1. End Show © Copyright Pearson Prentice Hall Slide 1 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. 11.2

2. End Show Slide 2 of 42 © Copyright Pearson Prentice Hall Types of Chemical Reactions > Five general types of chemical reactions: combination (synthesis) decomposition single-replacement double-replacement combustion See websites for videos and animations http://www.youtube.com/watch?v=i-HHvx1VC_8&NR=1 http://www.youtube.com/watch?v=tE4668aarck&feature=related Classifying Reactions 11.2

3. Classifying Reactions Combination Reactions A combination reaction is a chemical change in which two or more substances react to form a single new substance. 11.2

5. for Conceptual Problem 11.4

6. End Show Slide 6 of 42 © Copyright Pearson Prentice Hall 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. 11.2

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10. for Conceptual Problem 11.5

11. End Show Slide 11 of 42 © Copyright Pearson Prentice Hall 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. 11.2

12. End Show Slide 12 of 42 © Copyright Pearson Prentice Hall Types of Chemical Reactions > Classifying Reactions The activity series of metals lists metals in order of decreasing reactivity. For a single-replacement reaction to occur, the element that is displaced must be less active than the element that is doing the displacing. Metals above Hydrogen in the activity series will replace H from acids. Zn(s) + 2 HCl (aq) → H 2 (g) + ZnCl 2 (aq) Metals below Hydrogen in the activity series will not react with acids. 11.2

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16. for Conceptual Problem 11.6

17. End Show Slide 17 of 42 © Copyright Pearson Prentice Hall 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. 11.2

21. End Show Slide 21 of 42 © Copyright Pearson Prentice Hall Types of Chemical Reactions > Classifying Reactions Combustion Reactions (see regents ref tables) 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. 11.2

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24. © Copyright Pearson Prentice Hall Slide 24 of 42 End Show Note your regents reference tables are helpful for writing equations for combustion reactions Examples:

25. End Show Slide 25 of 42 © Copyright Pearson Prentice Hall Types of Chemical Reactions > Predicting the Products of a Chemical Reaction How can you predict the products of the five general types of reactions? The number of elements and/or compounds reacting is a good indicator of possible reaction type and thus possible products. 11.2

26. End Show Slide 26 of 42 © Copyright Pearson Prentice Hall Types of Chemical Reactions > Predicting the Products of a Chemical Reaction 11.2

27. End Show Slide 27 of 42 © Copyright Pearson Prentice Hall Types of Chemical Reactions > Predicting the Products of a Chemical Reaction 11.2

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30. End Show Slide 30 of 42 © Copyright Pearson Prentice Hall Types of Chemical Reactions > Predicting the Products of a Chemical Reaction 11.2

31. End Show © Copyright Pearson Prentice Hall Slide 31 of 42 Section Quiz -or- Continue to: Launch: Assess students’ understanding of the concepts in Section 11.2. 11.2 Section Quiz.

32. © Copyright Pearson Prentice Hall Slide 32 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 11.2 Section Quiz.

33. © Copyright Pearson Prentice Hall Slide 33 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 11.2 Section Quiz.

34. © Copyright Pearson Prentice Hall Slide 34 of 42 End Show Reactions in Aqueous Solution Structures in limestone caverns are formed when carbon dioxide converts calcium hydrogen carbonate into calcium carbonate. The calcium carbonate precipitates and forms dramatic stalactites and stalagmites. You will learn to predict the formation of precipitates and write equations to describe the reactions that produce them. 11.3

35. © Copyright Pearson Prentice Hall Slide 35 of 42 End Show When AgNO 3 (aq) and NaCl (aq) are mixed, a white precipitate of AgCl (s) is formed. We can write a balanced equation to describe this double-replacement reaction: AgNO 3 (aq) + NaCl (aq) → AgCl (s) + NaNO 3 (aq) Two other types of equations can be written for this reaction (complete ionic equation and a net-ionic equation) A complete ionic equation is an equation that shows dissolved ionic compounds as dissociated free ions. 11.3

36. © Copyright Pearson Prentice Hall Slide 36 of 42 End Show Net Ionic Equations An ion that appears on both sides of an equation and is not directly involved in the reaction is called a spectator ion. The net ionic equation is an equation for a reaction in solution that shows only those particles that are directly involved in the chemical change. 11.3

37. © Copyright Pearson Prentice Hall Slide 37 of 42 End Show Net Ionic Equations Complete ionic equation: Sodium ions and nitrate ions are not changed during the chemical reaction of silver nitrate and sodium chloride so the net ionic equation is 11.3

38. © Copyright Pearson Prentice Hall Slide 38 of 42 End Show Predicting the Formation of a Precipitate How can you predict the formation of a precipitate in a double-replacement reaction? You can predict the formation of a precipitate by using the general rules for solubility of ionic compounds and by using the regents reference tables. 11.3

39. © Copyright Pearson Prentice Hall Slide 39 of 42 End Show Predicting the Formation of a Precipitate Will a precipitate form when a sodium carbonate solution is mixed with a barium nitrate solution? Hints: what are the products? and are those products soluble? (Use your reference tables). 11.3

40. © Copyright Pearson Prentice Hall Slide 40 of 42 End Show Predicting the Formation of a Precipitate Balanced equation: Ba(NO 3 ) 2 + Na 2 CO 3 (aq)→ BaCO 3 (s) + 2 NaNO 3 (aq) Complete ionic equation: Ba 2+ (aq) + 2 NO 3 - (aq) + 2 Na + (aq) + CO 3 2- (aq) → BaCO 3 (s) + 2 Na + (aq)+ 2 NO 3 - (aq) Net Ionic equation: Sodium nitrate is soluble but barium carbonate is insoluble. The net ionic equation is 11.3

41. © Copyright Pearson Prentice Hall Slide 41 of 42 End Show 2. Which one of the following products of double-replacement reactions would NOT form a precipitate? a.AgCl b.PbSO 4 c.Mg(OH) 2 d.Mo(NO 3 ) 2 11.3 Section Quiz.

42. © Copyright Pearson Prentice Hall Slide 42 of 42 End Show 3. Which reaction will NOT produce a precipitate from aqueous solution? a.Hg 2 (NO 3 ) 2 + KCl b.FeSO 4 + Ba(OH) 2 c.Pb(NO 3 ) 2 + Na 2 CO 3 d.NaBr + Al 2 (SO 4 ) 2 11.3 Section Quiz