OPENER # - CHAPTER 8 - NOV __, 2012 Balance the following equations: CO (g) + N2O5 (g) O2( g) --> + H2O (l) --> CO2 (g) HNO3 (aq) PCl5 (l) + H2O (l) --> H3PO4 (aq) CH4 (g) + Br2 (g) --> CBr4 (l) C5H10O2 (l) Cr(OH) 3 (s) + + O2 (g) --> CO2 (g) HClO4 (aq) --> + + HCl (aq) HBr (g) + H2O (l) Cr(ClO4) 3 (aq) Chapter menu + H2O (l) Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. S.15.C.6 Identify the physical state for each substance in a reaction equation Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Chemical Equations and Chemical Reactions Table of Contents Section 2 Types of Chemical Reactions Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Section 2 Types of Chemical Reactions Objectives • Define and give general equations for synthesis, decomposition, single-displacement, and doubledisplacement 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. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Section 2 Types of Chemical Reactions 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. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. 8.2 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. Slide of 42 6 © Copyright Pearson Prentice Hall End Show 8.2 Types of Chemical Reactions > Classifying Reactions Classifying Reactions What are the five general types of reactions? Slide of 42 7 © Copyright Pearson Prentice Hall End Show Chapter 8 Section 2 Types of Chemical Reactions • There are several ways to classify chemical reactions. • 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 Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Section 2 Types of Chemical Reactions 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 • A and X can be elements or compounds. • AX is a compound Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Visual Concepts Synthesis Reactions Click below to watch the Visual Concept. http://my.hrw.com/sh/hc6_003036809x/s Visual Concept tudent/ch08/sec02/vc00/hc608_02_v00fs .htm Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Synthesis A + B AB + Chapter 8 Section 2 Types of Chemical Reactions 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. • Almost all metals react with oxygen to form oxides. • example: 2Mg(s) + O2(g) 2MgO(s) • Group 2 elements react in a similar manner, forming oxides with the formula MO, where M represents the metal. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Section 2 Types of Chemical Reactions Synthesis Reactions, continued Reactions of Elements with Oxygen and Sulfur, continued • The Group 1 metals form oxides with the formula M2O. • example: Li2O • The Group 1 and Group 2 elements react similarly with sulfur, forming sulfides with the formulas M2S and MS, respectively. 16Rb(s) + S8(s) 8Rb2S(s) 8Ba(s) + S8(s) 8BaS(s) Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Section 2 Types of Chemical Reactions Synthesis Reactions, continued Reactions of Elements with Oxygen and Sulfur, continued • Nonmetals also undergo synthesis reactions with oxygen to form oxides. • example: Sulfur reacts to form sulfur dioxide. S8(s) + 8O2(g) 8SO2(g) • example: Hydrogen reacts with oxygen to form dihydrogen monoxide (water). 2H2(g) + O2(g) 2H2O(g) Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Section 2 Types of Chemical Reactions 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. • 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) + Cl2(g) 2NaCl(s) Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Section 2 Types of Chemical Reactions Synthesis Reactions, continued Reactions of Metals with Halogens, continued • Group 2 metals react with the halogens to form ionic compounds with the formula MX2. • example: Mg(s) + F2(g) MgF2(s) • Fluorine is so reactive that it combines with almost all metals. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Section 2 Types of Chemical Reactions Synthesis Reactions, continued Synthesis Reactions with Oxides • Active metals are highly reactive metals. • Oxides of active metals react with water to produce metal hydroxides. • example: Calcium oxide reacts with water to form calcium hydroxide. CaO(s) + H2O(l) Ca(OH)2(s) Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Section 2 Types of Chemical Reactions 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. • example: SO2(g) + H2O(l) H2SO3(aq) • Certain metal oxides and nonmetal oxides react with each other in synthesis reactions to form salts. • example: CaO(s) + SO2(g) CaSO3(s) Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. 8.2 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. Slide of 42 19 © Copyright Pearson Prentice Hall End Show Decomposition AB A + B Chapter 8 Section 2 Types of Chemical Reactions Decomposition Reactions • In a decomposition reaction, a single compound undergoes a reaction that produces two or more simpler substances: elements or compounds. • Decomposition reactions are the opposite of synthesis reactions. • They are represented by the following general equation. AX A+X • AX is a compound. • A and X can be elements or compounds. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Section 2 Types of Chemical Reactions Decomposition Reactions, continued Decomposition of Binary Compounds • The decomposition of a substance by an electric current is called electrolysis. • example: 2H O(l) electricity 2H2 (g) + O2 (g) 2 • Oxides of the less-active metals, which are located in the lower center of the periodic table, decompose into their elements when heated. • example: 2HgO(s) 2Hg(l) + O2 (g) Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Visual Concepts Electrolysis Click below to watch the Visual Concept. http://my.hrw.com/sh/hc6_003036809x/st Visual Concept udent/ch08/sec02/vc02/hc608_02_v02fs. htm Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Section 2 Types of Chemical Reactions Decomposition Reactions, continued Decomposition of Metal Carbonates CaCO3 (s) CaO(s) + CO2 (g) Decomposition of Metal Hydroxides Ca(OH)2 (s) CaO(s) + H2O(g) Decomposition of Metal Chlorates 2KClO3 (s) MnO 2KCl(s) + 3O2 (g) (s) 2 Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Section 2 Types of Chemical Reactions Decomposition Reactions, continued Decomposition of Acids • 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. H2CO3 (aq) CO2 (g) + H2O(l) Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. 8.2 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. Slide of 42 26 © Copyright Pearson Prentice Hall End Show Chapter 8 Section 2 Types of Chemical Reactions Single-Displacement Reactions • In a single-displacement reaction, also known as a replacement reaction, one element replaces a similar element in a compound. • 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. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Single Displacement AX + B A + BX Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Section 2 Types of Chemical Reactions Single-Displacement Reactions Displacement of a Metal in a Compound by Another Metal • Aluminum is more active than lead. 2Al(s) + 3Pb(NO3)2(aq) 3Pb(s) + 2Al(NO3)3(aq) Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Section 2 Types of Chemical Reactions Single-Displacement Reactions, continued Displacement of Hydrogen in Water by a Metal • The most-active metals, such as those in Group 1, react vigorously with water to produce metal hydroxides and hydrogen. 2Na(s) + 2H2O(l) 2NaOH(aq) + H2(g) • Less-active metals, such as iron, react with steam to form a metal oxide and hydrogen gas. 3Fe(s) + 4H2O(g) Fe3O4(s) + 4H2(g) Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Section 2 Types of Chemical Reactions Single-Displacement Reactions, continued Displacement of Hydrogen in an Acid by a Metal • 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) H2(g) + MgCl2(aq) Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Section 2 Types of Chemical Reactions Single-Displacement Reactions, continued Displacement of Halogens • Fluorine is the most-active halogen. • It can replace any of the other halogens in their compounds. • In Group 17 each element can replace any element below it, but not any element above it. Cl2(g) + 2KBr(aq) 2KCl(aq) + Br2(l) F2(g) + 2NaCl(aq) 2NaF(aq) + Cl2(g) Br2(l) + KCl(aq) no reaction Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. 8.2 Types of Chemical Reactions > Classifying Reactions The activity series of metals lists metals in order of decreasing reactivity. Slide of 42 34 © Copyright Pearson Prentice Hall End Show Chapter 8 Section 2 Types of Chemical Reactions Double-Displacement Reactions • In double-displacement reactions, the ions of two compounds exchange places in an aqueous solution to form two new compounds. • 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. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Section 2 Types of Chemical Reactions Double-Displacement Reactions, continued • A double-displacement reaction is represented by the following general equation. AX + BY AY + BX • A, X, B, and Y in the reactants represent ions. • AY and BX represent ionic or molecular compounds. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Double Displacement AX + BY AY + BX Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Section 2 Types of Chemical Reactions 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. • example: 2KI(aq) + Pb(NO3)2(aq) PbI2(s) + 2KNO3(aq) • The precipitate forms as a result of the very strong attractive forces between the Pb2+ cations and the I anions. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Section 2 Types of Chemical Reactions Double-Displacement Reactions, continued Formation of a Gas FeS(s) + 2HCl(aq) H2S(g) + FeCl2(aq) Formation of Water HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l) Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. 8.2 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. Slide of 42 41 © Copyright Pearson Prentice Hall End Show Slide of 42 © Copyright Pearson Prentice Hall End Show Slide of 42 © Copyright Pearson Prentice Hall End Show Slide of 42 © Copyright Pearson Prentice Hall End Show 8.2 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. Slide of 42 45 © Copyright Pearson Prentice Hall End Show Chapter 8 Section 2 Types of Chemical Reactions Combustion Reactions • In a combustion reaction, a substance combines with oxygen, releasing a large amount of energy in the form of light and heat. • example: combustion of hydrogen 2H2(g) + O2(g) 2H2O(g) • example: combustion of propane C3H8(g) + 5O2(g) 3CO2(g) + 4H2O(g) Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Visual Concepts Combustion Reaction Click below to watch the Visual Concept. http://my.hrw.com/sh/hc6_003036809x/stu Visual Concept dent/ch08/sec02/vc05/hc608_02_v05fs.ht m Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. 8.2 Types of Chemical Reactions > Predicting the Products of a Chemical Reaction Predicting the Products of a Chemical Reaction How can you predict the products of the five general types of reactions? Slide of 42 48 © Copyright Pearson Prentice Hall End Show 8.2 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. Slide of 42 49 © Copyright Pearson Prentice Hall End Show Chapter 8 Section 2 Types of Chemical Reactions Determining Reaction Types Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Section 2 Types of Chemical Reactions Identifying Reactions and Predicting Products Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Section 2 Types of Chemical Reactions Identifying Reactions and Predicting Products Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Section 2 Types of Chemical Reactions Identifying Reactions and Predicting Products Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Section Review pg. 284 #2, 3, 4 Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Section Review pg. 284 #2, 3, 4 ANSWERS Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. 8.2 Section Quiz. Assess students’ understanding of the concepts in Section 8.2. Continue to: -or- Launch: Section Quiz Slide of 42 © Copyright Pearson Prentice Hall End Show 8.2 Section Quiz. 1. What type of reaction is described by the following equation? 6Li + N2 2Li3N a. combination reaction b. decomposition reaction c. single-replacement reaction d. combustion reaction Slide of 42 © Copyright Pearson Prentice Hall End Show 8.2 Section Quiz. 2. Balance the following equation and indicate whether it represents a combustion, combination, or decomposition reaction. H2SO4 H2O2 + SO2 a. H2SO4 H2O2 + SO2, combination reaction b. H2SO4 H2O2 + SO2, decomposition reaction c. H2SO4 2H2O2 + SO2, combination reaction d. H2SO4 2H2O2 + SO2, decomposition reaction Slide of 42 © Copyright Pearson Prentice Hall End Show 8.2 Section Quiz. 3. Predict the missing product in the following unbalanced equation. Pb(NO3)2 + KOH KNO3 + ____________ a. PbOH2 b. Pb(OH)4 c. Pb(OH)2 d. PbOH Slide of 42 © Copyright Pearson Prentice Hall 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. Slide of 25 © Copyright Pearson Prentice Hall 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 Slide of 28 © Copyright Pearson Prentice Hall End Show End of Chapter 8.2 Show Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Standardized Test Preparation 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 and sometimes less than the total mass of themore products. D. always equal to the total mass of the products. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Standardized Test Preparation 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 and sometimes less than the total mass of themore products. D. always equal to the total mass of the products. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Standardized Test Preparation Multiple Choice 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. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Standardized Test Preparation Multiple Choice 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. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Standardized Test Preparation Multiple Choice 3. Which is the correct chemical equation for the following formula equation: (NH4)2S NH3 + H2S? A. 2(NH4)2S B. 2(NH4)2S 2NH3 + H2S2 2NH3 + H2S C. (NH4)2S 2NH3 + H2S D. None of the above Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Standardized Test Preparation Multiple Choice 3. Which is the correct chemical equation for the following formula equation: (NH4)2S NH3 + H2S? A. 2(NH4)2S B. 2(NH4)2S 2NH3 + H2S2 2NH3 + H2S C. (NH4)2S 2NH3 + H2S D. None of the above Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Standardized Test Preparation Multiple Choice 4. Select the missing reactant(s) for the doubledisplacement reaction that produces PF5 and AsCl3. A. PCl5 and AsF3 B. PCl3 and AsF5 C. PCl3 and AsF3 D. None of the above Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Standardized Test Preparation Multiple Choice 4. Select the missing reactant(s) for the doubledisplacement reaction that produces PF5 and AsCl3. A. PCl5 and AsF3 B. PCl3 and AsF5 C. PCl3 and AsF3 D. None of the above Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Standardized Test Preparation Multiple Choice 5. Select the missing reactant for the following combustion reaction: 2______ + 15O2 14CO2 + 6H2O. A. C14H12 B. C14H12O4 C. C7H6 D. C7H6O2 Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Standardized Test Preparation Multiple Choice 5. Select the missing reactant for the following combustion reaction: 2______ + 15O2 14CO2 + 6H2O. A. C14H12 B. C14H12O4 C. C7H6 D. C7H6O2 Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Standardized Test Preparation Multiple Choice 6. A mixture consists of Ag, Pb, and Fe metals. Which of these metals will react with ZnCl2? A. Ag(s) B. Pb(s) C. Fe(s) D. None of these metals Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Standardized Test Preparation Multiple Choice 6. A mixture consists of Ag, Pb, and Fe metals. Which of these metals will react with ZnCl2? A. Ag(s) B. Pb(s) C. Fe(s) D. None of these metals Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Standardized Test Preparation Multiple Choice 7. Which of the following statements is true about the reaction 2F2 + 2H2O 4HF + O2? A. Two grams of O2 are produced when 2 g F2 reacts with 2 g H2O. B. Two moles of HF are produced when 1 mol F2 reacts with 1 mol H2O. C. For every 2 mol O2 produced, 6 mol HF are produced. D. For every 1 mol H2O that reacts, 2 mol O2 are produced. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Standardized Test Preparation Multiple Choice 7. Which of the following statements is true about the reaction 2F2 + 2H2O 4HF + O2? A. Two grams of O2 are produced when 2 g F2 reacts with 2 g H2O. B. Two moles of HF are produced when 1 mol F2 reacts with 1 mol H2O. C. For every 2 mol O2 produced, 6 mol HF are produced. D. For every 1 mol H2O that reacts, 2 mol O2 are produced. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Standardized Test Preparation Short Answer 8. Determine the products and write a balanced equation for the reaction of solid magnesium and water. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Standardized Test Preparation Short Answer 8. Determine the products and write a balanced equation for the reaction of solid magnesium and water. Answer: Mg(s) + 2H2O(l) Mg(OH)2(aq) + H2(g) Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Standardized Test Preparation Short Answer 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. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Standardized Test Preparation Short Answer 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: FeCl3(aq) + 3NaOH(aq) Fe(OH)3(s) + 3NaCl(s) Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Standardized Test Preparation 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. AX EX MX RX A _____ no reaction reaction no reaction E reaction _____ reaction reaction M no reaction no reaction _____ no reaction R reaction no reaction reaction _____ Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Standardized Test Preparation 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. 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 singledisplacement 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. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Standardized Test Preparation Extended Response 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? Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved. Chapter 8 Standardized Test Preparation Extended Response 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 + 2Cl2 Ca(OCl)2 + 2NaCl + H2O. If 2 mol NaOH react, then 1 mol Ca(OCl)2 can be produced. Chapter menu Resources Copyright © by Holt, Rinehart and Winston. All rights reserved.