1. Types of Reactions

2. Diatomic Elements BrINClHOF or 7H Club These elements are never alone

3. Reminder
When writing an ionic compound- cross the charges!

4. Combination/Synthesis
Two or more reactants combine to form one product.
Na +Cl2  NaCl

5. Decomposition One reactant forms multiple products
Often break down into elements
H2O  H2 + O2

6. Single Replacement Starts with one compound and one element.
If the single element is a metal replace the metal. If the single element is nonmetal, replace the nonmetal.
Will only replace if more active
K + NaOH  KOH + Na
F2 + AgI  AgF + I2

8. Double Replacement Two compounds, metals switch places.
Usually happens dissolved in water
AgNO3 + HCl  AgCl + HNO3

9. Combustion
Something made of carbon and hydrogen react with oxygen. Burning! Always produce CO2 and H2O
CH4 + O2  CO2 + H2O

10. N2 + 3H2 -----> 2NH3

11. 2NaI + F2 ---> 2NaF + I2 

12. 2AgCl + BaBr2 ----> 2AgBr + BaCl2

13. C2H6 + 5O2 ---> 3H2O + 2CO2

14. 2H2O ---->2H2 + O2

15. CaO --> Ca + O2 (

16. 6 O2 + C6H12O6 --> 6 H2O + 6 CO2 

17. 3 KOH + H3PO4 --> K3PO4 + 3 H2O 

18. 2 KNO3 --> 2 KNO2 + O2