1. 5 Types of Chemical Reactions

2. 1. Combustion Reactions
Occurs when oxygen reacts with a hydrocarbon to produce water and carbon dioxide.
A hydrocarbon is a compound containing only Carbon, Hydrogen and sometimes oxygen.
Example:
C10H8(s) + 12O2 (g)  10CO2 (g) + 4H2O(g)

3. 1. Combustion Reactions
Combustion reactions - 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”:
1) Fuel (hydrocarbon) 2) Oxygen 3) Something to ignite the reaction (spark)

4. Combustion Reactions In general: CxHy + O2  CO2 + H2O
Products 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 C8H18)

5. Combustion
Example
C5H O2  CO2 + H2O
Write the products and balance the following combustion reaction:
C10H O2  8 5 6

6. 2. Synthesis (or Combination)
the combination of 2 or more substances to form a compound
only one product
A + B  AB
Example: Cu + O2  2CuO

7. Synthesis
H2(g) + Cl2(g)  2 HCl(g)

8. 2. Synthesis
Example C + O2 O C +  O C
General: A + B  AB

9. Ex. Synthesis Reaction

10. Practice Predict the products. Na(s) + Cl2(g)  Mg(s) + F2(g) 
Al(s) + F2(g)  2 2
NaCl(s)
MgF2(s) 2 3 2
AlF3(s)
Now, balance them.

11. 3. Decomposition
a compound breaks down into 2 or more simpler substances
only one reactant
Examples:
2H2O(l)  2H2(g) + O2 (g)
H2CO3 (aq)  H2O (l) + CO2 (g)
AB  A + B

12. Decomposition
2 H2O(l)  2 H2(g) + O2(g)

13. 3. Decomposition
Example: NaCl  Cl Na Cl + Na
General: AB  A + B

14. Ex. Decomposition Reaction

15. A + BC  B + AC 4. Single Replacement
Occurs when a single element reacts with an ionic compound and switches places with one of the elements in the compound.
A + BC  B + AC

16. 4. Single Displacement General Form: AB + C  AC + B
Cation Displacement
Al + CuCl2 (aq)  Cu + AlCl3(aq)
Anion Displacement
Cl2 + KBr  KCl + Br2

17. Cu(s) + 2AgNO3(aq)  Cu(NO3)2(aq) + 2Ag(s)
Single Replacement
Cu(s) + 2AgNO3(aq)  Cu(NO3)2(aq) + 2Ag(s)

18. Went from neutral (0) to (+2) Went from (+2) to Neutral (0)
4. Single Displacement
Example: Zn + CuCl2
Zn was oxidized
Went from neutral (0) to (+2)  Zn Cl Cu + Cl Zn Cu +
Cu was reduced
Went from (+2) to Neutral (0)
General: AB + C  AC + B

19. Ex. Single Replacement Reaction

21. Single Replacement Reactions
Write and balance the following single replacement reaction equation:
Zn(s) HCl(aq)  ZnCl2 + H2(g) 2
NaCl(s) + F2(g)  NaF(s) + Cl2(g)
Al(s)+ Cu(NO3)2(aq) 2 2 2 3 3
Cu(s)+ Al(NO3)3(aq) 2

22. AB + CD  AD + CB 5. Double Replacement
ions in two compounds “change partners”
cation of one compound combines with anion of the other
AB + CD  AD + CB

23. Pb(NO3)2(aq) + K2CrO4(aq)  PbCrO4(s) + 2KNO3(aq)
Double Replacement
Pb(NO3)2(aq) + K2CrO4(aq)  PbCrO4(s) + 2KNO3(aq)
Usually produce a solid product (precipitate)!

24. 5. Double displacement General: AB + CD  AD + CB Example: MgO + CaS 

25. Double Replacement Reactions
Think about it like “foil”ing in algebra, first and last ions go together + inside ions go together
Example:
AgNO3(aq) + NaCl(s)  AgCl(s) + NaNO3(aq)
Another example:
K2SO4(aq) + Ba(NO3)2(aq)  KNO3(aq) + BaSO4(s) 2

26. 5.5 – Acid/Base Neutralization Reactions

27. Steps to Classifying Reactions
1. Does the reaction contain oxygen, carbon dioxide and water? If Yes, then it is combustion
Do simple molecules form one more complicated product? If yes, then it is synthesis/combination.
3. Does a single reactant break apart to 2 or more simpler products? Then it is decomposition

28. Steps to Classifying Reactions Continued. . . .
4. Is there an ionic compound and a single element on the reactant side and product side? Then it is single displacement. 5. Are all compounds ionic? Then it is double displacment/Replacement.

29. Examples C3H7OH + O2  CO2 + H2O Mg + O2  MgO H2O2  H2O + O2
Al + CuCl2  Cu + AlCl3
Pb(NO3)2 + KI  PbI2 + KNO3
Combustion
Synthesis
Decomposition
Single Displacement
Double Displacement
MgO

30. Practice Predict the products. HCl(aq) + AgNO3(aq) 
CaCl2(aq) + Na3PO4(aq) 
Pb(NO3)2(aq) + BaCl2(aq) 
FeCl3(aq) + NaOH(aq) 
H2SO4(aq) + NaOH(aq) 
KOH(aq) + CuSO4(aq) 

31. Mixed Practice State the type & predict the products. BaCl2 + H2SO4 
21/10/99
Mixed Practice
State the type & predict the products.
BaCl2 + H2SO4 
C6H12 + O2 
Zn + CuSO4 
Cs + Br2 
FeCO3 