Quantitative Chemistry
Stoichiometry is a branch of chemistry that deals with the quantitative analysis of chemical reactions. It is a generalization of mole conversions to chemical reactions. The foundation of stoichiometry is understanding the 6 types of chemical reactions. The 6 types of reactions are;
synthesis (formation),
decomposition,
single replacement (SR),
double replacement (DR),
neutralization, and
combustion.
Synthesis
Synthesis reactions combine two elements to make a compound
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A+B -> AB
Examples:
4Fe + P4 -> 4FeP
Here is a helpful video for synthesis reaction:
Decompostion
Decomposition is the reverse of Synthesis. Always assume that compounds decompose into elements during decomposition.
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AB -> A+B
Examples:
Ca(NO2)2 -> Ca + 2(NO2)
Here is a helpful video for decomposition reactions:
Single Replacement (SR)
In single replacement reactions the metals switch places.
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A + BC -> B + AC
Here is a helpful video on single replacement reactions.
Examples:
Sr + 2LiF -> 2Li + SrF2
Double Replacement (DR)
In double replacement reactions the non-metals in each compound switch places.
-
AB + CD -> AD + BC
Examples:
BeI2 + Na2(SO3) -> Be(SO3) + 2NaI
Here is a helpful video on double replacement reactions:
Neutralization
A neutralization reaction is a reaction between an acid and a base
Examples:
HCl + NaOH -> NaCl + HOH
Here is a helpful video on neutralization reactions:
Combustion
A combustion reaction is a reaction of something (usually hydrocarbon) with air. Hydrocarbon combustion always produces CO2 + H2O
Examples:
CH3OH + O2 -> CO2 + 2H2O
Here is a helpful video on combustion reactions:
And that wraps up the 6 chemical reactions!
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