1. Types of Chemical Reactions

2. The word “synthesize” means to produce.
Synthesis Reactions
A + B  AB
The word “synthesize” means to produce.
How to identify:
2 elements  one product.

3. Synthesis Reaction Ex. 4Fe + 3O2  2Fe2O3
Iron + Oxygen  Iron (III) Oxide

4. Decomposition Reactions
AB  A + B
How to identify: they always have only one reactant.

5. Decomposition Rxn. Ex. H2CO3  CO2 + H2O
Carbonic acid  Carbon dioxide + Water

6. A single metal replaces another one in a compound.
Single Replacement
A + BC  AC + B
A single metal replaces another one in a compound.

7. Double Replacement AB + CD  AD + CB
The metals in two compounds switch places.
(2 compounds  2 new compounds)

8. An organic compound is any compound containing C, H, and sometimes O.
Combustion
Organic cmpd. + O2  CO2 + H2O
An organic compound is any compound containing C, H, and sometimes O.

9. Predicting Products of Reactions

10. Write the formula correctly by balancing charges.
Synthesis
Two elements 
Write the formula correctly by balancing charges.

11. Synthesis cont... Nonmetal oxide + water  Acid
Combine atoms from both reactants. Start acid formula with H.

12. Decomposition
Binary Compound 
Break into elements.

13. Decomposition cont...
Metal Carbonate  Metal oxide + CO2

14. Single Replacement Metal + Compound(aq)  Use “activity series”
If the lone metal is higher than the one in the compound there will be a reaction.
If not, write “N.R.” in the products.

15. Ex. 2Al(s) + 3Pb(NO3)2(aq)  3Pb(s) + 2Al(NO3)3(aq)
Al is more reactive (“fun”) and kicks Pb out of the “friendship”

16. Compound(aq) + Compound(aq) 
Double Replacement
Compound(aq) + Compound(aq) 
Use the Solubility Table from your book. If both products are SOLUBLE, write “N.R.” in the products.

17. Completely perfect combustion, but not reality.
Organic + O2 
CO2 + H2O
Completely perfect combustion, but not reality.

18. Reactions in Aqueous Solution

19. Ions in Solution
When ionic compounds dissolve in water they break apart:
“NaCl(aq)” means Na+(aq) + Cl-(aq)
“CaCl2(aq)” means Ca+2(aq) + 2Cl-(aq)

20. Ionic Equations Becomes
In a “complete ionic equation” you split the aqueous compounds into their ions:
NaCl(aq) + AgNO3(aq) NaNO3(aq) + AgCl(s)
Becomes
Na+(aq) + Cl-(aq) + Ag+(aq) + NO3-(aq)  Na+(aq) + NO3-(aq) + AgCl(s)

21. Ionic Equations
Some of the ions don’t change from one side to the other (Na+ and NO3-). They are “spectator ions”.

22. Ag+(aq) + Cl-(aq)  AgCl(s)
Net Ionic Equations
“Net” means
“after adjustments and deductions”.
Writing the net ionic equation you leave the spectator ions out.
Ag+(aq) + Cl-(aq)  AgCl(s)

23. Examples Balance these, then write the complete ionic equation:
Pb(ClO4)2(aq) + NaI(aq) PbI2(s) + NaClO4(aq)
Zn(s) + HCl(aq)  ZnCl2(aq) + H2(g)

24. Examples Now give the net ionic equation of the two reactions.
Pb+2(aq) + 2I-(aq)  PbI2(s)
Zn(s) + 2H+(aq)  Zn+2(aq) + H2(g)

25. Keep in Mind
When you have the SAME coefficient for ALL of the reactants AND products, reduce them to ONE.