2. Single Replacement Reactions  A single replacement reaction occurs when atoms of an element replace the atoms of a second element in a compound.  This happens due to the activity series of metals. A reactive metal replaces any metal that is less reactive.

3. Activity Series of Metals  Li  K  Ba  Ca  Na  Mg  Al  Zn  Fe  Ni  Sn  Pb  H  Cu

4. Sample  Zn + H 2 SO 4  ZnSO 4 + H 2  Sn + NaNO 3  ?

5. Examples  Al + H 2 SO 4   Cl 2 + KI   Cu + FeSO 4   Li + H 2 O 

6. Double Replacement Reactions  A double replacement reaction involves an exchange of positive ions between two compounds.  NaOH + H 2 SO 4  Na 2 SO 4 + H 2 0 (UB)  BaCl 2 + K 2 CO 3  BaCO 3 + KCl (UB)

7. Combustion Reactions  In a combustion reaction oxygen reacts with another substance producing energy in the form of heat and light.  Combustion reactions require O 2 and form CO 2 and H 2 O as byproducts.  C 6 H 6 + O 2  CO 2 + H 2 O

8. Combination Reactions  A combination reaction is when two or more substances react to form a single substance  S + O 2  SO 2  Ca + S   Fe + O2  Iron (II) oxide  P + O2  diphosphorus pentoxide

9. Decomposition Reactions  A decomposition reaction is when a single compound is broken down ito two or more simpler products.  CaCO 3  CaO + CO 2  Ag 2 O 