Stoichiometry!

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

- 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.

- 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.

- 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!