Name
Period
Date
Chapter 3 Review Sheet: Matter & Its Properties
STATES OF MATTER
1.
Draw a diagram to represent 8 particles in each state of matter. (HINT: Recall that
plasma is gas-like but with one major difference.)
SOLID
LIQUID
GAS
PLASMA
CLASSIFICATION OF MATTER
Classify the following as element (E), compound (C), heterogeneous mixture (H), or solution (S).
2.
neon gas
4.
clean air
3.
orange juice
5.
carbon dioxide (CO2)
6.
Compare and contrast a mixture and a compound. How are they alike/different?
7.
How are homogeneous and heterogeneous mixtures different? Give examples of each
(not listed above).
8.
List and explain several ways to separate mixtures including distillation, chromatography
and filtration.
9.
How could you separate a mixture of sand and sugar?
10. Explain the Law of Conservation of Mass.
11. Distinguish between a gas and a vapor.
Matter & Its Properties – Ch. 3
CHEM
PROPERTIES & CHANGES IN MATTER
Classify the following properties of matter as chemical (C) or physical (P).
12. flexible
14. boils at 20C
13. combustible
15. low reactivity
Classify the following physical properties of matter as extensive (E) or intensive (I).
16. melting point
18. volume
17. mass
19. density
Classify the following as chemical changes (C) or physical changes (P).
20. grapes fermenting
25. eggs cooking
21. copper melting
26. iron rusting
22. recycling aluminum
27. wood burning
23. gasoline exploding
28. mixing cake batter
24. water evaporating
___________
29. baking a cake
List the terms for the physical changes below:
30. liquid  solid
33. gas  liquid
31. solid  liquid
34. solid  gas
32. liquid  gas
35. gas  solid
DENSITY
D
M
V
Solve the following density problems. Show your work and put the correct units!
36. What is a derived unit? Make sure you could make a density graph!!
37. What is the density of a substance with a mass of 37.72 grams and a volume of 6.70 cm3?
38. The density of sugar is 1.59 g/cm3. The mass of a sample is 4.0 g. What is the volume of
the sample?
39. The density of clay is 2.2 g/cm3. What is the mass of a 5.00 cm3 sample?
40. You have a substance that has a mass of 92.0 g and a volume of 115 mL. Can this
substance float on water? Why or why not?
Matter & Its Properties – Ch. 3
CHEM
Chapter 3 Review Sheet: Matter & Its Properties Answers
1.
2. E
4. S
3. H
5. C
6. mixture contains more than one substance physically combined, compound has more than
one substance chemically combined; mixtures can be separated using physical means,
compounds cannot; compounds have a fixed composition, mixtures do not; compounds are
pure substances, mixtures are not; both are combinations of materials and made of pure
substances
7. homogeneous mixtures, also called solutions, have a uniform composition throughout,
examples are Kool-Aid, tea, saltwater; heterogeneous mixtures do not have a uniform
composition, examples are OJ, milk, granite, Italian dressing
8. you can separate mixtures by density, magnetic attraction, particle size, distillation –
separating substances with different boiling points, chromatography – separating substances
with different polarity/solubility, filtration – separating substances using filter paper so liquid
pass through and solids do not
9. to separate sand and sugar – add water, sugar will dissolve, filter sand out, boil water to
leave sugar
10. law of conservation of mass says mass is neither created nor destroyed, mass of reactants
= mass of products in a chemical reaction
11. gas is phase of matter where particles are not bound to each other and are able to move
freely, vapor is term used for gaseous state of substances that are solids or liquids at room
temperature
volume on x-axis, slope is
12. P
25. C
density)
13. C
26. C
37. 5.55 g/cm3
14. P
27. C
38. 2.5 cm3
15. C
28. P
39. 11 g
16. I
29. C
40. Yes, because its
17. E
30. freezing
density is 0.80 g/mL and
that is less than the
18. E
31. melting
density of water which is
19. I
32. evaporation
1.0 g/mL
20. C
33. condensation
21. P
34. sublimation
22. P
35. deposition
23. C
36. a combination of base
units (mass on y-axis,
24. P
Ch. 3 – Matter & Its Properties
CHEM