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05_CTR_ch20 7/12/04 8:17 AM Page 517 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 517 05_CTR_ch20 7/12/04 8:17 AM Page 518 Name ___________________________ Date ___________________ Class __________________ ________ 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. 518 Core Teaching Resources © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 20. In the equation given, identify the substance oxidized, the substance reduced, the oxidizing agent, and the reducing agent. Zn ! Cu2! y Zn2! ! Cu 05_CTR_ch20 7/12/04 8:17 AM Page 519 Name ___________________________ 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 © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 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 519 05_CTR_ch20 7/12/04 8:17 AM Page 520 Name ___________________________ Date ___________________ Class __________________ ________ 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 Core Teaching Resources © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. ________ 17. "3 05_CTR_ch20 7/12/04 8:17 AM Page 521 Name ___________________________ Date ___________________ Class __________________ 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. © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 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 521 05_CTR_ch20 7/12/04 8:17 AM Page 522 Name ___________________________ Date ___________________ Class __________________ ________ 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" 522 Core Teaching Resources © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. ________ 14. half-reaction method 05_CTR_ch20 7/12/04 8:17 AM Page 523 Name ___________________________ 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 © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 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 523 05_CTR_ch20 7/12/04 8:17 AM Page 524 Name ___________________________ Date ___________________ Class __________________ 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 Core Teaching Resources © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. f. CrO2 ! ClO" y CrO42" ! Cl" (basic solution) 05_CTR_ch21 7/12/04 8:18 AM Page 543 Name ___________________________ Date ___________________ Class __________________ 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 © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 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 543 05_CTR_ch21 7/12/04 8:18 AM Page 544 Name ___________________________ Date ___________________ Class __________________ 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. 544 Core Teaching Resources © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. ________ 12. dry cell 05_CTR_ch21 7/12/04 8:18 AM Page 545 Name ___________________________ 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 © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 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 545 05_CTR_ch21 7/12/04 8:18 AM Page 546 Name ___________________________ Date ___________________ Class __________________ 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. 546 Core Teaching Resources © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. ________ 12. electrical potential 05_CTR_ch21 7/12/04 8:18 AM Page 547 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. © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 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 547 05_CTR_ch21 7/12/04 8:18 AM Page 548 Name ___________________________ Date ___________________ Class __________________ 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. 548 Core Teaching Resources © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. ________ 13. electrolysis 05_CTR_ch21 7/12/04 8:18 AM Page 549 Name ___________________________ 21 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) © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 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 549 05_CTR_ch22 7/12/04 8:19 AM Page 567 Name ___________________________ Date ___________________ Class __________________ 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 © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 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 567 05_CTR_ch22 7/12/04 8:19 AM Page 568 Name ___________________________ Date ___________________ Class __________________ ________ 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. 568 Core Teaching Resources © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. Part D Questions and Problems 05_CTR_ch22 7/12/04 8:19 AM Page 569 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 © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 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 05_CTR_ch22 7/12/04 8:19 AM Page 570 Name ___________________________ 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 © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 19. Name this compound, using the IUPAC system. 05_CTR_ch22 7/12/04 8:19 AM Page 571 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. © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 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 05_CTR_ch22 7/12/04 8:19 AM Page 572 Name ___________________________ 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 Core Teaching Resources © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. ________ 17. isomers 05_CTR_ch22 7/12/04 8:19 AM Page 573 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 © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 27. Draw the cis and trans isomers for 3-hexene. Chapter 22 Hydrocarbon Compounds 573 05_CTR_ch22 7/12/04 8:19 AM Page 574 Name ___________________________ 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. © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. joined in a ring with a 1. 05_CTR_ch22 7/12/04 8:19 AM Page 575 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. © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 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 05_CTR_ch22 7/12/04 8:19 AM Page 578 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 © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. b. 3,4-diethylhexane 05_CTR_ch22 7/12/04 8:19 AM Page 579 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 © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 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 05_CTR_ch22 7/12/04 8:19 AM Page 580 Name ___________________________ 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. © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 580 Core Teaching Resources 05_CTR_ch23 7/12/04 8:19 AM Page 601 Name ___________________________ 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 © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 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 05_CTR_ch23 7/12/04 8:19 AM Page 602 Name ___________________________ 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 Core Teaching Resources © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. Part D Problems 05_CTR_ch23 7/12/04 8:19 AM Page 603 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 © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 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 05_CTR_ch23 7/12/04 8:19 AM Page 604 Name ___________________________ 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 © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. Part D Problems 05_CTR_ch23 7/12/04 8:19 AM Page 605 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 © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 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 05_CTR_ch23 7/12/04 8:19 AM Page 606 Name ___________________________ 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 Core Teaching Resources © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. ________ 17. dehydrogenation reaction 05_CTR_ch23 7/12/04 8:19 AM Page 607 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 © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 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 05_CTR_ch23 7/12/04 8:19 AM Page 608 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 Core Teaching Resources © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. ________ 13. addition polymer 05_CTR_ch23 7/12/04 8:19 AM Page 609 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 © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. @ 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 609 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. 610 Core Teaching Resources © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. b. propene