1. Predicting Products
Chemical Reactions

2. Combustion Reactions Always have similar reactants:
CnHn + O2
Always create the same products:
CO2 + H2O
Balance!
C3H8 + O2 
CH3CH2OH + O2 
CO2 + H2O
CO2 + H2O

3. Single Replacement A + BX  AX + B
Single element replaces one of the elements in compound
NEVER carry a subscript, only the charge of the ion!
Use your polyatomic ion charges
Use the periodic table/ periodic table of ions
HNO3 + Zn  ???

4. Single Replacement
First - decide if the single element forms a cation or an anion and give it the ionic charge.
Zinc is the single element and will form a +2 cation.
Second, determine which element in the compound the single element will replace.
Cations can only replace cations, anions can only replace anions. (positive replaces positive, negative replaces negative ions)
In this reaction, the hydrogen acts as the cation. Zinc should replace hydrogen.
Next, check the activity series to determine if the reaction will occur.

5. Activity Series
Activity series - a list of elements based on reactivity.
An element in the activity series can replace any element below it.
Since zinc is replacing hydrogen, zinc must be above hydrogen in the activity series for the reaction to occur.
It is, so the reaction occurs.

7. Single Replacement Form products with correct subscripts
Balance equation
2 HNO3 + Zn  H2 + Zn(NO3)2

8. Double Replacement AX + BY  AY + BX Again…No subscript, only charge!
Two compounds and the partners will switch!
Again…No subscript, only charge!
AgNO3 + NaCl  ???

9. Double Replacement Assign charges to each of the ions.
Positive replaces positive (or negative replaces negative)
Compounds MUST have a cation and an anion
Form products and give them the correct subscripts
Balance the equation.
AgNO3 + NaCl  ???

10. Double Replacement
Ag+1 and Na+1 will switch. Na+1 will compound with NO3-1 and Ag+1 will compound with Cl-1
AgNO3 + NaCl  AgCl + NaNO3

11. Double Replacement AgNO3 + NaCl  AgCl + NaNO3
Pb(NO3)2 + CuSO4  PbSO4 + Cu(NO3)2

12. Double Replacement NaOH + FeCl3  ??? Pb(NO3)2 + KI  ???
NaCl + Fe(OH)3
Pb(NO3)2 + KI  ???
PbI2 + KNO3
CaCl2 + NaOH  ???
NaCl + Ca(OH)2

13. Decomposition AX  A + X Acids decompose into water and an oxide.
Compound breaks apart into two smaller elements/compounds
Acids decompose into water and an oxide.
H2CO3 H2O + CO2
Metallic hydroxides (anything with a metal and an OH) decompose to form a metallic oxide and water.
Mg(OH)2  MgO + H2O
Metallic carbonates decompose to form a metallic oxide and carbon dioxide.
Li2CO3  Li2O + CO2

14. Synthesis A + X  AX Again…No subscript, only charge! Na + Cl2  ???
Two simple elements combine to form one compound.
Again…No subscript, only charge!
Na + Cl2  ???

15. Synthesis
Assign charges to each of the ions (if you have a metal and a nonmetal) to create an ionic compound.
Form the product and give it the correct subscripts.
Balance the equation.
2 Na + Cl2  2 NaCl

16. Predicting Products Activity
Match the Reactants with the Products
Take a sheet of paper with you
Your name on paper
Write each equation out
4 in group – 2 per group member
3 in group – 3 per group member
Balance the equation
List the reaction
Combustion, Decomposition, Single Replacement, Double Replacement, Synthesis
Staple group together and turn in when finished