Download Physical Science Chapters 6 and 7 Test Review Answer Section

Physical Science Chapters 6 and 7 Test Review
Name ______________________
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____
1. The only sure evidence for a chemical reaction is
a. the formation of a gas.
b. a color change.
c. the production of one or more new substances.
d. changes in properties.
____
2. Which is the correct chemical equation for the following statement? Sodium reacts with oxygen in a 2 to 1
ratio to produce sodium oxide.
a. 4 Na + O2  2 Na2O
b. Na2O a + O2
c. Na2O + O2 a
d. Na2 + O2 aO
____
3. In a chemical equation, numbers often appear in front of a chemical formula. These numbers tell you the
a. number of atoms in each molecule in the reaction.
b. number of elements in the reaction.
c. number of molecules or atoms of each substance in the reaction.
d. number of molecules in each atom in the reaction.
____
4. Which of the following does NOT increase the number of particles of a substance available to react in a
chemical reaction?
a. increasing the concentration
b. increasing the surface area
c. adding a catalyst
d. increasing the mass
____
5. One example of a chemical change is
a. filtering.
b. burning wood.
c. boiling water.
d. crushing a can.
____
6. How is a solute different from a solvent in a solution?
a. The solute is present in a smaller amount.
b. The solute is present in a greater amount.
c. The solute is a solid and the solvent is a liquid.
d. The solute is a liquid and the solvent is a gas.
____
7. When a solid compound dissolves in water,
a. it breaks up into individual crystals.
b. it always conducts electricity.
c. its particles surround individual water molecules.
d. each of its particles becomes surrounded by water molecules.
____
8. How would a solute affect the boiling point of water?
a. The water will boil at a lower temperature.
b. The water will boil at a higher temperature.
c. The water will not boil.
d. The boiling point will be the same as the freezing point.
____
9. If two unidentified solids of the same texture and color have different solubilities in 100 grams of water at
20°C, you could conclude that
a. they are the same substance.
b. they are different substances.
c. they have different melting points.
d. their solubilities will be the same if the water temperature is increased.
____ 10. Which is a characteristic property of acids?
a. They turn blue litmus paper red.
b. They turn red litmus paper blue.
c. They taste bitter.
d. They do not react with metals.
____ 11. In a water solution, how do acids differ from bases?
a. Acids form hydrogen ions (H+), while bases form hydroxide ions (OH–).
b. Acids turn litmus blue, while bases turn litmus red.
c. Acids form salts, but bases do not.
d. Hydrogen ions (H+) remain dissolved, but hydroxide ions (OH–) do not.
____ 12. If you have a solution of a strong acid and a solution of a weak acid of equal concentration and volume, then
the
a. strong acid will have a lower pH.
b. strong acid will have a higher pH.
c. two solutions will have the same pH.
d. weak acid will produce more hydrogen ions.
____ 13. Neutralization is a reaction between a(n)
a. acid and a base.
b. acid and a metal.
c. base and a salt.
d. salt and water.
____ 14. What does a neutralization reaction produce?
a. acids
b. bases
c. water and a salt
d. carbonated water
____ 15. The presence of H ions in a solutions indicates that the solution is
a. acidic.
c. neutral.
b. basic.
____ 16. This indicates the ratio of the elements in a compound.
a. chemical equation
c. chemical symbol
b. chemical formula
____ 17. In a chemical equation, this number tell us the how many atoms or molecules of a substance take part in the
reaction.
a. subscript
c. superscript
b. coefficient
____ 18. What type of reaction is this: CO2 C + O2
a. decomposition
c. single replacement
b. synthesis
d. double replacement
____ 19. A polar solute would dissolve in this type of solvent.
a. polar
c. dilute
b. nonpolar
d. concentrated
____ 20. Which of the following is a balanced chemical equation?
a. Ba(CN)2 + 2 H2SO4  BaSO4 + 2HCN
c. Cu + O2  2CuO
b. 2Na + MgSO4  Na2SO4 + Mg
d. 2 H2 + O2  H2O
Matching
a.
b.
c.
d.
e.
f.
g.
exothermic
coefficient
chemical formula
inhibitor
activation energy
chemical symbol
subscript
h.
i.
j.
k.
l.
m.
n.
precipitate
chemical equation
products
matter
reactants
catalyst
indicator
____ 21. A solid that forms from solution during a chemical reaction.
____ 22. Anything that has mass and takes up space.
____ 23. The substances on the left side of a chemical equation.
____ 24. The substances on the right side of a chemical equation.
____ 25. A chemical reaction that gives off heat.
____ 26. The one- or two-letter abbreviation for an element.
____ 27. The combination of symbols that shows the ratio of elements in a compound.
____ 28. A short, easy way to show a chemical reaction using symbols.
____ 29. A number placed in front of a chemical formula in a chemical equation.
____ 30. The small number to the lower right of a chemical symbol that tells the number of atoms of that element.
____ 31. The minimum amount of energy required to start a chemical reaction.
____ 32. A material that increases the rate of reaction by lowering the activation energy.
____ 33. A material used to slow the rate of a chemical reaction.
____ 34. A material used to determine the pH of a substance.
Physical Science Chapters 6 and 7 Test Review
Answer Section
MULTIPLE CHOICE
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C
PTS: 1
DIF: L1
CaPS.6.1.2 Explain how you can tell when a chemical reaction occurs.
S 8.5.a
BLM: knowledge
A
PTS: 1
DIF: L2
CaPS.6.2.1 Identify what information a chemical equation contains.
S 8.5.b
BLM: analysis
C
PTS: 1
DIF: L2
CaPS.6.2.3 Explain what a balanced chemical equation must show.
S 8.5.b
BLM: comprehension
C
PTS: 1
DIF: L1
CaPS.6.3.2 Identify factors that affect the rate of a chemical reaction.
S 8.5.a
BLM: knowledge
B
PTS: 1
DIF: L2
CaPS.6.1.1 State how changes in matter can be described.
S 8.5.c
BLM: comprehension
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PTS: 1
DIF: L2
CaPS.7.1.1 State the characteristics of solutions, colloids, and suspensions.
S 8.5.d
BLM: comprehension
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PTS: 1
DIF: L1
CaPS.7.1.2 Describe what happens to the particles of a solute when a solution forms.
S 8.5.d
BLM: knowledge
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PTS: 1
DIF: L1
CaPS.7.1.3 Explain how solutes affect the freezing point and boiling point of a solvent.
S 8.5.d
BLM: knowledge
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PTS: 1
DIF: L2
CaPS.7.2.2 Explain why solubility is useful in identifying substances.
S 8.5.d
BLM: comprehension
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PTS: 1
DIF: L1
CaPS.7.3.1 Name the properties of acids and bases.
STA: S 8.5.e
knowledge
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DIF: L2
CaPS.7.4.1 State what kinds of ions acids and bases form in water.
S 8.5.e
BLM: comprehension
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PTS: 1
DIF: L2
CaPS.7.4.2 Explain what pH tells you about a solution.
STA: S 8.5.e
comprehension
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PTS: 1
DIF: L1
CaPS.7.4.3 Describe what happens in a neutralization reaction.
S 8.5.e
BLM: knowledge
C
PTS: 1
DIF: L1
CaPS.7.4.3 Describe what happens in a neutralization reaction.
S 8.5.a
BLM: knowledge
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