3. Chapter Menu Chemical Reactions Section 9.1 Reactions and Equations Section 9.2 Classifying Chemical Reactions Exit Click a hyperlink or folder tab to view the corresponding slides.

4. Section 9-1 Section 9.1 Reactions and Equations Recognize evidence of chemical change. Represent chemical reactions with equations. Balance chemical equations.

5. Section 9-1 Section 9.1 Reactions and Equations chemical change: a process involving one or more substances changing into a new substance chemical reaction reactant product chemical equation coefficient

6. Section 9-1 Chemical Reactions Chemical reaction:hemical reaction The process by which one or more substances are rearranged to form different substances.

7. Section 9-1 Chemical Reactions (cont.) Evidence of a chemical reaction –Change in temperature –Change in color –Odor, gas, or bubbles

8. Section 9-1 Representing Chemical Reactions (cont.) A chemical equation is a statement that uses chemical formulas to show the identities and relative amounts of the substances involved in a chemical reaction.chemical equation

9. Section 9-1 Representing Chemical Reactions Two parts of chemical equations ReactantsReactants are the starting substances. ProductsProducts are the substances formed in the reaction.

10. Section 9-1

11. Representing Chemical Reactions (cont.) aluminum(s) + bromine(l) → aluminum bromide(s) Chemical Reaction in words What state are the reactants? What state is the product?

12. Section 9-1 Representing Chemical Reactions (cont.) Skeleton equations use atomic symbols Al(s) + Br(l) → AlBr 3 (s) Notice the product is a correct molecular formula

13. Solid lithium reacts with chlorine gas to produce solid lithium chloride. Example 1

14. Solid lithium reacts with chlorine gas to produce solid lithium chloride. lithium(s) + chlorine(g)  lithium chloride(s) Example 1 word equation

15. Solid lithium reacts with chlorine gas to produce solid lithium chloride. lithium(s) + chlorine(g)  lithium chloride(s) Li(s) + Cl 2 (g)  LiCl(s) Remember a lot of atoms are diatomic in nature Example 1 skeleton equation

16. Nitrogen gas reacts with oxygen gas to produce nitrogen dioxide gas. Example 2

17. Nitrogen gas reacts with oxygen gas to produce nitrogen dioxide gas. nitrogen(g) + oxygen(g)  nitrogen dioxide(g) Example 2 word equation

18. Nitrogen gas reacts with oxygen gas to produce nitrogen dioxide gas. nitrogen(g) + oxygen(g)  nitrogen dioxide(g) N 2 (g) + O 2 (g)  NO 2 (g) Example 2 skeleton equation

19. Solid iron reacts with aqueous copper (II) nitrate to produce solid copper and aqueous iron (II) nitrate. Example 3

20. Solid iron reacts with aqueous copper (II) nitrate to produce solid copper and aqueous iron (II) nitrate. Iron(s) + copper(II) nitrate(aq)  copper(s) + iron(II) nitrate(aq) Remember nitrate is ( NO 3 ) - Example 3 word equation

21. Solid iron reacts with aqueous copper (II) nitrate to produce solid copper and aqueous iron (II) nitrate. Iron(s) + copper(II) nitrate(aq)  copper(s) + iron(II) nitrate(aq) Fe(s) + Cu(NO 3 ) 2 (aq)  Cu(s) + Fe(NO 3 ) 2 (aq) Example 3 skeleton equation

22. Section 9-1 Balancing Chemical Equations Balanced equation for the reaction between aluminum and bromine.

23. Section 9-1 Balancing Chemical Equations (cont.) A coefficient in a chemical equation is the number written in front of a reactant or product.coefficient It describes the lowest whole- number ratio. Yeah!!!!

24. Section 9-1 Balancing Chemical Equations (cont.) Balanced equations represent the Law of Conservation of Mass

25. Section 9-1 Balancing Chemical Equations (cont.)

26. Li(s) + Cl 2 (g)  LiCl(s) 1 Li 2 Cl 1 Li 1 Cl Example 1 balanced equation

27. Li(s) + Cl 2 (g)  LiCl(s) 1 Li 2 Cl 1 Li 1 Cl need 2 Cl on this side Example 1 balanced equation

28. Li(s) + Cl 2 (g)  LiCl(s) 1 Li 2 Cl 1 Li 1 Cl need 2 Cl on this side put 2 in front of LiCl Li(s) + Cl 2 (g)  2LiCl(s) 1 Li 2 Cl 2 Li 2 Cl Example 1 balanced equation

29. Li(s) + Cl 2 (g)  LiCl(s) 1 Li 2 Cl 1 Li 1 Cl need 2 Cl on this side Li(s) + Cl 2 (g)  2LiCl(s) 1 Li 2 Cl 2 Li 2 Cl bc molecule need 2 Li on this side put 2 in front of Li only Example 1 balanced equation

30. Li(s) + Cl 2 (g)  LiCl(s) 1 Li 2 Cl 1 Li 1 Cl need 2 Cl on this side Li(s) + Cl 2 (g)  2LiCl(s) 1 Li 2 Cl 2 Li 2 Cl bc molecule Need 2 Li 2Li(s) + Cl 2 (g)  2LiCl(s) 2 Li 2 Cl 2 Li 2 Cl all balanced Example 1 balanced equation

31. N 2 (g) + O 2 (g)  NO 2 (g ) Example 2 balanced equation

32. N 2 (g) + O 2 (g)  NO 2 (g) 2N 2O 1N 2O not balanced put 2 in front of NO 2 N 2 (g) + O 2 (g)  2NO 2 (g) 2N 2O 2N 4O not balanced put 2 in front of O 2 N 2 (g) + 2O 2 (g)  2NO 2 (g) 2N 4O 2N 4O balanced Example 2 balanced equation

33. Fe(s) + Cu(NO 3 ) 2 (aq)  Cu(s) + Fe(NO 3 ) 2 (aq) Example 3 balanced equation

34. Fe(s) + Cu(NO 3 ) 2 (aq)  Cu(s) + Fe(NO 3 ) 2 (aq) 1Fe 1Cu 2(NO 3 ) 1Cu 1Fe 2(NO 3 ) balanced Example 3 balanced equation

35. Solid potassium reacts with liquid water to produce hydrogen gas and a water (aqueous) solution of potassium hydroxide. Hydroxide is OH - Practice 1 balanced equation

36. Solid potassium reacts with liquid water to produce hydrogen gas and a water (aqueous) solution of potassium hydroxide. Potassium(s) + water(l)  hydrogen(g) + potassium hydroxide(aq) K(s) + H 2 O(l)  H 2 (g) + KOH(aq) Practice 1 balanced equation

37. Solid potassium reacts with liquid water to produce hydrogen gas and a water (aqueous) solution of potassium hydroxide. Potassium(s) + water(l)  hydrogen(g) + potassium hydroxide(aq) K(s) + H 2 O(l)  H 2 (g) + KOH(aq) 2K(s) + 2H 2 O(l)  H 2 (g) + 2KOH(aq) Practice 1 balanced equation

38. Calcium chloride and sodium carbonate in water (aqueous) solution produce solid calcium carbonate and a water solution of sodium chloride. Carbonate is (CO 3 ) -2 Practice 2 balanced equation

39. Calcium chloride and sodium carbonate in water (aqueous) solution produce solid calcium carbonate and a water solution of sodium chloride. Calcium chloride(aq) + sodium carbonate(aq)  calcium carbonate(s) + sodium chloride(aq) CaCl 2 (aq) + Na 2 (CO 3 )(aq)  Ca(CO 3 )(s) + NaCl(aq) Practice 2 balanced equation

40. Calcium chloride and sodium carbonate in water (aqueous) solution produce solid calcium carbonate and a water solution of sodium chloride. Calcium chloride(aq) + sodium carbonate(aq)  calcium carbonate(s) + sodium chloride(aq) CaCl 2 (aq) + Na 2 (CO 3 )(aq)  Ca(CO 3 )(s) + NaCl(aq) CaCl 2 (aq) + Na 2 (CO 3 )(aq)  Ca(CO 3 )(s) + 2NaCl(aq) Practice 2 balanced equation

41. Liquid bromine and solid lithium iodide react to form solid lithium bromide and solid iodine. Practice 3 balanced equation

42. Liquid bromine and solid lithium iodide react to form solid lithium bromide and solid iodine. bromine(l) + lithium iodide(s)  lithium bromide(s) + iodine(s) Br 2 (l) + LiI(s)  LiBr(s) + I 2 (s) Practice 3 balanced equation

43. Liquid bromine and solid lithium iodide react to form solid lithium bromide and solid iodine. bromine(l) + lithium iodide(s)  lithium bromide(s) + iodine(s) Br 2 (l) + LiI(s)  LiBr(s) + I 2 (s) Br 2 (l) + 2LiI(s)  2LiBr(s) + I 2 (s) Practice 3 balanced equation

44. A.A B.B C.C D.D Section 9-1 Section 9.1 Assessment Which of the following is NOT a chemical reaction? A.a piece of wood burning B.a car rusting C.an ice cube melting into water D.red litmus paper turning blue

45. A.A B.B C.C D.D Section 9-1 Section 9.1 Assessment What is the coefficient of bromine in the equation 2Al(s) + 3Br 2 (l) → 2AlBr 3 (s)? A.1 B.2 C.3 D.6

46. End of Section 9-1

47. Section 9-2 Section 9.2 Classifying Chemical Reactions Classify chemical reactions. Identify the characteristics of different classes of chemical reactions.

48. Section 9-2 Section 9.2 Classifying Chemical Reactions (cont.) Types of chemical reactions: Synthesis Combustion Decomposition Replacement reactions

49. Section 9-2 Section 9.2 Classifying Chemical Reactions metal: an element that is a solid at room temperature, a good conductor of heat and electricity, and is generally shiny synthesis reaction combustion reaction decomposition reaction single-replacement reaction double-replacement reaction precipitate

50. Section 9-2 Types of Chemical Reactions Synthesis reactionynthesis reaction two or more substances react produce a single product.

51. Section 9-2 Types of Chemical Reactions (cont.) Synthesis Example

52. Section 9-2 Types of Chemical Reactions (cont.) Combustion Reactionombustion Reaction oxygen combines with a substance release energy in the form of heat and light

53. Section 9-2 Types of Chemical Reactions (cont.) This is also a synthesis reaction. Combustion Example

54. Section 9-2 Decomposition Reactions Decomposition Reactionecomposition Reaction a single compound breaks down into two or more elements or new compounds Often require an energy source, such as heat, light, or electricity.

55. Section 9-2 Replacement Reactions Single Replacement ReactionSingle Replacement Reaction. the atoms of one element replace the atoms of another element in a compound A + BX → AX + B

56. Section 9-2 Replacement Reactions (cont.) A metal will not always replace a metal in a compound dissolved in water because of differing reactivities. An activity series can be used to predict if reactions will occur.

57. Section 9-2 Replacement Reactions (cont.) Halogens frequently replace other halogens in replacement reactions. Halogens also have different reactivities and do not always replace each other.

58. Section 9-2 Replacement Reactions (cont.) Double replacement reactions An ion exchange between two compounds

59. Section 9-2 Replacement Reactions (cont.) Precipitate the solid product produced during a chemical reaction All double replacement reactions produce either water, a gas, or a precipitate.

60. Section 9-2 Replacement Reactions (cont.)

61. Section 9-2 Replacement Reactions (cont.)

62. A.A B.B C.C D.D Section 9-2 Section 9.2 Assessment Which of the following is NOT one of the four types of reactions? A.deconstructive B.synthesis C.single replacement D.double replacement

63. A.A B.B C.C D.D Section 9-2 Section 9.2 Assessment The following equation is what type of reaction? KCN(aq) + HBr(aq) → KBr(aq) + HCN(g) A.deconstructive B.synthesis C.single replacement D.double replacement

64. End of Section 9-2

65. Section 9-3 Section 9.3 Reactions in Aqueous Solutions Describe aqueous solutions. Write complete ionic and net ionic equations for chemical reactions in aqueous solutions. Predict whether reactions in aqueous solutions will produce a precipitate, water, or a gas.

66. Section 9-3 Section 9.3 Reactions in Aqueous Solutions Double-replacement reactions occur between substances in aqueous solutions and produce precipitates, water, or gases.

67. Section 9-3 Section 9.3 Reactions in Aqueous Solutions (cont.) aqueous solution solute solvent complete ionic equation spectator ion net ionic equation solution: a uniform mixture that might contain solids, liquids, or gases

68. Section 9-3 Aqueous Solutions Aqueous Solution contains one or more dissolved substances (called solutes) in watersolutes Solvent the most plentiful substance in a solution Water is always the solvent in an aqueous solution.

69. Section 9-3 Aqueous Solutions (cont.) There are many possible solutes—sugar and alcohol are molecular compounds that exist as molecules in aqueous solutions. Compounds that produce hydrogen ions in aqueous solutions are acids.

70. Section 9-3 Aqueous Solutions (cont.) Ionic compounds can also be solutes in aqueous solutions. When ionic compounds dissolve in water, their ions separate in a process called dissociation.

71. Section 9-3 Types of Reactions in Aqueous Solutions When two solutions that contain ions as solutes are combined, the ions might react. If they react, it is always a double replacement reaction. Three products can form: precipitates, water, or gases.

72. Section 9-3 Types of Reactions in Aqueous Solutions (cont.) 2NaOH(aq) + CuCl 2 (aq) → 2NaCl(aq) + Cu(OH) 2 (s) Aqueous solutions of sodium hydroxide and copper(II) chloride react to form the precipitate copper(II) hydroxide.

73. Section 9-3 Types of Reactions in Aqueous Solutions (cont.) Complete ionic equations Show all of the particles in a solution as they actually exist 2Na + (aq) + 2OH – (aq) + Cu 2+ (aq)+ 2Cl – (aq) → 2Na + (aq) + 2Cl – (aq) + Cu(OH) 2 (s)

74. Section 9-3 Types of Reactions in Aqueous Solutions (cont.) Spectator Ions Ions that do not participate in a reaction and are not usually written in ionic equations. Net Ionic EquationsNet Ionic Equations. Formulas that include only the particles that participate in reactions 2OH – (aq) + Cu 2+ (aq) → Cu(OH) 2 (s)

75. Section 9-3 Types of Reactions in Aqueous Solutions (cont.) Some reactions produce more water molecules. No evidence of a chemical reaction is observable. HBr(aq) + NaOH(aq) → H 2 O(l) + NaBr(aq) Without spectator ions H + (aq) + OH – (aq) → H 2 O(l)

76. Section 9-3 Types of Reactions in Aqueous Solutions (cont.) Gases that are commonly produced are carbon dioxide, hydrogen cyanide, and hydrogen sulfide. 2HI(aq) + Li 2 S(aq) → H 2 S(g) + 2LiI(aq)

77. Section 9-3 Types of Reactions in Aqueous Solutions (cont.) Produce carbon dioxide gas mix vinegar and baking soda HCl(aq) + NaHCO 3 (aq) → H 2 CO 3 (aq) + NaCl(aq) H 2 CO 3 (aq) decomposes immediately H 2 CO 3 (aq) → H 2 O(l) + CO 2 (g)

78. Section 9-3 Types of Reactions in Aqueous Solutions (cont.) Two reactions can be combined and represented by a single chemical reaction.

79. Section 9-3 Types of Reactions in Aqueous Solutions (cont.) Reaction 1 HCl(aq) + NaHCO 3 (aq) → H 2 CO 3 (aq) + NaCl(aq) Reaction 2 H 2 CO 3 (aq) → H 2 O(l) + CO 2 (g) Combined equation HCl(aq) + NaHCO 3 (aq) + H 2 CO 3 (aq) → H 2 CO 3 (aq) + NaCl(aq) + H 2 O(l) + CO 2 (g) Overall equation HCl(aq) + NaHCO 3 (aq) → H 2 O(l) + CO 2 (g) + NaCl(aq)

80. A.A B.B C.C D.D Section 9-3 Section 9.3 Assessment What is the solvent in an aqueous solution? A.hydrogen B.sodium ions C.water D.alcohol

81. A.A B.B C.C D.D Section 9-3 Section 9.3 Assessment An equation that includes only the particles that participate in a reaction is called: A.net ionic equation B.spectator ions C.complete ionic equation D.reduced ionic equation

82. End of Section 9-3

83. Resources Menu Chemistry Online Study Guide Chapter Assessment Standardized Test Practice Image Bank Concepts in Motion

84. Study Guide 1 Section 9.1 Reactions and Equations Key Concepts Some physical changes are evidence that indicate a chemical reaction has occurred. Word equations and skeleton equations provide important information about a chemical reaction. A chemical equation gives the identities and relative amounts of the reactants and products that are involved in a chemical reaction. Balancing an equation involves adjusting the coefficients until the number of atoms of each element is equal on both sides of the equation.

85. Study Guide 2 Section 9.2 Classifying Chemical Reactions Key Concepts Classifying chemical reactions makes them easier to understand, remember, and recognize. Activity series of metals and halogens can be used to predict if single-replacement reactions will occur.

86. Study Guide 3 Section 9.3 Reactions in Aqueous Solutions Key Concepts In aqueous solutions, the solvent is always water. There are many possible solutes. Many molecular compounds form ions when they dissolve in water. When some ionic compounds dissolve in water, their ions separate. When two aqueous solutions that contain ions as solutes are combined, the ions might react with one another. The solvent molecules do not usually react. Reactions that occur in aqueous solutions are double- replacement reactions.

87. A.A B.B C.C D.D Chapter Assessment 1 The law of conservation of mass requires what in a chemical reaction equation? A.both sides of the equation to contain the same substances B.the reactants to have the same amount of molecules as the products C.both sides to have the same amount of atoms of each element D.the products to have fewer molecules than the reactants

88. A.A B.B C.C D.D Chapter Assessment 2 A reaction that gives off heat is what type of reaction? A.single replacement reaction B.double replacement reaction C.synthesis reaction D.combustion reaction

89. A.A B.B C.C D.D Chapter Assessment 3 Ions that are present in a solution and do not participate in a chemical reaction when another substance is added are called ____. A.spectator ions B.reactants C.products D.net ions

90. A.A B.B C.C D.D Chapter Assessment 4 A double replacement reaction produces all of the following except ____. A.gases B.solids C.light D.water

91. A.A B.B C.C D.D Chapter Assessment 5 What type of reaction is the following? 2H 2 O(l) + energy → H 2 (g) + O 2 (g) A.synthesis reaction B.decomposition reaction C.combustion reaction D.replacement reaction

92. A.A B.B C.C D.D STP 1 What type of reaction is the following? 2H 2 (g) + O 2 (g) → 2H 2 O(l) A.replacement reaction B.synthesis C.combustion reaction D.double replacement reaction

93. A.A B.B C.C D.D STP 2 A precipitate forms in a double replacement reaction only if: A.the reactivities of the compounds differ B.the new compound is denser than water C.the new compound is soluble in water D.the new compound is not soluble in water

94. A.A B.B C.C D.D STP 3 A ____ is a statement that uses chemical formulas to show the identities and relative amounts of the substances involved in a chemical reaction. A.word equation B.skeleton equation C.chemical equation D.balanced equation

95. A.A B.B C.C D.D STP 4 Predict the type of reaction. LiBr 2 (aq) + 2NaOH (aq) → ____ A.synthesis reaction B.combustion reaction C.single replacement reaction D.double replacement reaction

96. A.A B.B C.C D.D STP 5 Which reactions are essentially the opposite of synthesis reactions? A.single-replacement B.decomposition C.combustion D.double-replacement

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110. CIM Table 9.2 Steps for Balancing Equations Figure 9.15 The Forming of a Precipitate Table 9.4 Types of Chemical Reactions

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