1. I. States of Matter (p.12) Kinetic Molecular Theory States of Matter
Ch. 1 - Matter
I. States of Matter (p.12)
Kinetic Molecular Theory
States of Matter

2. A. Kinetic Molecular Theory
KMT
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 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, fluorescent light bulbs, CRTs

7. Ch. 1 - Matter II. Classification of Matter (p.15-17, 397-398)
Matter Flowchart
Pure Substances
Mixtures
C. Johannesson

8. Warm-Up
What is the difference between a homogeneous and heterogeneous mixture? (how can you tell the difference?)
C. Johannesson

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
C. Johannesson

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

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

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)
C. Johannesson

13. B. Pure Substances Law of Definite Composition
A given compound always contains the same, fixed ratio of elements.
Law of Multiple Proportions
Elements can combine in different ratios to form different compounds.
C. Johannesson

14. Two different compounds, each has a definite composition.
B. Pure Substances
For example…
Two different compounds, each has a definite composition.
C. Johannesson

15. C. Mixtures Variable combination of 2 or more pure substances.
Heterogeneous
Homogeneous
C. Johannesson

16. C. Mixtures Solution homogeneous very small particles
no Tyndall effect
Tyndall Effect
particles don’t settle
EX: rubbing alcohol
C. Johannesson

17. C. Mixtures Colloid heterogeneous medium-sized particles
Tyndall effect
particles don’t settle
EX: milk
C. Johannesson

18. C. Mixtures Suspension heterogeneous large particles Tyndall effect
particles settle
EX: fresh-squeezed lemonade
C. Johannesson

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

20. Ch. 1 - Matter III. Properties & Changes in Matter (p.11-14)
Extensive vs. Intensive
Physical vs. Chemical
C. Johannesson

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

22. A. Extensive vs. Intensive
Examples:
boiling point
volume
mass
density
conductivity
intensive
extensive
C. Johannesson

23. 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
C. Johannesson

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

25. 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
C. Johannesson

26. 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
C. Johannesson

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

28. Ch. 9 - Classification of Matter
I. Describing Matter (p )
Physical Property
Physical Change
Chemical Change
Chemical Property

29. A. Physical Property
A characteristic of a substance that can be observed without changing its identity.
can be used to separate mixtures
EX: magnetism, density

30. B. Physical Change
A change in the form of a substance without changing its identity.
properties remain the same
reversible
can be used to separate mixtures
EX: dissolving, grinding

31. C. Chemical Change A change in the identity of a substance.
properties change
irreversible
Signs: color change, formation of a gas/solid, release of light/heat
EX: burning, rusting

32. D. Chemical Property
A characteristic that indicates whether a substance can undergo a specific chemical change.
EX: flammability, reactivity