Single Replacement Single Replacement Reactions are reactions that involve an element replacing one part of a compound. The products include the displaced element and a new compound. The more reactive element (metal or nonmetal) will always end up as part of the compound; if the more reactive element is already in the compound, no reaction will occur.

2KBr + Cl2  2KCl + Br2 SINGLE REPLACEMENT: An element replacing one part of a compound forms a new element & compound TIPS: Single element & a compound Element can be diatomic: BrINClHOF

Double Replacement Double Replacement reactions is where two reactant compounds exchange ions to form two new products that are compounds. The ions/elements from the reactants must appear in the produces. No new elements are added during the reaction.

NaCl + AgBr  AgCl + NaBr DOUBLE REPLACEMENT: 2 reactant compounds exchange ions to form 2 new products that are compounds TIPS: 2 compounds both sides Must produce a solid, liquid, gas Precipitation Reaction

Combustion Reactions Combustion Reactions occur when hydrocarbons or carbohydrates burn in oxygen. The products are ALWAYS water and carbon dioxide. Oxygen = O2

2C2H6 + 7O2  4CO2 + 6H2O COMBUSTION: A carbohydrate or hydrocarbon is burned in air (O2) to form carbon dioxide and water TIPS: Only products are CO2 & H2O Reactant must have O2

Decomposition Reactions Decomposition Reactions occur when a single reactant is broken down into two or more products, sometimes spontaneously and sometimes with the addition of heat.

2KClO3  2KCl + 3O2 DECOMPOSITION: Single reactant is broken down into 2 or more products TIPS: Always 1 Reactant Redox Rxn

Synthesis Reaction Synthesis Reaction occurs when two substances combine to form a single new substance. A more complex product is always formed in synthesis rxns. This is the most common type of reaction.

H2 + Cl2  2HCl SYNTHESIS: 2 substances combine to form 1 new substance TIPS: Always 1 product produced Redox Rxn