1. Predicting the Products of Chemical Reactions

2. Classify the reaction… then write the products.
COMBUSTION:
Reactants: hydrocarbon and oxygen
Products: H2O and CO2
If a metal reacts w/ O2 → metal oxide
If a nonmetal reacts w/ O2 → nonmetal oxide.

3. CxHy + O2  Carbon Dioxide + water
Can also be CxHyOz
A oxygen as a reactant indicates a combustion reaction.
Write CO2 and H2O as products and then balance (this is the hard part!)
C4H O2 
CO2
+ H2O

4. SYNTHESIS: A + B  AB Product: Contain both reactants
(remember to balance the charges for ionic compounds)
A + B  AB
Na(s) + Cl2(g)  2NaCl
2 elements indicates synthesis
Write Charges for each then write compound
Na+ Cl-
NaCl
Balance Reaction

5. Product: break into two elements or compounds
DECOMPOSITION:
Product: break into two elements or compounds
AB  A + B
Single reactant = decomposition reaction.
Separate to elements
Remember diatomics or less complex compounds (we will be memorizing some of these later!)
2MgO  2Mg + O2
NH4OH  NH3+ H2O

6. SINGLE REPLACEMENT: Product: Metal replaces metal (cations) or…
Nonmetal replaces non-metal (anions)
Remember to take into account the charges on the cation and anion and write the formula correctly!
You MUST check your activity series

7. If element is a non-metal, it replaces the anion.
AB + C  AC + B or
AB + C → BC + A
AB is an ionic compound and C is an element.
If element is a metal, it replaces the cation.
CuSO4 + Zn Cu+ ZnSO4
If element is a non-metal, it replaces the anion.
2 LiI + F2 2LiF +I2
Remember correct charges
Remember the diatomics!
Then balance at the end.

8. Product: Cations and anions switch with cations and anions
DOUBLE REPLACEMENT:
Product: Cations and anions switch with cations and anions
It is helpful to separate each compound into their cation and anionic parts with their charges.
Balance charges with new chemical formulas in products!!! 

9. Balance at the end!  AB + CD  Double Displacement
AB and CD are both ionic compounds.
Separate each compound
Write their charges.
Switch places and re-write new compounds.
Pb2+ I K+ NO3-
2 Pb(NO3) KI PbI KNO3
Balance at the end! 

10. Diatomics!
Remember the elements that exist in diatomic form.
They are gases at room temperature!
H2 N2 O2 F2 Cl2 , Br2 , I2

11. Solubility Rules 1. Most alkali metal salts AND NH4+ salts ARE soluble
2. Cl-, Br-, I- are soluble, *except for Ag+, Hg+2, Pb+2
3. F- are soluble, *except for IIA metals
4. NO3-, ClO3-, ClO4-, and CH3COO- are soluble
5. SO4-2 are soluble, *except for Ca2+ , Sr+2, Ba+2, Ag+, Pb+2, Hg2+
6. CO3-2, PO4-3, C2O4-2, CrO4-2, S-2, OH-, and O-2 are INSOLUBLE
(rule 1 takes priority!)
It can be assumed that ionic compounds. that dissolve in water are strong electrolytes and are therefore soluble.