cells. Source: W. G. Moffatt, et al., The Structure and Properties of Materials, Vol. 1, John Wiley & Sons, 1976.

  25. Face-Centered Cubic Crystal Structure Figure 1.3 The face-centered cubic (fcc) crystal structure: (a) hard-ball model; (b) unit cell; and (c) single crystal with many unit cells. Source: W. G. Moffatt, et al., The Structure and Properties of Materials, Vol. 1, John Wiley & Sons, 1976.

  26. Hexagonal Close-Packed Crystal Structure Figure 1.4 The hexagonal close-packed (hcp) crystal structure: (a) unit cell; and (b) single crystal with many unit cells. Source: W. G. Moffatt, et al., The Structure and Properties of Materials, Vol. 1, John Wiley & Sons, 1976.

  27. Imperfections (Defects) in Crystals • Imperfections often arise due to inability of solidifying material to continue replication of unit cell,e.g., grain boundaries in metals • It is in fact: Deviation in the regular pattern of the crystalline lattice structure. Studying about imperfections is important: Imperfection is bad: a perfect diamond (with no flaws) is more valuable than one containing imperfections. Imperfection is good: the addition of an alloying ingredient in a metal to increase its strength (this is an imperfection which is introduced purposely).

  28. Types of defects or imperfections • Point defects, • Line defects, • Surface defects.

  29. Point Defects Imperfections in crystal structure involving either a single atom or a few number of atoms Dislocation of an atom Extra atom present Figure 2.9 Point defects: (a) vacancy, (b) ion‑pair vacancy (Schottky), (c) interstitialcy, (d) displaced ion (Frenkel Defect).

  30. Defects in a Single-Crystal Lattice Figure 1.9 Schematic illustration of types of defects in a single-crystal lattice: self-interstitial, vacancy, interstitial, and substitutional.

  31. Line Defects Defect happens along a line ( Connected group of point defects that forms a line in the lattice structure) • Most important line defect is a dislocation, which can take two forms: • Edge dislocation • Screw dislocation

  32. Edge Dislocation Figure 2.10 Line defects: (a) edge dislocation Edge of an extra plane of atoms that exists in the lattice

  33. Movement of an Edge Dislocation Figure 1.10 Movement of an edge dislocation across the crystal lattice under a shear stress. Dislocations help explain why the actual strength of metals in much lower than that predicted by theory.

  34. Screw Dislocation Figure 2.10 Line defects: (b) screw dislocation Spiral within the lattice structure wrapped around an imperfection line, like a screw is wrapped around its axis

  35. Surface Defects Imperfections that extend in two directions to form a boundary • Examples: • External:the surface of a crystalline object is an interruption in the lattice structure • Internal:grain boundaries are internal surface interruptions

  36. Elastic Strain

  37. Elastic Strain When a crystal experiences a gradually increasing stress, it first deforms elastically • If force is removed lattice structure returns to its original shape Figure 2.11 Deformation of a crystal structure: (a) original lattice: (b) elastic deformation, with no permanent change in positions of atoms.

  38. Plastic Strain If stress is higher than forces holding atoms in their lattice positions, a permanent shape change occurs Figure 2.11 Deformation of a crystal structure: (c) plastic deformation (slip), in which atoms in the lattice are forced to move to new "homes“.

  39. Effect of Dislocations on Strain • In the series of diagrams, the movement of the dislocation allows deformation to occur under a lower stress than in a perfect lattice. • Slip involves the relative movement of atoms on the opposite sides of a plane in the lattice, called slip plane. Figure 2.12 Effect of dislocations in the lattice structure under stress.

  40. Slip on a Macroscopic Scale • When a lattice structure with an edge dislocation is subjected to a shear stress, the material deforms much more readily than in a perfect structure. • Dislocations are a good‑news‑bad‑news situation • Good news in manufacturing – the metal is easier to form • Bad news in design – the metal is not as strong as the designer would like

  41. Twinning • A second mechanism of plastic deformation in which atoms on one side of a plane (the twinning plane) are shifted to form a mirror image of the other side Figure 2.13 Twinning, involving the formation of an atomic mirror image on the opposite side of the twinning plane: (a) before, and (b) after twinning.

  42. Polycrystalline Nature of Metals • A block of metal may contain millions of individual crystals, called grains • Such a structure is called polycrystalline • Each grain has its own unique lattice orientation; but collectively, the grains are randomly oriented in the block

  43. Crystalline Structure • How do polycrystalline structures form? • As a block of metal cools from the molten state and begins to solidify, individual crystals nucleate at random positions and orientations throughout the liquid • These crystals grow and finally interfere with each other, forming at their interface a surface defect ‑ a grain boundary • Grain boundaries are transition zones, perhaps only a few atoms thick Grain Grain boundary Growth of crystals in metals

  44. Noncrystalline (Amorphous) Structures

  45. Noncrystalline (Amorphous) Structures • Many materials are noncrystalline • Water and air have noncrystalline structures • A metal loses its crystalline structure when melted • Some important engineering materials have noncrystalline forms in their solid state: • Glass • Many plastics • Rubber

  46. Features of Noncrystalline Structures • Two features differentiate noncrystalline (amorphous) from crystalline materials: • Absence of long‑range order in molecular structure • Differences in melting and thermal expansion characteristics What are the differences between them?

  47. Crystalline versus Noncrystalline Figure 2.14 Difference in structure between: (a) crystalline and (b) noncrystalline materials. The crystal structure is regular, repeating, and denser The noncrystalline structure is random and less tightly packed.

  48. Solidification Alloy Metal Pure Metal

  49. Volumetric Effects Figure 2.15 Characteristic change in volume for a pure metal (a crystalline structure), compared to the same volumetric changes in glass (a noncrystalline structure). Tg=glass temperature Tm=melting temperature

  50. Summary: Characteristics of Metals • Crystalline structuresin the solid state, almost without exception • BCC, FCC, or HCP unit cells • Atoms held together by metallic bonding • Properties: high strength and hardness, high electrical and thermal conductivity • FCC metals are generally ductile