1. Great and Glorious Test Day
Starter S-105
Test Day
Great and Glorious Test Day
Yahoo
Yipee
Yah

2. Starter S-101 What is the chemical formula for Hydrochloric Acid
Nitrogen Dioxide
Iron (II) Phosphate

3. Chapter 11
Chemical Reactions

4. 11.1 Describing Chemical Reactions
Chapter 11
11.1 Describing Chemical Reactions

5. 11.1 Describing Chemical Reactions
Writing Chemical Reactions
Word Equations – gives the names of compounds and elements in the equation
reactants  products
Reactants – compounds and elements before the reaction
Products – compounds and elements after the reaction

6. 11.1 Describing Chemical Reactions
Different compounds, or elements are separated by a plus sign
Copper + Oxygen  Copper (II) Oxide
These are often converted from descriptions of the reaction

7. 11.1 Describing Chemical Reactions
When antiseptic hydrogen peroxide is put in an open cut bubbles of oxygen form rapidly. Water is also produced.
Reaction – reactants
hydrogen peroxide

8. 11.1 Describing Chemical Reactions
When antiseptic hydrogen peroxide in an open cut bubbles of oxygen from rapidly. Water is also produced.
Reaction – products
hydrogen peroxide

9. 11.1 Describing Chemical Reactions
When antiseptic hydrogen peroxide in an open cut bubbles of oxygen from rapidly. Water is also produced.
Reaction – products
hydrogen peroxide  oxygen + water

10. 11.1 Describing Chemical Reactions
When a stove burner is lit, methane gas reacts with oxygen to form carbon dioxide and water.
Reaction – reactants
methane gas + oxygen

11. 11.1 Describing Chemical Reactions
When a stove burner is lit, methane gas reacts with oxygen to carbon dioxide and water.
Reaction – products
methane gas + oxygen

12. 11.1 Describing Chemical Reactions
When a stove burner is lit, methane gas reacts with oxygen to carbon dioxide and water.
Reaction – products
methane gas + oxygen  carbon dioxide + water

13. 11.1 Describing Chemical Reactions
Chemical Equations – replace the names of compounds and elements with the chemical formula
hydrogen peroxide  oxygen + water
H2O2  O2 + H2O
Remember diatomic elements

14. 11.1 Describing Chemical Reactions
methane gas + oxygen  carbon dioxide + water
CH4 + O2  CO2 + H2O

15. 11.1 Describing Chemical Reactions
Usually the state of
each compound
or element is
given beside the
formula
CH4(g)+ O2(g)  CO2(g) + H2O(g)
Solid
(s)
Liquid
(l)
Gas
(g)
Aqueous
(aq)

16. Starter S-102 When solutions of potassium iodide and
lead (II) nitrate are mixed in a beaker, a
brilliant yellow solid is formed.
This solid when analyzed turns
out to be lead (II) iodide.
Further analysis shows that
potassium nitrate is now dissolved
in the water.
Write the word equation.
Write the chemical equation

17. Starter S-106
A chunk of iron is placed in a solution of hydrochloric acid. A gas bubbles out of the solution that is tested and found to be hydrogen. The solution left in the test tube is iron (III) chloride.

18. Starter S-107
Water is placed in a test tube and zapped with electricity. Two gases are produced. One makes a glowing wooden split light up, so it is oxygen. The other causes a small explosion when a burning wooden splint is placed in it, so it is hydrogen.

19. 11.1 Describing Chemical Reactions
Balancing Chemical Equations – both sides of a chemical equation have the same number of each atom
Mass is conserved
Balancing Demo

20. 11.1 Describing Chemical Reactions
Example
Al + O2  Al2O3
1. Write elements on each side and how many of each are present

21. 11.1 Describing Chemical Reactions
Example
Al + O2  Al2O3
Al – 1 Al – 2
O – 2 O – 3
2. Add one element at a time to the side that doesn’t have enough

22. 11.1 Describing Chemical Reactions
Al + O2  Al2O3
Al – 2 Al – 2
O – 2 O – 3

23. 11.1 Describing Chemical Reactions
Al O2
Al + O2  Al2O3
Al – 2 Al – 2
O – 4 O – 3

24. 11.1 Describing Chemical Reactions
Al O2 Al2O3
Al + O2  Al2O3
Al – 2 Al – 4
O – 4 O – 6

25. 11.1 Describing Chemical Reactions
Al,Al,Al O2 Al2O3
Al + O2  Al2O3
Al – 4 Al – 4
O – 4 O – 6

26. 11.1 Describing Chemical Reactions
Al,Al,Al O2,O2 Al2O3
Al + O2  Al2O3
Al – 4 Al – 4
O – 6 O – 6
Balanced
3. Count the number of each compound or element – write a coefficient for each

27. 11.1 Describing Chemical Reactions
4Al + 3O2  2Al2O3

28. 11.1 Describing Chemical Reactions
Balance the following equations
Cu + AgNO3  Cu(NO3)2 + Ag

29. 11.1 Describing Chemical Reactions
Balance the following equations
Cu + 2AgNO3  Cu(NO3)2 + 2Ag
FeCl3 + NaOH  Fe(OH)3 + NaCl

30. 11.1 Describing Chemical Reactions
Balance the following equations
Cu + 2AgNO3  Cu(NO3)2 + 2Ag
FeCl3 + 3NaOH  Fe(OH)3 + 3NaCl
CS2 + Cl2  CCl4 + S2Cl2

31. 11.1 Describing Chemical Reactions
Balance the following equations
Cu + 2AgNO3  Cu(NO3)2 + 2Ag
FeCl3 + 3NaOH  Fe(OH)3 + 3NaCl
CS2 + 3Cl2  CCl4 + S2Cl2
AgNO3 + H2S  Ag2S + HNO3

32. 11.1 Describing Chemical Reactions
Balance the following equations
Cu + 2AgNO3  Cu(NO3)2 + 2Ag
FeCl3 + 3NaOH  Fe(OH)3 + 3NaCl
CS2 + 3Cl2  CCl4 + S2Cl2
2AgNO3 + H2S  Ag2S + 2HNO3
Zn(OH)2 + H3PO4  Zn3(PO4)2 + H2O

33. 11.1 Describing Chemical Reactions
Balance the following equations
Cu + 2AgNO3  Cu(NO3)2 + 2Ag
FeCl3 + 3NaOH  Fe(OH)3 + 3NaCl
CS2 + 3Cl2  CCl4 + S2Cl2
2AgNO3 + H2S  Ag2S + 2HNO3
3Zn(OH)2 + 2H3PO4  Zn3(PO4)2 + 6H2O
Fe2O3 + H2  Fe + H2O

34. 11.1 Describing Chemical Reactions
Balance the following equations
Cu + 2AgNO3  Cu(NO3)2 + 2Ag
FeCl3 + 3NaOH  Fe(OH)3 + 3NaCl
CS2 + 3Cl2  CCl4 + S2Cl2
2AgNO3 + H2S  Ag2S + 2HNO3
3Zn(OH)2 + 2H3PO4  Zn3(PO4)2 + 6H2O
Fe2O3 + 3H2  2Fe + 3H2O

35. Starter S-107
Balance
C6H6 + O2  CO2 + H2O
CH3CH2OH + O2  CO2 + H2O

36. 11.2 Types of Chemical Reactions
Chapter 11
11.2 Types of Chemical Reactions

37. 11.2 Type of Chemical Reactions
11.2 Types of Chemical Reactions
You will need to know and predict the product for 6 types of chemical reactions
Synthesis
Form
Example
Synthesis

38. 11.2 Type of Chemical Reactions
11.2 Types of Chemical Reactions
2. Decomposition
Form
Example
Decomposition

39. 11.2 Type of Chemical Reactions
11.2 Types of Chemical Reactions
3. Single Replacement Reaction
Form
Example
For metals, the reactions occurs if
the metal is more reactive than the
the one in the compound
Single

40. 11.2 Type of Chemical Reactions
11.2 Types of Chemical Reactions
4. Double Replacement Reaction
Form
Example
Double

41. 11.2 Type of Chemical Reactions
11.2 Types of Chemical Reactions
5. Combustion Reaction
Form
Example
Combustion

42. 11.2 Type of Chemical Reactions
11.2 Types of Chemical Reactions
6. Acid/Base Neutralization Reaction
Form
Example
The substance AB is called a
Chemical Salt
Acid Base

43. 11.2 Type of Chemical Reactions
11.2 Types of Chemical Reactions
Reactions are predicted based on recognizing forms.

44. Starter S-110 What type of reaction is this? CaCl2 + Pb(NO3)2 
Write the complete balanced equation

45. Objective
I can perceive and predict products for at least six different types of chemical reactions.

46. 11.2 Type of Chemical Reactions
11.2 Types of Chemical Reactions
Reaction
AgNO3 + NaCl 
Type:
Double Replacement
Products:
AgNO3 + NaCl  AgCl + NaNO3
Balanced:

47. 11.2 Type of Chemical Reactions
11.2 Types of Chemical Reactions
Reaction
Pb + AgNO3 
Type:
Single Replacement
Products:
Pb + AgNO3  Ag + Pb(NO3)2
Balanced:
Pb + 2AgNO3  2Ag + Pb(NO3)2

48. 11.2 Type of Chemical Reactions
11.2 Types of Chemical Reactions
Reaction
FeCl3 + KOH 
Type:
Double Replacement
Products:
FeCl3 + KOH  Fe(OH)3 + KCl
Balanced:
FeCl3 + 3KOH  Fe(OH)3 + 3KCl

49. 11.2 Type of Chemical Reactions
11.2 Types of Chemical Reactions
Reaction
NaOH + H2SO4 
Type:
Acid Base Neutralization
Products:
NaOH + H2SO4  Na2SO4 + H2O
Balanced:
2NaOH + H2SO4  Na2SO4 + 2H2O

50. 11.2 Type of Chemical Reactions
11.2 Types of Chemical Reactions
Reaction
C2H8 + O2 
Type:
Combustion
Products:
C2H8 + O2  CO2 + H2O
Balanced:
C2H8 + 4O2  2CO2 + 4H2O

51. 11.2 Type of Chemical Reactions
11.2 Types of Chemical Reactions
Reaction
NH3 
Type:
Decomposition
Products:
NH3  N2 + H2
Balanced:
2NH3  N2 + 3H2

52. 11.2 Type of Chemical Reactions
11.2 Types of Chemical Reactions
Reaction
Bi(NO3)3 + H2S 
Type:
Double Replacement
Products:
Bi(NO3)3 + H2S  Bi2S3 + HNO3
Balanced:
2Bi(NO3)3 + 3H2S  Bi2S3 + 6HNO3

53. 11.2 Type of Chemical Reactions
11.2 Types of Chemical Reactions
Reaction
Ca + F2 
Type:
Synthesis
Products:
Ca + F2  CaF2
Balanced:

54. Starter S-112 What type of reaction is C2H5OH + O2 
Write and balance the reaction

55. 11.3 Reactions in Aqueous Solutions
Chapter 11
11.3 Reactions in Aqueous Solutions

56. 11.2 Type of Chemical Reactions
11.3 Reactions in Aqueous Solution
Many reactions take place in water – aqueous
For example, the reaction of Silver Nitrate and Sodium Chloride
But in a solution, most ionic compounds have dissociated to form ions

57. 11.2 Type of Chemical Reactions
11.3 Reactions in Aqueous Solution
That is they are really in this form
This is called the Complete Ionic Equation
Notice – the solid is not broken into ions, only what is in solution

58. 11.2 Type of Chemical Reactions
11.3 Reactions in Aqueous Solution
Look carefully at the equation
There are Na+ and NO3- ions that stay the same
These are called Spectator Ions
A Net Ionic Equation shows only ions that actually do something in a reaction

59. 11.2 Type of Chemical Reactions
11.3 Reactions in Aqueous Solution
Net Ionic Equation
Try this one

60. 11.2 Type of Chemical Reactions
11.3 Reactions in Aqueous Solution
Practice
Equation
Compete Ionic Equations
Net Ionic Equation

61. Starter S-113 Write the complete ionic and net ionic equations for
Fe(NO3)3(aq) + 3NaOH(aq)  Fe(OH)3(s) + 3NaNO3(aq)
Complete Ionic
Fe+3(aq)+3NO3-(aq) + 3Na+(aq)+3OH-(aq) Fe(OH)3(s)+ 3Na+(aq)+3NO3-(aq)
Net Ionic
Fe+3(aq)+3OH-(aq) Fe(OH)3(s)

62. Starter S-115 A. Write the complete ionic and net ionic equations for
Cu(s) + AgNO3(aq)  Ag(s) + Cu(NO3)2(aq)
random squirrel with light saber

63. Practice

64. 11.2 Type of Chemical Reactions
11.3 Reactions in Aqueous Solution
Precipitate – separates from a solution as a solid
Predicted using a solubility
chart
In the reaction
Is either product a solid?
Chart

65. 11.2 Type of Chemical Reactions
11.3 Reactions in Aqueous Solution
AgCl – insoluble
NaNO3

66. 11.2 Type of Chemical Reactions
11.3 Reactions in Aqueous Solution
AgCl – insoluble - solid
NaNO3

67. 11.2 Type of Chemical Reactions
11.3 Reactions in Aqueous Solution
AgCl – insoluble - solid
NaNO3 – soluble

68. 11.2 Type of Chemical Reactions
11.3 Reactions in Aqueous Solution
AgCl – insoluble - solid
NaNO3 – soluble - aqueous

69. Starter S-115 A. Write the complete ionic and net ionic equations for
Cu(s) + AgNO3(aq)  Ag(s) + Cu(NO3)2(aq)
B. Which of the following are soluble
Cu(OH)2
Mg(NO3)2
AgCl random squirrel with light saber

70. Starter S-117
Predict the products of the following reaction. Determine the correct states for the products
AgNO3(aq) + NaCl(aq) 

71. Starter S-117
Test

72. Starter S-119
Predict the products of the following reaction. Determine the correct states for the products
KOH + Mg(NO3)2 

73. Starter S-120
Predict the products of the following reaction. Determine the correct states for the products
Cu(NO3)2 + Fe(OH)3 

74. Starter S-122
How would you identify the following aqueous solutions? Name a simple test.
AgNO3
H2SO4
KOH
Cu(NO3)2
CoCl2

75. Starter S-122 If 12.0 g of AgCl react What is the molar mass of AgCl?
How many moles of AgCl are present as a reactant?
Silver chloride precipitate