1. OB: intro to 5 chemical reactions (5)
1. In a chemical reaction bonds are broken and new ones form. New substances form, these new substances have their own properties. There are a variety of kinds of reactions which we will learn about, learn to recognize, and then to write balanced chemical equations for.
The first kind of reaction is called the SYNTHESIS REACTION.
2. n a synthesis reaction, smaller reactants combine to form larger products.
3. A + B AB (this is the abstract)
4. Reactants form into products

2. 6. When bonds form, energy is released.
Examples of word equations… 5. A WORD EQUATION shows the chemical reaction in WORDS not symbols.
Hydrogen and oxygen synthesize into water
Carbon and oxygen combine into carbon monoxide
Carbon monoxide and oxygen synthesize into carbon dioxide
Iron and oxygen form into iron (III) oxide (or rust)
In each case, smaller reactants form into larger products.
6. When bonds form, energy is released.
To break bonds, energy must be absorbed.
We will memorize 5 kinds of chemical reactions this week.

3. 10. Demo #1 Synthesis Reactions
Hydrogen
Oxygen in air
With a flame, we will ignite the hydrogen, allowing it to combine with the oxygen in the air, synthesizing into water (in a FAST AND LOUD WAY!)

4. 11. Abstract examples: A + B AB or X + YZ XYZ
12. Word equation: hydrogen and oxygen yields water
14. Skeleton:
15. Balanced Equation:
16. Balanced Thermochemical Equation: _________________________________

5. Abstract examples: A + B AB or X + YZ XYZ
SYNTHESIS REACTION – Demo diagram #1
Abstract examples: A + B AB or X + YZ XYZ
Word equation: hydrogen and oxygen yields water
Skeleton: H2 + O H2O
Balanced Equation: 2H2(G) + O2(G) H2O(G)
Balanced Thermochemical Equation: H2(G) + O2(G) H2O(G) Energy

6. 17. A synthesis reaction always has two or more smaller reactants combining into larger products.
18. Today’s reaction was exothermic, but sometimes these reactions can absorb energy (heat) and are called endothermic.
We start with a skeleton, then work out the balancing.
19. We cannot “fix” subscripts, they are set by formula rules. We can adjust ratios by adding coefficients.

7. From the word equation, write the skeleton equation, then balance the chemical reaction. Add phase symbols where ever you can.
20. Sodium + chlorine yields sodium chloride

8. Na + Cl2 NaCl 2Na(S) + Cl2(G) 2NaCl(S)
From the word equation, write the skeleton equation, then balance the chemical reaction. Add phase symbols where ever you can.
20. Sodium + chlorine yields sodium chloride
Na + Cl NaCl
2Na(S) + Cl2(G) NaCl(S)
For the next few slides, write the word equation, under it write a skeleton equation, then write a balanced chemical equation.

9. 21. Iron + Oxygen synthesizes to iron III oxide (rust)

10. 21. Iron + Oxygen synthesizes to iron III oxide (rust)
4Fe(S) + 3O2(G) Fe2O3(S)

11. 22. Aluminum + Nitrogen synthesize into aluminum nitride

12. 22. Aluminum + Nitrogen synthesize into aluminum nitride
2Al(S) + N2(G) AlN(S)

13. 23. Potassium and chlorine make potassium chloride

14. 23. Potassium and chlorine make potassium chloride
2K(S) + Cl2(G) KCl(S)

15. H2 + O2 H2O C + O2 CO CO + O2 CO2 Fe + O2 Fe2O3
24. Examples of skeleton equations… Balance them now.
H O H2O
C + O CO
CO O CO2
Fe O Fe2O3

16. 2H2 + O2 2H2O 2C + O2 2CO 2CO + O2 2CO2 4Fe + 3O2 2Fe2O3
24. Examples of skeleton equations… Balance them now.
2H O H2O
2C + O CO
2CO O CO2
4Fe O Fe2O3

17. PbO Pb + O2 (skeleton) 2PbO 2Pb + O2 (balanced)
OB: All about decomposition reactions
25. Decomposition reactions are the opposite of synthesis, where a larger reactant is broken down into 2 or more smaller products
26. AB A + B or XYZ X + YZ
27. In a decomposition reaction there is always ONE REACTANT, and 2 or more products
Examples….
Lead II oxide decomposes into lead and oxygen
PbO Pb + O (skeleton)
2PbO Pb + O (balanced)

18. hydrogen peroxide decomposes into water & oxygen gas
Demo Decomposition Reaction
29. Decomposition reactions require one reactant to break down into 2 or more smaller products
30. Abstract: ABC AB + C
31. Word equation
hydrogen peroxide decomposes into water & oxygen gas
32. Skeleton equation H2O H2O + O2

19. 35. You need to add a CATALYST
33. Balanced Chemical Reaction
2H2O2(L) H2O(L) + O2(G)
[back and forth, back and forth, pull your hair if you need to. Count the atoms on the reactant side and compare to the product side.
Four hydrogen in reactant, four in product, four oxygen in reactant, = 4 in product]
This reaction is SO SLOW, that watching it is for the birds (you can put that in your notes).
You can’t hurry love, you just have to wait… but in chemistry you can hurry things up.
35. You need to add a CATALYST

20. 2H2O2(L) 2H2O(L) + O2(G) + energy
36. PUT CATALYST on the arrow where it belongs.
2H2O2(L) H2O(L) + O2(G) + energy KI
By adding the potassium iodide catalyst, things go much faster. Write that catalyst above the arrow in the reaction. That shows it’s been added, but it does not affect the reaction except for how fast it goes.
The exact same reaction occurs with a catalyst as without, but when things happen fast, they appear to be different. There is NO DIFFERENCE in products, or amount of energy released, it’s just FASTER.

21. 37. Draw a picture
Excitement pops out the top, because the reaction is LOTS faster than before.
No catalyst, slow, decomposition happens, energy is released slowly
Add the KI catalyst
H2O2
becomes water

22. Use the following decomposition reaction word equations to create skeleton equations which you will balance properly with PHASE SYMBOLS.
38.
Magnesium nitride decomposes into magnesium & nitrogen.

23. Use the following decomposition reaction word equations to create skeleton equations which you will balance properly with PHASE SYMBOLS.
38. Magnesium nitride decomposes into magnesium & nitrogen.
Mg3N2(S) Mg(S) + N2(G)

24. 39. Magnesium carbonate decomposes into carbon dioxide & magnesium oxide

25. 39. Magnesium carbonate decomposes into carbon dioxide & magnesium oxide
MgCO3(S) CO2(G) + MgO(S)

26. 40. Iron (II) oxide decomposes

27. 40. Iron (II) oxide decomposes
2FeO(S) O2(G) + 2Fe(S)

28. 41A. AMMONIA gas decomposes
41B. Hydrogen monochloride gas decomposes

29. 2HCl(G) H2(G) + Cl2(G) 2NH3(G) N2(G) + 3H2(G) NH3(G) N2(G) + H2(G)
41. AMMONIA decomposes
NH3(G) N2(G) + H2(G)
2NH3(G) N2(G) + 3H2(G)
42. Hydrogen monochloride gas decomposes into hydrogen & chlorine gases
HCl(G) H2(G) + Cl2(G)
2HCl(G) H2(G) + Cl2(G)

30. Dinitrogen Pentoxide Decomposes into nitrogen and oxygen.

31. 41C.
Dinitrogen Pentoxide Decomposes into nitrogen and oxygen.
2N2O5(G) N2(G) + 5O2(G)

32. OB: Single Replacement Reactions or, connecting my love for Janet to Table J Single Replacement reactions (SR) starts with an aqueous solution and atoms being added to it.

33. 44. In this reaction, the atoms may have a high enough reactivity level to replace an ion in solution, bumping it out as a precipitate.
45. Example…
A(S) + BC(AQ) AC(AQ) + B(S) atoms + cation/anion solution become different cation/anion solution + different atoms
46. The atom A is put into the aqueous solution BC. A REPLACES B in solution, forming a new solution AC, and B falls out of the solution as a solid precipitate.
47. Predicting these reactions requires the Activity Series (Table J for Janet)

34. Mg(S) + HCl(AQ) Mg(S) metal is added to HCl(AQ) solution
48. Demo
Mg(S) metal is added to HCl(AQ) solution
Mg(S) + HCl(AQ)
49. There are 3 parts to this reaction so far: the Mg atom, the H+1 cation, & the Cl-1 anion
2 of these are on one side of table J, which 2?

35. Mg(S) + HCl(AQ) MgCl2(AQ) + H2(G)
50. It’s the Mg and H that are both on the left side of the table. Since Mg is higher up, that means Mg has a higher activity level, it will have the ability to bump the hydrogen cation out of solution. BALANCE THE SKELETON NOW
Mg(S) + HCl(AQ) MgCl2(AQ) + H2(G)

36. Mg(S) + 2HCl(AQ) MgCl2(AQ) + H2(G)
51. Balanced:
Mg(S) + 2HCl(AQ) MgCl2(AQ) + H2(G)
The ratio of Mg:HCl:MgCl2:H2 is 1:2:1:1,
John Dalton is happy.

37. 53. Single Replacement reactions start with ONE AQ solution
54. Abstract A(S) + BC(AQ) AC(AQ) + B(S)
55. Word Equation: copper into silver nitrate solution reacts… Write the SKELETON REACTION, then balance this equation.

38. Products: solid silver precipitate & Copper(I)nitrate
56. Write the SKELETON REACTION:
Cu(S) + AgNO3(AQ) CuNO3(AQ) + Ag(S)
Products: solid silver precipitate & Copper(I)nitrate
Copper replaces Silver in solution, the silver forms a solid precipitate.
Thinking of TOPIC-B? This is the “P”

39. Love + Table J Charlie gets married with a band of Gold (Au) from Janet…

40. 58. draw
Charlie’s Wedding Band
Made of
Solid gold!
HCl(AQ)

41. My wedding band is too important to leave to chance!
Table J tells us when reactions will happen, or not.
59. Au(S) + HCl (AQ) no reaction
60. Why? Because Au is lower on table J than H is, Gold is not active enough to bump out the hydrogen from solution!
My wedding band is too important to leave to chance!

42. Balance these SR reactions or write an X for no reaction
61. Mg(S)+ Zn(NO3)2(AQ)
Na(S) + Sn(NO3)2(AQ)
63. Cl2(G)+ KBr(AQ)

43. Balance these SR reactions or write an X for no reaction
61. Mg(S)+ Zn(NO3)2(AQ) Mg(NO3)2(AQ) + Zn(S)
Na(S) + Sn(NO3)2(AQ) NaNO3(AQ) + Sn(S)
63. Cl2(G)+ KBr(AQ) this one is special or different. Why?

44. 63. Cl2(G)+ 2KBr(AQ) 2KCl(AQ) + Br2(L)
This is an ANION REPLACEMENT type of SR. The chlorine replaces the bromine. The potassium hangs out.
The phase symbol here for bromine is probably liquid.

45. Balance these SR reactions or write an X for no reaction
Zn(S)+ H2SO4(AQ)
Li(S) + Co(NO3)3(AQ)
Au(S)+ KCl(AQ)

46. Balance these SR reactions or write an X for no reaction
Zn(S)+ H2SO4(AQ) ZnSO4(AQ) + H2(G)
65. 3Li(S) + Co(NO3)3(AQ) LiNO3(AQ) Co(S)
Au(S)+ KCl(AQ) X NO REACTION, gold is below potassium on table J

47. AB(AQ) + XY(AQ) AY(AQ) + XB(S)
OB: Double Replacement Reactions (4/5)
67. It takes 2 aqueous solutions to begin a double replacement reaction.
68. The cations switch anions with each other.
69. The reaction occurs if a precipitate forms in the products.
70. If no precipitate forms, a mixture formed, but no chemical reaction happened.
71. In the abstract:
AB(AQ) + XY(AQ) AY(AQ) + XB(S)

48. Double Replacement Table F
72. Must start with 2 AQ solutions, must end with 1 AQ solution + 1 SOLID PRECIPITATE
73. How will you know if a product is soluble in water (dissolves), or insoluble (a precipitate)? Use…
Table F
Take it out now…

49. Write on your tables FIRST, label the tops of each of the 4 columns.
Aqueous
SOLID
SOLID
Aqueous

50. Cu+2 and NO3-1 and NH4+1 and CO3-2
74. Example reaction:
Copper (II) nitrate solution + ammonium carbonate solutions combine…
First we must write the formulas correctly (watch ion charges)
Cu+2 and NO and NH4+1 and CO3-2

51. Now we balance, then check table F for aqueous or solid
Cations switch their Anions
Cu(NO3)2(AQ) (NH4)2CO3(AQ) NH4NO3 + CuCO3
Next, we check to see if our products are written properly according to ion charges
Ammonium + nitrate are in 1:1 ratio OK,
Cu+2 + CO also 1:1 OKAY
Now we balance, then check table F for aqueous or solid
Cu(NO3)2(AQ) (NH4)2CO3(AQ) NH4NO3 + CuCO3

52. AQ is aqueous, dissolved into water S is insoluble, or solid it water
75. Let’s look at table F. What’s AQ, what’s S?
Cu(NO3)2(AQ) + (NH4)2CO3(AQ) NH4NO3(AQ) + CuCO3(S)
2 aqueous solutions to start aqueous solution + 1 solid precipitate = DR
AQ is aqueous, dissolved into water
S is insoluble, or solid it water

53. Sodium hydroxide and copper (II) sulfate solutions combine…
Mental Plans for Double Replacement Reactions
AQ solutions combine, if you get 1 (AQ) and 1 (S) precipitate to form then a double replacement reaction occurred.
77. If 2 AQ solutions result in 2 different AQ solutions, nothing really happened.
78. Abstract: FG(AQ) + XY(AQ) FY + XG [one AQ + one S!]
79. Word equation:
Sodium hydroxide and copper (II) sulfate solutions combine…
80. Skeleton, then balance this:
81. Balanced:

54. Let’s Look at Table F now, and practice
82. Every solution on the left side is soluble (dissolves in water).
There are only a couple of exceptions. _________________________________
83. The Halides (F, Cl, Br, and I) make solid some compounds And the sulfates make some too. What are the these exceptions? ___________________________________________________________
84. Every solution on the right side is insoluble (makes a solid precipitate in water) but there are exceptions there too ____________________________________________________________ Name 3 ions that ALWAYS make AQ solutions without any exceptions:

55. Let’s Look at Table F now, and practice
82. Every solution on the left side is soluble (dissolves in water).
There are only a couple of exceptions. Some Halides, some sulfates., and sometimes Ca+2, Sr+2, and Ba+2
The Halides (F, Cl, Br, and I) make solid some compounds And the sulfates make some too. What are the these exceptions? For Halides the exceptions are: Ag+1 Pb+2 and Hg2+2 For Sulfates the exceptions are: Ag+1 Ca+2 Sr+2 Ba+2 and Pb+2
84. Every solution on the right side is insoluble (makes a solid precipitate in water) but there are exceptions there too mostly Group 1 and Ammonium, but a few extra too (look!) Name 3 ions that ALWAYS make AQ solutions without any exceptions: ammonium, nitrates, acetates, hydrogen carbonates, and the chlorates (plus all group 1 cation compounds)

56. 86. Check the names + formulas on Table F. Are these compounds AQ or S ?
Silver chloride
AgCl
Magnesium nitrate
Mg(NO3)2
Sodium hydroxide
NaOH
Calcium nitrate
CaNO3
Strontium sulfate
SrSO4
Barium acetate
Ba(C2H3O2)2
Aluminum chlorate
Al(ClO3)3
Lead (II) bromide
PbBr2
Lithium sulfide
LiS
Ammonium chromate
(NH4)2CrO4

57. 86. Check the name to the formula. Are these compounds AQ or S ?
formulas
AQ or S ?
Silver chloride
AgCl S 
Magnesium nitrate
Mg(NO3)2
 AQ
Sodium hydroxide
NaOH
Calcium nitrate
CaNO3
Strontium sulfate
SrSO4  S
Barium acetate
Ba(C2H3O2)2
Aluminum chlorate
Al(ClO3)3
Lead (II) bromide
PbBr2
Lithium sulfide
LiS
AQ 
Ammonium chromate
(NH4)2CrO4

58. Finish the word problems, do the formulas, balance the equations, complete the phase symbols for both products.
87. Sodium chloride + lead (II) acetate solutions combine…
88.

59. Finish the word problems, do the formulas, balance the equations, complete the phase symbols for both products.
Sodium chloride + lead (II) acetate solutions combine… into sodium acetate and Lead (II) chloride
88.
2NaCl(AQ) + Pb(C2H3O2)2(AQ) NaC2H3O2(AQ) + PbCl2(S)

60. Finish the word problems, do the formulas, AND balance the equations, complete the phase symbols for both products.
89. Potassium phosphate + calcium chloride solutions combine…

61. 2K3PO4(AQ) + 3CaCl2(AQ) 6KCl(AQ) + Ca3(PO4)2(S)
Finish the word problems, do the formulas, balance the equations, complete the phase symbols for both products.
89.
Potassium phosphate + calcium chloride solutions combine into potassium chloride and calcium phosphate
2K3PO4(AQ) + 3CaCl2(AQ) KCl(AQ) + Ca3(PO4)2(S)

62. Finish the equations, balance the equations, complete the phase symbols for both products.
90. BaCl2(AQ) + RbOH(AQ)
91. NH4CrO4(AQ) + Ca(NO3)2(AQ)

63. Finish the equations, balance the equations, complete the phase symbols for both products.
90. BaCl2(AQ) + 2RbOH(AQ) RbCl(AQ) Ba(OH)2(S)
91. (NH4)2CrO4(AQ) + Ca(NO3)2(AQ) NH4NO3(AQ) + CaCrO4(S)

64. OB: Combustion Reactions
92. Combustion reactions require a hydrocarbon compound to combine rapidly with oxygen, forming oxygen and carbon dioxide, and lots of energy.
There is little challenge recognizing these reactions, and the products NEVER vary.
93. Hydrocarbon: a compound made of carbon and hydrogen.
94. Oxygenated hydrocarbon: a compound made of carbon, hydrogen and oxygen. These also combust, but the balancing is one step more work for you.

65. Hydrocarbon + oxygen carbon dioxide + water
95. Examples of hydrocarbons: methane, propane, butane, octane, wax.
96. Examples of oxygenated hydrocarbons: ethanol (alcohol), wood, ethers, acetone.
97. Every single combustion reaction looks like this:
Hydrocarbon + oxygen carbon dioxide + water
98. First practice example: the simplest of all hydrocarbons, methane combusts.
We set up the skeleton reaction, then YOU balance this while I take attendance.
CH O CO H2O

66. CH4(G) + 2O2(G) CO2(G) + 2H2O(G)
John Dalton, simple whole number ratio check: 1:2:1:2 all okay.
Due to the heat released, the water is a gas too.
Balance these, we’ll see how you did on the next slide.
99. C2H6(G) + O2(G)
C3H8(G) + O2(G)

67. 2C2H6(G) + 7O2(G) 4CO2(G) + 6H2O(G)
C3H8(G) + 5O2(G) H2O(G) + 3CO2(G)
101. Combustion reactions always have a hydrocarbon* and oxygen reacting to form water and carbon dioxide.
*you could switch in an oxygenated hydrocarbon too

68. 103. Abstract: Hydrocarbon + O2 CO2 + H2O
Demo for Combustion Reactions
102. Combustion reactions require a hydrocarbon (or oxygenated hydrocarbon) to combine with oxygen, forming carbon dioxide, water + HEAT (always exothermic!)
103. Abstract: Hydrocarbon + O CO2 + H2O
The “abstract” is not too abstract because of the limitations of the reaction.
104. Word Equation:
Methanol + oxygen yields carbon dioxide & water
(Methanol is NOT the “alcohol” in wine and beer)

69. CH3OH(G)+ O2(G) CO2(G)+ H2O(G) + energy!
105. BALANCE THIS REACTION TO SEE IT, IT’S CERTAINLY WORTH IT!
CH3OH(G)+ O2(G) CO2(G)+ H2O(G) + energy!

70. 2CH3OH(G)+ 3O2(G) 2CO2(G) + 4H2O(G)
BALANCE THIS REACTION TO SEE IT, IT’S CERTAINLY WORTH IT!
2CH3OH(G)+ 3O2(G) CO2(G) + 4H2O(G)
+ energy!
106. Is John Dalton happy? ____
107. In an exothermic reaction, energy is a product.

71. 108. The easiest way to “spot” a combustion reaction is…

72. 108. The easiest way to “spot” a combustion reaction is…recognize a hydrocarbon that combines with oxygen, and ONLY forms carbon dioxide and water (and energy)!

73. Balance this combustion reaction… write the word equation and balance it too
109. Butane (C4H10) combusts.

74. 109. Butane (C4H10) combusts. 2C4H10 + 13O2 8CO2 + 10H2O +Energy
Balance this combustion reaction… write the word equation and balance it too
109. Butane (C4H10) combusts.
2C4H O CO H2O Energy

75. Balance this combustion reaction… write the word equation and balance it too
110. Octane (C8H18) combusts.

76. 110. Octane (C8H18) combusts. 2C8H18 + 25O2 16CO2 + 18H2O +Energy
Balance this combustion reaction… write the word equation and balance it too
110. Octane (C8H18) combusts.
2C8H O CO2 + 18H2O Energy

77. OB: recognizing chemical reactions, balancing practice. REVIEW
Get out reference tables.
White paper for notes too.

78. Synthesis and Decomposition Reactions:
SYNTH: 2 or more small things make one larger product
Or the reverse,
DECOMP: One large reactant breaks down into 2 or more smaller products.
Write balanced chemical equations from these 2 word equations.
S: phosphorous and chlorine gas form into phosphorous pentachloride gas.
D: Manganese VII oxide form manganese and oxygen gas

79. P(S) + Cl2(G) PCl5(G) P(S) + Cl2(G) PCl5(G)
phosphorous and chlorine gas form into phosphorous pentachloride gas
P(S) + Cl2(G) PCl5(G)
P(S) + Cl2(G) PCl5(G)
skeleton

80. P(S) + Cl2(G) PCl5(G) 2P(S) + 5Cl2(G) 2PCl5(G) balanced
phosphorous and chlorine gas form into phosphorous pentachloride gas
P(S) + Cl2(G) PCl5(G)
2P(S) + 5Cl2(G) PCl5(G)
skeleton
balanced

81. Manganese VII oxide form manganese and oxygen gas
Mn2O7(S) Mn(S) + O2(G)
skeleton

82. Mn2O7(S) Mn(S) + O2(G) 2Mn2O7(S) 4Mn(S) + 7O2(G)
Manganese VII oxide form manganese and oxygen gas
Mn2O7(S) Mn(S) + O2(G)
2Mn2O7(S) Mn(S) + 7O2(G)
skeleton

83. Single Replacement Reactions (table J)
Always start with one aqueous solution and an “atom”, and end with a different aqueous solution and a different atom. The atom can be diatomic. Sometimes it’s a cation switch, or an anion switch, or even nothing at all. Try writing balanced reactions for these three:
Sodium goes into silver nitrate solution
Bromine is added to lithium iodide solution
Tin is added to barium nitrate solution

84. Skeletons first Next Slide, balance them all!
Sodium goes into silver nitrate solution
Na(S) + AgNO3(AQ) NaNO3(AQ) + Ag(S)
Bromine is added to lithium iodide solution
Br2(L) + LiI (AQ) LiBr(AQ) + I(S)
Tin is added to barium nitrate solution
Sn(S) + Ba(NO3)2 (AQ) Sn(NO3)2(AQ) + Ba(S)

85. Na(S) + AgNO3(AQ) NaNO3(AQ) + Ag(S)
Sodium goes into silver nitrate solution
Na(S) + AgNO3(AQ) NaNO3(AQ) + Ag(S)
Bromine is added to lithium iodide solution
Br2(L) + 2LiI (AQ) LiBr(AQ) + I2(S)
Tin is added to barium nitrate solution
Sn(S) + Ba(NO3)2 (AQ) X
Already balanced!
Balanced!
No reaction!
OOPS!!!

86. Double Replacement Reactions
Start with two AQ ionic solutions, end with a different AQ solution and a precipitate
If your 2 AQ solutions form two new AQ solutions, then all you have is a mixture.
Vocab: soluble, insoluble, precipitate, aqueous, cations, anions.
Turn these two word equations into balanced chemical equations.
Lithium nitrate and potassium chloride solutions are poured together
Lead (II) hydrogen carbonate and Cobalt (III) sulfate solutions are poured together

87. switched + fixed on next slide
First the skeletons, then, balance and check table F
(just switch the ions around, next slide we’ll “fix ‘em”.)
Lithium nitrate and potassium chloride solutions are poured together
LiNO3(AQ) + KCl(AQ) LiCl + KNO3
Lead (II) hydrogen carbonate and Cobalt (III) sulfate solutions are poured together
Pb(HCO3)2(AQ) + Co2(SO4)3(AQ) PbSO CoHCO3

88. LiNO3(AQ) + KCl(AQ) LiCl + KNO3
First the skeletons, then, balance and check table F balanced on next slide
just switch the ions around, next slide we’ll “fix ‘em”.
Lithium nitrate and potassium chloride solutions are poured together
LiNO3(AQ) + KCl(AQ) LiCl + KNO3
Lead (II) hydrogen carbonate and Cobalt (III) sulfate solutions are poured together
Pb(HCO3)2(AQ) + Co2(SO4)3(AQ) PbSO Co(HCO3)3
ALL OK HERE
Lead is +2 ion, sulfate is -2, okay there
Cobalt is +3 ion, anion is only -1. FIXED

89. LiNO3(AQ) + KCl(AQ) LiCl(AQ ) + KNO3(AQ)
First the skeletons, then, balance and check table F balanced on next slide
(just switch the ions around, next slide we’ll “fix ‘em”.
Lithium nitrate and potassium chloride solutions are poured together
LiNO3(AQ) + KCl(AQ) LiCl(AQ ) + KNO3(AQ)
Lead (II) hydrogen carbonate and Cobalt (III) sulfate solutions are poured together
3Pb(HCO3)2(AQ) + Co2(SO4)3(AQ) PbSO4(S) + Co(HCO3)3(AQ)
Mixture!
Balanced!
Check table F for soluble or insoluble

90. Combustion are always a hydrocarbon + oxygen forming water and carbon dioxide with heat.
Vocab: hydrocarbon, oxygenated hydrocarbon, complete combustion, incomplete combustion, exothermic and endothermic.
Balance these two combustion reactions:
hexane combusts (C6H14)
Propanol combusts (C3H5OH) this is a type of alcohol.

91. C6H14(L) + O2(G) CO2(G) + H2O(G)
First the skeletons, then both balanced:
hexane combusts (C6H14)
C6H14(L) + O2(G) CO2(G) + H2O(G)
1-Propanol combusts (C3H5OH) this is a type of alcohol.
C3H5OH(L) + O2(G) CO2(G) + H2O(G)

92. 2C6H14(L) + 19O2(G) 12CO2(G) + 14H2O(G)
Balanced.
hexane combusts (C6H14)
2C6H14(L) + 19O2(G) CO2(G) H2O(G)
1-Propanol combusts (C3H5OH) this is a type of alcohol.
C3H5OH(L) + 4O2(G) CO2(G) + 3H2O(G)

93. CH4(G) + 2O2(G) → CO2(G) + 2H2O(G)
In Complete combustion, only carbon dioxide forms
CH4(G) + O2(G) → C(S) + 2H2O(G)
With Incomplete combustion, carbon will form because there is insufficient oxygen to make carbon dioxide.
Carbon is the chemical name for SOOT.