1. 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.

2. 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

3. 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.

4. 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

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

6. 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

7. 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.

8. 2KClO3  2KCl + 3O2 DECOMPOSITION:
Single reactant is broken down into 2 or more products
TIPS: Always 1 Reactant
Redox Rxn

9. 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.

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