1. Types of Chemical Reactions
Single Replacement Reactions
Double Replacement Reactions
Combustion Reactions

2. Recall Synthesis Reactions
Two or more substances combine to form one substance.
The general form is A + X AX
Decomposition Reactions
One substance reacts to form two or more substances.
The general form is AX  A+X

3. Single Replacement Reactions
A metal will replace a metal ion in a compound.
The general form is A + BX  AX + B
A nonmetal will replace a nonmetal ion in a compound.
The general form is Y+BX  BY + X

4. Single Replacement Reactions
Examples:
Ni + AgNO3 NiNO3 + Ag
Nickel replaces the metallic ion Ag+ (metal replaces metal ion)
The silver becomes free silver and the nickel becomes the nickel (II) ion.
Ni + AgNO3  Ag + Ni(NO3)2
Balance the equation:
Ni + 2AgNO3  2Ag + Ni(NO3)2

5. Thermite Reaction
Steve Spangler Video Thermite

6. Thermite Reaction Al + Fe2O3 
Aluminum will replace iron (III) as was seen in the video.
Iron (III) becomes Fe and aluminum metal becomes Al3+.
2Al + Fe2O3  Al2O3 + 2Fe

7. Double Replacement Reactions
Ions of two compounds exchange places with each other.
Reactants must be two ionic compounds, in aqueous solution
The general form is AX+BY = AY + BX

8. Remember the Demonstration!!!!!!!!
Word - Lead (II) Nitrate + Potassium Iodide --> Potassium Nitrate + Lead Iodide
Skeletal - Pb(NO3)2 (aq) + 2KI (aq) --> 2KNO3 (aq) + PbI2 (s)
What occurred???
This is a double displacement reaction

9. Double Replacement NaOH + CuSO4  The Na+ and Cu2+ switch places.
Na+ combines with SO42- to form Na2SO4.
Cu2+ combines with OH- to form Cu(OH)2
NaOH + CuSO4  Na2SO4 + Cu(OH)2
2NaOH + CuSO4  Na2SO4 + Cu(OH)2

10. Double Replacement CuSO4 + Na2CO3 
Cu2+ combines with CO32- to form CuCO3.
Na+ combines with SO42- to form Na2SO4.
CuSO4 + Na2CO3  CuCO3 + Na2SO4

11. 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

12. Recognition
You need to be able to recognize which reaction is taking place

13. Practice Examples: Synthesis H2 + O2 ® H2O ® Zn + H2SO4 ® HgO ®
KBr + Cl2 ®
AgNO3 + NaCl ®
Mg(OH)2 + H2SO3 ®
Synthesis
Decomposition
Single Displacement
Double Replacement

14. Combustion Reactions
Combustion means “add Oxygen” Normally, a compound composed of only C, H, (and maybe O) is reacted with oxygen – usually called “burning”
If the combustion is complete, the products will be CO2 and H2O.
If the combustion is incomplete, , the products will be CO (or possibly just C) and H2O.

15. Combustion Reaction
When a substance combines with oxygen, a combustion reaction results.
The combustion reaction may also be an example of an earlier type such as 2Mg + O2  2MgO.
The combustion reaction may be burning of a fuel.

16. Combustion Reactions
Combustion reactions involve light and heat energy released.
Natural gas, propane, gasoline, etc. are burned to produce heat energy.
Most of these organic reactions produce water and carbon dioxide.

17. Combustion Reaction
When hydrocarbon compounds CxHx are burned in oxygen, the products are water and carbon dioxide.
CH4 + O2  CO2 + H2O
CH4 + 2O2  CO2 + 2H2O
Demonstration

18. Combustion Reactions
Generally combustion reactions involve the burning of a Hydrocarbon (CxHx) in Oxygen.
Other elements can also burn with Oxygen
2Mg + O2  2MgO+ Energy
2H2 + O2  2H2O+ Energy (basis behind fuel cell energy)
P4 + 5O2  P4O10 + Energy (matches)

19. Practice Classify each of the following as to type: H2 + Cl2  2HCl
Synthesis
Ca + 2H2O  Ca(OH)2 + H2
Single Displacement

20. Practice 2CO + O2  2CO2 2KClO3  2KCl + 3O2 Synthesis and Combustion
Decomposition

21. Practice FeS + 2HCl  FeCl2 + H2S Zn + 2HCl  ? ZnCl2+ H2
Double Replacement
Zn + 2HCl  ? ZnCl2+ H2
Single Displacement