Chemical Reactions

Law of Conservation of Matter = matter can not be created nor destroyed just rearranged.  This is why we balance reactions.

Reactants = starting substances in a chemical reaction (left of arrow)

Products = ending substances from a chemical reaction (right of arrow)

Yield = to produce, to form

Coefficient = the number that comes before a chemical compound use to balance a chemical reaction/equation

Synthesis reaction = a reaction in which 2 simple substances react to form only one product.  Takes the form of A + B --> C

decompostition Reaction = opposite of a synthesis, one reactant breaks down into two or more simpler substances.  This usually requires heat.  Takes the form A --> B + C

Single replacement reaction = uses the activity series list, a more reactive element replaces a less reactive element.  Takes the form A +BC --> AC + B Always one element + a compound yields a new compond + a new element

Double replacement reaction = these usually produce common gases or precipitates (solublity rules - later)  The cations of two compounds mix and replace one another.  Takes the form AB + CD --> AD + CB  Always starts with 2  compounds to prduce 2 new ones

Combustion reaction = an organic material (hydrocarbon) is burned in air (oxygen gas) to produce carbon dioxide and water, large release of heat

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