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Resources
Chapter Presentation
Bellringer
Transparencies
Sample Problems
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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HW.SECTION REVIEW, pg.266
#(1-10)
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Section 8.1 Review
1. 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.
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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?
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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
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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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Sample Problem A , Practice pg. 269
Write a balanced equation for each of the
following.
1) P4 + O2 → P2O5
2 ) C3H8 + O2 → CO2 + H2O
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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.
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Sample Problem B , Practice pg. 271
Write a balanced chemical equation for each of the
following.
1) C2H2 + O2 → CO2 + H2O
2
5
4
2
2 ) Fe(OH)2 + H2O2 → Fe(OH)3
2
2
3) FeS2 + Cl2 → FeCl3 + S2Cl2
2
5
2
2
3) NH3+ O2 → NO + H2O
4
5
4
6
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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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Sample Problem C , Practice pg. 273
Write a balanced equation for each of the following.
1) 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
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4) Write
each of the following reactions as a word
equation, an unbalanced formula equation, and finally
as a balanced equation.
a) 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.
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Section Review pg. 274
5) Balance the following equations.
a. ZnS + O2 → ZnO + SO2
b. Fe2O3 + CO → Fe + CO2
c. AgNO3 + AlCl3 →AgCl + Al(NO3)3
d. Ni(ClO3)2 → NiCl2 + O2
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Section Review pg. 274
6) Balance the following equations.
a. (NH4)2Cr2O7 → Cr2O3 + N2 + H2O
b. NH3 + CuO → N2 + Cu + H2O
c. Na2SiF6 + Na → Si + NaF
d. C4H10 + O2 → CO2 + H2O
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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
Sample Problem D , practice pg. 279
Predict the product(s) and write a balanced equation for
each of the following reactions.
1) the reaction of butane, C4H10, with oxygen
2)the reaction of water with calcium oxide
3)the reaction of lithium with oxygen
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4)the decomposition of carbonic acid
5) The decomposition of nitrogen triiodide.
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6) The reaction of magnesium oxide and
water.
7) The decomposition of calcium carbonate.
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Homework
Copy and solve the following questions
Predict the product(s) and write a balanced equation for
each of the following reactions.
1. pentane, C5H12, reacting with oxygen.
2. Water reacting with potassium oxide.
3. Calcium reacting with oxygen.
4. The decomposition of sodium chloride.
5. The combustion of octane C8H18.
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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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Sample Problem E, practice pg. 282
For the following situations, write a balanced equation
if a reaction happens. Otherwise write “no reaction.”
1) 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.
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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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Predict the products of the following reations.
a. AgNO3(aq) + K2SO4(aq) →
b. H2SO4(aq) + KOH(aq) →
c. KI(aq) + Pb(NO3)2(aq) →
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Chapter 8
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HOMEWORK
SECTION REVIEW,
pg. 285, # ( 1- 10)
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Section 8.3 Review, pg. 285
8. Balance each of the equations below, and indicate the
type of reaction for each equation.
a. 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)
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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.
a. Ag(s) + H2O(l)
b. Mg(s) + Cu(NO3)2(aq)
c. Al(s) + O2(g)
d. H2SO4(aq) + KOH(aq)
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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.
a. HgO →
b. C3H7OH + O2 →
c. Zn + CuSO4 →
d. BaCl2 + Na2SO4 →
e. Zn + F2 →
f. C5H10 + O2 →
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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) + SO 24 (aq)
 Cu(s) + Zn2+(aq) + SO 24(aq)
• 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.
SO 24 (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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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.
a. Br2(l) + NaI(aq)→ NaBr(aq) + I2(s)
b. Ca(OH)2(aq) + HCl(aq) → CaCl2(aq) + H2O(l)
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c. Mg(s) + AgNO3(aq) → Ag(s) + Mg(NO3)2(aq)
d. AgNO3 + KBr →AgBr + KNO3
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e. Ni(s) + Pb(NO3)2(aq) →Ni(NO3)2(aq) + Pb(s)
f. Ca(s) + H2O(l) → Ca(OH)2(aq) + H2(g)
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HW.
SECTION REVIEW,
Pg. 289, # (8 -11)
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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
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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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Understanding Concepts
3. Of these reaction types, which has only one reactant?
A. decomposition
B. displacement
C. oxidation
D. synthesis
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Understanding Concepts
3. Of these reaction types, which has only one reactant?
A. decomposition
B. displacement
C. oxidation
D. synthesis
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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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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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Understanding Concepts
5. Differentiate between formula equations and balanced
chemical equations.
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Chapter 8
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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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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
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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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Reading Skills
7. What evidence is there that a chemical reaction has
occurred?
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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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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
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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
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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
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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
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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
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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
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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
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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
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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
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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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