This document provides information about Material Technology 1 course offered by PN. Norhazlina Bte Amon. The course covers topics like material structure, binary alloy systems, ferrous materials, metal working processes, corrosion and non-ferrous metals over 18 weeks. Students will be assessed through quizzes, theory tests and other tasks like end of chapter exercises and presentations.

1. JF302 – MATERIAL
TECHNOLOGY 1
LECTURER : PN.NORHAZLINA BTE AMON
(Coordinator)
Contact no. : 019-6462754

2. Course outline
SYNOPSIS
MATERIAL TECHNOLOGY 1 provides students an understanding on
pure metal, alloy and other non-metal materials that are
commonly used in the engineering field, including a study on metal
and alloy microstructure. Students also learn the processes of
metal work and specific materials used to produce engineering
components.

3. WEEKLY SCHEDULE
Week 1 : Students Registration
Week 2-3 :1.0 - MATERIAL STRUCTURE AND BINARY ALLOY SYSTEM
Week 4-5 :2.0 – FERROUS MATERIAL STRUCTURE AND BINARY ALLOY SYSTEM
Week 6-8 :3.0 – METAL WORK, CASTING PROCESS AND HEAT TREATMENT ON
STEEL
Week 9 : Mid-Semester Break
Week 10-12 :4.0 MATERIAL TESTING
Week 13-15 :5.0 CORROSION AND NON-FERROUS METAL
Week 16-17 :6.0 PLASTIC
Week 18-19 :Revision Week and Final Examination

4. GRADING (CONTINUOUS
ASSESSMENT)
No. Assessment Number
(minimum)
% total Week
1 Quiz 2 20 W2, W5, W10
2 Theory Test 2 40 W8, W15
3 Other Assessment Task
i. End of Chapter
ii. Presentation
2
1
20
20
W2, W5, W12
W16
Overall Total 8 100
REFERENCES :
Arens. W. F (2004). Contemporary Advertising. McGraw Hill. United States.
Brown B. C. (2007). The Complete Guide To Google Advertising Including Tips and Tricks and
Strategies to Create a Winning Advertising Plan. Atlantic Publishing Group Inc. Florida.
Ogivly. D. (1985). Ogivly on Advertising. Random House Inc. United States.
Sissors. J.Z. (2002). Advertising Media Planning. McGraw Hill. United States.
Well . W.D. (2005) Advertising : Principles and Pratice. United States.

5. Atomic Structure
• Atomic structure is made of:
 Protons: positive (+) charge
 Neutrons: no charge (neutral)
 Electrons: negative (-) charge
• The nucleus contains the mass of an atom: Protons +
Neutrons
• Layers of electrons that orbit around the nucleus are
called orbitals or energy-level shells.

6. Atomic Structure

7. Element
 In chemistry, an element is a pure
substances that cannot be broken
down into any simpler substances by
chemical method.
 Each element has its own atomic
mass, and a no. of protons and
electrons for an elements always
remains the same.

8.  Elements can bond with one another to form
compounds.
 These are some famous elements :
Iron(Fe), Gold(Au), Hydrogen(H),
Carbon(C), Oxygen(O)
 These are some compounds (combination of
elements)
Water(H2O), Carbon dioxide(CO2),
Ammonia (NH3)

9. Periodic Table of Elements

10. Crystalline & Amorphous
 Materials are either:
1. Crystalline
2. Non-crystalline – Amorphous
What is crystalline material?
 Crystalline solid must have an ordered arrangement
of atoms (occupy specific or predictable positions in
a 3D array).
 Crystalline materials include metals, many ceramics
and some polymers

11. Crystalline & Amorphous
 In an amorphous solid atoms do not possess well-
defined arrangement (atoms have no periodic
packing)
 Amorphous structures form in complex structures,
polymers, and rapidly cooled materials.

12. Why do we need to know the crystal structure?
• Crystal structure of a material affects its mechanical
properties (strength, toughness, ductility)
• Understanding crystal structures is essential in
understanding the crystalline materials.

13. Crystalline Structure
􀂄 Structure in which the 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 some polymers

14. Principals Metallic Crystal
Structures
 Most important engineering metals have one of the
following crystal structures:
◦ BCC - body centered cubic
◦ FCC - face centered cubic
◦ HCP – hexagonal close packed

15. Principals Metallic Crystal
Structures

16. BCC ( Body-Centered
Crystal)
Body-centered cubic (BCC) crystal structure:
(a)unit cell, with atoms indicated as point locations in a three-
dimensional axis system
(b) unit cell model showing closely packed atoms (sometimes
called the hard-ball model)
(c) repeated pattern of the BCC structure
Number of atoms in a BCC unit cell
 Each corner atom contributes
as 1/8
 There are 8 corner atoms/
BCC unit cell
• There is 1 atom in the centre
(non shared)
cellunitatomsatomsofnumber /2118
8
1


17. Number of atoms in a FCC unit cell
 Each corner atom contributes
as 1/8
 There are 8 corner atoms/
BCC unit cell
• Each face atom contributes
as ½
• There are 6 face atoms
cellunitatomsatomsofnumber /4
2
1
68
8
1


18. Crystal Structures for
Common Metals
(at Room Temperature)
 Body-centered cubic (BCC)
Chromium, Iron, Molybdenum, Tungsten
 Face-centered cubic (FCC)
Aluminum, Copper, Gold, Lead, Silver, Nickel
 Hexagonal close-packed (HCP)
Magnesium, Titanium, Zinc

19. TERMS USE IN
RECRYSTALLIZATION
PROCESS
Space Lattice & Unit Cell
 Lattice - A collection of points that divide space into
smaller equally sized segments.
 Unit cell - A subdivision of the lattice that still retains the
overall characteristics of the entire lattice.

20. Space Lattice & Unit Cell

21. Grain And Grain Boundary
 Grain – Most Crystalline solids are
composed of a collection of many crystals.
 Grain Boundary – There exist some atomic
mismatch within the region where two
grains meet.

22. Atomic Bonding
• Atomic bonding is the formation of compounds by combining two
or more elements
• In an atomic bonding electrons are gained, lost or shared
• There are 4 main types of bonding:
 Ionic bonding
 Covalent bonding
 Metallic bonding
 Van der waals
Primary Bonding
Secondary Bonding

23. Covalent Bonding
• In covalent bonding the electrons are shared between atoms
• Covalent bonds are more stable and stronger than ionic bonds
e.g; Diamond (Carbon)

24. Ionic Bonding
• Ionic bonding occurs
between + and – ions
• Requires electron transfer
between atoms forming
attracting ions
• Example: sodium chloride
(NaCl)
• Other compounds having
ionic bonding: MgO, CsCl

25. Characteristics of Ionic Bonding
• Ionic compounds are usually hard, rigid and
brittle: the results of ions being held in specific
positions

26. Metallic Bonding
◦ Valence electrons are detached from atoms, and
spread in an electron sea that glues the ions together
+ + + +
+ + + +
+ + + +

27. Secondary Bonding
-ex: Polymer (PVC)