1. MATTER; CHAPTER 3
Elements, Compounds, Mixtures

2. DEMO…
Place a black dot on the line drawn in
pencil on your filter paper and place it in
the beaker that has some water in the
bottom.
Make sure the dot is not under water.
Watch as we take notes. What do you
see?

3. ALL matter can be classified into 1 of 3
groups:
Elements
Compounds
Mixtures

4. ELEMENTS:
Simplest Pure substance
Made of ONE type of atom
Unique properties to identify
92 naturally occurring
Organized on Periodic table
with chemical symbols
3 main types…

6.  Could you identify these elements by their density?
 Could you identify these elements by their conductivity?
 Could you identify these elements by their reactivity to
oxygen?
 Could you identify these elements by their melting point?
Cobalt Iron Nickel
Melting Point: 1,495 oC 1,535 oC 1,455 oC
Density: 8.9 g/cm3 7.9 g/cm3 8.9 g/cm3
Conductivity Electric
and thermal
energy
Electric
and thermal
energy
Electric
and thermal
energy
Reactivity
oxygen
Unreactive Slowly forms
rust
Unreactive

7. So…..
 Can you identify elements by 1
property? Why or why not?
Cobalt Iron Nickel
Melting Point: 1,495 oC 1,535 oC 1,455 oC
Density: 8.9 g/cm3 7.9 g/cm3 8.9 g/cm3
Conductivity Electric
and thermal
energy
Electric
and thermal
energy
Electric
and thermal
energy
Reactivity
oxygen
Unreactive Slowly forms
rust
Unreactive

8. 1. Metals:
Shiny; good conductors, malleable,
ductile

9. 2. Nonmetals:
Dull; poor conductors, brittle

10. 3. Metalloids:
Semiconductors; Properties of both metals
and nonmetals

11. 1. What is an element?
2. Create a word web that shows
connections between the following:
Elements
Metals
Metalloids
Nonmetals
3. Describe these connections

12. Elements
Metalloids
NonmetalsMetals

13. Math and Science…
The human body is made of the following
elements:
Oxygen; 64.6%
Carbon; 18.0%
Hydrogen; 10.0%
Nitrogen; 3.1%
Calcium; 1.9%
Phosphorous; 1.1%
Other; 1.3%
This type of data would best be displayed using
______________ graph.
Create one.

14. Math and Science…
Percentages of Elements in the Human
Body
65%
18%
10%
3%
2%
1%
1%
Oxygen
Carbon
Hydrogen
Nitrogen
Calcium
Phosphorous
Other

15. HOW SMALL IS AN ATOM?
(Don’t memorize these numbers!)
An aluminum atom has a diameter of about
______________cm.
A A piece of aluminum foil is about
_________________atoms thick.
0.00000003
50,000

16. WHAT’S INSIDE AN ATOM?
Particle Charge Location Mass
Proton
Neutron
Electron
Positive
Neutral
(0)
Negligible
1/1836 amu
Electron
Clouds
Nucleus 1 amu
1 amuNucleus
Negative
Copy this chart in your notes and use pages 87-91 to fill it in.

17. ATOMS AND THE PERIODIC TABLE
Use the periodic table on page 158 to find sulfur and
copy its square exactly in your notes.
Use the key on page 158 to label each of the four
pieces of information found in this square.
16
S
Sulfur
32.1
Atomic Number
Chemical Symbol
Element Name
Atomic Mass

18. 1. Describe the 3 “classes” that
elements can be grouped into?
2. What is the smallest part of an
element?

19. HOW ARE ELEMENTS DIFFERENT?
Look at all of the different kinds of elements on
the periodic table.
If all protons are identical, all neutrons are
identical, and all electrons are identical, how do
we have such a variety of atoms?
It depends on the _______________________!PROTON NUMBER

20. 1. What is an element?
2.What is a compound?
3.How are elements and compounds
similar? Different?

21. THE NUMBER RULES!
All elements have a model that can be drawn to
show how their Protons, Neutrons, and Electrons
are arranged. Look at Nitrogen shown below:
7p+
7n
7e-

22. COMPOUNDS:
2 + elements chemically combined
Elements react with each other
Most substances on Earth
Different properties than original
elements

23. Molecules with more than 1 type of
atom
Chemical formulas
CH4
H2O
CH4

24. ???
 What is happening to the magnesium ribbon?

25. EX:
Magnesium + Oxygen  Magnesium Oxide

26. BOHR MODELS…
Represent compounds
Ex: H2O (water)
1 P
0 N
1 P
0 N
8 P
8 N

27. Can be separated by chemical
reactions

28. Flame Tests
Copy the chart in your notes:
Compound Flame Color
Calcium chloride
Potassium chloride
Sodium chloride
Barium chloride
Lithium chloride
Strontium chloride
Copper chloride

29. Flame Tests
 Is this a chemical or a physical change? Why?
 Do you think the flame colors are caused by the
chloride or the metals? Why?
 What color do you think sodium fluoride would
have? Why?

30. Warm up
1. What is happening to the
compounds in the soda?
2. What is a compound?
3. List 3 examples of compounds you
are familiar with.

31. Electrolysis…
Uses electric current
Separates water into H and O
Used to obtain aluminum, copper,
peroxide

32. Electrolysis…
Was this a chemical or physical
change? How do you know?
What type of matter is water
(element, compound, mixture) ?

33. 1. How are compounds and elements
alike?
2. How are compounds and elements
different?
3. What are 2 ways to break down a
compound?

34. MIXTURES:
2 + substances;
NOT chemically combined
NO chemical change
Identities of parts DO NOT
change
Physically separate parts

35. TYPES…
Homogeneous: looks like one
substance
Heterogeneous: different
substances visible

36. H2O
water
NaCl
salt

37. The Liberty Bell is a mixture of:
70% copper
25% tin
Small amounts of lead, zinc, arsenic, gold &
silver

38. Demo…
Look at the mixture at your
desk and figure out which one
you have.
See if the substance is
homogeneous or
heterogeneous.
Complete your chart. Share
your data with the class.

39. Mixture
ID
Mixture Homogeneous or
Heterogeneous?
How To
Separate?
A
B
C
D
E
F
G
H
I

40. Mixture Names
Sand and iron filings
Saltwater
Nuts and bolts
Soft drink (gas in liquid)
Saltwater and sand
Air
Coffee grounds and water
Blood
Steel (C + other elements
in iron)

41. 1. Describe your observations of the
flame tests. Was this chemical or
physical change?
2.Describe your observations of the
electrolysis experiment? Was this
chemical or physical change?

42. 1. Compare and contrast compounds
and mixtures.
2.What is the difference between
homogeneous and heterogeneous
mixtures?

43. SOLUTIONS:
Looks like 1 substance
Really 2 + substances
evenly distributed
Read page 76 in your textbook. Why is
perfume a solution?

44. Demo…
What do you notice about
the different beakers of
colored water?
How would you describe
them?

45. Solute: substance that is
dissolved
Solvent: substance that does
the dissolving
Water is the Universal Solvent

46. WARM UP
Retrieve your paper slip with the
marker streak. We completed these
a few days back.
1. Discuss and list some
QUALITATIVE observations
about this paper.
2. What type of substance was the
marker? (element, compound,
mixture, etc.)
3. Use your science terms to
support your answer to number
2.

47. EXTENSION
Chromatography
Can be used for many things…
Forensic analysis
Determine Unknown chemicals

48. A TASTY SOLUTION…
Group Members 1 & 4: allow the
candy to completely dissolve
without any help
Group Member 2: Allow the candy to
dissolve with only your tongue
moving it around
Group Member 3: Allow the candy to
dissolve with both tongue and teeth
***All members record time for shell
to dissolve

49. A TASTY SOLUTION…
In your solutions…
1. What was the solvent?
2. What was the solute?
3. What was the difference in
dissolving rate for the different
members?
4. What things can be done to
change the dissolving rate of a
substance?

50. Solubility is how much can
dissolve
Changes with conditions
Amount of solute is called
concentration

51. Solubility of various substances at increasing
temperatures
1. What is the independent variable? The dependent?
2. Which substance is more soluble at lower temps than at higher?
3. Which substance does not change its solubility much?

52. Why does a can of soda
get “flat” when it sits open
at room temperature?
When Temp Solubility of gas

53. Why can Mrs. Lock
dissolve more ice tea mix
when she boils the water
first?
When Temp Solubility of solids

54. SUSPENSIONS:
A mixture;
Particles are dispersed and
visible but may settle out
Can be separated by
filtration

55. WARM UP
1. Why are suspensions
considered mixtures?
2. Why is a snow globe a
good example of a
suspension?

56. WARM UP
1. What are the properties
of a solution?
2. What are the properties
of a suspension?

57. COLLOIDS:
Properties of solutions and
suspensions
Small particles
Mixed well; don’t settle out;
scatter light
Can’t be separated by filtration
Types of mixtures…

58. Demo…
Is this a colloid?
Why?

59. Why is this a colloid?

60. Why is this a colloid?

61. Type
Homogeneous or
Heterogeneous
1. Oil and water
2. Chicken broth
3. Milk
4. Granite (rock)
5. Soda (gas in liquid)
6. Salt water
7. Raisin bran
8. Toothpaste
9. Sand and water
10. Oil and vinegar
11. Mayonnaise
12. Kibble and Bits
Solution, Colloid, Suspension

62. WARM UP…
1. Take out your textbook
and uncover it
2. Clean any papers out of
the book-recycle them!
3. Get out a PENCIL for the
test