Types of Reactions: The Basics Synthesis reactions Decomposition reactions Single displacement reactions Double displacement reactions Combustion reactions You need to be able to identify each type.

1. Synthesis General: A + B  AB  Example C + O2 CO2  + O O *** Remember, even though the “Magic 7” have a subscript (ex/ O2), they are still considered just a single element***

Synthesis (combination) General: A + B  AB A synthesis reaction will always have: 2 or more reactants 1 product

Ex. Synthesis Reaction

2. Decomposition General: AB  A + B Example: NaCl Na + Cl   + Na Cl

Decomposition General: AB  A + B A decomposition reaction will always have: 1 reactant 2 or more products

Ex. Decomposition Reaction

3. Single Replacement (or single displacement) General: AB + C  AC + B Example: CuCl2 + Zn  ZnCl2 + Cu  Zn Cl Cu + Cl Zn Cu +

Single Replacement General: AB + C  AC + B A single replacement reaction will always have: 1 compound and 1 element as reactants 1 compound and 1 element as products

Ex. Single Replacement Reaction

4. Double replacement (double displacement) General: AB + CD  AD + CB Example: MgO + CaS  MgS + CaO S O  Mg Ca + O S Mg Ca +

Double Replacement General: AB + CD  AD + CB A double replacement reaction will always have: 2 compounds as reactants 2 compounds as products

5. Combustion Reactions C#H# Examples: CH4 C2H6 Combustion reactions - a hydrocarbon reacts with oxygen gas. This is also called burning!!! Hydrocarbons are compounds that contain only carbon and hydrogen C#H# Examples: CH4 C2H6

Combustion Reactions In general: C#H# + O2  CO2 + H2O Reactants are ALWAYS C#H# and O2 gas. Products are ALWAYS CO2 and H2O.

Combustion Example **note: the equation above is not balanced** C5H12 + O2  CO2 + H2O **note: the equation above is not balanced**

Mixed Practice State the reaction type BaCl2 + H2SO4  BaSO4 + HCl (equations are not balanced) BaCl2 + H2SO4  BaSO4 + HCl C6H12 + O2  CO2 + H2O Zn + CuSO4  Cu + ZnSO4 Cs + Br2  CsBr2 FeCO3  Fe + CO2