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2. Standardized Test Prep
Resources
Chapter Presentation
Bellringer
Transparencies
Sample Problems
Visual Concepts
Standardized Test Prep

3. Chapter 8 Table of Contents Section 1 Describing Chemical Reactions
Chemical Equations and Reactions
Chapter 8
Table of Contents
Section 1 Describing Chemical Reactions
Section 2 Balancing Chemical Equations
Section 3 Classifying Chemical Reactions
Section 4 Writing Net Ionic Equations

4. Section 1 Describing Chemical Reactions
Chapter 8
Bellringer
For the following situations, list observations that you think indicate that a chemical reaction has taken place:
a cut apple turns brown
an egg changes when it cooks
a log burns
a car rusts

5. Section 1 Describing Chemical Reactions
Chapter 8
Objectives
List evidence that suggests that a chemical reaction has occurred and evidence that proves that a chemical reaction has occurred.
Describe a chemical reaction by using a word equation and a formula equation.
Interpret notations in formula equations, such as those relating to states of matter or reaction conditions.

6. Chapter 8 Chemical Reaction
Section 1 Describing Chemical Reactions
Chapter 8
Chemical Reaction
A chemical reaction is the process by which one or more substances change into one or more new substances.
Reactants are the original substances in a chemical reaction.
Products are the substances that are created in a chemical reaction.

7. Chapter 8
Visual Concepts
Chemical Reaction

8. Evidence of a Chemical Reaction
Section 1 Describing Chemical Reactions
Chapter 8
Evidence of a Chemical Reaction

9. Signs of a Chemical Reaction
Chapter 8
Visual Concepts
Signs of a Chemical Reaction

10. Chapter 8
Visual Concepts
Precipitate

11. Evidence of a Chemical Reaction
Section 1 Describing Chemical Reactions
Chapter 8
Evidence of a Chemical Reaction
solution color changes
solution bubbles
copper is used up

12. Chemical Reaction Versus Physical Change
Section 1 Describing Chemical Reactions
Chapter 8
Chemical Reaction Versus Physical Change
chemical change – new substance forms with properties that differ from original substance
density
boiling point
melting point
physical change - changes of state
evaporation
condensation
melting
freezing

13. Reactions and Energy Changes
Section 1 Describing Chemical Reactions
Chapter 8
Reactions and Energy Changes
Energy can be released in a chemical reaction.
methane + oxygen  carbon dioxide + water + energy
Energy is a product.
Energy can be absorbed in a chemical reaction.
dinitrogen tetroxide + energy  nitrogen dioxide
Energy is a reactant.

14. Constructing a Chemical Equation
Section 1 Describing Chemical Reactions
Chapter 8
Constructing a Chemical Equation
A chemical equation shows the chemical formulas and relative amounts of all reactants and products.
A word equation contains the names of the reactants and products.
Equations must be balanced.

15. methane + oxygen  carbon dioxide + water
Section 1 Describing Chemical Reactions
Chapter 8
Writing a Word Equation or Formula Equation
methane + oxygen  carbon dioxide + water
?CH ?O2  ?CO ?H2O

16. Equations and Reaction Information
Section 1 Describing Chemical Reactions
Chapter 8
Equations and Reaction Information
Physical States
NaHCO3(s) + HC2H3O2(aq)  NaC2H3O2(aq) + CO2(aq) + H2O(l)
solid liquid
aqueous solutions
Reaction Conditions
350°C, kPa
N2(g) + 3H2(g)
2NH3(g)
catalyst

17. Equations and Reaction Information
Section 1 Describing Chemical Reactions
Chapter 8
Equations and Reaction Information

18. Chapter 8
Visual Concepts
Chemical Equation

19. HW.SECTION REVIEW, pg.266 #(1-10)

20. Section 8.1 Review What is a chemical reaction?
2. What is the only way to prove that a chemical
reaction has occurred?
3. When water boils on the stove, does a chemical change or a physical change take place?
4. Give four examples of evidence that suggests
that a chemical change probably is occurring.

21. Section15.2 Review
5. When propane gas, C3H8, is burned with oxygen, the products are carbon dioxide and water. Write an unbalanced formula equation for the reaction.
6. Assume that liquid water forms in item 5. Write a formula equation for the reaction that shows the physical states of all compounds.
7. What does “Mn” above the arrow in a formula
equation mean?

22. Section 8.1 Review
8. What symbol is used in a chemical equation to indicate the phrase “reacts with”?
9. Solid silicon and solid magnesium chloride form when silicon tetrachloride gas reacts with magnesium metal. Write a word equation and an unbalanced formula equation. Include all of the appropriate notations.
10. Magnesium oxide forms from magnesium metal and oxygen gas. Write a word equation and an unbalanced formula equation. Include all of the appropriate notations

23. sugar + flour + eggs + vanilla + salt  cake
Section 2 Balancing Chemical Equations
Chapter 8
Bellringer
Write a word equation for baking a cake.
Does the cake have the same properties as the ingredients?
Answer:
sugar + flour + eggs + vanilla + salt  cake
The properties are different.

24. Section 2 Balancing Chemical Equations
Chapter 8
Objectives
Relate the conservation of mass to the rearrangement of atoms in a chemical reaction.
Write and interpret a balanced chemical equation for a reaction, and relate conservation of mass to the balanced equation.

25. Reactions Conserve Mass
Section 2 Balancing Chemical Equations
Chapter 8
Reactions Conserve Mass
Mass cannot be created or destroyed by a chemical or physical change
Equations must be balanced.
?Na + ?H2O  ?NaOH + ?H2

26. Chapter 8 Balancing Equations
Section 2 Balancing Chemical Equations
Chapter 8
Balancing Equations
The number of atoms for each element must be the same on the reactants’ side and on the products’ side.
A coefficient multiplies the number of atoms of each element in the formula that follows.
H2O: 2 hydrogen atoms, 1 oxygen atom
2H2O: 4 hydrogen atoms, 2 oxygen atoms

27. Reading a Chemical Equation
Chapter 8
Visual Concepts
Reading a Chemical Equation

28. Balancing a Chemical Equation by Inspection
Chapter 8
Visual Concepts
Balancing a Chemical Equation by Inspection

29. Chapter 8 Balancing Equations Sample Problem A
Section 2 Balancing Chemical Equations
Chapter 8
Balancing Equations
Sample Problem A
Balance the equation for the reaction of iron(III) oxide with hydrogen to form iron and water.

30. Chapter 8 Balancing Equations Sample Problem A Solution
Section 2 Balancing Chemical Equations
Chapter 8
Balancing Equations
Sample Problem A Solution
Identify reactants and products.
reactants products
Fe2O H2  Fe + H2O
Count atoms 3 2 3
Reactants
Products
Balanced?
Unbalanced formula equation
Fe2O3 + H2
Fe + H2O
Iron atoms 2 1 no
Oxygen atoms 3
Hydrogen atoms
yes
Insert coefficients.

31. Reactions Conserve Mass
Section 2 Balancing Chemical Equations
Chapter 8
Reactions Conserve Mass
Balanced equations show mass conservation
?Na + ?H2O  ?NaOH + ?H2
2Na + 2H2O  2NaOH + H2
Never change subscripts to balance equations
Unbalanced: H2 + O2  H2O
Incorrect: H2 + O2  H2O2
H2O  H2O2
Correct: 2H2 + O2  2H2O

32. Sample Problem A , Practice pg. 269
Write a balanced equation for each of the following.
P4 + O2 → P2O5
2 ) C3H8 + O2 → CO2 + H2O

33. Sample Problem A , Practice pg. 269
3 ) Ca2Si + Cl2 → CaCl2 + SiCl4
4 )Silicon reacts with carbon dioxide to form silicon carbide, SiC, and silicon dioxide.

34. Sample Problem B , Practice pg. 271
Write a balanced chemical equation for each of the following.
1) C2H2 + O2 → CO2 + H2O
2 ) Fe(OH)2 + H2O2 → Fe(OH)3
FeS2 + Cl2 → FeCl3 + S2Cl2
NH3+ O2 → NO + H2O

35. Chapter 8 Balancing Equations
Section 2 Balancing Chemical Equations
Chapter 8
Balancing Equations
Sample Problem C
Aluminum reacts with arsenic acid, HAsO3, to form H2 and aluminum arsenate. Write a balanced equation for this reaction.

36. Chapter 8 Balancing Equations reactants products 2 6 3 2
Section 2 Balancing Chemical Equations
Chapter 8
Balancing Equations
Sample Problem C Solution
1. Identify reactants and products.
reactants products
Al + HAsO3  H Al(AsO3)3
2. Count Atoms 2 6 3 2
Reactants
Products
Balanced?
Unbalanced formula equation
Al + HAsO3
H2 + Al(AsO3)3
Iron atoms 1
yes
Oxygen atoms 2 no
Hydrogen atoms 3
3. Insert coefficients

37. Sample Problem C , Practice pg. 273
Write a balanced equation for each of the following.
HgCl2 + AgNO3 → Hg(NO3)2 + AgCl
2 ) Al + Hg(CH3COO)2 →Al(CH3COO)3 + Hg
3 ) Calcium phosphate and water are produced when calcium hydroxide reacts with phosphoric acid

38. HW.
Section 8.2 Review
Q(1-6)

39. 4) Write each of the following reactions as a word equation, an unbalanced formula equation, and finally as a balanced equation.
When heated, potassium chlorate decomposes into potassium chloride and oxygen.
b) Silver sulfide forms when silver and sulfur, S8, react.
c) Sodium hydrogen carbonate breaks down to form sodium carbonate, carbon dioxide, and water vapor.

40. Section Review pg. 274
5) Balance the following equations.
ZnS + O2 → ZnO + SO2
b. Fe2O3 + CO → Fe + CO2
c. AgNO3 + AlCl3 →AgCl + Al(NO3)3
d. Ni(ClO3)2 → NiCl2 + O2

41. Section Review pg. 274
6) Balance the following equations.
(NH4)2Cr2O7 → Cr2O3 + N2 + H2O
b. NH3 + CuO → N2 + Cu + H2O
c. Na2SiF6 + Na → Si + NaF
d. C4H10 + O2 → CO2 + H2O

42. Chapter 8 Bellringer Describe the following terms. synthesis
Section 3 Classifying Chemical Reactions
Chapter 8
Bellringer
Describe the following terms.
synthesis
decomposition
displacement

43. Section 3 Classifying Chemical Reactions
Chapter 8
Objectives
Identify combustion reactions, and write chemical equations that predict the products.
Identify synthesis reactions, and write chemical equations that predict the products.
Identify decomposition reactions, and write chemical equations that predict the products.

44. Chapter 8 Objectives, continued
Section 3 Classifying Chemical Reactions
Chapter 8
Objectives, continued
Identify displacement reactions, and use the activity series to write chemical equations that predict the products.
Identify double-displacement reactions, and write chemical equations that predict the products.

45. Chapter 8 Combustion Reactions
Section 3 Classifying Chemical Reactions
Chapter 8
Combustion Reactions
A combustion reaction is a reaction of a carbon-based compound with oxygen.
Combustion of propane:
C3H8 + 5O2  3CO2 + 4H2O
Combustion of ethanol:
CH3CH2OH + 3O2  2CO2 + 3H2O

46. Chapter 8
Visual Concepts
Combustion Reaction

47. CaO(s) + H2O(l)  Ca(OH)2(s)
Section 3 Classifying Chemical Reactions
Chapter 8
Synthesis Reactions
In a synthesis reaction a single compound forms from two or more reactants.
Two elements form a binary compound
C + O2  CO2
2C + O2 2CO
Two compounds form a ternary compound
CaO(s) + H2O(l)  Ca(OH)2(s)
CO2(g) + H2O(l)  H2CO3(aq)

48. Chapter 8
Visual Concepts
Synthesis Reactions

49. Decomposition Reactions
Section 3 Classifying Chemical Reactions
Chapter 8
Decomposition Reactions
In a decomposition reaction a single compound breaks down, often with the input of energy, into two or more elements or simpler compounds.
Decomposition of water
electricity
2H2O(l)
O2(g) + 2H2(g)
A metal carbonate decomposes to form a metal oxide and carbon dioxide.
heat
CaCO3(s)
CaO(s) + CO2(g)

50. Decomposition Reaction
Chapter 8
Visual Concepts
Decomposition Reaction

51. Chapter 8
Visual Concepts
Electrolysis

52. Decomposition Reactions, continued
Section 3 Classifying Chemical Reactions
Chapter 8
Decomposition Reactions, continued
Sample Problem D
Predicting Products
Predict the product(s) and write a balanced equation for the reaction of potassium with chlorine.

53. Decomposition Reactions, continued
Section 3 Classifying Chemical Reactions
Chapter 8
Decomposition Reactions, continued
Sample Problem D Solution
Reaction is most likely a synthesis reaction, so the product will be binary
Potassium will lose one electron to become a 1+ ion.
Chlorine will gain one electron to become a 1– ion.
K + Cl2  KCl
Balance the equation.
2K + Cl2  2KCl

54. Section 3 Classifying Chemical Reactions
Chapter 8
Sample Problem D , practice pg. 279
Predict the product(s) and write a balanced equation for each of the following reactions.
the reaction of butane, C4H10, with oxygen
2)the reaction of water with calcium oxide
3)the reaction of lithium with oxygen

55. 4)the decomposition of carbonic acid
5) The decomposition of nitrogen triiodide.

56. 6) The reaction of magnesium oxide and water.
7) The decomposition of calcium carbonate.

57. Homework Copy and solve the following questions
Predict the product(s) and write a balanced equation for each of the following reactions.
pentane, C5H12, reacting with oxygen.
Water reacting with potassium oxide.
Calcium reacting with oxygen.
The decomposition of sodium chloride.
The combustion of octane C8H18.

58. Displacement Reactions
Section 3 Classifying Chemical Reactions
Chapter 8
Displacement Reactions
In a displacement reaction a single element reacts with a compound and displaces another element from the compound.
2Al(s) + 3CuCl2(aq)  2AlCl3(aq) + 3Cu(s)
Aluminum displaces copper.

59. Single Displacement Reaction
Chapter 8
Visual Concepts
Single Displacement Reaction

60. Displacement Reactions, continued
Section 3 Classifying Chemical Reactions
Chapter 8
Displacement Reactions, continued
The activity series ranks the reactivity of elements

61. Chapter 8
Visual Concepts
Activity Series

62. Displacement Reactions, continued
Section 3 Classifying Chemical Reactions
Chapter 8
Displacement Reactions, continued
Sample Problem E
Determining Products by Using the Activity Series Magnesium is added to a solution of lead(II) nitrate. Will a reaction happen? If so, write the equation and balance it.

63. Displacement Reactions, continued
Section 3 Classifying Chemical Reactions
Chapter 8
Displacement Reactions, continued
Sample Problem E Solution
Identify the reactants.
Magnesium will attempt to displace lead from lead(II) nitrate.
Check the activity series.
Magnesium is more active than lead and displaces it.
Write the balanced equation.
Mg + Pb(NO3)2  Pb + Mg(NO3)2

64. Sample Problem E, practice pg. 282
For the following situations, write a balanced equation if a reaction happens. Otherwise write “no reaction.”
Aluminum is dipped into a zinc nitrate solution.
2 )Sodium is placed in cold water.
3 )Gold is added to a solution of calcium chloride.

65. HCl(aq) + NaOH(aq)  HOH(l) + NaCl(aq)
Section 3 Classifying Chemical Reactions
Chapter 8
Double-Displacement Reactions
In a double-displacement reaction two compounds in aqueous solution appear to exchange ions and form two new compounds.
One of the products must be a solid precipitate, a gas, or a molecular compound, such as water.
HCl(aq) + NaOH(aq)  HOH(l) + NaCl(aq)

66. Double-Displacement Reaction
Chapter 8
Visual Concepts
Double-Displacement Reaction

67. Precipitation Reaction
Chapter 8
Visual Concepts
Precipitation Reaction

68. Predict the products of the following reations.
a. AgNO3(aq) + K2SO4(aq) →
b. H2SO4(aq) + KOH(aq) →
c. KI(aq) + Pb(NO3)2(aq) →

69. Chapter 8

70. HOMEWORK
SECTION REVIEW, pg. 285, # ( 1- 10)

71. Section 8.3 Review, pg. 285
8. Balance each of the equations below, and indicate the type of reaction for each equation.
Cl2(g) + NaBr(aq) → NaCl(aq) + Br2(l)
b. CaO(s) + H2O(l) → Ca(OH)2(aq)
c. Ca(ClO3)2(s) → CaCl2(s) + O2(g)
d. AgNO3(aq) + K2SO4(aq) → Ag2SO4(s) + KNO3(aq)
e. Zn(s) + CuBr2(aq) → ZnBr2(aq) + Cu(s)
f. C8H18(l) + O2(g) → CO2(g) + H2O(g)

72. Section 8.3 Review, pg. 285
9. Predict whether a reaction would occur when the materials indicated are brought together. For each reaction that would occur, complete and balance the equation.
Ag(s) + H2O(l)
b. Mg(s) + Cu(NO3)2(aq)
c. Al(s) + O2(g)
d. H2SO4(aq) + KOH(aq)

73. Section 8.3 Review, pg. 285
10. Predict the products, write a balanced equation, and identify the type of reaction for each of the following reactions.
HgO →
b. C3H7OH + O2 →
c. Zn + CuSO4 →
d. BaCl2 + Na2SO4 →
e. Zn + F2 →
f. C5H10 + O2 →

74. Section 4 Writing Net Ionic Equations
Chapter 8
Bellringer
Write a definition for the word spectator in terms of the part spectators play in a sporting event.

75. Section 4 Writing Net Ionic Equations
Chapter 8
Objectives
Write total ionic equations for reactions in aqueous solutions.
Identify spectator ions and write net ionic equations for reactions in aqueous solutions.

76. Ionic Equations, continued
Section 4 Writing Net Ionic Equations
Chapter 8
Ionic Equations, continued
Ionic compounds dissolve in water
KI(aq) = K+(aq) + I–(aq)
Pb(NO3)2(aq) = Pb2+(aq) (aq)
Reaction between KI and Pb(NO3)2
2KI(aq) + Pb(NO3)2(aq)  PbI2(s) + 2KNO3(aq)
Total Ionic Equation
2K+(aq) + 2I–(aq) + Pb2+(aq) (aq)
 PbI2(s) + 2K+(aq) (aq)

77. 2I–(aq) + Pb2+(aq)  PbI2(s)
Section 4 Writing Net Ionic Equations
Chapter 8
Ionic Equations, continued
Spectator ions remain unchanged in the solution as aqueous ions. They do not react.
2K+(aq) + 2I–(aq) + Pb2+(aq) (aq)
 PbI2(s) + 2K+(aq) (aq)
The net ionic equation is the chemical equation that shows only the net change.
2I–(aq) + Pb2+(aq)  PbI2(s)

78. Chapter 8
Visual Concepts
Net Ionic Equation

79. Zn(s) + Cu2+(aq)  Cu(s) + Zn2+(aq)
Section 4 Writing Net Ionic Equations
Chapter 8
Ionic Equations, continued
Net Ionic equations can be used for displacement reactions.
Zn(s) + Cu2+(aq) (aq)  Cu(s) + Zn2+(aq) (aq)
net ionic equation
Zn(s) + Cu2+(aq)  Cu(s) + Zn2+(aq)

80. Ionic Equations, continued
Section 4 Writing Net Ionic Equations
Chapter 8
Ionic Equations, continued
Check atoms and charge to balance net ionic equations.
(aq) + Ba2+(aq)  BaSO4(s)
Charge: (2–) + (2+) =
Zn(s) + Cu2+(aq)  Cu(s) + Zn2+(aq)
Charge:

81. Practice
Write a total ionic equation for each of the following unbalanced formula equations. Identify the spectator ions, and write a net ionic equation for each reaction . Don’t forget to balance.
Br2(l) + NaI(aq)→ NaBr(aq) + I2(s)
b. Ca(OH)2(aq) + HCl(aq) → CaCl2(aq) + H2O(l)

82. c. Mg(s) + AgNO3(aq) → Ag(s) + Mg(NO3)2(aq)
d. AgNO3 + KBr →AgBr + KNO3

83. e. Ni(s) + Pb(NO3)2(aq) →Ni(NO3)2(aq) + Pb(s)
f. Ca(s) + H2O(l) → Ca(OH)2(aq) + H2(g)

84. HW.
SECTION REVIEW,
Pg. 289, # (8 -11)

85. Understanding Concepts
Chapter 8
Standardized Test Preparation
Understanding Concepts
1. What type of chemical reaction involves the exchange of the ions of two compounds in an aqueous solution to form two new compounds?
A. synthesis reaction
B. decomposition reaction
C. single-displacement reaction
D. double-displacement reaction

86. Understanding Concepts
Chapter 8
Standardized Test Preparation
Understanding Concepts
1. What type of chemical reaction involves the exchange of the ions of two compounds in an aqueous solution to form two new compounds?
A. synthesis reaction
B. decomposition reaction
C. single-displacement reaction
D. double-displacement reaction

87. Understanding Concepts
Chapter 8
Standardized Test Preparation
Understanding Concepts
2. Which of these sentences correctly states the law of conservation of mass?
F. In a chemical reaction, the mass of the products cannot exceed the mass of the reactants.
G. In a chemical reaction, the mass of the products is always equal to the mass of the reactants.
H. In a chemical reaction, the mass of the products is always less than the mass of the reactants.
I. In a chemical reaction, the mass of the products is always greater than the mass of the reactants.

88. Understanding Concepts
Chapter 8
Standardized Test Preparation
Understanding Concepts
2. Which of these sentences correctly states the law of conservation of mass?
F. In a chemical reaction, the mass of the products cannot exceed the mass of the reactants.
G. In a chemical reaction, the mass of the products is always equal to the mass of the reactants.
H. In a chemical reaction, the mass of the products is always less than the mass of the reactants.
I. In a chemical reaction, the mass of the products is always greater than the mass of the reactants.

89. Understanding Concepts
Chapter 8
Standardized Test Preparation
Understanding Concepts
3. Of these reaction types, which has only one reactant?
A. decomposition
B. displacement
C. oxidation
D. synthesis

90. Understanding Concepts
Chapter 8
Standardized Test Preparation
Understanding Concepts
3. Of these reaction types, which has only one reactant?
A. decomposition
B. displacement
C. oxidation
D. synthesis

91. Understanding Concepts
Chapter 8
Standardized Test Preparation
Understanding Concepts
4. Write a net ionic equation, excluding spectator ions, for the reaction:
Mg(s) + Zn(NO3)2(aq)  Zn(s) + Mg(NO3)2(aq)

92. Understanding Concepts
Chapter 8
Standardized Test Preparation
Understanding Concepts
4. Write a net ionic equation, excluding spectator ions, for the reaction:
Mg(s) + Zn(NO3)2(aq)  Zn(s) + Mg(NO3)2(aq)
Answer: Mg(s) + Zn2+(aq)  Mg2+(aq) + Zn(s)

93. Understanding Concepts
Chapter 8
Standardized Test Preparation
Understanding Concepts
5. Differentiate between formula equations and balanced chemical equations.

94. Understanding Concepts
Chapter 8
Standardized Test Preparation
Understanding Concepts
5. Differentiate between formula equations and balanced chemical equations.
Answer: Formula equations give the identity of the reactants and the products, but a balanced equation shows equal numbers of atoms of each element on both sides.

95. Understanding Concepts
Chapter 8
Standardized Test Preparation
Understanding Concepts
6. Write a balanced equation for this reaction:
iron(III) nitrate + lithium hydroxide 
lithium nitrate + iron(III) hydroxide

96. Understanding Concepts
Chapter 8
Standardized Test Preparation
Understanding Concepts
6. Write a balanced equation for this reaction:
iron(III) nitrate + lithium hydroxide 
lithium nitrate + iron(III) hydroxide
Answer: Fe(NO3)3 + 3LiOH  3LiNO3 + Fe(OH)3

97. Chapter 8 Reading Skills
Standardized Test Preparation
Reading Skills
Read the passage below. Then answer the questions.
A student places a strip of pure magnesium metal into a test tube containing a dilute solution of hydrochloric acid (hydrogen chloride dissolved in water). As the magnesium disappears, bubbles of a colorless gas form and the test tube becomes hot to the touch. If a lit match is placed near the top of the test tube, the gas that has been generated burns.

98. Chapter 8 Reading Skills
Standardized Test Preparation
Reading Skills
7. What evidence is there that a chemical reaction has occurred?

99. Chapter 8 Reading Skills
Standardized Test Preparation
Reading Skills
7. What evidence is there that a chemical reaction has occurred?
Answer: The gas that burns is a different chemical substance than any of the reactants, indicating a chemical reaction.

100. Chapter 8 Reading Skills
Standardized Test Preparation
Reading Skills
8. Based on the substances present in the reaction, what is the most likely identity of the reaction product that burns in air?
F. hydrogen
G. magnesium
H. oxygen
I. oxygen and hydrogen mixture

101. Chapter 8 Reading Skills
Standardized Test Preparation
Reading Skills
8. Based on the substances present in the reaction, what is the most likely identity of the reaction product that burns in air?
F. hydrogen
G. magnesium
H. oxygen
I. oxygen and hydrogen mixture

102. Chapter 8 Reading Skills
Standardized Test Preparation
Reading Skills
9. Which of these equations is a balanced chemical equation for the reaction described above?
A. Mg(s) + HCl(aq)  MgCl2(aq) + H2(g) + energy
B. Mg(s) + 2HCl(aq) + energy  MgCl2(aq) + H2(g)
C. Mg(s) + 2HCl(aq)  MgCl2(aq) + H2(g) + energy
D. 2Mg(s) + 2HCl(aq)  2MgCl2(aq) + H2(g) + energy

103. Chapter 8 Reading Skills
Standardized Test Preparation
Reading Skills
9. Which of these equations is a balanced chemical equation for the reaction described above?
A. Mg(s) + HCl(aq)  MgCl2(aq) + H2(g) + energy
B. Mg(s) + 2HCl(aq) + energy  MgCl2(aq) + H2(g)
C. Mg(s) + 2HCl(aq)  MgCl2(aq) + H2(g) + energy
D. 2Mg(s) + 2HCl(aq)  2MgCl2(aq) + H2(g) + energy

104. Interpreting Graphics
Chapter 8
Standardized Test Preparation
Interpreting Graphics
The table below shows the reactivity of selected
elements. Use it to answer questions 10 through 12.

105. Interpreting Graphics
Chapter 8
Standardized Test Preparation
Interpreting Graphics
10.Which of these elements will produce a flammable product when placed in water at room temperature?
F. aluminum
G. silver
H. sodium
I. zinc

106. Interpreting Graphics
Chapter 8
Standardized Test Preparation
Interpreting Graphics
10.Which of these elements will produce a flammable product when placed in water at room temperature?
F. aluminum
G. silver
H. sodium
I. zinc

107. Interpreting Graphics
Chapter 8
Standardized Test Preparation
Interpreting Graphics
11.Which of these combinations is most likely to cause a displacement reaction?
A. a zinc strip placed in a solution of aluminum
chloride
B. a nickel strip placed in a solution of calcium chloride
C. a silver strip placed in a solution of potassium
hydroxide
D. an aluminum strip placed in a solution of copper

108. Interpreting Graphics
Chapter 8
Standardized Test Preparation
Interpreting Graphics
11.Which of these combinations is most likely to cause a displacement reaction?
A. a zinc strip placed in a solution of aluminum
chloride
B. a nickel strip placed in a solution of calcium chloride
C. a silver strip placed in a solution of potassium
hydroxide
D. an aluminum strip placed in a solution of copper

109. Interpreting Graphics
Chapter 8
Standardized Test Preparation
Interpreting Graphics
12.What determines the order of the elements in the activity series?
F. increasing atomic number
G. increasing electronegativity
H. increasing ionization energy
I. experimentally determined reactivity

110. Interpreting Graphics
Chapter 8
Standardized Test Preparation
Interpreting Graphics
12.What determines the order of the elements in the activity series?
F. increasing atomic number
G. increasing electronegativity
H. increasing ionization energy
I. experimentally determined reactivity