Lecture 2 Metals and its properties Lecture

©2007 John Wiley & Sons, Inc. M P Groover, Fundamentals of Modern Manufacturing 3/e
METALS
1. Introduction
2. Alloys and Phase Diagrams
3. Ferrous Metals
4. Nonferrous Metals
5. Super alloys
6. Guide to the Processing of Metals

Metals
 Most elements are metals. 88 elements to the left of
the stairstep line are metals or metal like elements.

Metals: The Most Important
Engineering Material
 Metals can be seen all around us
 We use metals because they have many useful
properties
Electrical wires
(conduction, Free Electrons)
Frames for houses
( Mechanical Properties)
Taps
( Mechanical + Manufacturing properties)

Metals: The Most Important
Engineering Materials
 They have properties that satisfy a wide variety
of design requirements
 The manufacturing processes by which they
are shaped into products have been developed
and refined over many years
 Engineers understand metals

Why Metals Are Important
 High stiffness and strength - can be alloyed for
high rigidity, strength, and hardness
 Toughness - capacity to absorb energy better
than other classes of materials
 Good electrical conductivity - Metals are
conductors
 Good thermal conductivity - conduct heat better
than ceramics or polymers
 Easily processable
 Cost – the price of steel is very competitive
with other engineering materials

Starting Forms of Metals used in
Manufacturing Processes
 Cast metal - starting form is a casting
Metal Casting is the process in which molten metal is poured into a mould
that contains a hollow cavity of a desired geometrical shape and allowed to
cool down to form a solidified part.
 Wrought metal - Wrought metals are those that have been
shaped by hammers and other tools. The metals can be wrought after
casting. Wrought iron is a common material for gates and fences
 Powdered metal – Metal powder is a metal that has been
broken down into a powder form.
Powdered metals are often used to facilitate lubrication, corrosion
resistance or to create alloys. Metal powders commonly used in
manufacturing products: Aluminum Powder. Bismuth Powder

Metals
Physical Properties of Metals:
 Metals have Lustre (shininess)
 Good conductors of heat and electricity
 High density (heavy for their size)
 High melting point (due to complete crystal structure)
 Ductile (most metals can be drawn out into thin wires)
 Malleable (most metals can be hammered/drawn into
thin sheets)

Metals
Chemical Properties of Metals:
 Easily lose electrons
Conduction
Corrode easily. Corrosion is a gradual wearing away
due to same property. Create bonds with other e.g
(Example: silver tarnishing and iron rusting)
 How would you test for hardness?
 Electrical conductivity?
 Heat conductivity?

Metals Bonding Model
 In a solid sample of a metal:
1. Positive ions are arranged in a closely packed
structure. This is called a regular three
dimensional lattice of positive ions.
 The ions occupy fixed positions in a lattice

2. The Outermost electrons (valence electrons) of metals
wander freely through metallic lattice. These are called
delocalised electrons.
 Metal consists of cat ions held together by negatively-
charged electron "glue.“
 delocalised electrons are not associated with a single
atom or to a bond.

3. The ions in the lattice are held together by
electrostatic forces and delocalised electrons
Electrostatic forces are the forces between
particles that are caused by their electric
charges
This attraction extends throughout the lattice and
is called metallic bonding.

Limitations of Metal Bonding Model
 Some properties of metals cannot be explained
by the metallic bonding
1.The range of melting points, densities
2. Magnetic nature of cobalt iron and nickel
3. Differences in electrical conductivity
4. Solubility in water and corrosion

Metals Crystal Model
 Some of these limitations can be explained by the
metal crystal model
 Metals form crystals, large or small
Cat ions
Delocalised
electrons
between Cat
ions
Large
metal
crystals
small
metal
crystals

Explaining Properties of Metals
Why do metals have relatively high
boiling points?
 The strong attraction (electrostatic forces)
between the positive cat ions and
delocalised electrons holds the metallic
lattice together making it hard to loosen
the bonds.

Why are metals good conductors of
electricity and heat?
 Delocalised (free) electrons can move rapidly in
response to electric fields and transmit heat,
hence metals are a good conductors of
electricity and heat.

Why are metals malleable and ductile?
 The layers of atoms in metal are hard to pull
apart because of the electrons holding them
together, hence metals are tough.
 Individual atoms are not held to any other
specific atoms, hence atoms slip easily past one
another. Thus metals are ductile and malleable.

Why are metals hard?
 Strong electrostatic forces between the cat
ions and electrons make it difficult to
separate particles from one another
 Why are metals lustrous(shiny)?
 When light energy hits the delocalised
electrons they absorb the energy and jump
to high energy level, when they go back down
a level they release energy in the form of a
photon hence the shininess

Modifying Metals
 Few metals are used in their pure form
 Most metals need to be changed in some way so
they can be used. This may include treating the
metals and combining metals
Example: Iron is not hard enough by itself to be
used so we use steel.
Steel is made by mixing iron with about 2% carbon

3- Ways
To Modify the Metals
A: Alloys
B: Hardening
C: Heat Treatment

Alloying
 Properties of metals can be significantly altered
by adding other substances, usually a metal or
carbon.
 The substances are melted together and mixed
then allowed to cool. This is called an alloy.
 Note no chemical reaction has taken place it is
just a mixing of two metals

Hardening of Metals
 The way a metal is prepared can have a large
impact on how it behaves
 Many metals are prepared in the liquid state and
cooled. The rate at which it cools can have a
significant effect on the properties of the solid
(time for making crystals)

Arranging Crystals
 Small metal crystals make the
metal harder because the ions are
less able to move
 Smaller crystals also means there
is more disruption between crystals
making them brittle (easy to break)
 Larger metal crystals make the
metal soft

Heat Treatment
 There are three ways of treating a metal
with heat
1. Annealing
2. Quenching
3. Tempering

Treatment Process Effect on
metal
properties
Effect on metal
structure
Annealing A metal is heated to a
moderate
temperature and
allowed to cool slowly
The metal is
softer with
improved
ductility
Larger metal
crystals form
Quenching A metal is heated to a
moderate
temperature and
cooled quickly
(sometimes by
plunging into water
The metal is
harder and
brittle.
Tiny metals
crystals form.
Tempering A quenched metal is
heated (to a lower
temperature than is
used for quenching
and allowed to cool
The metal is
harder but
less brittle.
Crystals of
intermediate
size form.

Classification of Metals
 Ferrous - those based on iron
 Steels
 Cast irons
 Nonferrous - all other metals
 Aluminum, magnesium, copper, nickel,
titanium, zinc, lead, tin, molybdenum,
tungsten, gold, silver, platinum, and others
 Super alloys

Metals and Alloys
 Some metals are important as pure elements
(e.g., gold, silver, copper)
 Most engineering applications require the
enhanced properties obtained by alloying
 Through alloying, it is possible to increase
strength, hardness, and other properties
compared to pure metals

Alloys
An alloy = a mixture or compound of two or more
elements, at least one of which is metallic
 Two main categories:
1. Solid solutions
2. Intermediate phases

Solid Solutions
An alloy in which one element is dissolved in
another to form a single-phase structure
 A phase = any homogeneous mass of material,
such as a metal in which the grains all have the
same crystal lattice structure
 In a solid solution, the solvent or base element
is metallic, and the dissolved element can be
either metallic or nonmetal

Two Forms of Solid Solutions
1. Substitutional solid solution - atoms of solvent
element are replaced in its unit cell by
dissolved element
2. Interstitial solid solution - atoms of dissolving
element fit into vacant spaces between base
metal atoms in the lattice structure
 In both forms, the alloy structure is generally
stronger and harder than either of the
component elements

Two Forms of Solid Solutions
Figure 6.1 Two forms of solid solutions: (a) substitutional
solid solution, and (b) interstitial solid solution.

Intermediate Phases
 There are usually limits to the solubility of one
element in another
 When the amount of the dissolving element in
the alloy exceeds the solid solubility limit of the
base metal, a second phase forms in the alloy
 The term intermediate phase is used to
describe it because its chemical composition is
intermediate between the two pure elements
 Its crystalline structure is also different from
those of the pure metals

Types of Intermediate Phases
1. Metallic compounds – consist of a metal and
nonmetal, such as Fe3C
2. Intermetallic compounds - two metals that
form a compound, such as Mg2Pb
 In some alloy compositions, the intermediate
phase is mixed with the primary solid solution
to form a two-phase structure
 Some two-phase alloys are important because
they can be heat treated for much higher
strength than solid solutions

Phase Diagrams
A graphical means of representing the phases of
a metal alloy system as a function of
composition and temperature
 A phase diagram for an alloy system consisting
of two elements at atmospheric pressure is
called a binary phase diagram
 Other forms of phase diagrams are
discussed in texts on metallurgy and
materials science

Phase Diagrams
 Composition is plotted on the horizontal axis
and temperature on the vertical axis
 Any point in the diagram indicates the overall
composition and the phase or phases present
at the given temperature under equilibrium
conditions

Copper-Nickel Phase Diagram
Figure 6.2 Phase diagram for the copper-nickel alloy
system.

Copper-Nickel (Cu-Ni) Alloy System
 Solid solution alloy throughout entire range of
compositions below the solidus
 No intermediate solid phases in this alloy
system
 However, there is a mixture of phases (solid +
liquid) in the region bounded by the solidus and
liquidus

Chemical Compositions of Phases
 The overall composition of the alloy is given by
its position along the horizontal axis
 However, the compositions of liquid and solid
phases are not the same
 These compositions can be found by
drawing a horizontal line at the temperature
of interest
 Where the line intersects the solidus and
liquidus indicates the compositions of solid
and liquid phases, respectively

Example
Determine compositions of liquid and solid phases
in the Cu-Ni system at an aggregate composition
of 50% nickel and a temperature of 1316oC
(2400oF)

Inverse Lever Rule – Step 1
 The phase diagram can be used to determine
the amounts of each phase present at a given
temperature
 Using the horizontal line that indicates
overall composition at a given temperature,
measure the distances between the
aggregate composition and the intersection
points with the liquidus and solidus,
identifying the distances as CL and CS,
respectively

Inverse Lever Rule – Step 2
 The proportion of liquid phase present is given
by
L phase proportion =
 And the proportion of solid phase present is
given by
S phase proportion =
)
( CL
CS
CS

CL
CS
CL


Applications of the Inverse Lever Rule
 Methods for determining chemical composition
of phases and amounts of each phase are
applicable to the solid region of the phase
diagram as well as the liquidus-solidus region
 Wherever there are regions in which two phases
are present, these methods can be utilized
 When only one phase is present, the
composition of the phase is its aggregate
composition under equilibrium conditions, and
the inverse lever rule does not apply

Tin-Lead Phase Diagram
Figure 6.3 Phase diagram for the tin-lead alloy system.

Tin-Lead (Sn-Pb) Alloy System
 Widely used in soldering for making
electrical connections
 Sn-Pb system includes two solid phases,
alpha () and beta ()
-phase = solid solution of tin in lead at left
side of diagram
-phase = solid solution of lead in tin at
around 200C (375F) at right side of
diagram
 Between these solid solutions lies a mixture
of the two solid phases,  + 

Melting in the Tin-Lead Alloy System
 Pure tin melts at 232C (449F)
 Pure lead melts at 327C (621F)
 Tin-lead alloys melt at lower temperatures
 The diagram shows two liquidus lines that
begin at the melting points of the pure metals
and meet at a composition of 61.9% Sn
 This is the eutectic composition for the
tin-lead system

Ferrous Metals
Based on iron, one of the oldest metals known to
man
 Ferrous metals of engineering importance are
alloys of iron and carbon
 These alloys divide into two major groups:
 Steel
 Cast iron
 Together, they constitute approximately 85% of
the metal tonnage in the United States

Iron as a Commercial Product
 Electrolytic iron - the most pure, at about
99.99%, for research and other purposes
where the pure metal is required
 Ingot iron - contains about 0.1% impurities
(including about 0.01% carbon), used in
applications where high ductility or corrosion
resistance are needed
 Wrought iron - contains about 3% slag but very
little carbon, and is easily shaped in hot
forming operations such as forging

Steel and Cast Iron Defined
Steel = an iron-carbon alloy containing from
0.02% to 2.1% carbon
Cast iron = an iron-carbon alloy containing
from 2.1% to about 4% or 5% carbon
 Steels and cast irons can also contain
other alloying elements besides carbon

Iron and Steel Production
 Iron making - iron is reduced from its ores
 Steel making – iron is then refined to obtain
desired purity and composition (alloying)

Iron Ores Required in Iron-making
 The principal ore used in the production of iron
and steel is hematite (Fe2O3)
 Other iron ores include magnetite (Fe3O4),
siderite (FeCO3), and limonite (Fe2O3-xH2O,
where x is typically around 1.5)
 Iron ores contain from 50% to around 70% iron,
depending on grade (hematite is almost 70%
iron)
 Scrap iron and steel are also widely used today
as raw materials in iron- and steel making

Other Raw Materials in Iron-making
 Coke (C)
 Supplies heat for chemical reactions and
produces carbon monoxide (CO) to reduce
iron ore
 Limestone (CaCO3)
 Used as a flux to react with and remove
impurities in molten iron as slag
 Hot gases (CO, H2, CO2, H2O, N2, O2, and
fuels)
 Used to burn coke

Iron-making in a Blast Furnace
Blast furnace - a refractory-lined chamber with a
diameter of about 9 to 11 m (30 to 35 ft) at its
widest and a height of 40 m (125 ft)
 To produce iron, a charge of ore, coke, and
limestone are dropped into the top of a blast
furnace
 Hot gases are forced into the lower part of the
chamber at high rates to accomplish
combustion and reduction of the iron

Figure 6.5
Cross-section of
iron-making
blast furnace
showing major
components

Lecture 2 Metals and its properties Lecture

Chemical Reactions in Iron-Making
 Using hematite as the starting ore:
Fe2O3 + CO  2FeO + CO2
 CO2 reacts with coke to form more CO:
CO2 + C (coke)  2CO
 This accomplishes final reduction of FeO to
iron:
FeO + CO  Fe + CO2

Proportions of Raw Materials In
Iron-Making
 Approximately seven tons of raw materials are
required to produce one ton of iron:
 2.0 tons of iron ore
 1.0 ton of coke
 0.5 ton of limestone
 3.5 tons of gases
 A significant proportion of the byproducts are
recycled

Iron from the Blast Furnace
 Iron tapped from the blast furnace (called pig
iron) contains over 4% C, plus other impurities:
0.3-1.3% Si, 0.5-2.0% Mn, 0.1-1.0% P, and
0.02-0.08% S
 Further refinement is required for cast iron and
steel
 A furnace called a cupola is commonly used
for converting pig iron into gray cast iron
 For steel, compositions must be more closely
controlled and impurities brought to much
lower levels

Lecture 2 Metals and its properties Lecture

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