The document discusses the key properties and states of matter. It defines matter as anything that has mass and takes up space, and identifies three common states of matter - solids, liquids, and gases. It distinguishes between physical and chemical properties, and physical and chemical changes. The document also covers mixtures and solutions, the conservation of mass, and provides an example problem calculating the mass of a product in a chemical reaction.

1. Properties of Matter
Ch. 2

2. Quick Review
 Matter is anything that: a) has mass, and b) takes up
space
 Mass = a measure of the amount of ―stuff‖ (or material)
the object contains (don’t confuse this with weight, a
measure of gravity)
 Volume = a measure of the space occupied by the object

3. States of Matter
1) Solid- matter that can not flow (definite shape) and
has definite volume.
2) Liquid- definite volume but takes the shape of its
container (flows).
3) Gas- a substance without definite volume or shape
and can flow.
 Vapor- a substance that is currently a gas, but normally
is a liquid or solid at room temperature. (Which is
correct: ―water gas‖, or ―water vapor‖?)
4) Plasma- Ionized gas that contains positive ions and
electrons

4. Drawing the States of Matter
Solid Liquid Gas

5. States of Matter
Solid
Liquid
Gas
Definite
Volume?
YES
YES
NO
Definite
Shape?
YES
NO
NO
Result of a
Temperature
Increase?
Small
Expansion
Small
Expansion
Large
Expansion
Will it
Compress?
NO
NO
YES

6. The 6 Phase Changes
1.Melting: Solid to Liquid
2.Freezing: Liquid to Solid
3.Evaporation: Liquid to Gas
4.Condensation: Gas to Liquid
5.Sublimation: Solid to Gas
6.Deposition: Gas to Solid

7. Describing Matter
Properties used to describe matter can be
classified as:
1) Extensive – depends on the amount
of matter in the sample
- Mass, volume, calories are examples
2) Intensive – depends on the type of
matter, not the amount present
- Hardness, Boiling Point

8. Is Density Intensive or
Extensive?


9. Properties
Words that describe matter
(adjectives)
Physical Properties- a property that
can be observed and measured
without changing the material’s
composition.
Examples- color, hardness, m.p.,
b.p.

10. Properties
Chemical Properties- a property that
can only be observed by changing
the composition of the material.
Examples- ability to burn,
decompose, ferment, react with,
etc.

11. Physical Change
Physical change will change the visible
appearance, without changing the
composition of the material.
Can be reversible, or irreversible
Boil, melt, cut, bend, split, crack
Is boiled water still water?
***ALL 6 PHASE CHANGES ARE
PHYSICAL CHANGES!***

12. Chemical Change
Chemical Change - a change where
a new form of matter is made.
Rust, burn, decompose, ferment

13. Signs of a Chemical Change
1.Gas production
2.Precipitate formation
3.Energy production (light, sound)
4.Change in Temperature
5.Change in color
6.Change in chemical or physical property

14. Chemical vs. Physical Change
Ask yourself: Is anything new being
made?

15. 3 Types of Matter
1. Elements
2. Compounds
3. Mixtures
a. Heterogeneous
b. Homogeneous (Solutions)

16. Pure Substances
 Pure substances can be either
 Elements
 Compounds

17. 1. Elements
Simplest kind of matter
Cannot be broken down any
simpler and still have properties
of that element!
All one kind of atom.
Atoms– the smallest particle or
unit of an element that has the
properties of that element.

18. 2. Compounds
Substances that can be broken
down only by chemical methods
When broken down, the pieces
have completely different
properties than the original
compound.
Made of two or more atoms,
chemically combined (not just a
physical blend!)

19. 3. Mixtures
 Mixtures are a physical blend
of at least two substances;
have variable composition.
 Every part keeps it’s own
properties.
 They can be either:

20. 3. Mixtures (cont.)
1) Heterogeneous – the
mixture is not uniform in
composition
Ex. Chocolate chip cookie, gravel,
soil.

21. 3. Mixtures (cont.)
2) Homogeneous - same
composition throughout;
called ―solutions‖
• Kool-aid, air, salt water

22. More on Homogenous (solutions)
 Mixed molecule by molecule, thus too small to see the
different parts
 Can occur between any state of matter: gas in gas;
liquid in gas; gas in liquid; solid in liquid; solid in solid
(alloys), etc.
 Most common solutions consist of 1 or more substances
dissolved (the dissolved ―stuff‖ is called the solute) in a
liquid (called the solvent)
 If the solvent is water—aqueous solution
 A true solution will never separate or settle out on its
own.

23. Ways of Separating Mixtures
 Differences in physical properties can be used to
separate mixtures.
1) Filtration - separates a solid from the liquid in a
heterogeneous mixture (by size)
2) Distillation – separates a solution by boiling points
There are other ways as well: magnets, evporation
chromotography

24. Law of Conservation of
Mass/Matter

25. During any chemical reaction, the
mass of the products (right side of
arrow) is always equal to the mass of
the reactants (left side of arrow).
All the mass can be accounted
for:
Burning of wood results in products that
appear to have less mass as ashes;
where is the rest?

26. Example Problem
When methane gas burns, and reacts and
combines with oxygen to produce carbon
dioxide and water vapor. If 4 grams of
methane reacts with 16 grams of oxygen to
produce 11 grams of carbon dioxide, how
much water vapor is produced?