Download Part A Completion

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Name ___________________________
Date ___________________
Class __________________
THE MEANING OF OXIDATION
20.1 AND REDUCTION
Section Review
Objectives
• Define oxidation and reduction in terms of the loss or gain of oxygen or hydrogen
and the loss or gain of electrons
• State the characteristics of a redox reaction and identify the oxidizing agent and
reducing agent
Vocabulary
• oxidation-reduction reactions
• redox reactions
• oxidation
• reduction
• reducing agent
• oxidizing agent
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
© Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved.
1
, reactions are an important
1.
category of chemical reactions. Oxidation is considered to be any
2.
Oxidation–reduction, or
shift of electrons
2
from an atom. Reduction includes any
3.
shift of electrons
3
an atom. An oxidation reaction is always
4.
reaction. The substance that does the
5.
accompanied by a
oxidizing (the
the reducing (the
4
5
agent) is
7
agent) is
6
. The substance that does
8
.
6.
7.
8.
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 9. Reduction is the complete or partial gain of electrons by a substance.
________ 10. In the reaction 2Na ! Cl2 y 2NaCl, sodium is the reducing agent.
________ 11. In the reaction 2Na ! Cl2 y 2NaCl, sodium is being reduced.
Chapter 20 Oxidation-Reduction Reactions
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________ 12. To protect an iron ship hull, you should attach a metal that is easily
reduced.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A
Column B
________ 13. combustion
a. a metal that loses electrons easily
________ 14. oxidation
b. complete or partial loss of electrons or gain of oxygen
________ 15. oxidizing agent
c. oxidation of metals to metallic ions by oxygen and
water in the environment
________ 16. corrosion
d. a metal that resists corrosion
________ 17. zinc
e. a chemical change in which oxygen reacts with
another substance, often producing energy in the
form of heat and light
________ 18. gold
f. a substance that accepts electrons in a redox reaction
Part D Questions and Problems
Answer the following in the space provided.
19. Define oxidation and reduction in terms of the loss or gain of electrons.
21. Explain how putting a block of zinc or aluminum on the iron hull of a large ship
will protect the ship from corrosion.
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20. In the equation given, identify the substance oxidized, the substance reduced,
the oxidizing agent, and the reducing agent.
Zn ! Cu2! y Zn2! ! Cu
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20.2
Date ___________________
Class __________________
OXIDATION NUMBERS
Section Review
Objectives
• Determine the oxidation number of an atom of any element in a pure substance
• Define oxidation and reduction in terms of a change in oxidation number, and
identify atoms being oxidized or reduced in redox reactions
Vocabulary
• oxidation number
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
The oxidation number of an element in an uncombined state
1
is
. The oxidation number of a monatomic ion is the same
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in magnitude and
2
as its ionic
3
. The sum of the
4
. In a polyatomic ion, however, the sum is equal to the
5
. Oxidation numbers help you keep track of
transfer in redox reactions. An oxidation number increase is
7
, while a
8
2.
3.
4.
oxidation numbers of the elements in a neutral compound is
6
1.
–
5.
6.
7.
8.
is reduction.
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 9. Oxygen is more electronegative than chlorine.
________ 10. The oxidation number of each oxygen atom in most compounds is !2.
________ 11. The oxidation number of Cl in KClO3 is !1.
________ 12. The oxidation number of each hydrogen atom in most compounds is !1.
________ 13. The oxidation number for copper in a copper penny is "2.
Chapter 20 Oxidation-Reduction Reactions
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________ 14. In the reaction C ! H2O y CO ! H2, the oxidation number of the
hydrogen doesn’t change.
________ 15. In the reaction C ! H2O y CO ! H2, the oxidation number of the
carbon increases.
________ 16. An increase in the oxidation number of an atom indicates oxidation.
Part C Matching
Match the oxidation number of nitrogen in each formula in Column B to the correct
oxidation number in Column A.
Column A
Column B
a. N2
________ 18. "2
b. HNO3
________ 19. "1
c. NO
________ 20. 0
d. NH2OH
________ 21. !1
e. NH3
________ 22. !2
f. N2O3
________ 23. !3
g. N2O
________ 24. !4
h. N2H4
________ 25. !5
i. NO2
Part D Questions and Problems
Answer the following in the space provided.
26. Define oxidation and reduction in terms of a change in oxidation number.
27. Use the change in oxidation number to determine which elements are oxidized
and which are reduced in these reactions. (Note: It is not necessary to use
balanced equations.)
a. HNO3 ! HBr y NO ! Br2 ! H2O
b. KMnO4 ! HCl y MnCl2 ! Cl2 ! H2O ! KCl
c. Sb ! HNO3 y Sb2O5 ! NO ! H2O
d. C ! H2SO4 y CO2 ! SO2 ! H2O
520
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________ 17. "3
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BALANCING REDOX REACTIONS
20.3
Section Review
Objectives
• Balance a redox equation using the oxidation-number-change method
• Balance a redox equation by breaking a redox equation into oxidation and
reduction half-reactions and then using the half-reaction method
Vocabulary
• oxidation-number-change method
• half-reaction
• half-reaction method
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced is this section. Each blank can be completed with a term, short
phrase, or number.
1.
One method for balancing redox equations involves
1
of the substances that are
2.
oxidized and reduced. Coefficients are then used to make the
3.
increase in oxidation number equal to the decrease.
4.
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determining the change in
The
2
method is another way to write a
3
4
equation for a redox reaction. In this method, the net
equation is divided into
5
5.
6.
half-reactions. Each half-reaction
is balanced independently. Finally, the half-reactions are
6
7.
.
The half-reaction method is particularly useful in balancing
equations for
7
reactions.
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 8. The reduction half-reaction in the reaction MnO4!" Cl! y Mn2" "
Cl2 involves MnO4! y Mn2"
Chapter 20 Oxidation-Reduction Reactions
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________ 9. In an oxidation half-reaction, electrons occur on the right side of the
equation.
________ 10. Electrons never appear in a balanced redox reaction.
________ 11. 2e! " 2Cl! y Cl2 is a balanced half-reaction.
________ 12. To balance the oxygen in a half reaction involving MnO4! y Mn2",
2H2O will be added to the product side of the equation.
________ 13. In the equation 2FeBr2 " Br2 y 2FeBr3, the oxidation number of the
iron doesn’t change.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A
Column B
a. ions that are present but do not participate in or
change during the reaction
________ 15. spectator ions
b. Fe2" y Fe3" " e!
________ 16. anions
c. balancing a redox equation by first balancing the
oxidation and reduction half-reactions
________ 17. oxidation half-reaction
d. balancing a redox equation by comparing the increase
and decrease in oxidation numbers
________ 18. half-reaction
e. equation showing either the reduction or the oxidation
of a species in an oxidation-reduction reaction
________ 19. oxidation-numberchange method
f. ions that can serve as reducing agents
________ 20. reduction half-reaction
g. 2e! " Br2 y 2Br!
Part D Questions and Problems
Answer the following in the space provided.
21. Balance these redox equations using the oxidation-number-change method.
a. HNO3(aq) " HI(g) y NO(g) " I2(s) " H2O
b. HNO3(aq) " I2(s) y HIO3(aq) " NO2(g) " H2O(l)
22. Balance these redox equations using the half-reaction method.
a. H2S(aq) " HNO3(aq) y S(s) " NO(g) " H2O(l)
b. Fe2" " Cr2O72! y Fe3" " Cr3"
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________ 14. half-reaction method
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20
Date ___________________
Class __________________
OXIDATION-REDUCTION REACTIONS
Practice Problems
In your notebook, solve the following problems.
SECTION 20.1 THE MEANING OF OXIDATION AND REDUCTION
Determine what is oxidized and what is reduced in each reaction. Identify the
oxidizing agent and the reducing agent.
1. 2Sr ! O2 y 2SrO
2. 2Li ! S y 2Li2S
3. 2Cs ! Br2 y 2CsBr
4. 3Mg ! N2 y Mg3N2
5. 4Fe ! 3O2 y 2Fe2O3
6. Cl2 ! 2NaBr y 2NaCl ! Br2
7. Si ! 2F2 y SiF4
8. 2Ca ! O2 y 2CaO
9. Mg ! 2HCl y MgCl2 ! H2
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10. 2Na ! 2H2O y 2NaOH ! H2
SECTION 20.2 OXIDATION NUMBERS
1. Give the oxidation number of each kind of atom or ion.
a. Sn
c. S2"
e. Se
g. Sn4!
b. K!
d. Fe3!
f. Mg2!
h. Br"
2. Calculate the oxidation number of chromium in each of the following formulas.
a. Cr2O3
b. H2Cr2O7
c. CrSO4
d. CrO42"
3. Use the changes in oxidation number to determine which elements are oxidized
and which are reduced in these reactions. (Note: It is not necessary to use
balanced reactions.)
a. C ! H2SO4 y CO2 ! SO2 ! H2O
b. HNO3 ! HI y NO ! I2 ! H2O
c. KMnO4 ! HCl y MnCl2 ! Cl2 ! H2O ! KCl
d. Sb ! HNO3 y Sb2O5 ! NO ! H2O
4. For each reaction in problem 3 above, identify the oxidizing agent and reducing
agent.
Chapter 20 Oxidation-Reduction Reactions
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SECTION 20.3 BALANCING REDOX EQUATIONS
1. Balance these equations using the oxidation-number-change method.
a. C ! H2SO4 y CO2 ! SO2 ! H2O
b. H2S ! HNO3 y S ! NO ! H2O
c. HNO3 ! HI y NO ! I2 ! H2O
d. Sb ! HNO3 y Sb2O5 ! NO ! H2O
e. KMnO4 ! HCl y MnCl2 ! Cl2 ! H2O ! KCl
f. KIO4 ! KI ! HCl y KCl ! I2 ! H2O
g. Zn ! Cr2O72" ! H! y Zn2! ! Cr3! ! H2O
2. Write half-reactions for the oxidation and reduction processes for each of the
following reactions.
a. Fe2! ! MnO4" y Fe3! ! Mn2! (acidic solution)
b. Sn2! ! IO3" y Sn4! ! I" (acidic solution)
c. S2" ! NO3" y S ! NO (acidic solution)
d. Mn2! ! H2O2 y MnO2 ! H2O (basic solution)
3. Balance these reactions using the half-reaction method.
a. Zn ! HgO y ZnO22" ! Hg (basic solution)
b. Fe2! ! MnO4" y Fe3! ! Mn2! (acidic solution)
c. Sn2! ! IO3" y Sn4" ! I" (acidic solution)
d. S2" ! NO3" y S ! NO (acidic solution)
e. Mn2! ! H2O2 y MnO2 ! H2O (basic solution)
524
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f. CrO2 ! ClO" y CrO42" ! Cl" (basic solution)
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ELECTROCHEMICAL CELLS
21.1
Section Review
Objectives
• Use the activity series to identify which metal in a pair is more easily oxidized
• Identify the source of electrical energy in a voltaic cell
• Describe current technologies that use electrochemical processes to produce
electrical energy
Vocabulary
•
•
•
•
electrochemical process
electrochemical cell
voltaic cells
half-cell
•
•
•
•
• dry cell
• battery
• fuel cells
salt bridge
electrode
anode
cathode
Part A Completion
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Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
1.
Chemical processes can release or absorb energy. Any
2.
conversion between chemical energy and electrical is known as an
1
3.
. These processes always involve spontaneous redox
reactions in which a transfer of
2
4.
occurs. Electrochemical
cells that generate electrical energy are known as
3
5.
.
6.
The half-cells of an electrochemical cell are separated by a
porous plate or
4
7.
. This barrier prevents the contents of the
two half-cells from mixing, but permits the passage of
5
between the half-cells. Electrons are transferred through an external
circuit from the
the
7
6
, the electrode where oxidation occurs, to
, the electrode where reduction occurs.
Chapter 21 Electrochemistry
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Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 8. Nickel is below mercury in the activity series of metals.
________ 9. The reduction half-reaction in a voltaic cell occurs at the cathode.
________ 10. In a flashlight battery, the anode is the graphite rod.
________ 11. A salt bridge is part of a voltaic cell.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A
Column B
a. the electrode at which oxidation occurs
________ 13. voltaic cells
b. a group of voltaic cells that are connected together
________ 14. cathode
c. a voltaic cell in which a fuel substance undergoes oxidation
to continuously produce electrical energy
________ 15. battery
d. the electrode at which reduction occurs
________ 16. fuel cell
e. any device that converts chemical energy into electrical
energy or electrical energy into chemical energy
________ 17. electrochemical cell
f. electrochemical cells used to convert chemical energy into
electrical energy
________ 18. anode
g. a commercial voltaic cell in which the electrolyte is a moist
paste
Part D Problem
Answer the following in the space provided.
19. Describe the voltaic cell represented as
Mg(s) | MgSO4(aq) || PbSO4(aq) | Pb(s)
Sketch a diagram of the cell similar to the one shown in Figure 21.3 of
your textbook. Label the cathode and anode, and indicate the direction
of electron flow.
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________ 12. dry cell
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21.2
Date ___________________
Class __________________
HALF-CELLS AND CELL POTENTIALS
Section Review
Objectives
•
•
•
•
Identify the origin of the electrical potential of a cell
Explain the value of the standard reduction potential of the hydrogen half-cell
Describe how the standard reduction potential of a half-cell is determined
Interpret the meaning of a positive standard cell potential
Vocabulary
• electrical potential
• reduction potential
• standard hydrogen
• cell potential
• standard cell potential
electrode
Key Equation
E0cell ! E0red " E0oxid
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Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
1.
The measure of a voltaic cell’s ability to produce an electric
current is called its
1
, which is usually measured in volts. The
2
electrical potential of a cell results from a competition for
3.
between the two half-cells. The difference between the reduction
potentials of the two half-cells is called the
3
4.
5.
.
In comparing standard cell potentials for half-reactions, the
4
2.
5
serves as a reference and is assigned a value of
.
6.
7.
A negative value for the standard reduction potential means that
the tendency for this half-cell to be reduced is
6
than the
tendency for hydrogen ions to be reduced. If the calculated
standard cell potential for a given redox reaction is positive, then
the reaction is
7
.
Chapter 21 Electrochemistry
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Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 8. The half-cell that has a greater tendency to acquire electrons will be the
one in which oxidation occurs.
________ 9. In an electrochemical cell, the hydrogen half-cell is the reduction
half-cell.
________ 10. A positive value for a standard reduction potential means hydrogen ions
have a greater tendency to be reduced than the ions in this half-cell.
________ 11. If the cell potential for a given redox reaction is negative, the reaction is
spontaneous.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A
Column B
a. the difference between the reduction potentials of the
two half-cells
________ 13. reduction potential
b. the measure of a cell’s ability to produce an electric
current
________ 14. spontaneous reaction
c. the standard reduction potential of the hydrogen
electrode
________ 15. 0.00 V
d. the tendency of a given half-reaction to occur as a
reduction
________ 16. cell potential
e. standard reduction potential for the oxidation half-cell
________ 17. E0oxid
f. a reaction having a positive cell potential
Part D Problem
Answer the following in the space provided.
18. Compute the standard cell potential of a Mg | Mg2! || Cl2 | Cl" cell, using
standard electrode potentials.
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________ 12. electrical potential
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Name ___________________________
21.3
Date ___________________
Class __________________
ELECTROLYTIC CELLS
Section Review
Objectives
•
•
•
•
Distinguish between electrolytic and voltaic cells
Describe the process of electrolysis of water
Describe the process of electrolysis of brine
Explain how electrolysis is used in metal processing
Vocabulary
• electrolysis
• electrolytic cell
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
1.
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The process in which electrical energy is used to make a
1
nonspontaneous redox reaction go forward is called
3
2
.
3.
flow from the anode
4.
apparatus in which this process is carried out is called an
In this type of cell, as in voltaic cells,
2.
. The
5.
to the cathode through an external circuit. In an electrolytic cell,
electrons are driven by an outside power source such as a
5
4
.
6.
must
7.
be added to enable the water to conduct electricity. The products
8.
In the electrolysis of water, a small amount of
of the electrolysis of water are
6
and
7
. During the
electrolysis of brine, chloride ions are oxidized to produce chlorine
gas at the anode, and water is reduced to produce
8
at the cathode.
Chapter 21 Electrochemistry
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Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 9. During the electrolysis of brine, sodium metal is produced at the
cathode.
________ 10. An electrolytic cell drives a nonspontaneous reaction to completion.
________ 11. When a current is applied via two electrodes in water, oxygen and
hydrogen are produced.
________ 12. An object that is to be electroplated needs to be the cathode of the
electrolytic cell.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A
Column B
a. an electrolytic method for obtaining ultrapure metals
________ 14. electrolytic cell
b. the process in which electrical energy is used to make a
nonspontaneous reaction go forward
________ 15. brine
c. the deposition of a thin layer of metal on an object in an
electrolytic cell
________ 16. electroplating
d. an electrochemical cell used to cause a chemical change
through the application of electrical energy
________ 17. electrorefining
e. a concentrated solution of sodium chloride
Part D Questions and Problems
Answer the following in the space provided.
18. Distinguish between electrolytic and voltaic cells and list some applications
of each.
19. Sketch an electrolytic cell that could be used to silverplate a teaspoon. Label the
anode, cathode, and the direction of electron flow. Write the anode and cathode
reactions that occur.
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________ 13. electrolysis
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Date ___________________
Class __________________
ELECTROCHEMISTRY
Practice Problems
Use Table 21.2 to solve the following problems in your notebook.
SECTION 21.2 HALF-CELLS AND CELL POTENTIALS
1. Determine the cell reaction, the standard cell potential (E0cell) and the half-cell
that acts as the cathode for the voltaic cells composed of the following half-cells.
a. Mg2!(aq) ! 2e" y Mg(s)
Cl2(g) ! 2e" y 2Cl"(aq)
b. Ni2!(aq) ! 2e" y Ni(s)
Ag! (aq) ! e" y Ag(s)
c. MnO4"(aq) ! 8H!(aq) ! 5e" y Mn2!(aq) ! 4H2O (l)
Cd2!(aq) ! 2e" y Cd(s)
d. Br2(l)! 2e" y 2Br"(aq)
Na!(aq) ! e" y Na(s)
e. 2H!(aq) ! 2e" y H2(g)
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MnO2(s) ! 4H!(aq) ! 2e" y Mn2! (aq) ! 2H2O(l)
2. Calculate E0cell to determine whether the following redox reactions are
spontaneous as written.
a. Sn2!(aq) ! Ba(s) y Sn(s) ! Ba2!(aq)
b. 2Ag!(aq) ! 2Cl"(aq) y 2Ag(s) ! Cl2(g)
c. Zn(s) ! F2(g) y 2F"(aq) ! Zn2!(aq)
d. 2Li(s) ! Co2! (aq) y 2Li!(aq) ! Co(s)
e. 2I"(aq) ! K!(aq) y I2(s) ! K(s)
Chapter 21 Electrochemistry
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HYDROCARBONS
22.1
Section Review
Objectives
• Describe the relationship between number of valence electrons and bonding
in carbon
• Define and describe alkanes
• Relate the polarity of hydrocarbons to their solubility
Vocabulary
• hydrocarbons
• alkanes
• straight-chain alkanes
• homologous series
• condensed structural
formulas
• substituent
• alkyl group
• branched-chain alkane
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
1
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The branch of chemistry that deals with
is called
2
chemistry. Organic compounds that contain
only carbon and hydrogen are
4
3
. Carbon always forms
carbons can be arranged in a
7
6
5
10
9
3.
5.
chain or in a chain that
6.
. A hydrocarbon substituent is called an
8
7.
chain of carbons in the molecule. This chain is the
structure.
2.
bonds. The
group. The first step in naming branched-chain alkanes is to find
the
1.
4.
covalent bonds.
Alkanes contain only carbon-carbon
has
compounds
8.
9.
10.
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 11. Because a carbon atom contains 6 valence electrons, it forms 3
covalent bonds.
Chapter 22 Hydrocarbon Compounds
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________ 12. Straight-chain alkanes contain 10 carbon atoms.
________ 13. A substituent can take the place of a hydrogen atom on a parent
hydrocarbon molecule.
________ 14. Hydrocarbon structural formulas are numbered from right to left.
________ 15. When naming branched-chain hydrocarbons, the names of the
substituent alkyl groups are listed in alphabetical order.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A
Column B
________ 16. hydrocarbons
a. hydrocarbons that contain only single covalent bonds
________ 17. alkanes
b. a hydrocarbon substituent
________ 18. straight-chain alkanes
c. alkanes that contain one or more alkyl substituents
________ 19. substituent
d. organic compounds that contain only carbon and
hydrogen
________ 20. alkyl group
e. alkanes that contain any number of carbons one after
another in a chain
________ 21. branched-chain alkanes
f. atom or group of atoms that take the place of a
hydrogen atom in a hydrocarbon molecule
Answer the following in the space provided.
22. Name this compound, using the IUPAC system.
CH3
@
CH3 2 C 2 CH2 2 CH3
@
CH3
23. a. What is the total number of single bonds in a molecule of pentane, C5H12?
b. What is the total number of single bonds in a molecule of
2,2-dimethylpropane?
24. Write the structural formula for 3-ethyl-2,2,5-trimethyloctane.
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Part D Questions and Problems
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Name ___________________________
22.2
Date ___________________
Class __________________
UNSATURATED HYDROCARBONS
Section Review
Objectives
• Describe the difference between unsaturated and saturated hydrocarbons
• Distinguish the structures of alkenes and alkynes
Vocabulary
• saturated compounds
• unsaturated compounds
• alkenes
• alkynes
• aliphatic hydrocarbons
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
1
Alkenes are
hydrocarbons. That is, they contain one
2
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or more carbon-carbon
2.
bonds. Alkynes are also
unsaturated compounds. They contain one or more carboncarbon
3
bonds. Rotation is restricted about the multiple
Alkenes are named by finding the
5
corresponding
6
3.
4.
5.
bonds of alkenes and alkynes.
molecule that contains a
1.
4
chain in the
bond. The root name of the
7
is used, plus the ending
are numbered so that the carbon atoms of the
8
6.
7.
. Atoms
8.
have the
9.
lowest possible numbers. Alkynes are named in the same way,
except that the ending
9
is added to the alkane root.
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 10. An alkane with one or more alkyl groups is called an alkyne.
________ 11. Hydrocarbons are saturated.
Chapter 22 Hydrocarbon Compounds
569
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Date ___________________
Class __________________
________ 12. Parent alkene chains are numbered so that the carbons of the double
bond have the lowest possible numbers.
________ 13. Unsaturated hydrocarbons contain double bonds.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A
Column B
________ 14. unsaturated compounds
a. contain at least one carbon-carbon double bond
________ 15. saturated compounds
b. contain at least one carbon-carbon triple bond
________ 16. alkenes
c. organic compounds that contain double or triple
carbon-carbon bonds
________ 17. alkynes
d. hydrocarbons that contain the maximum number of
hydrogen atoms per carbon atom
Part D Questions and Problems
Answer the following in the space provided.
18. Name this compound using the IUPAC system.
CH3 2 CH2 CH3
@
@
CH2 2 C 3 CH 2 CH3
CH3 2 CH 2 CH 2 CH 2 CH 2 CH2 2 CH2 2 CH2 2 CH3
@
@
@
@
CH3 CH3 CH3 CH3
20. Name the following compound, using the IUPAC system.
H
@
H2C
@
H
H
@
H2 C2 H
@
H2C2H
@
22 C 22
@
H
H H H
@
@
@
C2C3C2H
@
H
21. Draw the structural formula for the following compound.
7-ethyl-2,4,9-trimethyl-5-decyne.
570
Core Teaching Resources
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19. Name this compound, using the IUPAC system.
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Name ___________________________
Date ___________________
Class __________________
ISOMERS
22.3
Section Review
Objectives
• Explain why structural isomers have different properties
• Describe the conditions under which geometric isomers are possible
• Identify optical isomers
Vocabulary
• isomers
• structural isomers
• stereoisomers
• geometric isomers
• trans configuration
• cis configuration
• asymmetric carbon
• optical isomers
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
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Isomers have the same
molecular
isomer of
4
2
3
1
formula but different
. For example, 2–methylpropane is a structural
2.
. Isomers are different compounds with different
3.
4.
.
5
isomers differ in the orientation of groups around
a double bond. The two possible double-bond configurations are
the
6
configuration and the
7
Geometric isomers are one type of
9
which is called an
10
cannot be
12
6.
7.
8
8.
. The other type
carbon. Isomers with an asymmetric
9.
10.
11.
isomers.
Models of optical isomers are like
5.
configuration.
contains a carbon atom with four different groups attached,
carbon are
1.
11
images, which
12.
.
Chapter 22 Hydrocarbon Compounds
571
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Date ___________________
Class __________________
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 13. Structural isomers are compounds with identical molecular structures.
________ 14. Compounds containing double bonds have cis, trans isomers.
________ 15. Isomers with the atoms joined in the same order are structural isomers.
________ 16. A carbon with four different groups attached is an asymmetric carbon.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A
Column B
a. a carbon with four different groups attached
________ 18. structural isomers
b. configuration with substituted groups on the same side of
the double bond
________ 19. stereoisomers
c. isomers that differ in the concentration of groups around
a double bond
________ 20. geometric isomers
d. molecules in which the atoms are joined in the same
order, but the arrangements of the atoms in space are
different
________ 21. trans configuration
e. compounds that have the same molecular formula, but
the atoms are joined in a different order
________ 22. cis configuration
f. configuration with substituted groups on opposite sides
of the double bond
________ 23. asymmetric carbon
g. pairs of molecules that differ only in the way four
different groups are arranged around a central carbon
atom
________ 24. optical isomers
h. compounds that have the same molecular formula but
different molecular structures
572
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________ 17. isomers
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Name ___________________________
Date ___________________
Class __________________
Part D Problems
Answer the following in the space provided.
25. Draw three structural isomers of pentane.
26. Identify the asymmetric carbon in this compound.
H
@2 1
CH3 2 CH2 2 CH2 2 C 2 CH3
@
F
5
4
3
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27. Draw the cis and trans isomers for 3-hexene.
Chapter 22 Hydrocarbon Compounds
573
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Date ___________________
Class __________________
HYDROCARBON RINGS
22.4
Section Review
Objectives
• Identify cyclic ring structures
• Describe bonding in benzene
Vocabulary
• cyclic hydrocarbons
• aromatic compound
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
1
Compounds with hydrocarbon rings are called
2
hydrocarbons. Benzene is the simplest form of an
compound. The benzene molecule consists of
4
3
2.
carbons
atom attached to each carbon.
Two different structures can be written for benzene in which
5
6
7.
7
8.
is also called toluene, while the dimethylbenzenes are known as
8
. 1,2–disubstitution on a benzene ring is also know as
9
disubstitution, while 1,3 is known as
574
11
disubstitution.
Core Teaching Resources
5.
structures.
Many substituted benzenes have common names.
known as
4.
6.
and single bonds alternate. The actual bonding in
benzene does not alternate between the
3.
10
, and 1,4 is
9.
10.
11.
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joined in a ring with a
1.
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Name ___________________________
Date ___________________
Class __________________
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 12. Aromatic compounds contain 6 carbon atoms.
________ 13. Benzene is the simplest arene.
________ 14. Compounds that contain rings are aromatic hydrocarbons.
________ 15. Another name for 1,3-dimethylbenzene is m-xylene.
________ 16. Aromatic compounds have pleasant odors.
Part C Matching
Match each description in Column B to the correct term in Column A.
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Column A
Column B
________ 17. cyclic hydrocarbons
a. when two or more equally valid structures can be
drawn for a molecule
________ 18. resonance
b. group of hydrocarbons that contain a benzene ring
or a ring with bonding like that of benzene
________ 19. phenyl group
c. name given to a benzene ring when it is a substituent
________ 20. aromatic compounds
d. organic compounds that contain hydrocarbon rings
Part D Problems
Answer the following in the space provided.
21. Draw the structural formula for propylbenzene.
22. Draw the structural formula for 3-phenyl-1-butene.
23. Name the following compounds, using the IUPAC system.
a.
CH2 2 CH2
^
%
CH2
CH2
@
@
CH2
CH2
%
^
CH2 2 CH2
b.
CH2CH3
@
%
CH2CH3
Chapter 22 Hydrocarbon Compounds
575
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Name ___________________________
22
Date ___________________
Class __________________
HYDROCARBON COMPOUNDS
Practice Problems
In your notebook, solve the following problems.
SECTION 22.1 HYDROCARBONS
1. Name this hydrocarbon, according to the IUPAC system.
CH3
CH3
@
@
CH3 2 CH2 2 CH2 2 C 2 CH2 2 C 2 CH3
@
@
CH2
CH2
@
@
CH3
CH3
2. Name this hydrocarbon, according to the IUPAC system.
CH3
CH3
@
@
CH3 2 CH 2 C 2 CH2 2 C 2 CH2 2 CH3
@
@
@
CH3 CH2
CH2
@
CH3
3. Write the structural formula for each of the following compounds.
a. 3-ethyl-2,3-dimethylpentane
c. 2,3,4,5-tetramethylnonane
4. Draw condensed structural formulas for the straight-chain alkanes with seven
and eight carbons.
5. How many single bonds are in a hexane molecule?
SECTION 22.2 UNSATURATED HYDROCARBONS
1. Name this compound, according to the IUPAC system.
CH3
@
CH3 2 C 3 CH 2 CH 2 CH3
@
CH2
@
CH3
2. Name this compound, according to the IUPAC system.
CH3
@
CH 4 C 2 CH 2 CH 2 CH3
@
CH3
578
Core Teaching Resources
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b. 3,4-diethylhexane
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Name ___________________________
Date ___________________
Class __________________
3. Name and draw all of the alkynes with the molecular formula C5H8.
4. Write structural formulas for the following hydrocarbons.
a. 3,5-dimethyl-1-hexene
b. 4-methyl-1-pentene
c. 3,3-dimethyl-1-butyne
SECTION 22.3 ISOMERS
1. Name this compound, according to the IUPAC system.
H
H
^
^
C3C
%
%
CH3
CH2CH3
2. Name this compound, according to the IUPAC system.
CH3 2 CH2
H
%
^
C3C
^
%
H
CH2 2 CH 2 CH3
@
CH3
3. Write the structural formula for trans–2–heptene.
4. Which of the following can exist as cis, trans isomers?
a. 2-butene
b. 1-butene
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c. 2-methyl-2-butene
d. 3-hexene
5. Identify the asymmetric carbon in the following compound.
5
4
3
2
1
CH3 2 CH2 2 CH 2 CH 2 CH3
@
@
CH3 CH3
6. Which of the following compounds have an asymmetric carbon?
a. CH3 2 CH 2 CH 2 CH3
@
@
OH CH3
b. CH3 2 CH 2 CH3
@
CH3
c. CH3 2 CH 2 F
@
OH
Chapter 22 Hydrocarbon Compounds
579
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Date ___________________
Class __________________
SECTION 22.4 HYDROCARBON RINGS
1. Name this compound, according to the IUPAC system.
^ CH2 CH3
@
CH3
2. Name this compound, according to the IUPAC system.
CH3 2 CH 3 CH 2 CH2 2 CH 2 CH3
@
3. Write structural formulas for the following compounds.
a. 1,3-dimethylcyclohexane
b. cis-1,2-diphenylethene
c. 1,4-diethylbenzene
SECTION 22.5 HYDROCARBONS FROM EARTH’S CRUST
1. Write a balanced equation for the complete combustion of 2-methylheptane.
2. Describe three types of fuels obtained by refining petroleum.
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580
Core Teaching Resources
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23.1
Date ___________________
Class __________________
INTRODUCTION TO FUNCTIONAL GROUPS
Section Review
Objectives
• Explain how organic compounds are classified
• Identify the IUPAC rules for naming halocarbons
• Describe how halocarbons can be prepared
Vocabulary
• functional group
• halocarbons
• alkyl halides
• aryl halides
• substitution reaction
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
1.
The chemical reactions of most organic compounds involve
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1
groups. Functional groups are the chemically
2
2.
parts of an organic molecule. Common functional groups include
3
the double and triple carbon-carbon bonds of
4
, respectively.
5
4.
and
5.
are a class of organic compounds
6.
containing one or more covalently bonded halogen atoms.
A common type of organic reaction is a
6
3.
7.
reaction in
which an atom or a group of atoms replaces another atom or group
8.
of atoms. For example, treating methane with bromine in the
9.
presence of a catalyst causes the substitution of a
8
with a
atom
10.
atom. Similarly, halogens on carbon chains are
readily replaced by hydroxide ions to produce an
10
7
9
and a
.
Chapter 23 Functional Groups
601
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Date ___________________
Class __________________
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 11. A functional group is a specific arrangement of atoms in an organic
compound that is capable of characteristic reactions.
________ 12. Many halocarbons are found in nature.
________ 13. A product of a substitution reaction is a hydrogen halide.
________ 14. The common name of CH3CH2CH2Br is propyl bromide.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A
Column B
________ 15. functional group
a. the reaction of chlorine with ethane to produce ethyl
chloride and hydrogen chloride
________ 16. alkyl halide
b. CH3CH2CH2CH2I
________ 17. substitution reaction
c. a class of organic compounds in which one or more
halogen atoms are joined to a carbon of an arene ring
________ 18. aryl halides
d. a specific arrangement of atoms in an organic compound
that is capable of characteristic chemical reactions
Answer the following in the space provided.
19. Identify the functional group in each of the following compounds.
O
a.
c.
OH
#
@
2C2H
CH3 2 C 2 CH3
@
H
b.
O
#
CH3 2 CH2 2 C 2 CH3
d.
O
#
CH3 2 CH2 2 CH2 2 C 2 OH
20. Give the structural formula for each compound.
a. o-chlorotoluene
b. 2,2-dichloropentane
602
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Part D Problems
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Name ___________________________
23.2
Date ___________________
Class __________________
ALCOHOLS AND ETHERS
Section Review
Objectives
•
•
•
•
Identify how alcohols are classified and named
Predict how the solubility of an alcohol varies with the length of its carbon chain
Name the reactions of alkenes that may be used to introduce functional groups
Construct the general structure of an ether and describe how ethers are named
Vocabulary
• alcohol
• hydroxyl group
• fermentation
• denatured alcohol
• addition reaction
• hydration reaction
• hydrogenation reaction
• ether
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
1
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Aliphatic alcohols can be classified as
4
1.
are organic compounds with a hydroxyl group.
2
3
,
2.
, or
alcohols depending on the number of R groups attached
4.
to the carbon with the hydroxyl group. For example, 2-propanol
represents a
5
alcohol. In general, alcohols are more soluble
6
8
7.
.
7
Alcohols can be prepared from alkenes by a
5.
6.
in water than alkanes containing comparable numbers of atoms
because they are capable of intermolecular
3.
reaction.
8.
is added at the carbon-carbon
9.
double bond of the alkene. Another form of addition reaction is
10.
In this type of reaction,
9
11.
. In this reaction, which is catalyzed by platinum or
palladium, hydrogen is added to the carbon-carbon double bonds
in a molecule to produce an
10
12.
.
Organic compounds whose general formula can be written as
R-O-R are called
11
. Ethers usually have
12
boiling
points than alcohols of comparable formula mass.
Chapter 23 Functional Groups
603
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Date ___________________
Class __________________
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 13. The addition of water to an alkene is called a hydration reaction.
________ 14. Hydrogenation of a double bond is an oxidation reaction.
________ 15.
2O2
is an ether.
________ 16. The benzene ring usually undergoes addition rather than substitution.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A
Column B
________ 17. hydration reaction
a. the production of ethanol from sugars by the action of
yeast or bacteria
________ 18. fermentation
b. the reaction of HBr with propene to form
1-bromopropane
________ 19. alcohols
c. the reaction of hydrogen with butene to form butane
________ 20. addition
d. a class of organic compounds whose structures contain
an –OH group
________ 21. hydrogenation
e. the addition of water to an alkene
Answer the following in the space provided.
22. Identify the following compounds as primary, secondary, or tertiary alcohols.
a.
b. CH3 2 CH2 2 OH
OH
@
CH3 2 CH2 2 C 2 CH3
@
CH3
23. Give the structure for the expected organic product from each reaction.
a. CH3
H
%
^
Pt
C3C
! H2 uy
^
%
H
CH3
b. CH3
H
604
%
^
C3C
^
%
H
!
H
! H2O uy
H
Core Teaching Resources
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Part D Problems
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Name ___________________________
23.3
Date ___________________
Class __________________
CARBONYL COMPOUNDS
Section Review
Objectives
•
•
•
•
Identify the structure of a carbonyl group as found in aldehydes and ketones
Construct the general formula for carboxylic acids and explain how they are named
Describe an ester
Explain how dehydration is an oxidation reaction
Vocabulary
• carbonyl group
• aldehydes
• ketones
• carboxylic acid
• carboxyl group
• fatty acids
• esters
• dehydrogenation reaction
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
1
A carbonyl group consists of a carbon atom and an
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atom joined by a
2
3
bond. Aldehydes,
1.
4
,
, and
3.
esters are all classes of organic compounds that contain carbonyl
5
groups. The general formula for an
The general formula of a
6
2.
can be written as RCHO. 4.
5.
can be written as RCOOH.
The simplest aldehyde is methanal, also called
7
6.
.
7.
Methanal is used industrially to manufacture synthetic resins.
8
.
8.
Organic compounds formed from the reaction of a carboxylic acid
9.
Ethanoic, propanoic, and butanoic acids are examples of
with an alcohol are called
9
could be synthesized by reacting
. For example, propyl ethanoate
10
with ethanoic acid.
Carbonyl-containing compounds and alcohols can be
interconverted using
11
10.
11.
12.
reactions. For example, the
primary alcohols methanol and ethanol can be converted to
aldehydes by treating them with acidified
12
.
Chapter 23 Functional Groups
605
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Date ___________________
Class __________________
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 13. Many continuous-chain carboxylic acids are called fatty acids.
________ 14. Benedict’s test is used to detect ketones.
________ 15. The hydrolysis of ethyl butanoate in an acid solution would yield
ethanoic acid and butanol.
________ 16. 2-methyl-2-propanol cannot be oxidized to propanone using acidified
potassium dichromate.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A
Column B
a. a group of atoms that consists of a carbonyl group attached
to a hydroxyl group
________ 18. esters
b. long continuous-chain carboxylic acids isolated from fats
________ 19. ketones
c. the loss of hydrogen
________ 20. fatty acids
d. a derivative of carboxylic acids in which the –OH of the
carbonyl group has be replaced by an –OR from an alcohol
________ 21. carboxyl group
e. organic compounds in which the carbon of the carbonyl
group is joined to two other carbons
Part D Problems
Answer the following in the space provided.
22. Show how alcohols, aldehydes, ketones, and carboxylic acids are related by
oxidation and reduction reactions.
23. Give the IUPAC name for the following compound.
O
#
CH3 CH2 C CH2 CH2 CH3
606
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________ 17. dehydrogenation
reaction
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Name ___________________________
Date ___________________
Class __________________
POLYMERIZATION
23.4
Section Review
Objectives
• Describe how additional polymers are formed
• Describe how condensation polymers are formed
Vocabulary
• polymer
• monomers
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms
that are introduced in this section. Each blank can be completed with a term, short
phrase, or number.
1
A
is a large molecule formed by the covalent bonding
of repeating smaller molecules.
2
polymerization occurs when 2.
3
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unsaturated monomers react to form a polymer.
polymers
3.
4.
are formed by the head-to-tail joining of monomer units.
4
1.
, formed by the joining of ethene molecules, is an
5.
5
6.
example of an addition polymer.
, formed by the joining of
dicarboxylic acids and dihydroxy alcohols, are examples of
condensation polymers. The physical properties of polymers, such
as hardness and rigidity, depend in part on the
6
of the
carbon chains in the polymer molecules.
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
________ 7. Polymerization reactions require a catalyst.
________ 8. Addition polymers form when unsaturated monomers react to form a
polymer.
Chapter 23 Functional Groups
607
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Name ___________________________
Date ___________________
Class __________________
________ 9. The condensation polymerization of a carboxylic acid with an amine
produces a polyester and water.
________ 10. Various types of nylon are polyamides.
________ 11. The basic repeating unit of polyvinyl chloride could be written as
Cl
@
CH2 2 CH
x
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A
________ 12. polymer
Column B
a.
@
CH2 2 CH
x
b. a large molecule formed by the covalent bonding of
repeating smaller molecules
________ 14. condensation
polymerization
c. polypropylene
________ 15. KevlarTM
d. requires that there be two functional groups on each
monomer molecule
________ 16. polystyrene
e. a tough, flexible, and flame-resistant condensation
polymer used to construct bullet-proof vests
Part D Questions and Problems
Answer the following in the space provided.
17. Show the addition polymerization of ethene to form polyethylene.
18. Describe the characteristics of a polyester. Give an example of a polyester.
608
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________ 13. addition polymer
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Name ___________________________
23
Date ___________________
Class __________________
FUNCTIONAL GROUPS
AND ORGANIC REACTIONS
Practice Problems
In your notebook, solve the following problems.
SECTION 23.1 INTRODUCTION TO FUNCTIONAL GROUPS
1. Identify the functional group in each of the following compounds.
a. CH3
CH3
b.
%
CH 2 O 2 CH2 CH3
^
O
#
CH3 2 CH2 2 CH2 2 C
%
c.
Br
@
CH3 2 CH 2 CH2 2 CH3
d.
CH3
@
CH3 2 C 2 OH
@
CH3
OH
2. What class of organic compounds do each of the following substances belong
to? Write IUPAC names for each structure.
^ Br
a.
b. CH3 CH Cl Br
c. H
H
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@
Br
%
^
C3C
^
%
Cl
H
3. Write the formulas of the expected products for the following reactions.
a. CH3
%
CH 2 CH2 2 CH2 2 Br ! NaOH y
^
CH3
b. CH4 ! 4Cl2
catalyst
JJJJH
4. Give the structural formula for each of the following compounds.
a. 1-bromo-3-ethylbenzene
b. 1-bromo-3,4-dimethylheptane
SECTION 23.2 ALCOHOLS AND ETHERS
1. Write the IUPAC names for each of the following compounds. Classify each
alcohol as primary, secondary, or tertiary.
a. CH3 CH CH2 CH3
@
OH
b. CH3 CH2 2 O 2
c. CH3
CH3
%
CH 2 CH2 2 CH2 2 OH
^
d. CH3CH2CH2CH2CH2OH
Chapter 23 Functional Groups
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05_CTR_ch23 7/12/04 8:19 AM Page 610
Name ___________________________
Date ___________________
Class __________________
2. Write the structural formulas for dipropyl ether, 2-methyl-1-butanol, and
2,3-butanediol. Which of these compounds is expected to be most soluble in
water?
3. Write an equation for the synthesis of
a. 2-chlorobutane from 1-butene and hydrogen chloride
b. bromobenzene from benzene and bromine
4. Classify each of the reactions in problem 3 as an addition or substitution reaction.
SECTION 23.3 CARBONYL COMPOUNDS
1. Write IUPAC names for each of the following compounds.
a.
d.
O
#
C
^ %
O
#
CH3 CH2 CH2 C
H
b.
O
#
CH3 CH2 2 C 2 CH3
c.
CH3 O
@
#
CH3 CH2 C CH2 C
%
e.
%
O CH2 CH3
O
#
2 CH 3 CH 2 C 2 H
OH
2. Write the IUPAC name of the expected product for the reduction of each of the
following compounds.
a. ethanoic acid
c. butanal
3. Write the IUPAC name of the expected product(s) for the oxidation of each of
the following compounds.
a. 2-pentanol
c. butane
b. octanal
4. Write an equation for the synthesis of
a. isopropyl butanoate from isopropanol and butanoic acid
b. butanoic acid from 1-butanol
5. Classify each of the reactions in problem 4 as an oxidation-reduction,
substitution, addition, or esterfication reaction.
SECTION 23.4 POLYMERIZATON
1. Draw the structures of propene (propylene) and tetrafluoroethene. Draw the
basic repeating units when each of these compounds polymerizes. Describe
some practical uses of each polymer.
2. Draw the basic repeating unit of polyethylene terephthalate (PET). Classify PET
as a polyamide or polyester. Is PET a condensation or addition polymer? Explain.
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Core Teaching Resources
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b. propene