1. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Balance the following equations: CO (g) + O 2 ( g) --> CO 2 (g) N 2 O 5 (g) + H 2 O (l) --> HNO 3 (aq) PCl 5 (l) + H 2 O (l) --> H 3 PO 4 (aq) + HCl (aq) CH 4 (g) + Br 2 (g) --> CBr 4 (l) + HBr (g) C 5 H 10 O 2 (l) + O 2 (g) --> CO 2 (g) + H 2 O (l) Cr(OH) 3 (s) + HClO 4 (aq) --> Cr(ClO 4 ) 3 (aq) + H 2 O (l) OPENER # - CHAPTER 8 - NOV __, 2012

2. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu S.15.C.6 Identify the physical state for each substance in a reaction equation

3. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Table of Contents Chapter 8 Chemical Equations and Chemical Reactions Section 2 Types of Chemical Reactions

4. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Objectives Define and give general equations for synthesis, decomposition, single-displacement, and double- displacement reactions. Classify a reaction as a synthesis, decomposition, single-displacement, double-displacement, or combustion reaction. List three kinds of synthesis reactions and six kinds of decomposition reactions. Section 2 Types of Chemical Reactions Chapter 8

5. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Objectives, continued List four kinds of single-displacement reactions and three kinds of double-displacement reactions. Predict the products of simple reactions given the reactants. Section 2 Types of Chemical Reactions Chapter 8

6. End Show © Copyright Pearson Prentice Hall 6 Slide of 42 Types of Chemical Reactions The heat and smoke of burning charcoal are the products of a combustion reaction. Combustion is one of the five general types of chemical reactions. If you can recognize a reaction as being a particular type, you may be able to predict the products of the reaction. 8.2

7. End Show © Copyright Pearson Prentice Hall 7 Slide of 42 Types of Chemical Reactions > Classifying Reactions What are the five general types of reactions? 8.2

8. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu There are several ways to classify chemical reactions. Section 2 Types of Chemical Reactions Chapter 8 The classification scheme described in this section provides an introduction to five basic types of reactions: synthesis or combination or composition decomposition single-displacement (or replacement) double-displacement (or replacement) combustion reactions

9. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Synthesis Reactions In a synthesis reaction, also known as a composition or combination reaction, two or more substances combine to form a new compound. This type of reaction is represented by the following general equation. A + X AX Section 2 Types of Chemical Reactions Chapter 8 A and X can be elements or compounds. AX is a compound

10. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Visual Concepts Click below to watch the Visual Concept. Visual Concept Chapter 8 Synthesis Reactions http://my.hrw.com/sh/hc6_003036809x/s tudent/ch08/sec02/vc00/hc608_02_v00fs.htm

11. Synthesis  A + B  AB  + 

12. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Synthesis Reactions, continued Reactions of Elements with Oxygen and Sulfur One simple type of synthesis reaction is the combination of an element with oxygen to produce an oxide of the element. Section 2 Types of Chemical Reactions Chapter 8 Almost all metals react with oxygen to form oxides. Group 2 elements react in a similar manner, forming oxides with the formula MO, where M represents the metal. example: 2Mg(s) + O 2 (g) 2MgO(s)

13. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Synthesis Reactions, continued Reactions of Elements with Oxygen and Sulfur, continued The Group 1 and Group 2 elements react similarly with sulfur, forming sulfides with the formulas M 2 S and MS, respectively. Chapter 8 Section 2 Types of Chemical Reactions The Group 1 metals form oxides with the formula M 2 O. example: Li 2 O 16Rb(s) + S 8 (s) 8Rb 2 S(s) 8Ba(s) + S 8 (s) 8BaS(s)

14. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Synthesis Reactions, continued Reactions of Elements with Oxygen and Sulfur, continued Nonmetals also undergo synthesis reactions with oxygen to form oxides. Section 2 Types of Chemical Reactions Chapter 8 example: Sulfur reacts to form sulfur dioxide. S 8 (s) + 8O 2 (g) 8SO 2 (g) example: Hydrogen reacts with oxygen to form dihydrogen monoxide (water). 2H 2 (g) + O 2 (g) 2H 2 O(g)

15. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Synthesis Reactions, continued Reactions of Metals with Halogens Most metals react with the Group 17 elements, the halogens, to form either ionic or covalent compounds. Section 2 Types of Chemical Reactions Chapter 8 Group 1 metals react with halogens to form ionic compounds with the formula MX, where M is the metal and X is the halogen. example: 2Na(s) + Cl 2 (g) 2NaCl(s)

16. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Synthesis Reactions, continued Reactions of Metals with Halogens, continued Group 2 metals react with the halogens to form ionic compounds with the formula MX 2. Section 2 Types of Chemical Reactions Chapter 8 example: Mg(s) + F 2 (g) MgF 2 (s) Fluorine is so reactive that it combines with almost all metals.

17. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Synthesis Reactions, continued Synthesis Reactions with Oxides Active metals are highly reactive metals. Section 2 Types of Chemical Reactions Chapter 8 Oxides of active metals react with water to produce metal hydroxides. example: Calcium oxide reacts with water to form calcium hydroxide. CaO(s) + H 2 O(l) Ca(OH) 2 (s)

18. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Synthesis Reactions, continued Synthesis Reactions with Oxides, continued Many oxides of nonmetals in the upper right portion of the periodic table react with water to produce oxyacids. Section 2 Types of Chemical Reactions Chapter 8 example: SO 2 (g) + H 2 O(l) H 2 SO 3 (aq) Certain metal oxides and nonmetal oxides react with each other in synthesis reactions to form salts. example: CaO(s) + SO 2 (g) CaSO 3 (s)

19. End Show Slide of 42 © Copyright Pearson Prentice Hall 19 Types of Chemical Reactions > Classifying Reactions Decomposition Reactions A decomposition reaction is a chemical change in which a single compound breaks down into two or more simpler products. 8.2

20. Decomposition  A B  A + B  

21. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Decomposition Reactions Decomposition reactions are the opposite of synthesis reactions. Section 2 Types of Chemical Reactions Chapter 8 In a decomposition reaction, a single compound undergoes a reaction that produces two or more simpler substances: elements or compounds. They are represented by the following general equation. AX A + X AX is a compound. A and X can be elements or compounds.

22. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Decomposition Reactions, continued Decomposition of Binary Compounds The decomposition of a substance by an electric current is called electrolysis. Section 2 Types of Chemical Reactions Chapter 8 example: Oxides of the less-active metals, which are located in the lower center of the periodic table, decompose into their elements when heated. example:

23. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Visual Concepts Click below to watch the Visual Concept. Visual Concept Electrolysis Chapter 8 http://my.hrw.com/sh/hc6_003036809x/st udent/ch08/sec02/vc02/hc608_02_v02fs. htm

24. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Decomposition Reactions, continued Decomposition of Metal Carbonates Section 2 Types of Chemical Reactions Chapter 8 Decomposition of Metal Hydroxides Decomposition of Metal Chlorates

25. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Decomposition Reactions, continued Decomposition of Acids Section 2 Types of Chemical Reactions Chapter 8 Certain acids decompose into nonmetal oxides and water. example: Carbonic acid is unstable and decomposes readily at room temperature to produce carbon dioxide and water.

26. End Show Slide of 42 © Copyright Pearson Prentice Hall 26 Types of Chemical Reactions > Classifying Reactions Single-Replacement Reactions A single-replacement reaction is a chemical change in which one element replaces a second element in a compound. 8.2

27. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Single-Displacement Reactions In a single-displacement reaction, also known as a replacement reaction, one element replaces a similar element in a compound. Section 2 Types of Chemical Reactions Chapter 8 Many single-displacement reactions take place in aqueous solution. Single-displacement reactions can be represented by the following general equations. A + BX AX + B or Y + BX BY + X A, B, X, and Y are elements. AX, BX, and BY are compounds.

28. Single Displacement  AX + B  A + BX

29. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu

30. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Single-Displacement Reactions Displacement of a Metal in a Compound by Another Metal Aluminum is more active than lead. 2Al(s) + 3Pb(NO 3 ) 2 (aq) 3Pb(s) + 2Al(NO 3 ) 3 (aq) Section 2 Types of Chemical Reactions Chapter 8

31. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Single-Displacement Reactions, continued Displacement of Hydrogen in Water by a Metal Section 2 Types of Chemical Reactions Chapter 8 The most-active metals, such as those in Group 1, react vigorously with water to produce metal hydroxides and hydrogen. 2Na(s) + 2H 2 O(l) 2NaOH(aq) + H 2 (g) Less-active metals, such as iron, react with steam to form a metal oxide and hydrogen gas. 3Fe(s) + 4H 2 O(g) Fe 3 O 4 (s) + 4H 2 (g)

32. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Single-Displacement Reactions, continued Displacement of Hydrogen in an Acid by a Metal Section 2 Types of Chemical Reactions Chapter 8 The more-active metals react with certain acidic solutions, such as hydrochloric acid and dilute sulfuric acid, replacing the hydrogen in the acid. The reaction products are a metal compound (a salt) and hydrogen gas. Mg(s) + 2HCl(aq) H 2 (g) + MgCl 2 (aq)

33. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Single-Displacement Reactions, continued Displacement of Halogens Section 2 Types of Chemical Reactions Chapter 8 Fluorine is the most-active halogen. In Group 17 each element can replace any element below it, but not any element above it. Cl 2 (g) + 2KBr(aq) 2KCl(aq) + Br 2 (l) F 2 (g) + 2NaCl(aq) 2NaF(aq) + Cl 2 (g) Br 2 (l) + KCl(aq) no reaction It can replace any of the other halogens in their compounds.

34. End Show Slide of 42 © Copyright Pearson Prentice Hall 34 Types of Chemical Reactions > Classifying Reactions The activity series of metals lists metals in order of decreasing reactivity. 8.2

35. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Double-Displacement Reactions In double-displacement reactions, the ions of two compounds exchange places in an aqueous solution to form two new compounds. Section 2 Types of Chemical Reactions Chapter 8 One of the compounds formed is usually a precipitate, an insoluble gas that bubbles out of the solution, or a molecular compound, usually water. The other compound is often soluble and remains dissolved in solution.

36. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Double-Displacement Reactions, continued A double-displacement reaction is represented by the following general equation. AX + BY AY + BX Section 2 Types of Chemical Reactions Chapter 8 A, X, B, and Y in the reactants represent ions. AY and BX represent ionic or molecular compounds.

37. Double Displacement  AX + BY  AY + BX 

38. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu

39. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Double-Displacement Reactions, continued Formation of a Precipitate The formation of a precipitate occurs when the cations of one reactant combine with the anions of another reactant to form an insoluble or slightly soluble compound. Section 2 Types of Chemical Reactions Chapter 8 example: 2KI(aq) + Pb(NO 3 ) 2 (aq) PbI 2 (s) + 2KNO 3 (aq) The precipitate forms as a result of the very strong attractive forces between the Pb 2+ cations and the I − anions.

40. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Double-Displacement Reactions, continued Formation of a Gas FeS(s) + 2HCl(aq) H 2 S(g) + FeCl 2 (aq) Formation of Water HCl(aq) + NaOH(aq) NaCl(aq) + H 2 O(l) Section 2 Types of Chemical Reactions Chapter 8

41. End Show Slide of 42 © Copyright Pearson Prentice Hall 41 Types of Chemical Reactions > Classifying Reactions Double-Replacement Reactions A double-replacement reaction is a chemical change involving an exchange of positive ions between two compounds. 8.2

42. © Copyright Pearson Prentice Hall Slide of 42 End Show

43. © Copyright Pearson Prentice Hall Slide of 42 End Show

44. © Copyright Pearson Prentice Hall Slide of 42 End Show

45. Slide of 42 © Copyright Pearson Prentice Hall 45 Types of Chemical Reactions > Classifying Reactions Combustion Reactions A combustion reaction is a chemical change in which an element or a compound reacts with oxygen, often producing energy in the form of heat and light. 8.2

46. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Combustion Reactions In a combustion reaction, a substance combines with oxygen, releasing a large amount of energy in the form of light and heat. Section 2 Types of Chemical Reactions Chapter 8 example: combustion of hydrogen 2H 2 (g) + O 2 (g) 2H 2 O(g) example: combustion of propane C 3 H 8 (g) + 5O 2 (g) 3CO 2 (g) + 4H 2 O(g)

47. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Visual Concepts Click below to watch the Visual Concept. Visual Concept Chapter 8 Combustion Reaction http://my.hrw.com/sh/hc6_003036809x/stu dent/ch08/sec02/vc05/hc608_02_v05fs.ht m

48. End Show Slide of 42 © Copyright Pearson Prentice Hall 48 Types of Chemical Reactions > Predicting the Products of a Chemical Reaction How can you predict the products of the five general types of reactions? 8.2

49. End Show © Copyright Pearson Prentice Hall 49 Slide of 42 Types of Chemical Reactions > Predicting the Products of a Chemical Reaction The number of elements and/or compounds reacting is a good indicator of possible reaction type and thus possible products. 8.2

50. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Determining Reaction Types Section 2 Types of Chemical Reactions Chapter 8

51. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Identifying Reactions and Predicting Products Section 2 Types of Chemical Reactions Chapter 8

52. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 2 Types of Chemical Reactions Chapter 8 Identifying Reactions and Predicting Products

53. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Identifying Reactions and Predicting Products Section 2 Types of Chemical Reactions Chapter 8

54. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section Review pg. 284 #2, 3, 4

55. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section Review pg. 284 #2, 3, 4 ANSWERS

56. End Show © Copyright Pearson Prentice Hall Slide of 42 Section Quiz -or- Continue to: Launch: Assess students’ understanding of the concepts in Section 8.2. 8.2 Section Quiz.

57. © Copyright Pearson Prentice Hall Slide of 42 End Show 1. What type of reaction is described by the following equation? 6Li + N 2 → 2Li 3 N a.combination reaction b.decomposition reaction c.single-replacement reaction d.combustion reaction 8.2 Section Quiz.

58. © Copyright Pearson Prentice Hall Slide of 42 End Show 2. Balance the following equation and indicate whether it represents a combustion, combination, or decomposition reaction. H 2 SO 4 → H 2 O 2 + SO 2 a.H 2 SO 4 → H 2 O 2 + SO 2, combination reaction b.H 2 SO 4 → H 2 O 2 + SO 2, decomposition reaction c.H 2 SO 4 → 2H 2 O 2 + SO 2, combination reaction d.H 2 SO 4 → 2H 2 O 2 + SO 2, decomposition reaction 8.2 Section Quiz.

59. © Copyright Pearson Prentice Hall Slide of 42 End Show 8.2 Section Quiz. 3. Predict the missing product in the following unbalanced equation. Pb(NO 3 ) 2 + KOH → KNO 3 + ____________ a.PbOH 2 b.Pb(OH) 4 c.Pb(OH) 2 d.PbOH

60. © Copyright Pearson Prentice Hall Slide of 25 End Show Online Self-Check Quiz Complete the online Quiz and record answers. Ask if you have any questions about your answers. click here for online Quiz 8.2 (8 questions) You must be in the “Play mode” for the slideshow for hyperlink to work.

61. © Copyright Pearson Prentice Hall Slide of 28 End Show VIDEOS FOR ADDITIONAL INSTRUCTION Additional Videos for Section 8.2: Types of Chemical Reactions Types of Reactions Synthesis Reactions Decomposition Reaction Single Replacement Reaction Double Replacement Reactions Combustion Reactions

62. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu End of Chapter 8.2 Show

63. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Multiple Choice 1. According to the law of conservation of mass, the total mass of the reacting substances is A. always more than the total mass of the products. B. always less than the total mass of the products. C. sometimes more and sometimes less than the total mass of the products. D. always equal to the total mass of the products. Standardized Test Preparation Chapter 8

64. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 1. According to the law of conservation of mass, the total mass of the reacting substances is A. always more than the total mass of the products. B. always less than the total mass of the products. C. sometimes more and sometimes less than the total mass of the products. D. always equal to the total mass of the products. Standardized Test Preparation Chapter 8 Multiple Choice

65. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 2. To balance a chemical equation, you may adjust the A. coefficients. B. subscripts. C. formulas of the products. D. either the coefficients or the subscripts. Standardized Test Preparation Chapter 8 Multiple Choice

66. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 2. To balance a chemical equation, you may adjust the A. coefficients. B. subscripts. C. formulas of the products. D. either the coefficients or the subscripts. Standardized Test Preparation Chapter 8 Multiple Choice

67. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 3.Which is the correct chemical equation for the following formula equation: (NH 4 ) 2 S NH 3 + H 2 S? A. 2(NH 4 ) 2 S 2NH 3 + H 2 S 2 B. 2(NH 4 ) 2 S 2NH 3 + H 2 S C. (NH 4 ) 2 S 2NH 3 + H 2 S D. None of the above Standardized Test Preparation Chapter 8 Multiple Choice

68. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 3.Which is the correct chemical equation for the following formula equation: (NH 4 ) 2 S NH 3 + H 2 S? A. 2(NH 4 ) 2 S 2NH 3 + H 2 S 2 B. 2(NH 4 ) 2 S 2NH 3 + H 2 S C. (NH 4 ) 2 S 2NH 3 + H 2 S D. None of the above Standardized Test Preparation Chapter 8 Multiple Choice

69. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 4. Select the missing reactant(s) for the double- displacement reaction that produces PF 5 and AsCl 3. A. PCl 5 and AsF 3 B. PCl 3 and AsF 5 C. PCl 3 and AsF 3 D. None of the above Standardized Test Preparation Chapter 8 Multiple Choice

70. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 4. Select the missing reactant(s) for the double- displacement reaction that produces PF 5 and AsCl 3. A. PCl 5 and AsF 3 B. PCl 3 and AsF 5 C. PCl 3 and AsF 3 D. None of the above Standardized Test Preparation Chapter 8 Multiple Choice

71. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 5. Select the missing reactant for the following combustion reaction: 2______ + 15O 2 14CO 2 + 6H 2 O. A. C 14 H 12 B. C 14 H 12 O 4 C. C 7 H 6 D. C 7 H 6 O 2 Standardized Test Preparation Chapter 8 Multiple Choice

72. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 5. Select the missing reactant for the following combustion reaction: 2______ + 15O 2 14CO 2 + 6H 2 O. A. C 14 H 12 B. C 14 H 12 O 4 C. C 7 H 6 D. C 7 H 6 O 2 Standardized Test Preparation Chapter 8 Multiple Choice

73. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 6. A mixture consists of Ag, Pb, and Fe metals. Which of these metals will react with ZnCl 2 ? A. Ag(s) B. Pb(s) C. Fe(s) D. None of these metals Standardized Test Preparation Chapter 8 Multiple Choice

74. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 6. A mixture consists of Ag, Pb, and Fe metals. Which of these metals will react with ZnCl 2 ? A. Ag(s) B. Pb(s) C. Fe(s) D. None of these metals Standardized Test Preparation Chapter 8 Multiple Choice

75. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Standardized Test Preparation Chapter 8 Multiple Choice 7. Which of the following statements is true about the reaction 2F 2 + 2H 2 O 4HF + O 2 ? A.Two grams of O 2 are produced when 2 g F 2 reacts with 2 g H 2 O. B. Two moles of HF are produced when 1 mol F 2 reacts with 1 mol H 2 O. C. For every 2 mol O 2 produced, 6 mol HF are produced. D. For every 1 mol H 2 O that reacts, 2 mol O 2 are produced.

76. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 7. Which of the following statements is true about the reaction 2F 2 + 2H 2 O 4HF + O 2 ? A.Two grams of O 2 are produced when 2 g F 2 reacts with 2 g H 2 O. B. Two moles of HF are produced when 1 mol F 2 reacts with 1 mol H 2 O. C. For every 2 mol O 2 produced, 6 mol HF are produced. D. For every 1 mol H 2 O that reacts, 2 mol O 2 are produced. Standardized Test Preparation Chapter 8 Multiple Choice

77. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Short Answer 8. Determine the products and write a balanced equation for the reaction of solid magnesium and water. Standardized Test Preparation Chapter 8

78. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 8. Determine the products and write a balanced equation for the reaction of solid magnesium and water. Answer: Mg(s) + 2H 2 O(l) Mg(OH) 2 (aq) + H 2 (g) Standardized Test Preparation Chapter 8 Short Answer

79. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 9. A precipitation of iron(III) hydroxide is produced by reacting an aqueous solution of iron(III) chloride with an aqueous solution of sodium hydroxide. Write a balanced chemical equation. Standardized Test Preparation Chapter 8 Short Answer

80. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 9. A precipitation of iron(III) hydroxide is produced by reacting an aqueous solution of iron(III) chloride with an aqueous solution of sodium hydroxide. Write a balanced chemical equation. Answer: FeCl 3 (aq) + 3NaOH(aq) Fe(OH) 3 (s) + 3NaCl(s) Standardized Test Preparation Chapter 8 Short Answer

81. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Extended Response 10. List the hypothetical metals A, E, M, and R in increasing order of reactivity by using the reaction data in the table below. The reaction of interest is of the form C + ZX CX + Z. Explain your reasoning. AXEXMXRX A _____ no reactionreactionno reaction Ereaction _____ reaction Mno reaction _____ no reaction Rreactionno reactionreaction _____ Standardized Test Preparation Chapter 8

82. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Answer: The metals in increasing order of reactivity are M, A, R, and E. M is the least reactive because it shows no reaction in a single-displacement reaction with any of the other metals. A is the next least reactive because it will react in a single- displacement reaction with only M. E is the most reactive metal of the series because E will react in a single-displacement reaction with the other three metals. Standardized Test Preparation Chapter 8 Extended Response 10. List the hypothetical metals A, E, M, and R in increasing order of reactivity by using the reaction data in the table below. The reaction of interest is of the form C + ZX CX + Z. Explain your reasoning.

83. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 11. Calcium hypochlorite, Ca(OCl) 2, is a bleaching agent produced from sodium hydroxide, calcium hydroxide, and chlorine. Sodium chloride and water are also produced in the reaction. Write the balanced chemical equation. If 2 mol NaOH react, how many moles of calcium hypochlorite can be produced? Standardized Test Preparation Chapter 8 Extended Response

84. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 11. Calcium hypochlorite, Ca(OCl) 2, is a bleaching agent produced from sodium hydroxide, calcium hydroxide, and chlorine. Sodium chloride and water are also produced in the reaction. Write the balanced chemical equation. If 2 mol NaOH react, how many moles of calcium hypochlorite can be produced? Answer: The balanced chemical equation is 2NaOH + Ca(OH) 2 + 2Cl 2 Ca(OCl) 2 + 2NaCl + H 2 O. If 2 mol NaOH react, then 1 mol Ca(OCl) 2 can be produced. Standardized Test Preparation Chapter 8 Extended Response