Classifying Chemical Reactions

Synthesis

Multiples combine to make ONE PRODUCT (also known as: combination reaction)

Decomposition

ONE REACTANT breaks down to multiple products (think of decomposing: breaking elements down)

Single replacement

is a chemical reaction where one element replaces another in a compound

Double replacement

2 compounds (ionic) on each side ( 1 element + compound = 2 compounds)

definition: 2 ionic compounds that are in each side of the equation.

Combustion

the same: oxygen is alone as a reactant

different: amount of products and the form of products and reactants

*oxygen is air which is fuel to a fire = combustion.

definition: a type of chemical reaction between a fuel and and oxygen that produces energy in the form of light and heat.

Synthesis equation:

Zn + S = ZnS

Decomposition equation:

Al2S3 —> Al + S

Single Replacement equation:

H2SO4 + Fe —> H2 + FeSO4

Double Replacement equation

PbCl4 + AgNO3 —> Pb(NO3)2 + AgCl

Combustion equation:

One product: A + O2 —> AO2

2 products: C2H3 + O2 —> CO2 + H2O

Synthetic Combustion:

Fe + O2 —> Fe2O3

Hydrocarbon

a compound made up of only two elements: hydrogen and carbon

Combustion (Hydrocarbon) equation:

C4H12 + O2 —> H2O + CO2