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
Take the shape of the container
fixed volume

5. B. Four States of Matter Gases
high KE - particles can separate and move throughout 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. Another look at all the states of matter

8. II. Matter Flowchart Pure Substances Mixtures
Ch. 1 - Matter
II. Matter Flowchart
Pure Substances
Mixtures

9. 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

10. A. Matter Flowchart Examples: graphite pepper sugar (sucrose) paint
soda
element
hetero. mixture
compound
homo. mixture
solution

11. B. Pure Substances Element composed of identical atoms
EX: copper wire, aluminum foil

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

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

14. C. Mixtures Solution homogeneous very small particles
particles don’t settle
EX: rubbing alcohol

15. C. Mixtures Colloid heterogeneous medium-sized particles
particles don’t settle
EX: milk

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

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

18. Ch. 1 - Matter III. Properties & Changes in Matter
Extensive vs. Intensive
Physical vs. Chemical

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

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

21. B. 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

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

23. B. 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

24. B. 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

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

26. How would you separate the following mixture?
IRON FILINGS, SALT, CHALK POWDER AND WATER
Dissolve as much of the mixture as possible
Add water and stir
Filter the mixture so that the soluble salt will be obtained in the filtrate and the insoluble chalk powder will be the residue on the filter paper
Place the dry mixture into a beaker
Dry out the filter paper to keep the dry chalk powder
 Use a magnet to attract and extract the iron filings from the dry mixture
 Pour the filtrate into an evaporating basin to evaporate the water and leave behind the salt