1. Predicting Reactions

2. Terminology Na(s) + H2O(ℓ)  NaOH(aq) + H2(g)
Sodium and water are the reactants
Reactants – the starting materials for a reaction
Sodium hydroxide and hydrogen are the products
Products – what is created by the reaction

3. Symbols in Reactions Na(s) + H2O(ℓ)  NaOH(aq) + H2(g) (s) (ℓ) (g)
Solid
(ℓ)
Liquid (does not describe a solution)
(g)
Gas
(aq)
Aqueous – dissolved in water, solution

4. Symbols in Reactions Delta over the reaction arrow
Heat is continually added to make the reaction happen
Formula over the reaction arrow
Catalyst
Participates in the reaction but is not consumed
Speeds up the reaction
In this example, iron is a catalyst.

5. Diatomic Molecules
Certain elements exist in nature as diatomic molecules
Br2 I2 N2
Cl2 H2 O2 F2
BrINClHOF
Any time chemists refer to one of these elements in its natural state we are speaking of the diatomic molecule

6. Types of Reactions A + B  AB AB  A + B AB + C  AC + B
Synthesis
AB  A + B
Decomposition
AB + C  AC + B
Single Replacement
AB + CD  AD + CB
Double Replacement
CXHYOZ + O2  CO2 + H2O
Combustion Reaction

7. How to Tell Which is Which
Does the reaction have oxygen as a reactant and carbon dioxide and water as products?
Combustion
Does your reaction have two or more chemicals combining to form one compound?
Synthesis
Does your reaction have one compound being broken into two or more compounds?
Decomposition

8. How to Tell Which is Which
Does the reaction have any reactants that are only one element?
Single Replacement
Does the reaction have two reactants and two products that switched “partners”?
Double Replacement

9. Practice
Classify each reaction as one of the five basic reaction types:
Al + HCl  AlCl3 + H2
Cu(OH)2  CuO + H2O
CH4 + O2  CO2 + H2O
P4O10 + H2O  H3PO4
AgNO3 + NaOH  AgOH + NaNO3

10. Balancing Reactions Consider the following reaction: H2 + O2  H2O
There is a problem with this reaction
Where did the second oxygen atom go?
Must have the same number of atoms of each type on both sides of the reaction.
Balancing the reaction.

11. Balancing Reactions In order to balance a reaction
Change or add coefficients to compounds
Never add a coefficient to one element in a compound
Never add or change a subscript

12. Balancing Practice
H O2  H2O

13. Balancing Practice
C3H O2  CO H2O

14. Balancing Practice
FeCl Na2S  NaCl Fe2S3

15. Balancing Practice
Ca(NO3)2 + Na3PO4  NaNO3 + Ca3(PO4)2

16. Balancing Practice
Na H2O  NaOH H2

17. Balancing Practice
C2H O2  CO H2O

18. Predicting Reactions

19. Predicting Reactions
Solutions of copper(II) chloride and sodium carbonate are mixed
What type of reaction is this?
What are the names of the products?
Which product is the precipitate?
Insoluble ionic compounds will form precipitates during reactions.
Precipitates are solids.

20. Predicting Double Replacement Reactions
Solutions of copper(II) sulfate and sodium chloride are mixed
Where is my precipitate?
What are the names of my products?
Why is there no precipitate?
If two solutions of ionic compounds are mixed and no precipitate forms, then we say that no reaction has occurred.

21. Double Replacement Practice
For the following reactions, write the complete reaction that occurs using all appropriate symbols. If no reaction occurs write NR. Balance the reaction using the lowest whole number coefficients possible.
Silver nitrate solution is mixed with a sodium sulfate solution.

22. Double Replacement Practice
For the following reactions, write the complete reaction that occurs using all appropriate symbols. If no reaction occurs write NR. Balance the reaction using the lowest whole number coefficients possible.
Solutions of ammonium chloride and lead(II) acetate are mixed.

23. Double Replacement Practice
For the following reactions, write the complete reaction that occurs using all appropriate symbols. If no reaction occurs write NR. Balance the reaction using the lowest whole number coefficients possible.
Solutions of copper(II) sulfate and iron(III) chloride are mixed.

24. Double Replacement Practice
For the following reactions, write the complete reaction that occurs using all appropriate symbols. If no reaction occurs write NR. Balance the reaction using the lowest whole number coefficients possible.
Solutions of lead(II) nitrate and sodium iodide are mixed.

25. Predicting More Reactions

26. A Series of Reactions Add 6M HCl to What type of reaction is this?
Copper
Iron
Magnesium
Zinc
What type of reaction is this?

27. Single Replacement Predictions
Write the balanced reaction for each metal.
What is the gas being produced?
Which metal is the most active?
Which metal is the least active?

28. Single Replacement Predictions
Most Active Mg Zn Fe Cu
Least Active
A more complete listing is on your reference table.

29. Activity Series Most Active Elements are at the top
These will replace anything below it in a compound
These elements are more stable in compounds.
Least Active Elements are at the bottom
These elements are more stable by themselves.
No Reaction Occurs when the elements are already in their more stable positions.

30. Two Activity Series The two activity series are not connected.
Please draw a big fat line between them on your reference table.

31. Single Replacement Practice
For the following reactions, write the complete reaction that occurs using all appropriate symbols. If no reaction occurs write NR. Balance the reaction using the lowest whole number coefficients possible.
Aluminum metal is added to a solution of copper(II) sulfate

32. Single Replacement Practice
For the following reactions, write the complete reaction that occurs using all appropriate symbols. If no reaction occurs write NR. Balance the reaction using the lowest whole number coefficients possible.
Magnesium metal is added to a solution of potassium chloride

33. Single Replacement Practice
For the following reactions, write the complete reaction that occurs using all appropriate symbols. If no reaction occurs write NR. Balance the reaction using the lowest whole number coefficients possible.
Lithium metal is added to water.

34. Single Replacement Practice
For the following reactions, write the complete reaction that occurs using all appropriate symbols. If no reaction occurs write NR. Balance the reaction using the lowest whole number coefficients possible.
Chlorine gas is bubbled through a solution of sodium bromide.

35. Other Types of Reactions
Predicting other types of reactions is as simple as following a pattern.
You have all the patterns you need on your reference table.

36. Practice Problems
For the following reactions, write the complete reaction that occurs using all appropriate symbols. If no reaction occurs write NR. Balance the reaction using the lowest whole number coefficients possible.
Calcium hydroxide is heated strongly.

37. Practice Problems
For the following reactions, write the complete reaction that occurs using all appropriate symbols. If no reaction occurs write NR. Balance the reaction using the lowest whole number coefficients possible.
Propane (C3H8) is burned in oxygen.

38. Practice Problems
For the following reactions, write the complete reaction that occurs using all appropriate symbols. If no reaction occurs write NR. Balance the reaction using the lowest whole number coefficients possible.
Powdered aluminum is added to liquid bromine

39. Practice Problems
For the following reactions, write the complete reaction that occurs using all appropriate symbols. If no reaction occurs write NR. Balance the reaction using the lowest whole number coefficients possible.
Sucrose (C12H22O11) is burned in oxygen

40. Practice Problems
For the following reactions, write the complete reaction that occurs using all appropriate symbols. If no reaction occurs write NR. Balance the reaction using the lowest whole number coefficients possible.
Hydrogen gas is mixed with nitrogen gas in the presence of an iron catalyst.

41. Practice Problems
For the following reactions, write the complete reaction that occurs using all appropriate symbols. If no reaction occurs write NR. Balance the reaction using the lowest whole number coefficients possible.
Magnesium chlorate is heated strongly.

42. Practice Problems
For the following reactions, write the complete reaction that occurs using all appropriate symbols. If no reaction occurs write NR. Balance the reaction using the lowest whole number coefficients possible.
Sodium hydrogen carbonate is heated strongly.

43. Additional Practice Problems
For the following reactions, write the complete reaction that occurs using all appropriate symbols. If no reaction occurs write NR and explain why. Balance the reaction using the lowest whole number coefficients possible.
Fluorine gas is bubbled through an aluminum iodide solution.
Nickel(II) carbonate is heated strongly.
Solutions of zinc chloride and calcium nitrate are mixed.
Warm calcium metal is added to chlorine gas.
Acetone (C3H6O) is burned in air.

44. 3F2(g) + 2AlI3(aq)  2AlF3(aq) + 3I2(s)
This:
ZnCl2(aq) + Ca(NO3)2(aq)  Zn(NO3)2(aq) + CaCl2(aq) No Reaction
Ca(s) + Cl2(g)  CaCl2(s)
C3H6O(ℓ) + 4O2(g)  3CO2(g) + 3H2O(g)

45. Additional Practice Problems.
For the following reactions, write the complete reaction that occurs using all appropriate symbols. If no reaction occurs write NR and explain why. Balance the reaction using the lowest whole number coefficients possible.
Silver metal is added to molten sulfur.
Tin metal is added to a solution of manganese(II) chloride.
A solution of carbonic acid (H2CO3) is warmed.
Potassium metal is added to water.
Solutions of barium chloride and aluminum sulfate are mixed
Methane gas is burned in air

46. 2Ag(s) + S(ℓ)  Ag2S(s)
No Reaction
H2CO3(aq)  H2O(ℓ) + CO2(g)
2K(s) + 2H2O(ℓ)  2KOH(aq) + H2(g)
3BaCl2(aq) + Al2(SO4)3(aq)  3BaSO4(s) + 2AlCl3(aq)
CH4(g) + 2O2(g)  CO2(g) + 2H2O(ℓ)

47. 3BaCl2(aq) + Al2(SO4)3(aq)  3BaSO4(s) + 2AlCl3(aq)

48. Why Do We Have No Reaction?
Solutions of ammonium chloride and potassium phosphate are mixed.
Write the balanced reaction that would occur if this reaction happened

49. Why No Reaction? 3NH4Cl(aq) + K3PO4(aq)  (NH4)3PO4(aq) + 3KCl(aq)
What happens to ionic compounds when they dissolve in water?
NH4Cl really looks like NH4+(aq) and Cl-(aq)
K3PO4 really looks like 3K+(aq) and PO43-(aq)
3NH4+(aq) + 3Cl-(aq) + 3K+(aq) + PO43-(aq)  3NH4+(aq) + PO43-(aq) + 3K+(aq) + 3Cl-(aq)
No difference from one side to the other.
Everything cancels out.

50. Net Ionic Equations Net Ionic Equations
Write things that are ionized in solution as separate ions.
Dissolved ionic compounds.
Everything else write like normal.
Don’t write anything that cancels out from both sides.
Things that cancel are called spectator ions
Must be mass balanced and charge balanced.

51. Net Ionic Practice Problems
Solutions of barium chloride and potassium sulfate are mixed.

52. Net Ionic Practice Problems
Solutions of ammonium carbonate and calcium chloride are mixed.

53. Net Ionic Practice Problems
Magnesium is added to a solution of copper(II) nitrate

54. Net Ionic Practice Problems
Solutions of sodium phosphate and lead(II) nitrate are mixed.

55. Net Ionic Practice Problems
Solutions of sodium phosphate and lead(II) nitrate are mixed.
2Na3PO4(aq)+3Pb(NO3)2(aq)6NaNO3(aq)+Pb3(PO4)2(s)
6Na+(aq)+2PO43-(aq)+3Pb2+(aq)+6NO3-(aq)
6Na+(aq)+ 6NO3-(aq) + Pb3(PO4)2(s)
2PO43-(aq)+3Pb2+(aq)  Pb3(PO4)2(s)

56. Net Ionic Practice Problems
Solutions of sodium phosphate and lead(II) nitrate are mixed.