User:Milton Beychok/Sandbox: Difference between revisions
imported>Milton Beychok |
imported>Milton Beychok No edit summary |
||
| Line 1: | Line 1: | ||
==Typical | ==Typical 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:<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> | ||
| Line 20: | Line 20: | ||
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: | 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]] | * [[hydrogen peroxide]] → water + [[oxygen]] (Hydrogen peroxide spontaneously decomposes into water and gaseous oxygen) | ||
::2H<sub>2</sub>O<sub>2</sub> → 2H<sub>2</sub>O + O<sub>2</sub> | ::2H<sub>2</sub>O<sub>2</sub> → 2H<sub>2</sub>O + O<sub>2</sub> | ||
* [[calcium carbonate]] → [[calcium oxide]] + carbon dioxide | * [[calcium carbonate]] → [[calcium oxide]] + carbon dioxide (When heated calcium carbonate decomposes into calcium oxide and gaseous carbon dioxide) | ||
::CaCO<sub>3</sub> → CaO + CO<sub>2</sub> | ::CaCO<sub>3</sub> + heat → CaO + CO<sub>2</sub> | ||
'''''Single displacement reaction:''''' (also referred to as '''''substitution''''' or '''''single replacement''''' reaction) | '''''Single displacement reaction:''''' (also referred to as '''''substitution''''' or '''''single replacement''''' reaction) | ||
| Line 30: | Line 30: | ||
This is a reaction characterized by one element being displaced from a compound by another element. Examples include: | This is a reaction characterized by one element being displaced from a compound by another element. Examples include: | ||
* [[ | * [[copper]] + [[hydrochloric acid]] → [[copper chloride]] + hydrogen | ||
:: | ::Cu + 2HCl → CuCl<sub>2</sub> + H<sub>2</sub> | ||
* [[ | * [[zinc]] + [[copper sulfate]] → copper + zinc sulfate | ||
:: | ::Zn + CuSO<sub>4</sub> → Cu + ZnSO<sub>4</sub> | ||
'''''Metathesis reaction:''''' (also referred to as '''''exchange''''' or '''''double displacement''''' or '''''double replacement''''' reaction) | '''''Metathesis reaction:''''' (also referred to as '''''exchange''''' or '''''double displacement''''' or '''''double replacement''''' reaction) | ||
Revision as of 17:28, 8 October 2010
Typical 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 + Cl2 → 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 (Hydrogen peroxide spontaneously decomposes into water and gaseous oxygen)
- 2H2O2 → 2H2O + O2
- calcium carbonate → calcium oxide + carbon dioxide (When heated calcium carbonate decomposes into calcium oxide and gaseous carbon dioxide)
- CaCO3 + heat → 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:
- copper + hydrochloric acid → copper chloride + hydrogen
- Cu + 2HCl → CuCl2 + H2
- zinc + copper sulfate → copper + zinc sulfate
- Zn + CuSO4 → Cu + ZnSO4
Metathesis reaction: (also referred to as exchange or double displacement or double replacement reaction) This is a reaction in which the chemical elements from two compounds displace each other to form new, different compounds. It may also be defined as a reaction in which two compounds exchange bonds or ions in order to form new, different compounds. Examples include:
- sodium sulfate + barium chloride → barium chloride + barium sulfate
- Na2SO4 + BaCl2 → BaSO4 + 2NaCl
Precipitation reaction: (also referred to as aqueous metathesis)
- Calcium chloride + silver nitrate → calcium nitrate +silver chloride
- CaCl2 (aq) + 2 AgNO3 (aq) --> Ca(NO3)2 (aq) + 2 AgCl (s)
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.