1. Review!

2. State
Solid
Liquid
Gas
Volume
Shape
Packing of
particles
Particle
mobility

3. State
Solid
Liquid
Gas
Volume
definite
indefinite
Shape
Packing of
particles
Particle
mobility

4. State
Solid
Liquid
Gas
Volume
definite
indefinite
Shape
Packing of
particles
Particle
mobility

5. State
Solid
Liquid
Gas
Volume
definite
indefinite
Shape
Packing of
particles
tight
in-between
loose
Particle
mobility

6. State
Solid
Liquid
Gas
Volume
definite
indefinite
Shape
Packing of
particles
tight
in-between
loose
Particle
mobility
least
most

8. Free Write
What is a material?
List 5 examples of materials

9. Material Webster’s Definition: “Solid Stuff”
The elements or substance or the parts of which something is composed or can be made
“Solid Stuff”

10. Free Write Material Categories
List anything and everything you know about the following categories:
Metal
Ceramic
Polymer
Composite
Definition, description, properties, examples, uses, etc……

11. Materials I.D. Lab Pick one item from the collection
Be ready to classify it into one of the categories and give your reason

12. Metals Malleable - easily shaped by forming Optically reflective
Excellent conductors of electricity & heat
Crystalline structure
Metallic Bonding

13. Ceramics Non-metallic material normally prepared by heating a powder
Highly crystalline

14. Glass
Hard
Brittle
Non-crystalline (amorphous)
Ionic bonding

15. Polymers
Repeated links of hydrogen & carbon that make long molecules or networks that are tangled or cross-linked together
Mainly plastics and rubber
Covalent bonding

16. Composites
Mixtures of two or more bonded materials

17. Ideal Materials Endless and readily available source of supply
Cheap to refine and produce
Energy efficient
Strong, stiff, and dimensionally stable at all temperatures
Lightweight
Corrosion resistant
No harmful effects on the environment or people
Biodegradable
Numerous secondary uses

18. History and Materials Stone Age Bronze Age Iron Age
What age are we in now??????

19. Stuff – The Materials the World is Made of by Ivan Amato

20. Atomic Structure and the Periodic Table

21. Atoms
smallest particle of an element that has the properties of the element
made of 3 basic subatomic particles
there are now many more subatomic particles – theoretical physics

22. Subatomic Particles Name Protons (p or +) Neutrons (n) Electrons (e-)
Charge
Location
Mass
“Job”
Number

23. Subatomic Particles Charge +1 No charge -1 Protons (p or +)
Name
Protons (p or +)
Neutrons (n)
Electrons (e-)
Charge +1
No charge -1
Location
Mass
“Job”
Number

24. Subatomic Particles Location in nucleus in shells around nucleus
Name
Protons (p or +)
Neutrons (n)
Electrons (e-)
Charge +1
No charge -1
Location
in nucleus
in shells
around nucleus
Mass
“Job”
Number

25. nucleus small, dense center of atom
contains almost all the mass of the atom
contains protons and neutrons

27. in shells around nucleus
Subatomic Particles
Name
Protons (p or +)
Neutrons (n)
Electrons (e-)
Charge +1
No charge -1
Location
in nucleus
in shells around nucleus
Mass
≈ 1 amu
≈ 2000x smaller
“Job”
Number

28. Atomic Mass Unit (amu)
metric unit to measure the mass of VERY small objects (particles)
a unit to measure the mass of atoms
Just like we have light years for measuring very large distances

29. in shells around nucleus
Subatomic Particles
Name
Protons (p or +)
Neutrons (n)
Electrons (e-)
Charge +1
No charge -1
Location
in nucleus
in shells around nucleus
Mass
≈ 1 amu
≈ 2000 x smaller
“Job”
Determines
identity of
element
Supplies proper
mass to hold
nucleus together
bonding/
how it reacts
Number

30. Subatomic Particles Number Atomic # Atomic mass – atomic # =
Name
Protons (p or +)
Neutrons (n)
Electrons (e-)
Charge +1
No charge -1
Location
in nucleus
in shells around nucleus
Mass
≈ 1 amu
≈ 2000 x smaller
“Job”
Determines identity of element
Supplies proper mass to hold nucleus together
Determines bonding/ how it reacts
Number
Atomic #
Atomic mass – atomic # =
# of neutrons
Same as # of protons

31. # of protons atomic number whole number on periodic table
number of protons in an atom of an element
does NOT vary in an element – the same in all atoms of an element
Use the flexcam and a copy of the periodic tables they have in their notebooks to show them the location of the atomic number and atomic mass.
Try several examples.

32. # of electrons atoms are neutral (+) = (-)
# of protons = # of electrons
p = e-
Do several examples.

33. atomic mass (weight)
decimal number on the periodic table – it is for all the atoms of the element
number of protons plus the number of neutrons – it’s an average on the table
weighted average of all the isotopes of that element
the mass of one atom is a whole number
use the average weight of students analogy (all girls = 100 lbs, all boys = 200 lbs. – same # of girls and boys – more girls than boys)

34. Isotopes
iso = same
atoms of the same element with different numbers of neutrons
have different atomic masses but the same atomic number
some are stable, some are radioactive (carbon-12 and carbon-14)

36. # of neutrons atomic mass n + p - atomic # - p # of neutrons n
Work some sample problems on how to determine the # of protons, electrons, and neutrons in an atom of an element. Let the students choose the elements.

37.
Info on all the elements

39. Periodic Table rows How is the periodic table arranged?
arranged by increasing atomic number
rows
called periods
tells number of electron shells
number them down the left side of the periodic table – 1 through 7
discuss the history of the periodic table briefly.
Use the overhead to show them how to mark/label the rows.

40.
Periodic table lesson plans

41. Periodic Table columns called families or groups
elements in same column have similar chemical properties
same number of valence electrons

42. Periodic Table valence electrons electrons in outermost shell
involved in bonding
number the columns on your periodic table with the correct number of valence electrons
Use the overhead to show them how to mark/label the columns.

45. Element one kind of atom basic building blocks on periodic table
make up everything
over 100
represented by symbols
examples:
gold (Au)
sulfur (S)
zinc (Zn)
chlorine (Cl)

46. Compound 2 or more elements chemically combined
properties different from elements making it up
elements combine in definite ratios
represented by formulas
examples:
water – H2O
salt – NaCl
carbon dioxide – CO2

47. Mixture 2 or more substances physically combined
components can retain some of their properties
mixed in any ratio
no formula
examples:
salt water
bronze
kool-aid
fruit jello
brass

48. Metals
Ceramics/
glass
Polymers
Type of matter
Type of elements
Type of structure
Type of bonding

49. Metals Ceramics/ glass Polymers Type of matter Type of elements
element or mixture
compound OR mixture of compounds
mostly compounds
Type of elements
Type of structure
Type of bonding

50. Metals Ceramics/ glass Polymers Type of matter Type of elements
element or mixture
compound OR mixture of compounds
mostly compounds
Type of elements
metallic elements
metals with nonmetals OR semimetals with nonmetals
nonmetals
Type of structure
Type of bonding

51. Metals Ceramics/ glass Polymers Type of matter Type of elements
element or mixture
compound OR mixture of compounds
mostly compounds
Type of elements
metallic elements
metals with nonmetals OR semimetals with nonmetals
nonmetals
Type of structure
crystalline
ceramics = crystalline
glass = amorphous
mostly amorphous with some regions of crystallinity
Type of bonding

52. Metals Ceramics/ glass Polymers Type of matter Type of elements
element or mixture
Compound OR mixture of compounds
mostly compounds
Type of elements
metallic elements
metals with nonmetals OR semimetals with nonmetals
nonmetals
Type of structure
crystalline
ceramics = crystalline
glass = amorphous
mostly amorphous with some regions of crystallinity
Type of bonding
metallic
bonding
ionic bonding and network covalent bonding
covalent bonding and weak intermolecular forces

53. Metals 1 to 3 valence electrons givers of electrons lose electrons
make (+) ions
left side of periodic table

54. Nonmetals 5 to 8 valence electrons takers of electrons gain electrons
make (-) ions
right side of periodic table

55. Ion atom with a charge atom has gained or lost electrons
gained e- = (-) charge
lost e- = (+) charge
(+) ion = cation
(-) ion = anion

56. Bonding
atoms achieve a stable number of electrons (ionic and covalent)
involves valence electrons
make compounds and/or solids
fill out types of bonding chart using overhead
show overhead of metallic bonding
draw examples of ionic bonding – use skeletal models - MgO, NaCl, CaCl2, K2S
draw examples of covalent bonding – use skeletal models – CO2, H2O, O2

57. Metallic Bonding
All pure metals have metallic bonding & therefore exist as metallic structures. 
Metallic bonding consists of a regular arrangement of cations surrounded by a mobile sea of electrons.

59. Metallic Bonding
Each atom donates its valence electrons to the “whole”
Atom becomes a cation because it gave away its negative particles
Donated electrons form an electron cloud
Electron cloud binds all the cations together

60. Metallic Bonding
Valence electrons are shared by all atoms in the material
Electrons are free to drift throughout the material
Provides unique properties only found in metals
shiny metallic luster
good electrical and thermal conductivity
many others ...

61. Metallic Bonds: Mellow dogs with plenty of bones to go around
These bonds are best imagined as a room full of puppies who have plenty of bones to go around and are not possessive of any one particular bone.  This allows the electrons to move through the substance with little restriction. 

62. http://www. matsceng. ohio-state

63. Ionic Bonding

65. Sodium lets Chlorine use its valance electron

66. http://www. matsceng. ohio-state

67. http://www. matsceng. ohio-state

68. Ionic Bonds: One big greedy thief dog!
Ionic bonding can be best imagined as one big greedy
dog stealing the other dog's bone.  If the bone
represents the electron that is up for grabs, then when
the big dog gains an electron he becomes negatively
charged and the little dog who lost the electron
becomes positively charged. 
The two ions (that's where
the name ionic comes from)
are attracted very strongly
to each other as a result of
the opposite charges.

69. Covalent Bonding

71. http://www. matsceng. ohio-state

73. Covalent Bonds: Dogs of equal strength.
Covalent bonds can be thought of as two or more dogs
with equal attraction to the bones.  Since the dogs
(atoms) are identical, then the dogs share the pairs of
available bones evenly.  Since one dog does not have
more of the bone than the other dog, the charge is
evenly distributed among
both dogs.  The molecule
is not“ polar" meaning one
side does not have more
charge than the other.

74. Covalent Network Solid
REMEMBER THIS FOR POLYMERS
only covalent bonds
extremely large molecules or networks
usually have at least one element from carbon family
very strong and hard
very high melt T°
some glass and ceramics, diamond
polymers are usually not because they make linear chains instead of networks

75. Surprise!