1. The document discusses classifying matter and describes the differences between elements, compounds, mixtures and pure substances. 2. It explains that elements are the simplest substances that cannot be broken down further, while compounds are formed by combining two or more elements. 3. Mixtures contain combinations of substances that are not chemically bonded, and can be separated using physical properties, whereas compounds require chemical changes to separate.

1. TO GET YOU THINKING…
If you were asked to describe a grapefruit to
someone who had never seen one, what would
you tell the person?

2. MATTER Senior Science

3. SECTION 1: CLASSIFYING MATTER
Today, there are rules for how a newly discovered element is to be named. In earlier times,
elements were named for people, places, and foreign words, among other things. Match
each element to how it was named. You may also use an element’s symbol as a clue.
___ Berkelium (Bk) a. Noble Prize winner who studied relativity
___ Curium (Cm) b. Latin name (ferrum)
___ Einsteinium (Es) c. powerful mythological beings
___ Gold (Au) d. home of California university where element was first made
___ Krypton (Kr) e. Greek word for violet (iodes)
___ Iron (Fe) f. Nobel Prize winner who studied radioactive elements
___ Iodine (I) g. Greek word for hidden (kryptos)
___ Titanium h. Latin name (aurum)

4. SECTION 1: CLASSIFYING MATTER
By the end of this section, you should be able to:
 Identify six examples of physical properties of matter.
 Explain what happens to matter during a physical change.

5. WHAT IS MATTER?
 Matter is anything that has mass and takes up space.
 Every sample of matter in the universe is either an element, a
compound, or a mixture.

6. ELEMENTS, THE SIMPLEST SUBSTANCES
An element is a pure substance that cannot be separated into
simpler substances by physical or chemical means.
A substance in which there is only one type of particle is a pure
substance. Elements are made of particles called atoms.

8. ELEMENTS, THE SIMPLEST SUBSTANCES
Each element is represented by a 1 or 2 letter symbol that is
used worldwide.
Atoms can be made up of millions of molecules.
Molecules are the smallest unit of a substance that can exist by
itself and retain all of a substance’s chemical properties.

9. COMPOUNDS
A compound is a substance made up of atoms of 2 or more
elements joined together by chemical bonds.
Compounds have unique properties.

11. COMPOUNDS
Chemical formulas represent compounds.

13. PURE SUBSTANCES AND MIXTURES
 Elements and compounds are pure substances, but mixtures are
not.
 A pure substance is a sample of matter, either a single element
or a single compound, that has definite chemical and physical
properties.
 Mixtures are combinations of two or more substances that are
not chemically combined.

14. PURE SUBSTANCES AND MIXTURES
Mixtures are classified by how thoroughly the substances mix.
heterogeneous mixture: substances aren’t mixed uniformly and are
not evenly distributed
homogeneous mixture: substances are evenly distributed, and the
mixture is the same throughout
miscible: substances that can be mixed
immiscible: substances that cannot be mixed

17. SECTION 1 REVIEW ?S
p.50 #2-7

18. TO GET YOU THINKING…
Physical properties are often used to separate a mixture into its
original components. Imagine that you have been given a mixture
of sand, sugar, and iron filings. You know that iron is attracted to
a magnet, sugar dissolves in water and sand does not, and sugar
has a higher boiling point than water.
1. What do you separate in the first step? How?
2. What is separated out in the second step? How?
3. What happens in the third step?

19. PHYSICAL PROPERTIES
 A physical property of matter can be observed or measured
without changing the matter’s identity.

20. PHYSICAL PROPERTIES
 You use physical properties to identify matter. They can be
observed or measured.
 Ex: shape, color, odor, texture, state, strength, hardness,
magnetism, ability to conduct electricity or heat

22. PHYSICAL PROPERTIES
 The temperature and pressure at which a solid becomes a liquid
is called the melting point.
 The temperature and pressure at which a liquid becomes a gas
is called the boiling point.

24. PHYSICAL PROPERTIES
 Density is the amount of matter in a given space, or volume.
 Density =
mass
volume
 The most common units are g/cm3
or g/mL.
 Density is different than weight.

25. DENSITY PRACTICE PROBLEMS
p.54 #1-3

26. CHEMICAL PROPERTIES
 Chemical properties describe matter based on its ability to
change into new matter that has different properties.
 Flammability and reactivity are two chemical properties.

27. PHYSICAL VS CHEMICAL PROPERTIES
 Physical and chemical properties are different.
 Physical properties can be observed without changing the
identity of a substance.
 Chemical properties can be observed only in situations in which
the identity of the substance changes.

28.  The properties that are most useful in identifying a substance
are characteristic properties. These properties are always the
same no matter the size of the sample. They can be chemical or
physical properties.

29. SECTION 2 REVIEW ?S
p.58 #2, 4-7

30. TO GET YOU THINKING…
For each step involved in making bread, decide whether a physical or a
chemical change occurs, or whether a mixture or compound is formed.
a. stir flour and dry oatmeal mixture formed compound formed
b. heat the water physical change chemical change
c. melt the shortening physical change chemical change
d. beat the eggs physical change chemical change
e. blend molasses with water mixture formed compound formed
f. bake the bread physical change chemical change

31. SECTION 3: CHANGES OF MATTER
By the end of this section, you should be able to:
 Explain what happens during a chemical change.
 Distinguish between physical and chemical changes.

32. PHYSICAL CHANGES
 Physical changes do not change the identity of the matter
involved.
 Changing the size or state of matter are physical changes.

33. CHEMICAL CHANGES & NEW SUBSTANCES
 During a chemical change a substance changes chemical
properties.
 Some common signs of chemical changes includes a change in
color, odor, production of heat/light/sound, and fizzing.
 Chemical changes change the identity of the matter involved.

35. PHYSICAL VS. CHEMICAL CHANGES
 Physical changes do not change the composition of a substance
while chemical changes do.
 Many physical changes are easily reversed, but most chemical
changes cannot easily be reversed.

36. MIXTURES VS COMPOUNDS
 Mixtures can be separated by physical changes, but compounds must
be broken down by chemical changes.
Examples of separating a mixture:
Separating saltwater into its parts by heating it: When the water
evaporates, the salt remains.
Using a distillation device to heat a mixture whose components have
different boiling points: The component that boils and evaporates
first separates from the mixture.
Using a centrifuge: The mixture spins rapidly until the components
separate.

37. MIXTURES VS COMPOUNDS
 Some compounds can be broken down through chemical changes.
Examples of separating a compound:
When mercury(II) oxide is heated, it breaks down into the elements
mercury and oxygen.
When a current is passed through melted table salt, the elements
sodium and chlorine are produced.
When you open a bottle of soda, carbonic acid in the soda breaks
down into carbon dioxide and water.

38. SECTION 3 ?S
p.64 #3-7

39. CHAPTER REVIEW QUESTIONS
p.70-71 #1-21, 24-27