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Resources
Chapter Presentation
Bellringer
Transparencies
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Visual Concepts
Standardized Test Prep
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Chapter 8
Chemical Equations and
Reactions
Table of Contents
Section 1 Describing Chemical Reactions
Section 2 Balancing Chemical Equations
Section 3 Classifying Chemical Reactions
Section 4 Writing Net Ionic Equations
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Chapter 8
Section 1 Describing Chemical
Reactions
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
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Chapter 8
Section 1 Describing Chemical
Reactions
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.
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Chapter 8
Section 1 Describing Chemical
Reactions
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.
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Chapter 8
Visual Concepts
Chemical Reaction
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Chapter 8
Section 1 Describing Chemical
Reactions
Evidence of a Chemical Reaction
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Chapter 8
Visual Concepts
Signs of a Chemical Reaction
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Chapter 8
Visual Concepts
Precipitate
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Chapter 8
Section 1 Describing Chemical
Reactions
Evidence of a Chemical Reaction
• solution color changes
• solution bubbles
• copper is used up
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Chapter 8
Section 1 Describing Chemical
Reactions
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
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Chapter 8
Section 1 Describing Chemical
Reactions
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.
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Chapter 8
Section 1 Describing Chemical
Reactions
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.
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Chapter 8
Section 1 Describing Chemical
Reactions
Writing a Word Equation or Formula Equation
methane + oxygen  carbon dioxide + water
?CH4
+
?O2

?CO2
+ ?H2O
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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, 25 000 kPa
N2(g) + 3H2(g)
2NH3(g)
catalyst
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Chapter 8
Section 1 Describing Chemical
Reactions
Equations and Reaction Information
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Chapter 8
Visual Concepts
Chemical Equation
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Chapter 8
Section 2 Balancing Chemical
Equations
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.
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Chapter 8
Section 2 Balancing Chemical
Equations
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.
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Chapter 8
Section 2 Balancing Chemical
Equations
Reactions Conserve Mass
• Mass cannot be created or destroyed by a chemical
or physical change
• Equations must be balanced.
?Na + ?H2O  ?NaOH + ?H2
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Chapter 8
Section 2 Balancing Chemical
Equations
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
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Chapter 8
Visual Concepts
Reading a Chemical Equation
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Chapter 8
Visual Concepts
Balancing a Chemical Equation by Inspection
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Chapter 8
Section 2 Balancing Chemical
Equations
Balancing Equations
Sample Problem A
Balance the equation for the reaction of iron(III) oxide
with hydrogen to form iron and water.
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Chapter 8
Section 2 Balancing Chemical
Equations
Balancing Equations
Sample Problem A Solution
1. Identify reactants and products.
reactants
products
Fe2O3 + 3 H2  2 Fe + 3 H2O
2. Count atoms
Reactants
Products Balanced?
Fe2O3 + H2
Fe + H2O
Iron atoms
2
1
no
Oxygen atoms
3
1
no
Hydrogen atoms
2
2
yes
Unbalanced formula equation
3. Insert coefficients.
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Chapter 8
Section 2 Balancing Chemical
Equations
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
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Chapter 8
Section 2 Balancing Chemical
Equations
Reactions Conserve Mass
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Chapter 8
Section 2 Balancing Chemical
Equations
Polyatomic Ions can be balanced as a group
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Chapter 8
Section 2 Balancing Chemical
Equations
Balancing Equations
Sample Problem C
Aluminum reacts with arsenic acid, HAsO3, to form H2
and aluminum arsenate. Write a balanced equation for
this reaction.
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Chapter 8
Section 2 Balancing Chemical
Equations
Balancing Equations
Sample Problem C Solution
1. Identify reactants and products.
reactants
products
2 Al + 6HAsO3  3H2 + 2 Al(AsO3)3
2. Count Atoms
Reactants
Products
Al + HAsO3
H2 + Al(AsO3)3
Iron atoms
1
1
yes
Oxygen atoms
1
2
no
Hydrogen atoms
1
3
no
Unbalanced formula equation
Balanced?
3. Insert coefficients
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Chapter 8
Section 3 Classifying Chemical
Reactions
Bellringer
• Describe the following terms.
• synthesis
• decomposition
• displacement
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Chapter 8
Section 3 Classifying Chemical
Reactions
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.
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Chapter 8
Section 3 Classifying Chemical
Reactions
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.
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Chapter 8
Section 3 Classifying Chemical
Reactions
Combustion Reactions
• A combustion reaction is a reaction of a carbonbased compound with oxygen.
Combustion of propane:
C3H8 + 5O2  3CO2 + 4H2O
Combustion of ethanol:
CH3CH2OH + 3O2  2CO2 + 3H2O
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Chapter 8
Visual Concepts
Combustion Reaction
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Chapter 8
Section 3 Classifying Chemical
Reactions
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)
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Chapter 8
Visual Concepts
Synthesis Reactions
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Chapter 8
Section 3 Classifying Chemical
Reactions
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
2H2O(l)
electricity
O2(g) + 2H2(g)
• A metal carbonate decomposes to form a metal
oxide and carbon dioxide.
CaCO3(s)
heat
CaO(s) + CO2(g)
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Chapter 8
Visual Concepts
Decomposition Reaction
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Chapter 8
Visual Concepts
Electrolysis
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Chapter 8
Section 3 Classifying Chemical
Reactions
Decomposition Reactions, continued
Sample Problem D
Predicting Products
Predict the product(s) and write a balanced equation
for the reaction of potassium with chlorine.
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Chapter 8
Section 3 Classifying Chemical
Reactions
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
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Chapter 8
Section 3 Classifying Chemical
Reactions
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.
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Chapter 8
Visual Concepts
Single Displacement Reaction
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Chapter 8
Section 3 Classifying Chemical
Reactions
Displacement Reactions, continued
• The activity series ranks the reactivity of elements
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Chapter 8
Visual Concepts
Activity Series
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Chapter 8
Section 3 Classifying Chemical
Reactions
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.
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Chapter 8
Section 3 Classifying Chemical
Reactions
Displacement Reactions, continued
Sample Problem E Solution
1. Identify the reactants.
Magnesium will attempt to displace lead from
lead(II) nitrate.
2. Check the activity series.
Magnesium is more active than lead and displaces
it.
3. Write the balanced equation.
Mg + Pb(NO3)2  Pb + Mg(NO3)2
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Chapter 8
Section 3 Classifying Chemical
Reactions
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)
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Chapter 8
Visual Concepts
Double-Displacement Reaction
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Chapter 8
Visual Concepts
Precipitation Reaction
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Chapter 8
Identifying
Reactions and
Predicting Products
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Chapter 8
Section 4 Writing Net Ionic
Equations
Bellringer
• Write a definition for the word spectator in terms
of the part spectators play in a sporting event.
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Chapter 8
Section 4 Writing Net Ionic
Equations
Objectives
• Write total ionic equations for reactions in aqueous
solutions.
• Identify spectator ions and write net ionic equations
for reactions in aqueous solutions.
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Chapter 8
Section 4 Writing Net Ionic
Equations
Ionic Equations, continued
• Ionic compounds dissolve in water
KI(aq) = K+(aq) + I–(aq)
Pb(NO3)2(aq) = Pb2+(aq) + 2NO3(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) + 2NO3 (aq)
 PbI2(s) + 2K+(aq) + 2NO3 (aq)
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Chapter 8
Section 4 Writing Net Ionic
Equations
Ionic Equations, continued
• Spectator ions remain unchanged in the solution as
aqueous ions. They do not react.
2K+(aq) + 2I–(aq) + Pb2+(aq) + 2NO3(aq)
 PbI2(s) + 2K+(aq) + 2NO3 (aq)
• The net ionic equation is the chemical equation that
shows only the net change.
2I–(aq) + Pb2+(aq)  PbI2(s)
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Chapter 8
Visual Concepts
Net Ionic Equation
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Chapter 8
Section 4 Writing Net Ionic
Equations
Ionic Equations, continued
• Net Ionic equations can be used for displacement
reactions.
Zn(s) + Cu2+(aq) + SO24 (aq)
 Cu(s) + Zn2+(aq) + SO2(aq)
4
• net ionic equation
• Zn(s) + Cu2+(aq)  Cu(s) + Zn2+(aq)
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Chapter 8
Section 4 Writing Net Ionic
Equations
Ionic Equations, continued
• Check atoms and charge to balance net ionic
equations.
SO24 (aq) + Ba2+(aq)  BaSO4(s)
Charge:
(2–) + (2+) = 0
0
Zn(s) + Cu2+(aq)  Cu(s) + Zn2+(aq)
Charge:
2+
2+
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Chapter 8
Writing a Net Ionic Equation
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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
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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
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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.
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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.
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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
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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
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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)
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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)
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Chapter 8
Standardized Test Preparation
Understanding Concepts
5. Differentiate between formula equations and balanced
chemical equations.
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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.
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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
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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
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Chapter 8
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.
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Chapter 8
Standardized Test Preparation
Reading Skills
7. What evidence is there that a chemical reaction has
occurred?
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Chapter 8
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.
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Chapter 8
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
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Chapter 8
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
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Chapter 8
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
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Chapter 8
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
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Chapter 8
Standardized Test Preparation
Interpreting Graphics
The table below shows the reactivity of selected
elements. Use it to answer questions 10 through 12.
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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
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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
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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
chloride
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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
chloride
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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
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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
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