ch02 nature of materials
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THE NATURE OF MATERIALS
Manufacturing Processes, 1311
Dr Simin NasseriSouthern Polytechnic State University
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THE NATURE OF MATERIALS
1. Atomic Structure and the Elements
2. Bonding between Atoms and Molecules
3. Crystalline Structures
4. Noncrystalline (Amorphous) Structures
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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
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Atomic Structure and the Elements
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Atomic Structure and the Elements
The basic structural unitof 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 chemicalbuilding blocks of all matter
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Element Groupings
The elements can begrouped into families and
relationships established
between and within the
families by means of the
Periodic Table
Metalsoccupy the left and
center portions of the table
Nonmetals are on right
Between them is a
transition zone containing
metalloidsor semi-metals
Metals Metalloids orSemimetals
NonMetals
Beryllium Be Boron B Helium He
LithiumLi SiliconSi NeonNe
Magnesium Mg ArsenicAs ArgonAr
Cadmium
Cd Antimony
Sb Krypton
Kr
Copper- Cu Polonium - Po Xenon Xe
Iron Fe Tellurium - Te Radon Rn
Zinc Zn Germanium - Ge FluorineF
Titanium Ti Chlorine Cl
GoldAu Oxygen O
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Figure 2.1 Periodic Table of Elements. Atomic number and symbol are listedfor the 103 elements.
Periodic Table
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Question?
What are the noble metals?
Copper
Silver
Gold
Noble metals (precious metals) are metals that are resistant to corrosion or oxidation, unlike most base metals.
Platinum (Pt), Palladium (Pd)
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Bonding between Atoms and Molecules
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Bonding between Atoms and Molecules
Atomsare held together in molecules by varioustypes of bonds
1. Primary bonds- generally associated with formation
of molecules
2. Secondary bonds- generally associated withattraction between molecules
Primary bonds are much stronger than secondary
bonds
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Bonding between Atoms and Molecules
Primary
Bonding
Secondary
Bonding
Ionic
Covalent
Metallic
Dipole forces
London forces
Hydrogen bonding
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Primary Bonds
Characterized by strong atom-to-atom attractionsthat involve exchange of valence electrons
Following forms:
Ionic
Covalent
Metallic
The ones on the outer shell
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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
elementto increase electron count in the outermost shell.
Properties:
Poor Ductility
Low Electrical Conductivity
Example: Sodium Chloride (NaCl)
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Covalent Bonding
Figure 2.4Second form of
primary bonding:
(b) covalent
Outer electrons are shared between two local atoms ofdifferent elements.
Properties:
High HardnessLow Electrical Conductivity
Examples: Diamond, Graphite
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Metallic Bonding
Figure 2.4 Thirdform of primary
bonding: (c) metallic
Outer shell electrons are shared by all atoms to forman electron cloud.
Properties:
- Good Conductor
(Heat and Electricity)- Good Ductility
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Secondary Bonds
Secondary bonds involve attraction forcesbetween 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:
1. Dipole forces
2. London forces
3. Hydrogen bonding
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Macroscopic Structures of Matter
Atoms and molecules are the building blocksof 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 twostructures:
Crystalline
Noncrystalline
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Crystalline Structures
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Crystalline Structure
Structure in which atoms are located at regularand recurring positions in three dimensions
Unit cell- basic geometric groupingof 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 manyceramics and somepolymers
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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:
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Question?
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!!
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Three Crystal Structures in Metals
1. Body-centered cubic (BCC)2. Face centered cubic (FCC)
3. Hexagonal close-packed (HCP)
Figure 2.8 Three types of crystal structure in metals.
# of atoms in unit cell: 9 # of atoms: 14 # of atoms: 17
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Crystal Structures for Common Metals
Room temperature crystal structures for some of thecommon 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
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Imperfections (Defects) in Crystals
Imperfections often arise due to inability ofsolidifying material to continue replicationof 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).
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Types of defects or imperfections
Point defects, Line defects,
Surface defects.
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Point Defects
Imperfections in crystal structure involving eithera single atom or a few number of atoms
Figure 2.9 Point defects: (a) vacancy, (b) ion-pair vacancy (Schottky),
(c) interstitialcy, (d) displaced ion (Frenkel Defect).
Extra atom present
Dislocation of an atom
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Line Defects
Defect happens along a line( Connected group of pointdefects that forms a line in the lattice structure)
Most important line defect is a dislocation, which cantake two forms:
Edge dislocation
Screw dislocation
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Edge Dislocation
Figure 2.10 Line
defects: (a) edge
dislocation
Edge of an extra plane of atoms that exists inthe lattice
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Screw Dislocation
Figure 2.10 Line
defects: (b) screw
dislocation
Spiral within the lattice structure wrapped aroundan imperfection line, like a screw is wrapped
around its axis
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Surface Defects
Imperfections that extend in two directionstoform a boundary
Examples:
External:the surface of a crystalline object
is an interruption in the lattice structure
Internal:grain boundaries are internal
surface interruptions
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Elastic Strain
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Elastic Strain
When a crystal experiences a graduallyincreasing stress, it first deforms elastically
If force is removed lattice structure returns toits original shape
Figure 2.11 Deformation of a crystal structure: (a) original lattice: (b)
elastic deformation, with no permanent change in positions of atoms.
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Plastic Strain
If stress is higher than forces holding atoms intheir 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.
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Effect of Dislocations on Strain
In the series of diagrams, the movement of the dislocationallows deformation to occur under a lower stress than in aperfect lattice.
Slipinvolves 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.
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Slip on a Macroscopic Scale
When a lattice structure with an edge dislocationis subjected to a shear stress, the material
deforms much more readilythan in a perfect
structure.
Dislocations are a good-news-bad-news situation
Good newsin manufacturingthe metal is easier to
form
Bad newsin designthe metal is not as strong as thedesigner would like
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Twinning
A second mechanism of plastic deformationin
which atoms on one side of a plane (the twinningplane) are shifted to form a mirror imageof theother 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.
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Polycrystalline Nature of Metals
A block of metal may containmillions 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
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Crystalline Structure
Growth of crystals in metals
Grain
How do polycrystallinestructures form? As a block of metal
cools from the moltenstate and begins tosolidify, individualcrystals nucleate atrandom positions and
orientations throughoutthe liquid
These crystals grow andfinally interfere witheach other, forming attheir interface a surfacedefect - a grainboundary
Grain boundaries aretransition zones, perhapsonly a few atoms thick
Grain
boundary
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Noncrystalline (Amorphous) Structures
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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
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Features of Noncrystalline Structures
Two features differentiate noncrystalline(amorphous) from crystalline materials:
1. Absence of long-range order in
molecular structure
2. Differences in melting and thermal
expansion characteristics
What are the
differences
between
them?
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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 randomand less tightly packed.
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Solidification
Alloy Metal Pure Metal
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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
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Summary: Characteristics of Metals
Crystalline structuresin the solid state, almostwithout exception
BCC, FCC, or HCP unit cells
Atoms held together by metallic bonding
Properties: high strength and hardness, high
electrical and thermal conductivity
FCC metalsare generally ductile
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Summary: Characteristics of Ceramics
Most ceramics have crystalline structures,while glass(SiO2) is amorphous
Molecules characterized by ionic or covalent
bonding, or both
Properties: high hardness and stiffness,
electrically insulating, refractory, and
chemically inert
Refractorymaterials retain their strength at high temperatures. Theyare used to make crucibles and linings for furnaces, kilns and
incinerators.
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Summary: Characteristics of Polymers
Many repeating mersin molecule held togetherby covalent bonding
Polymers usually carbon plusone or more
other elements: H, N, O, and Cl
Amorphous(glassy) structure or mixture of
amorphous and crystalline
Properties: low density, high electrical
resistivity, and low thermal conductivity,
strength and stiffness vary widely
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