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There is no universally accepted list of the typical, important inorganic reactions. Although there are numerous available sources (books, journal and Internet websites) that include such lists, they all differ to some extent from each other. The inorganic reaction types listed and explained below were drawn from many of the available sources:<ref name=Cotton/><ref name=Cox>{{cite book|author=P.A. Cox|title=Inorganic Chemistry|edition=2nd Edition|publisher=Taylor & Francis|year=2004|id=ISBN 1-85996-289-0}}</ref><ref>[http://www.files.chem.vt.edu/RVGS/ACT/notes/Types_of_Equations.html Types of Equations] From the website of the [[Virginia Polytechnic Institute and State University]] (Virgina Tech). A list of many similar, excellent chemistry articles are available [http://www.files.chem.vt.edu/RVGS/ACT/notes/ACT-notes.html here].</ref><ref name=About1>[http://chemistry.about.com/cs/generalchemistry/a/aa072103a.htm Types of Inorganic Chemical Reactions] By Dr. Anne Marie Helmenstine on the website of About.com: Chemistry.</ref><ref name=About2>[http://chemistry.about.com/od/chemicalreactions/a/reactiontypes.htm Types of Chemical Reactions] By Dr. Anne Marie Helmenstine on the website of About.com: Chemistry.</ref> | There is no universally accepted list of the typical, important inorganic reactions. Although there are numerous available sources (books, journal and Internet websites) that include such lists, they all differ to some extent from each other. The inorganic reaction types listed and explained below were drawn from many of the available sources:<ref name=Cotton/><ref name=Cox>{{cite book|author=P.A. Cox|title=Inorganic Chemistry|edition=2nd Edition|publisher=Taylor & Francis|year=2004|id=ISBN 1-85996-289-0}}</ref><ref>[http://www.files.chem.vt.edu/RVGS/ACT/notes/Types_of_Equations.html Types of Equations] From the website of the [[Virginia Polytechnic Institute and State University]] (Virgina Tech). A list of many similar, excellent chemistry articles are available [http://www.files.chem.vt.edu/RVGS/ACT/notes/ACT-notes.html here].</ref><ref name=About1>[http://chemistry.about.com/cs/generalchemistry/a/aa072103a.htm Types of Inorganic Chemical Reactions] By Dr. Anne Marie Helmenstine on the website of About.com: Chemistry.</ref><ref name=About2>[http://chemistry.about.com/od/chemicalreactions/a/reactiontypes.htm Types of Chemical Reactions] By Dr. Anne Marie Helmenstine on the website of About.com: Chemistry.</ref> | ||
'''''Synthesis reaction:''''' (also referred to as '''''combination''''' or '''''composition''''' reaction) | '''''Synthesis reaction:''''' (also referred to as '''''combination''''' or '''''composition''''' reaction) | ||
This is a reaction in which two or more reactants combine to form a single product, where each reactant is a chemical element or compound and the reaction product consist of the two reactants. Examples include: | This is a reaction in which two or more reactants combine to form a single product, where each reactant is a chemical element or compound and the reaction product consist of the two reactants. Examples include: | ||
*[[sodium]] + [[chlorine]] → [[sodium chloride]] | *[[sodium]] + [[chlorine]] → [[sodium chloride]] | ||
::2Na + Cl <sub>2</sub> → 2NaCl | ::2Na + Cl <sub>2</sub> → 2NaCl | ||
| Line 18: | Line 18: | ||
'''''Decomposition reaction:''''' (may be '''''thermal''''', '''''electrolytic''''' or '''''catalytic''''' decomposition reaction) | '''''Decomposition reaction:''''' (may be '''''thermal''''', '''''electrolytic''''' or '''''catalytic''''' decomposition reaction) | ||
This is a reaction in which a chemical compound is separated into elements or simpler compounds. It is often defined as the exact opposite of a synthesis reaction. Examples include: | |||
* [[hydrogen peroxide]] → water + [[oxygen]] | |||
::2H<sub>2</sub>O<sub>2</sub> → 2H<sub>2</sub>O + O<sub>2</sub> | |||
* [[calcium carbonate]] → [[calcium oxide]] + carbon dioxide | |||
::CaCO<sub>3</sub> → CaO + CO<sub>2</sub> | |||
'''''Single displacement reaction:''''' (also referred to as '''''substitution''''' or '''''single replacement''''' reaction) | |||
This is a reaction characterized by one element being displaced from a compound by another element. Examples include: | |||
* [[zinc]] + [[hydrochloric acid]] → [[zinc chloride]] + hydrogen | |||
::Zn + 2HCl → ZnCl<sub>2</sub> + H<sub>2</sub> | |||
Revision as of 14:16, 8 October 2010
Typical of inorganic chemical reactions
There is no universally accepted list of the typical, important inorganic reactions. Although there are numerous available sources (books, journal and Internet websites) that include such lists, they all differ to some extent from each other. The inorganic reaction types listed and explained below were drawn from many of the available sources:[1][2][3][4][5]
Synthesis reaction: (also referred to as combination or composition reaction)
This is a reaction in which two or more reactants combine to form a single product, where each reactant is a chemical element or compound and the reaction product consist of the two reactants. Examples include:
- 2Na + Cl 2 → 2NaCl
- CO2 + H2O → H2CO3
- 2H2 + S → H2S
Decomposition reaction: (may be thermal, electrolytic or catalytic decomposition reaction)
This is a reaction in which a chemical compound is separated into elements or simpler compounds. It is often defined as the exact opposite of a synthesis reaction. Examples include:
- hydrogen peroxide → water + oxygen
- 2H2O2 → 2H2O + O2
- calcium carbonate → calcium oxide + carbon dioxide
- CaCO3 → CaO + CO2
Single displacement reaction: (also referred to as substitution or single replacement reaction)
This is a reaction characterized by one element being displaced from a compound by another element. Examples include:
- zinc + hydrochloric acid → zinc chloride + hydrogen
- Zn + 2HCl → ZnCl2 + H2
Double replacement reaction: (also referred to as metathesis or exchange reaction)
Acid-base reaction: (also referred to as neutralization)
Redox reaction: (also referred to as oxidation-reduction reaction)
Precipitation reaction: (also referred to as aqueous metathesis reaction)
- ↑ Cite error: Invalid
<ref>tag; no text was provided for refs namedCotton - ↑ P.A. Cox (2004). Inorganic Chemistry, 2nd Edition. Taylor & Francis. ISBN 1-85996-289-0.
- ↑ Types of Equations From the website of the Virginia Polytechnic Institute and State University (Virgina Tech). A list of many similar, excellent chemistry articles are available here.
- ↑ Types of Inorganic Chemical Reactions By Dr. Anne Marie Helmenstine on the website of About.com: Chemistry.
- ↑ Types of Chemical Reactions By Dr. Anne Marie Helmenstine on the website of About.com: Chemistry.