1. I. States of Matter Kinetic Energy States of Matter
Ch. 1 - Matter
I. States of Matter
Kinetic Energy
States of Matter

2. A. Kinetic Energy Particles of matter are always in motion.
The kinetic energy (speed) of these particles increases as temperature increases.

3. B. Four States of Matter Solids
very low KE - particles vibrate but can’t move around
fixed shape
fixed volume

4. B. Four States of Matter Liquids
low KE - particles can move around but are still close together
Variable shape
fixed volume

5. B. Four States of Matter Gases
high KE - particles can separate and move to fill the container
variable shape
variable volume

6. B. Four States of Matter Plasma
very high KE - particles collide with enough energy to break into charged particles (+/-)
gas-like, variable shape & volume
stars

7. I. Matter Flowchart Pure Substances Mixtures
Ch. 1 - Matter
I. Matter Flowchart
Pure Substances
Mixtures

8. Can it be physically separated?
A. Matter Flowchart
MATTER
yes no
Can it be physically separated?
MIXTURE
PURE SUBSTANCE
Is the composition uniform? no
yes
Can it be chemically decomposed? no
yes
Homogeneous Mixture
(solution)
Heterogeneous Mixture
Compound
Element
Colloids
Suspensions

9. A. Matter Flowchart Example: Pure substance or Mixture
Type of Pure substance or Type of mixture
1. Graphite (carbon)
2. Pepper
3. Sugar (sucrose)
4. Soda
Type of Matter:
Pure substance or Mixture
Type of Pure substance or Type of mixture
Pure substance
element
Mixture
Heterogeneous
compound
Homogeneous

10. B. Pure Substances Element composed of identical atoms
EX: Cu, Al, H2, O2

11. B. Pure Substances Compound 2 or more elements in a fixed ratio
properties differ from those of individual elements
EX: table salt (NaCl); water (H2O)

12. C. Mixtures Combination of 2 or more pure substances. Heterogeneous
Homogeneous

13. C. Mixtures A. Homogenous solution very small particles
particles don’t settle
EX: rubbing alcohol

14. C. Mixtures B. Hetergeneous 1. Colloid medium-sized particles
particles don’t settle
EX: milk

15. C. Mixtures Suspension heterogeneous large particles particles settle
EX: fresh-squeezed lemonade

16. C. Mixtures Examples: mayonnaise muddy water fog saltwater
Italian salad dressing
colloid
suspension
solution

17. II. Properties & Changes in Matter
Ch. 1 - Matter
II. Properties & Changes in Matter

18. A. Extensive vs. Intensive
Extensive Property
depends on the amount of matter present
Intensive Property
depends on the identity of substance, not the amount

19. A. Extensive vs. Intensive
Examples:
boiling point
volume
mass
density
conductivity
intensive
extensive

20. Physical vs. Chemical Physical Property
can be observed without changing the identity of the substance
Chemical Property
describes the ability of a substance to undergo changes in identity

21. Physical vs. Chemical Examples: melting point flammable density
magnetic
tarnishes in air
physical
chemical

22. Physical vs. Chemical Physical Change
changes the form of a substance without changing its identity
properties remain the same
Chemical Change
changes the identity of a substance
products have different properties

23. Physical vs. Chemical Signs of a Chemical Change
change in color or odor
formation of a gas
formation of a precipitate (solid)
change in light or heat

24. Physical vs. Chemical Examples: rusting iron dissolving in water
burning a log
melting ice
grinding spices
chemical
physical