1. Types of Chemical Reactions

2. Types of Chemical Reactions Review Reactants: Zn + I 2 Product: Zn I 2

3. Types of Chemical Reactions Review: At the conclusion of our time together, you should be able to: 1.List the 5 basic types of chemical reactions 2.Use this list to describe a reaction

4. Decomposition Simple Reactions Synthesis (Combination) Single Replacement Double Replacement

5. Decomposition Synthesis Single Replacement Double Replacement ABAB + AB AB + ABAB + C + C ABAB + C + CDD

6. Decomposition Synthesis Single Replacement Double Replacement ABAB + AB AB + ABAB + C + C ABAB + C + CDD

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9. Types of Reactions There are five types of chemical reactions we have talked about: There are five types of chemical reactions we have talked about: 1. Synthesis reactions 2. Decomposition reactions 3. Single displacement reactions 4. Double displacement reactions 5. Combustion reactions You need to be able to identify the type of reaction and predict the product(s) You need to be able to identify the type of reaction and predict the product(s)

10. Steps to Writing Reactions Some steps for doing reactions Some steps for doing reactions 1. Identify the type of reaction 2. Predict the product(s) using the type of reaction as a model 3. Balance it Don’t forget about the diatomic elements! (BrINClHOF) or (7 + 1) For example, Oxygen is O 2 as an element. In a compound, it can’t be a diatomic element because it’s not an element anymore, it’s a compound!

11. 1. Synthesis reactions Synthesis reactions occur when two substances (generally elements) combine and form a compound. (Sometimes these are called combination or addition reactions.) Synthesis reactions occur when two substances (generally elements) combine and form a compound. (Sometimes these are called combination or addition reactions.) reactant + reactant  1 product Basically: A + B  AB Basically: A + B  AB Example: 2H 2 + O 2  2H 2 O Example: 2H 2 + O 2  2H 2 O Example: C + O 2  CO 2 Example: C + O 2  CO 2

12. Synthesis Reactions Here is another example of a synthesis reaction Here is another example of a synthesis reaction

13. Practice Predict the products. Write and balance the following synthesis reaction equations. Predict the products. Write and balance the following synthesis reaction equations. Sodium metal reacts with chlorine gas Sodium metal reacts with chlorine gas Na (s) + Cl 2(g)  Na (s) + Cl 2(g)  Solid Magnesium reacts with fluorine gas Solid Magnesium reacts with fluorine gas Mg (s) + F 2(g)  Mg (s) + F 2(g)  Aluminum metal reacts with fluorine gas Aluminum metal reacts with fluorine gas Al (s) + F 2(g)  Al (s) + F 2(g)  NaCl MgF 2 AlF 3

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15. 2. Decomposition Reactions Decomposition reactions occur when a compound breaks up into the elements or in a few to simpler compounds Decomposition reactions occur when a compound breaks up into the elements or in a few to simpler compounds 1 Reactant  Product + Product 1 Reactant  Product + Product In general: AB  A + B In general: AB  A + B Example: 2 H 2 O  2H 2 + O 2 Example: 2 H 2 O  2H 2 + O 2 Example: 2 HgO  2Hg + O 2 Example: 2 HgO  2Hg + O 2

16. Decomposition Reactions Another view of a decomposition reaction: Another view of a decomposition reaction:

17. Decomposition Exceptions Carbonates and chlorates are special case decomposition reactions that do not go to the elements. Carbonates and chlorates are special case decomposition reactions that do not go to the elements. Carbonates (CO 3 2- ) decompose to carbon dioxide and a metal oxide Carbonates (CO 3 2- ) decompose to carbon dioxide and a metal oxide Example: CaCO 3  CO 2 + CaO Example: CaCO 3  CO 2 + CaO Chlorates (ClO 3 - ) decompose to oxygen gas and a metal chloride Chlorates (ClO 3 - ) decompose to oxygen gas and a metal chloride Example: 2 Al(ClO 3 ) 3  2 AlCl 3 + 9 O 2 Example: 2 Al(ClO 3 ) 3  2 AlCl 3 + 9 O 2 There are other special cases, but we will not explore those in this class There are other special cases, but we will not explore those in this class

18. Practice Predict the products. Then, write and balance the following decomposition reaction equations: Predict the products. Then, write and balance the following decomposition reaction equations: Solid Lead (IV) oxide decomposes PbO 2(s)  Solid Lead (IV) oxide decomposes PbO 2(s)  Aluminum nitride decomposes Aluminum nitride decomposes AlN (s)  AlN (s)  Pb + O 2 Al + N 2

19. Practice Identify the type of reaction for each of the following synthesis or decomposition reactions, and write the balanced equation: N 2(g) + O 2(g)  BaCO 3(s)  Co (s) + S (s)  NI 3(s)  (Co = +3) Nitrogen monoxide 2 NO BaO + CO 2 Co 2 S 3 2, 3, 1 N 2 + I 2 2, 1, 3

20. 3. Single Replacement Reactions Single Replacement Reactions occur when one element replaces another in a compound. Single Replacement Reactions occur when one element replaces another in a compound. A metal can replace a metal (+) OR a nonmetal can replace a nonmetal (-). A metal can replace a metal (+) OR a nonmetal can replace a nonmetal (-). element + compound  element + compound element + compound  element + compound A + BC  AC + B (if A is a metal) OR A + BC  BA + C (if A is a nonmetal) (remember the cation always goes first!) When H 2 O splits into ions, it splits into H + and OH - (not H+ and O -2 !!)

21. Single Replacement Reactions Another view: Another view:

22. A displacement reaction: metallic copper with silver nitrate Cu + Ag NO 3 Ag + Cu(NO 3 ) 2

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24. Single Replacement Reactions Write and balance the following single replacement reaction equation: Write and balance the following single replacement reaction equation: Zinc metal reacts with aqueous hydrochloric acid Zinc metal reacts with aqueous hydrochloric acid Zn (s) + HCl (aq)  Zn (s) + HCl (aq)  ZnCl 2 + H 2(g) Note: Zinc replaces the hydrogen ion in the reaction 2

25. Single Replacement Reactions Sodium chloride solid reacts with fluorine gas Sodium chloride solid reacts with fluorine gas NaCl (s) + F 2(g)  NaF (s) + Cl 2(g) NaCl (s) + F 2(g)  NaF (s) + Cl 2(g) Note that fluorine replaces chlorine in the compound Aluminum metal reacts with aqueous copper (II) nitrate Aluminum metal reacts with aqueous copper (II) nitrate Al (s) + Cu(NO 3 ) 2(aq)  Al (s) + Cu(NO 3 ) 2(aq)  Al(NO 3 ) 3(aq) + Cu 2, 3, 2, 3 Demo Time!! 22

26. Types of Chemical Reactions: At the conclusion of our time together, you should be able to: 1.List the 5 basic types of chemical reactions 2.Use this list to describe a reaction What are the 3 types of chemical reactions that we’ve covered so far???

27. 4. Double Replacement Reactions Double Replacement Reactions occur when a metal replaces a metal in a compound and a nonmetal replaces a nonmetal in a compound Double Replacement Reactions occur when a metal replaces a metal in a compound and a nonmetal replaces a nonmetal in a compound Compound + compound  compound+ compound Compound + compound  compound+ compound AB + CD  AD + CB AB + CD  AD + CB

28. Double Replacement Reactions Think about it like “foil”ing in algebra, first and last ions go together + inside ions go together Think about it like “foil”ing in algebra, first and last ions go together + inside ions go together Example: Example: AgNO 3(aq) + NaCl (s)  AgCl (s) + NaNO 3(aq) AgNO 3(aq) + NaCl (s)  AgCl (s) + NaNO 3(aq) Another example: Another example: K 2 SO 4(aq) + Ba(NO 3 ) 2(aq)  KNO 3(aq) + BaSO 4(s) 2

29. 3 Driving Forces for Double Replacement Reactions Water Forms Gas Forms Solid Forms If one of the above is not a product, there will be no reaction.

30. Practice Predict the products. Don’t balance the equation. Predict the products. Don’t balance the equation. 1. HCl (aq) + AgNO 3 (aq)  2. CaCl 2 (aq) + Na 3 PO 4 (aq)  3. Pb(NO 3 ) 2(aq) + BaCl 2 (aq)  4. Demo Time!! AgCl + HNO 3 NaCl + Ca 3 (PO 4 ) 2 Ba(NO 3 ) 2 + PbCl 2

31. 5. Combustion Reactions Combustion reactions occur when a hydrocarbon reacts with oxygen gas. Combustion reactions occur when a hydrocarbon reacts with oxygen gas. This is also called burning!!! In order to burn something you need the 3 things in the “fire triangle”: This is also called burning!!! In order to burn something you need the 3 things in the “fire triangle”: 1) A Fuel (hydrocarbon) 2) Oxygen to burn it with 3) Something to ignite the reaction (spark) 1) A Fuel (hydrocarbon) 2) Oxygen to burn it with 3) Something to ignite the reaction (spark)

32. Combustion Reactions In general: C x H y + O 2  CO 2 + H 2 O In general: C x H y + O 2  CO 2 + H 2 O Products in combustion are ALWAYS carbon dioxide and water. (although incomplete burning does cause some by- products like carbon monoxide) Products in combustion are ALWAYS carbon dioxide and water. (although incomplete burning does cause some by- products like carbon monoxide) Combustion is used to heat homes and run automobiles (octane, as in gasoline, is C 8 H 18 ) Combustion is used to heat homes and run automobiles (octane, as in gasoline, is C 8 H 18 )

33. Combustion Reactions Combustion Reactions Edgar Allen Poe’s drooping eyes and mouth are potential signs of CO poisoning.

34. Combustion Example Example C 5 H 12 + O 2  CO 2 + H 2 O C 5 H 12 + O 2  CO 2 + H 2 O Write the products and balance the following combustion reaction: Write the products and balance the following combustion reaction: C 10 H 22 + O 2  C 10 H 22 + O 2  CO 2 + H 2 O 568 20 31 22 2

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36. Types of Chemical Reactions Review: Let’s see if you can: 1.List the 5 basic types of chemical reactions 2.Use this list to describe a reaction

37. Mixed Practice State the type, predict the products, and balance the following reactions: State the type, predict the products, and balance the following reactions: 1. BaCl 2 + H 2 SO 4  2. C 6 H 12 + O 2  3. Zn + CuSO 4  4. Cs + Br 2  5. FeCO 3  Double Displacement Combustion Single Displacement Synthesis Decomposition

38. I don’t feel so stupid now…