Polyatomic ion: Difference between revisions
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A '''polyatomic ion''' is an [[ion]] consisting of a [[molecule]] with [[Covalent bond|covalently bonded]] [[atom]]s or of a [[complex (chemistry)|metal complex]] that can be considered as acting as a single unit in the context of [[acid]] and [[Base (chemistry)|base]] [[chemistry]] or in the formation of [[salt]]s. The prefix poly- means many in Greek. Note, a polyatomic ion is also referred to in older works as a [[radical (chemistry)|radical]]. In current usage the term radical refers to [[free radical]]s which are uncharged species with an unpaired electron. Some can be used in decomposition reactions, providing spectacular results, such as | {{subpages}} | ||
A '''polyatomic ion''' is an [[ion]] consisting of a [[molecule]] with [[Covalent bond|covalently bonded]] [[atom]]s or of a [[complex (chemistry)|metal complex]] that can be considered as acting as a single unit in the context of [[acid]] and [[Base (chemistry)|base]] [[chemistry]] or in the formation of [[salt]]s. The prefix poly- means many in Greek. Note, a polyatomic ion is also referred to in older works as a [[radical (chemistry)|radical]]. In current usage the term radical refers to [[free radical]]s which are uncharged species with an unpaired electron. Some can be used in decomposition reactions, providing spectacular results, such as H<sub>2(g)</sub>, O<sub>2(g)</sub> and I<sub>2(s)</sub>. | |||
'''Hydroxide Ions and Ammonium Ions''' | '''Hydroxide Ions and Ammonium Ions''' | ||
* A Hydroxide ion is made of one oxygen ion and one hydrogen ion: its chemical formula is ( | * A Hydroxide ion is made of one oxygen ion and one hydrogen ion: its chemical formula is (OH)<sup>-</sup>. It has a negative charge. | ||
* An [[Ammonium]] ion is made up of one nitrogen atom and four hydrogen atoms: its Chemical Formula is ( | * An [[Ammonium]] ion is made up of one nitrogen atom and four hydrogen atoms: its Chemical Formula is (NH<sub>4</sub>)<sup>+</sup>. It has a positive charge. | ||
A large polyatomic ion will often be considered as the [[conjugate acid]] or conjugate base of a neutral molecule, for example the conjugate acid of [[adrenaline]] at the [[amine]] group. | A large polyatomic ion will often be considered as the [[conjugate acid]] or conjugate base of a neutral molecule, for example the conjugate acid of [[adrenaline]] at the [[amine]] group. | ||
Note that many of the common negatively-charged [[anion]]ic polyatomic ions are conjugate bases of acids derived from the [[oxide]]s of non-metallic elements. For example the [[sulfate]] or | Note that many of the common negatively-charged [[anion]]ic polyatomic ions are conjugate bases of acids derived from the [[oxide]]s of non-metallic elements. For example the [[sulfate]] or SO<sub>4</sub><sup>2-</sup> ion is derived from [[sulfuric acid|H<sub>2</sub>SO<sub>4</sub>]] which can be regarded as [[sulfur trioxide|SO<sub>3</sub>]] + [[water|H<sub>2</sub>O]]. | ||
There are two "rules" that can be used for making the learning of polyatomic ions somewhat easier. First, when the prefix bi- is added to a name, a hydrogen is added to the ion's formula and its charge reduced by 1. This reduction is a function of the hydrogen ion being a +1 charge. An alternate to the bi- prefix is to use the word hydrogen in its place. | There are two "rules" that can be used for making the learning of polyatomic ions somewhat easier. First, when the prefix bi- is added to a name, a hydrogen is added to the ion's formula and its charge reduced by 1. This reduction is a function of the hydrogen ion being a +1 charge. An alternate to the bi- prefix is to use the word hydrogen in its place. | ||
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carbonate becomes bicarbonate or hydrogen carbonate | carbonate becomes bicarbonate or hydrogen carbonate | ||
CO<sub>3</sub><sup>2-</sup> becomes HCO<sub>3</sub><sup>-</sup> | |||
The second rule looks at the number of oxygens in an ion. Consider the chlorate family: | The second rule looks at the number of oxygens in an ion. Consider the chlorate family: | ||
{| | {| | ||
|- | |- | ||
|| [[perchlorate]]|| style="padding:.5em"| | || [[perchlorate]]|| style="padding:.5em"| ClO<sub>4</sub><sup>-</sup> | ||
|- style="height:120%" | |- style="height:120%" | ||
|| [[chlorate]]|| style="padding:.5em"| | || [[chlorate]]|| style="padding:.5em"| ClO<sub>3</sub><sup>-</sup> | ||
|- style="height:120%" | |- style="height:120%" | ||
|| [[chlorite]]|| style="padding:.5em"| | || [[chlorite]]|| style="padding:.5em"| ClO<sub>2</sub><sup>-</sup> | ||
|- style="height:120%" | |- style="height:120%" | ||
|| [[hypochlorite]]|| style="padding:.5em"| | || [[hypochlorite]]|| style="padding:.5em"| ClO<sup>-</sup> | ||
|} | |} | ||
First, think of the -ate ion as being the "base" name, in which case the addition of a per- prefix adds an oxygen. Changing the -ate suffix to -ite will reduce the oxygens by one, and keeping the suffix -ite and adding the prefix hypo- reduces the number of oxygens by two. In all situations, the charge is not affected. | First, think of the -ate ion as being the "base" name, in which case the addition of a per- prefix adds an oxygen. Changing the -ate suffix to -ite will reduce the oxygens by one, and keeping the suffix -ite and adding the prefix hypo- reduces the number of oxygens by two. In all situations, the charge is not affected. | ||
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|- | |- | ||
| [[acetate]] | | [[acetate]] | ||
| CH<sub>3</sub>COO<sup>-</sup> or C<sub>2<sub>H<sub>3<sub>O<sub>2</sub><sup>-</sup> | | CH<sub>3</sub>COO<sup>-</sup> or C<sub>2</sub>H<sub>3</sub>O<sub>2</sub><sup>-</sup> | ||
|- | |- | ||
| [[aluminate]] | | [[aluminate]] | ||
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== External links == | == External links == | ||
* [http://www2.pvc.maricopa.edu/tutor/chem/chem130/nomenclature/polyatomicion.html List of polyatomic ions] | * [http://www2.pvc.maricopa.edu/tutor/chem/chem130/nomenclature/polyatomicion.html List of polyatomic ions] | ||
* [http://antoine.frostburg.edu/chem/senese/101/compounds/polyatomic.shtml A Beginner's Guide To Polyatomic Ions.] | * [http://antoine.frostburg.edu/chem/senese/101/compounds/polyatomic.shtml A Beginner's Guide To Polyatomic Ions.] | ||
* [http://www.chemistry.wustl.edu/~edudev/LabTutorials/PeriodicProperties/Ions/ions.html Tables of Common Polyatomic Ions. Also a source for PDB files] ([[Protein Data Bank|PDB information]]) | * [http://www.chemistry.wustl.edu/~edudev/LabTutorials/PeriodicProperties/Ions/ions.html Tables of Common Polyatomic Ions. Also a source for PDB files] ([[Protein Data Bank|PDB information]]) | ||
Revision as of 10:20, 13 November 2007
A polyatomic ion is an ion consisting of a molecule with covalently bonded atoms or of a metal complex that can be considered as acting as a single unit in the context of acid and base chemistry or in the formation of salts. The prefix poly- means many in Greek. Note, a polyatomic ion is also referred to in older works as a radical. In current usage the term radical refers to free radicals which are uncharged species with an unpaired electron. Some can be used in decomposition reactions, providing spectacular results, such as H2(g), O2(g) and I2(s).
Hydroxide Ions and Ammonium Ions
- A Hydroxide ion is made of one oxygen ion and one hydrogen ion: its chemical formula is (OH)-. It has a negative charge.
- An Ammonium ion is made up of one nitrogen atom and four hydrogen atoms: its Chemical Formula is (NH4)+. It has a positive charge.
A large polyatomic ion will often be considered as the conjugate acid or conjugate base of a neutral molecule, for example the conjugate acid of adrenaline at the amine group.
Note that many of the common negatively-charged anionic polyatomic ions are conjugate bases of acids derived from the oxides of non-metallic elements. For example the sulfate or SO42- ion is derived from H2SO4 which can be regarded as SO3 + H2O.
There are two "rules" that can be used for making the learning of polyatomic ions somewhat easier. First, when the prefix bi- is added to a name, a hydrogen is added to the ion's formula and its charge reduced by 1. This reduction is a function of the hydrogen ion being a +1 charge. An alternate to the bi- prefix is to use the word hydrogen in its place.
Example:
carbonate becomes bicarbonate or hydrogen carbonate
CO32- becomes HCO3-
The second rule looks at the number of oxygens in an ion. Consider the chlorate family:
| perchlorate | ClO4- |
| chlorate | ClO3- |
| chlorite | ClO2- |
| hypochlorite | ClO- |
First, think of the -ate ion as being the "base" name, in which case the addition of a per- prefix adds an oxygen. Changing the -ate suffix to -ite will reduce the oxygens by one, and keeping the suffix -ite and adding the prefix hypo- reduces the number of oxygens by two. In all situations, the charge is not affected.
It is important to note that these rules will not work with all polyatomic ions, but they do work with the most common ones (sulfate, phosphate, nitrate, chlorate).
The most common type of file to view ion representations is a PDB which refers to Protein Databank. There are also now other kinds becoming available including CIF.