1. CHAPTER 10
Chemical Reactions
10.3 Types of Chemical Reactions

2. Chemical equations tell stories…
Reactants Products

3. Chemical equations tell stories…
Reactants Products
… and stories can be put into different categories

4. Chemical equations tell stories…
Reactants Products
… and stories can be put into different categories
Nonfiction
Science fiction
Adventure
Romance
History
Psychology
Children’s literature …

5. Chemical equations tell stories…
Reactants Products
… and stories can be put into different categories
Nonfiction
Science fiction
Adventure
Romance
History
Psychology
Children’s literature …
Synthesis / Decomposition
Single / Double replacement
Precipitate reaction
Polymerization reaction

6. Synthesis Synthesis reaction
Two compounds combine to make a third compound

7. Synthesis Synthesis reaction
Two compounds combine to make a third compound
Example:

8. Synthesis Synthesis reaction
Two compounds combine to make a third compound
Example:
One compound
Another compound
A third compound

9. Synthesis Synthesis reaction
Two compounds combine to make a third compound
magnesium oxide
magnesium hydroxide
water

10. Synthesis Synthesis reaction
Two compounds combine to make a third compound
magnesium oxide
magnesium hydroxide
water
One compound
Another compound
A third compound

11. Synthesis Synthesis reaction
Two compounds combine to make a third compound
magnesium oxide
magnesium hydroxide
water
Milk of magnesia,
a common medicine, is a suspension of Mg(OH)2 in water

12. Decomposition Decomposition reaction
One compound breaks apart into two or more compounds or elements

13. Decomposition Decomposition reaction
One compound breaks apart into two or more compounds or elements
Example:
Decomposition of water

14. Decomposition Decomposition reaction
One compound breaks apart into two or more compounds or elements
Example:
Decomposition of water
One compound
Two new compounds

15. Decomposition Decomposition reaction
One compound breaks apart into two or more compounds or elements
Example:
Decomposition of ozone

16. Decomposition Decomposition reaction
One compound breaks apart into two or more compounds or elements
Example:
Decomposition of ozone
One compound
Two new compounds

17. calcium carbonate (in limestone)
Decomposition
Decomposition reaction
One compound breaks apart into two or more compounds or elements
At 825oC:
calcium carbonate (in limestone)
calcium oxide (lime)
carbon dioxide

18. calcium carbonate (in limestone)
Decomposition
Decomposition reaction
One compound breaks apart into two or more compounds or elements
At 825oC:
calcium carbonate (in limestone)
calcium oxide (lime)
carbon dioxide
One compound
Two new compounds

19. Synthesis
A new compound is formed

20. Synthesis Decomposition A new compound is formed
A compound is broken down

21. Single replacement Single replacement reaction
Two compounds swap a single element or polyatomic ion

22. Single replacement Single replacement reaction
Two compounds swap a single element or polyatomic ion
Example:

23. Single replacement Single replacement reaction
Two compounds swap a single element or polyatomic ion
Example:

24. Single replacement Single replacement reaction
Two compounds swap a single element or polyatomic ion
Another example:

25. Single replacement Single replacement reaction
Two compounds swap a single element or polyatomic ion
Another example:

26. Double replacement Double replacement reaction
Two compounds exchange parts

27. Double replacement Pb(NO3)2(aq) + 2KI(aq) PbI2(s) + 2KNO3(aq)
Double replacement reaction
Two compounds exchange parts
Example:
Pb(NO3)2(aq) + 2KI(aq) PbI2(s) + 2KNO3(aq)

28. Double replacement Pb(NO3)2(aq) + 2KI(aq) PbI2(s) + 2KNO3(aq)
Double replacement reaction
Two compounds exchange parts
Example:
Pb(NO3)2(aq) + 2KI(aq) PbI2(s) + 2KNO3(aq)

29. Synthesis Decomposition Single replacement A new compound is formed
A compound is broken down
Single replacement
An element or ion is swapped

30. Synthesis Decomposition Single replacement Double replacement
A new compound is formed
Decomposition
A compound is broken down
Single replacement
An element or ion is swapped
Double replacement
Two element or ion are swapped

31. Pb(NO3)2(aq) + 2KI(aq) PbI2(s) + 2KNO3(aq)
This equation was used as an example for a double replacement reaction.
Pb(NO3)2(aq) + 2KI(aq) PbI2(s) + 2KNO3(aq)

32. Precipitate reaction Pb(NO3)2(aq) + 2KI(aq) PbI2(s) + 2KNO3(aq)
An insoluble compound is formed
This equation was used as an example for a double replacement reaction.
It is also a precipitate reaction.
Pb(NO3)2(aq) + 2KI(aq) PbI2(s) + 2KNO3(aq)

33. Double replacement
Pb(NO3)2(aq) + 2KI(aq) PbI2(s) + 2KNO3(aq)

34. Double replacement
Pb(NO3)2(aq) + 2KI(aq) PbI2(s) + 2KNO3(aq)

35. Double replacement
Pb(NO3)2(aq) + 2KI(aq) PbI2(s) + 2KNO3(aq)

36. Precipitate reaction Pb(NO3)2(aq) + 2KI(aq) PbI2(s) + 2KNO3(aq)
An insoluble compound is formed
This equation was used as an example for a double replacement reaction.
It is also a precipitate reaction.
Pb(NO3)2(aq) + 2KI(aq) PbI2(s) + 2KNO3(aq)
Insoluble PbI2
Solid
(precipitate)
K+ K+ NO3–
Dissolved ions

37. There are solubility rules we can follow
Precipitate reaction
Can we predict if a reaction product is going to be soluble or insoluble in water?
Yes!
There are solubility rules we can follow
PbI2(s) + 2KNO3(aq)
Solid
(precipitate)
K+ K+ NO3–
Dissolved ions

38. Precipitate reaction
Solubility rules for common ionic compounds in water

39. Precipitate reaction PbI2(s) + 2KNO3(aq)
Solubility rules for common ionic compounds in water
PbI2(s) + 2KNO3(aq)
Solid
(precipitate)
K+ K+ NO3–
Dissolved ions

40. Precipitate reaction PbI2(s) + 2KNO3(aq)
Solubility rules for common ionic compounds in water
PbI2(s) + 2KNO3(aq)
Solid
(precipitate)
K+ K+ NO3–
Dissolved ions

41. Precipitate reaction PbI2(s) + 2KNO3(aq)
Solubility rules for common ionic compounds in water
PbI2(s) + 2KNO3(aq)
Solid
(precipitate)
K+ K+ NO3–
Dissolved ions

42. Precipitate reaction
Minerals such as Mg2+ and Ca2+ leach into our water supply and cause a phenomenon known as “water hardness.”

43. Precipitate reaction
Minerals such as Mg2+ and Ca2+ leach into our water supply and cause a phenomenon known as “water hardness.”
How can we remove magnesium and calcium ions, which are soluble in water?

44. Precipitate reaction
Minerals such as Mg2+ and Ca2+ leach into our water supply and cause a phenomenon known as “water hardness.”
We can add Na2CO3 and cause a precipitate reaction
Precipitates are easy to remove!

45. Precipitate reaction
Predict what happens when silver nitrate (AgNO3) is mixed with sodium chloride (NaCl). Follow the steps and write the complete balanced equation.

46. Precipitate reaction
Predict what happens when silver nitrate (AgNO3) is mixed with sodium chloride (NaCl). Follow the steps and write the complete balanced equation.
Asked: The reaction that represents the mixing of AgNO3 and NaCl
Given: Formulas for both reactant solutions
Relationships: Solubility rules tell us that group 1 metal ions (here Na+) and nitrates are soluble, but chlorides of silver are insoluble.

47. Precipitate reaction
Predict what happens when silver nitrate (AgNO3) is mixed with sodium chloride (NaCl). Follow the steps and write the complete balanced equation.
Asked: The reaction that represents the mixing of AgNO3 and NaCl
Given: Formulas for both reactant solutions
Relationships: Solubility rules tell us that group 1 metal ions (here Na+) and nitrates are soluble, but chlorides of silver are insoluble.
Solve: AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) According to the solubility table, sodium nitrate is soluble and dissociates into Na+(aq) and NO3–(aq). Silver chloride is insoluble and forms a precipitate.

48. Precipitate reaction
Predict what happens when silver nitrate (AgNO3) is mixed with sodium chloride (NaCl). Follow the steps and write the complete balanced equation.
Asked: The reaction that represents the mixing of AgNO3 and NaCl
Given: Formulas for both reactant solutions
Relationships: Solubility rules tell us that group 1 metal ions (here Na+) and nitrates are soluble, but chlorides of silver are insoluble.
Solve: AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) According to the solubility table, sodium nitrate is soluble and dissociates into Na+(aq) and NO3–(aq). Silver chloride is insoluble and forms a precipitate.
Discussion: We know the precipitate is AgCl because it does not have a group 1 metal ion or nitrate. All ions are balanced.

49. Synthesis Decomposition Single replacement Double replacement
A new compound is formed
Decomposition
A compound is broken down
Single replacement
An element or ion is swapped
Double replacement
Two element or ion are swapped
Precipitate reaction
A precipitate is formed

50. Polymerization + Polymerization
A reaction that assembles a polymer through repeated additions of smaller molecular fragments (monomers)
monomers
Note that this is also a synthesis reaction +

51. Polymerization + + Polymerization
A reaction that assembles a polymer through repeated additions of smaller molecular fragments (monomers)
monomers + +

52. Polymerization + + Polymerization
A reaction that assembles a polymer through repeated additions of smaller molecular fragments (monomers)
monomers + +
repeatedly add a monomer

53. Polymerization + + Polymerization
A reaction that assembles a polymer through repeated additions of smaller molecular fragments (monomers)
monomers + +
a polymer
repeatedly add a monomer

54. Glucose C6H12O6

55. Two glucose monomers react and produce a molecule of water
Glucose C6H12O6
Two glucose monomers react and produce a molecule of water

56. Two glucose monomers react and produce a molecule of water
Water H2O
Glucose C6H12O6
Two glucose monomers react and produce a molecule of water

57. Two glucose monomers react and produce a molecule of water
This reaction is called dehydration synthesis
(a synthesis involving a “loss” of water)
Water H2O
Glucose C6H12O6
Two glucose monomers react and produce a molecule of water

58. Starch [C6H10O5]n

59. Synthesis Decomposition A new compound is formed
A compound is broken down

60. Synthesis Decomposition Single replacement Double replacement
A new compound is formed
Decomposition
A compound is broken down
Single replacement
An element or ion is swapped
Double replacement
Two element or ion are swapped

61. Synthesis Decomposition Single replacement Double replacement
A new compound is formed
Decomposition
A compound is broken down
Single replacement
An element or ion is swapped
Double replacement
Two element or ion are swapped
Precipitate reaction
A precipitate is formed
Polymerization
A polymer is assembled

62. Synthesis Decomposition Single replacement Double replacement
A new compound is formed
Decomposition
A compound is broken down
Single replacement
An element or ion is swapped
Double replacement
Two element or ion are swapped
Precipitate reaction
A precipitate is formed
Polymerization
A polymer is assembled