1. Types of Reactions and Predicting Products

2. Types of Reactions There are four main types of chemical reactions: Synthesis Synthesis Decomposition Decomposition Single Displacement/Replacement Single Displacement/Replacement Double Displacement/Replacement Double Displacement/Replacement There are also (1) combustion and (2) neutralization reactions

3. Synthesis Synthesis: Two or more reactants combine to form one new product e.g., 2Mg + O 2 2MgO

4. Synthesis Other examples of a synthesis (…combining or coming together) reaction… 3Ca + 2P  Ca 3 P 2 H 2 + S0 4  H 2 SO 4 S + Zn  ZnS 4Cs + O 2  2 Cs 2 O

5. Decomposition Decomposition: One reactant breaks down into two or more products e.g., 2H 2 O  2H 2 + O 2

6. Decomposition More examples of a decomposition ( … breaking apart … ) reaction (one reactant breaking apart into two or more products) 2KClO 3  2KCl + O 2 2KClO 3  2KCl + O 2

7. Single Displacement Single Displacement: A single element replaces one component of a compound e.g. MgBr 2 + Cl 2  MgCl 2 + Br 2 In this case, negative ions replace negative ions…

8. Single Displacement Other examples of a single displacement reaction (…one replacing another…) Fe + CuSO 4  Cu + FeSO 4 Ca + 2NaCl  CaCl 2 + 2Na 2(H 3 PO 4 ) + 6K  3H 2 + 2(K 3 PO 4 )

9. Double Displacement Double Displacement: Parts of two compounds switch places e.g. 3NaOH + FeCl 3  Fe(OH) 3 + 3NaCl Remember that positive ions always pair with negative ions.

10. Combustion And remember that there also exist combustion reactions e.g. Combustion of hydrocarbons like methane…. CH 4 + 2O 2  CO 2 + 2H 2 O