The document discusses various engineering materials including metals, ceramics, polymers, composites, and their composition and bonding. It describes that engineering materials are used for construction and manufacturing and enable exploration of new product designs. Metals can be ferrous or non-ferrous, and ceramics are hard, brittle materials. Atoms bond through ionic bonds, covalent bonds, or metallic bonds depending on whether they involve the transfer or sharing of electrons.

2. TOPICS
• Types of Engineering Materials
• Engineering Materials Composition
• Bonding and Molecules
GROUP 1
Frigillana, Samuel
Gomez, Jazreal
Valerio, Paulo
Santos, Patrick
Bacay, Kate Cloadine
Coile, John Michael
Aquino, Mark Gil

3. What is Engineering Materials?
Materials that are used as raw material for
any sort of construction or manufacturing
in an organized way not only in the field of
engineering, but in a day to day basis
because of their properties and
characteristics.

4. What is Engineering Materials?
These materials enable people to
explore in the design and
implementation of new products to
improve the quality of our modern
life. Proper study of these materials
is necessary in order to exploit all
the great characteristics that makes
us want a better lifestyle.

5. Engineering Materials

6. Metals
A kind of engineering material made with
mostly metallic and small amount of non
metallic elements.
Can be classified as ferrous and non-
ferrous

7. Metals
Ferrous Non Ferrous
Pure
Ferrous
Metals
Ferrous
Alloys
Pure Non
Ferrous
Metals
Non
Ferrous
Alloys
Copper Alum.
Zinc Tin
Brass Bronze Solder
Lead Silver
Gold Mercury
Mercury is the only non
ferrous metal that is liquid at
room temperature.
Copper
+
Zinc
Copper
+
Tin
Lead
+
Tin
Alloying.
Iron
Steel
High
Speed
Steel
High Speed Steel
Cutting Tools

8. Ferrous Metals
Metals that consist mostly of iron and small amounts of
other elements. Ferrous metals are prone to rusting if
exposed to moisture. Ferrous metals can also be picked up
by a magnet. The rusting and magnetic properties in
ferrous metals are both down due to the iron. Typical
ferrous metals include mild steel, cast iron and steel.
Examples:
1. Mild Steel.
2. Cast Iron.
3. High Carbon Steel.
4. High Speed Steel.
5. Stainless Steel.
Rusting
Magnetism

9. Non – Ferrous Metal
Metals that do not have any iron in them at all. This means
that Non-ferrous metals are not attracted to a magnet and
they also do not rust in the same way when exposed to
moisture. Typical Non-ferrous metals include copper,
aluminum (coke cans), tin and zinc.
Examples:
1. Aluminium.
2. Copper.
3. Zinc.
4. Tin.
5. Lead.
6. Silver.
7. Gold.
8. Magnesium.
Lead
Tin
Zinc

10. Ceramics
Inorganic, nonmetallic materials that consist of metallic and
nonmetallic elements bonded together primarily by ionic and/ or
covalent bonds
Its chemical compositions vary considerably, from simple
compounds to mixtures of many complex phases bonded
together.
Ceramics used for engineering applications, can be divided into
two groups: 1) Traditional ceramic materials
2) Advanced ceramic materials
Typically hard and brittle with low toughness and ductility
Usually good electrical and thermal insulators
Normally have relatively high melting temperatures and high
chemical stability in many hostile environments

11. Ceramics

12. Glass
Glassy materials are hard, brittle, and non-
crystalline. The lack of crystalline grains often
results in optical transparency. The glass we are
used to is a ceramic usually consisting of a
mixture of silicates or sometimes borates or
phosphates formed by fusion of silica or of
oxides of boron or phosphorus with a flux and a
stabilizer into a mass that cools to a rigid
condition without crystallization.

13. Polymers
Plastics/polymers are made up of millions of
repeated links to make long molecules or
networks that are tangled or crosslinked together.
Almost all polymers use carbon atoms in very
long chains. The carbon atoms may be attached
to other carbon, oxygen, nitrogen, and hydrogen
atoms. Polymers may or may not have an orderly
arrangement of atoms.

14. Composite Materials
Composites are mixtures of two or more bonded
materials. Composites are the mixture of multiple
materials, which in combination offer superior
properties to the materials alone. Structural
composites usually refer to the use of fibers
which are embedded in a plastic. These
composites offer high strength with very little
weight.

15. Conductors
Material which contains movable electric charges
called electrons. These electric charges will
move when an electric potential difference is
applied across separate points on the material.
This flow of charge is what is meant by electric
current.

16. Insulators
Material that resists the flow of electric current.
An insulating material has atoms with tightly
bonded valence electrons. These materials are
used in parts of electrical equipment intended to
support and separate electrical conductors
without passing current through themselves.

17. Semiconductors
Material that has a resistivity value between that of a
conductor and an insulator. The conductivity of a
semiconductor material can be varied under an external
electrical field. Devices made from semiconductor
materials are the foundation of modern electronics,
including radio, computers, telephones, and many other
devices. Solar photovoltaic panels are large semiconductor
devices that directly convert light energy into electrical
energy.

18. Composition of Materials

19. Atoms
We used to say that the atom was the smallest unit of
which matter was composed and indivisible. Also, the atom
is considered as the basic structural unit of matter.
Each atom is composed of a positively charged nucleus
surrounded by a sufficient number of negatively charged
electrons so that the charges are balanced and neutrons
which carry no charge. The number of electrons identifies
the atomic number and the element of the atom.

20. Structure of an Atom
Atoms have three
basic particles:
1. Proton
2. Neutron
3. Electron
The protons and
neutrons are found
inside the nucleus.
The electrons orbit
the nucleus on
shells.
Key
Proton
Neutron
Electro
n

21. Structure of an Atom
shell
proton
neutron
electron
nucleus

22. Atoms
When the atoms have gained or lost one or more
electrons, it is called as Ions.
Losing of an electron makes the atom electropositive
since there will be a positively charged proton without
its balancing electron. Such an ion is called positive
ion.
While gaining an electron makes the atom
electronegative since there is no spare positively
charged proton in the nucleus to balance the
additional electron. Such an ion is called negative
ion.

23. Ions

24. Cations and Anions

25. Arrangement of electrons
Electrons are arranged in shells that move around the
nucleus situated in the center of the atom.
Shell (n)
1st shell 2 electrons
2nd shell 8 electrons
3rd shell 18 electrons
4th shell 32 electrons

26. Why atoms form bonds
Electrons are in energy levels around the
nucleus (electron cloud).
The higher the energy level, the more
energy is required for an electron to
occupy that part of the cloud.
The outermost part of the electron cloud
contains the valence electrons – that is
the valence shell.
Maximum number of valence electrons in
an atom is 8.

27. Bonding of atoms
When two or more atoms, either of one type or
different types of atom, are joined together
chemically, the unit which is produced is called a
molecule. This process is called chemical
bonding.

28. Chemical Bonding
A chemical bond is a lasting attraction between
atoms that enables the formation of chemical
compounds. The bond may result from the
electrostatic force of attraction between atoms
with opposite charges, or through the sharing of
electrons

29. Atoms are stable
when they have 8
valence electrons.
When the atoms
have 8 electrons, it is
called an octet.
Atoms must lose,
gain or share
electrons to attain
the octet.
 Atoms that form bonds with other atoms by sharing them
or transferring them is known as the Octet Rule.

30. There is always an exception!
Hydrogen and Helium
Hydrogen needs only
one more to fill its
valence shell.
Helium has a full
valence shell – it is
stable and does not
bond with other atoms.

31. Bond…. Chemical Bonds
Ionic Bonds
They are formed when atoms gain or
lose electrons.
If the compound has a metal, then it is
an ionic bond.
Ex.
Na Cl
x
x x
x x
x
x

32. Ionization
When atoms gain or lose an electron, they become
an ion.
A Na atom has 11 positively charged protons and
11 negatively charged electrons.
When it loses 1 electron to become more stable, it has 11
protons (+) and 10 electrons (-) and has a +1 charge.
Cl has 17 protons.
When Cl gains 1 electron to complete the octet, it has 17
protons (+) and 18 electrons (-).
It is now an ion with a –1 charge.

33. Opposites Attract
Since the Na has a + charge and the Cl has a –
charge, the two atoms are attracted together and
form an ionic bond.
They have a 1:1 ratio when they combine…..

34. Covalent Bonds
Atoms that share electrons form covalent bonds.
If the atoms have a covalent bond and are the same
type of atom…. They are diatomic molecules.
Ex.
Cl Cl
x
x x
x x
x
x
x
x x
x x
x
x

35. Element Bonding Formula
Hydrogen H-H H2
Oxygen O-O O2
Nitrogen N-N N2
Fluorine F-F F2
Chlorine Cl-Cl Cl2
Bromine Br-Br Br2
Iodine I-I I2

36. Hydrogen Bonds
A hydrogen bond is the attractive force
between the hydrogen attached to an
electronegative atom of one molecule and
an electronegative atom of a different
molecule.
Usually the electronegative atom is
oxygen, nitrogen, or fluorine, which has a
partial negative charge.

37. Example of Hydrogen Bond
Each hydrogen atom is covalently bonded to the oxygen
via a shared pair of electrons. Oxygen also has two
unshared pairs of electrons. Thus there are 4 pairs of
electrons surrounding the oxygen atom, two pairs involved
in covalent bonds with hydrogen, and two unshared pairs
on the opposite side of the oxygen atom. Oxygen is an
"electronegative“ atom compared with hydrogen.

38. Metallic Bonds
Metallic bonding is the type of bonding found
in metallic elements. This is the electrostatic
force of attraction between positively charged
ions and delocalized outer electrons.
Metallic bonding refers to the interaction
between the delocalized electrons and the
metal nuclei.

39. Example of Metallic Bond
As the metal cations and the electrons are oppositely
charged, they will be attracted to each other, and also to
other metal cations. These electrostatic forces are called
metallic bonds, and these are what hold the particles
together in metals.

40. So you ask…. “How do I know if it is
covalent or ionic?”
Ionic bonds are formed by the attraction of
two oppositely charged particles.
Covalent bonds are formed when atoms
share electrons.
Typically bonds between metals and
nonmetals form ionic bonds.
Bonds between two nonmetals form covalent
bonds.

41. THANK YOU!

42. Q&A
TOPICS:
1. Types of Engineering Materials
2. Engineering Materials
Composition
3. Bonding and Molecules

43. 1. What is the main tittle of the report?
2. Describe the word Engineering materials.
3-5. Give at least 3 Engineering materials.(3pts)
6.What kind of Engineering material is metal?
7. Metal can be classified as ?
8. The materials are hard, brittle, and non-
crystalline. The lack of crystalline grains often results
in optical transparency is called?
9. It is made up of millions of repeated links to make
long molecules or networks that are tangled or
crosslinked together is called?

44. 10.The three basic components of an atom are:
A. protons, neutrons, and ions B. protons, neutrons, and electrons
B. C. protons, neutrinos, and ions
11. A single proton has what electrical charge?
A. no charge B. positive charge C. negative charge
12.What is a chemical bond that involves sharing a pair of electrons
between atoms in a molecule?
A. A cation B. An ion C. A covalent bond D. An ionic bond
13. A chemical bond in which one atom loses an electron to form a
positive ion and the other atom gains an electron to form a negative ion is
a (an)
A. Ionic bond B. Cation C. Covalent bond D. Sigma bond

45. 14. What is the basis of hydrogen bond?
A. Attraction forces between hydrogen atom bonded with another
hydrogen atom
B. Attraction forces between hydrogen atom bonded with a high
electronegativity atom (F, O, N)
C. Attraction forces between hydrogen atom bonded with a high
electronegativity atom (F, O, N) with atom (F, O, N) of another molecule
D. Attraction forces between hydrogen atom with another hydrogen atom
of another molecule
15. Metallic bonding is...
A. a type of covalent bond.
B. a type of ionic bond.
C. an attraction between positive and negative ions.
D. an attraction between positive ions and electrons.

46. 16. The Maximum Number Of Valence Electron In An Atom?
A.12 B.3 C.8 D.5
17. Material Which Contains Movable Electric Charges Called Electrons..
A. Polymers B. Conductors C. Glass D. Electric Wire
18. Typically A Hard And Brittle With Low Toughness And Ductility..
A. Polymer B. Glass C.Ceramics D. Wood
19. This Material Which Use In Some Building, Establishment, Warehouse,
Kitchenware, Homeware And It's Too Fragile.
. A.Glass B.Bricks C.Metal D. Wood
20. The Arise In A Molecule Compromised Of Two Atoms With Equal And Opposite
Electrical Charge.
A.Positive Charg B.Electric Charge C.Dipole Forces. D. Forces
21-23. Give the Atoms three basic particles (3pts)
24-25.Explain and discuss chemical bond?

47. ANSWER KEYS
1. NATURE OF MATERIALS
2. MATERIALS THAT ARE USED AS RAW MATERIAL FOR ANY SORT OF CONSTRUCTION OR MANUFACTURING IN
THE FIELD OF ENGINEERING AND IN A DAY TO DAY BASIS.
3-5. METAL, PLASTIC, CERAMIC, COMPOSITION
6. A KIND OF ENGINEERING MATERIAL MADE WITH MOSTLY METALLIC AND SMALL AMOUNT OF NON METALLIC
ELEMENTS.
7. FERROUS AND NON-FERROUS
8. GLASS
9. POLYMERS
10.B 16.C 24-25.
11.B 17.B
12.C 18.C
13.A 19.A
14.C 20.C
15.D 21-23. PROTON, NEUTRON, ELECTRON