Difference between revisions of "Hydroxide" - New World Encyclopedia

Hydroxide
General
Systematic name	hydroxide; oxidanide; hydridooxygenate(1−)
Molecular formula	OH−
Molar mass	19.02 g/mol
CAS number	[14280-30-9]
	Except where noted otherwise, data are given for; materials in their standard state (at 25 °C, 100 kPa); Infobox disclaimer and references

Latest revision as of 22:31, 30 August 2016

In chemistry, hydroxide is the most common name for the diatomic anion OH⁻, consisting of oxygen and hydrogen atoms. It is one of the simplest diatomic ions known. The term "hydroxide" also refers to the class of compounds that contain the hydroxide ion. Common examples are sodium hydroxide, potassium hydroxide, and ammonium hydroxide.

Pellets of sodium hydroxide.

Hydroxide compounds and ions are relatively common in nature. Several mineral ores, such as bauxite and limonite, are hydroxides. In addition, hydroxides are widely used in human activities. For example, sodium hydroxide (lye) is useful as a strong base in industry, and potassium hydroxide is used in agriculture.

Hydroxide as a base

Most compounds containing the hydroxide ion are chemical bases. Thus, hydroxide ions are involved in numerous acid-base reactions, including the reaction known as neutralization.

A substance that produces hydroxide ions when dissolved in aqueous solution is called an Arrhenius base. One example is ammonia (NH₃):

NH₃(g) + H₂O(l) ⇌ NH₄⁺(aq) + OH⁻(aq)

Salts containing hydroxide are called base salts. Base salts will dissociate into a cation and one or more hydroxide ions in water, making the solution basic. Base salts will undergo neutralization reactions with acids. In general, an acid-alkali reactions can be simplified to

OH⁻(aq) + H⁺(aq) → H₂O (l)

Ions that do not participate in this reaction are called spectator ions and are not shown here.

Solubility

Most inorganic hydroxide salts are insoluble in water. Important exceptions are salts in which the cations are alkali metal ions and or NH₄⁺, Ba²⁺, Sr²⁺, Ca²⁺, or Tl⁺ ions.

Behavior as a ligand

The hydroxide ion is a type of ligand. Each oxygen atom in the OH⁻ ion has a "lone pair" (unshared pairs) of electrons in the outermost shell, and it forms bonds by donating this pair of electrons to an appropriate receiving atom. In this manner, a hydroxide ion behaves as a Lewis base. Examples include the aluminate ion [Al(OH)₄]⁻, and aurate ion [Au(OH)₄]⁻.

Uses of hydroxide

Hydroxides and hydroxide ions are relatively common. Many useful chemicals and chemical processes involve hydroxides or hydroxide ions. Sodium hydroxide (lye) is used in industry as a strong base, potassium hydroxide is used in agriculture, and iron hydroxide minerals such as goethite and limonite have been used as low grade brown iron ore. The aluminum ore bauxite is composed largely of aluminum hydroxides.

References
ISBN links support NWE through referral fees

Chang, Raymond. 2006. Chemistry. 9th ed. New York: McGraw-Hill Science/Engineering/Math. ISBN 0073221031 and ISBN 978-0073221038.
Cotton, F. Albert, and Geoffrey Wilkinson. 1980. Advanced Inorganic Chemistry. 4th ed. New York: Wiley. ISBN 0471027758.
McMurry, J., and R.C. Fay. 2004. Chemistry. 4th ed. Upper Saddle River, NJ: Prentice Hall. ISBN 0131402080.

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-| [[IUPAC nomenclature|Systematic name]]<ref>http://www.iupac.org/reports/provisional/abstract04/RB-prs310804/TableIX-3.04.pdf</ref>
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+In [[chemistry]], '''hydroxide''' is the most common name for the [[diatomic]] [[anion]] OH<sup>&minus;</sup>, consisting of [[oxygen]] and [[hydrogen]] [[atom]]s. It is one of the simplest diatomic ions known. The term "hydroxide" also refers to the class of compounds that contain the hydroxide ion. Common examples are [[sodium hydroxide]], [[potassium hydroxide]], and [[ammonium hydroxide]].
+{{toc}}
 [[Image:Sodium hydroxide.jpg|thumb|250px|Pellets of sodium hydroxide.]]
+Hydroxide compounds and ions are relatively common in nature. Several mineral ores, such as [[bauxite]] and [[limonite]], are hydroxides. In addition, hydroxides are widely used in human activities. For example, [[sodium hydroxide]] (lye) is useful as a strong base in industry, and [[potassium hydroxide]] is used in agriculture.
-In [[chemistry]], '''hydroxide''' is the most common name for the [[diatomic]] [[anion]] OH<sup>−</sup>, consisting of [[oxygen]] and [[hydrogen]] [[atom]]s, usually derived from the [[Dissociation (chemistry)|dissociation]] of a [[base (chemistry)|base]]. It is one of the simplest diatomic ions known.
+==Hydroxide as a base==
-[[Inorganic]] compounds that contain the [[hydroxyl]] group are referred to as hydroxides.
-==Hydroxide as a base==
+Most compounds containing the hydroxide ion are chemical [[base (chemistry)|base]]s. Thus, hydroxide ions are involved in numerous [[acid-base]] reactions, including the reaction known as [[neutralization]].
-Most compounds containing hydroxide are bases.
-An [[Arrhenius base]] is a substance that produces hydroxide ions when dissolved in [[aqueous solution]]. One example would be [[ammonia]] (NH<sub>3</sub>):
+A substance that produces hydroxide ions when dissolved in [[aqueous solution]] is called an [[Arrhenius base]]. One example is [[ammonia]] (NH<sub>3</sub>):
 :NH<sub>3</sub>(g) + H<sub>2</sub>O(l) {{unicode|⇌}} [[ammonium|NH<sub>4</sub><sup>+</sup>]](aq) + OH<sup>−</sup>(aq)
-Thus, hydroxide ions are heavily involved in [[acid-base]] reactions as well as the special double displacement reaction called [[neutralization]].
+Salts containing hydroxide are called [[base salts]]. Base salts will dissociate into a cation and one or more hydroxide ions in water, making the solution basic. Base salts will undergo [[neutralization reaction]]s with [[acid]]s. In general, an [[acid-alkali reaction]]s can be simplified to
-Salts containing hydroxide are called [[base salts]]. Base salts will dissociate into a cation and one or more hydroxide ions in water, making the solution basic. Base salts will undergo [[neutralisation reactions]] with [[acids]]. In general [[acid-alkali reactions]] can be simplified to
 :OH<sup>−</sup>[[Aqueous|(aq)]] + [[hydronium|H<sup>+</sup>]](aq) → [[water (molecule)|H<sub>2</sub>O]][[liquid|(l)]]
-by omitting [[spectator ion]]s.
+Ions that do not participate in this reaction are called [[spectator ion]]s and are not shown here.
 ==Solubility==
-Most inorganic hydroxide salts are [[insoluble]] in water, except for cations of [[alkali metal]]s and the cations [[Ammonium|NH<sub>4</sub><sup>+</sup>]], [[Barium|Ba<sup>2+</sup>]], [[Strontium|Sr<sup>2+</sup>]], [[Calcium|Ca<sup>2+</sup>]] or [[Thallium|Tl<sup>+</sup>]].
+Most inorganic hydroxide salts are [[insoluble]] in water. Important exceptions are salts in which the cations are [[alkali metal]] ions and or [[Ammonium|NH<sub>4</sub><sup>+</sup>]], [[Barium|Ba<sup>2+</sup>]], [[Strontium|Sr<sup>2+</sup>]], [[Calcium|Ca<sup>2+</sup>]], or [[Thallium|Tl<sup>+</sup>]] ions.
+==Behavior as a ligand==
+The hydroxide ion is a type of [[ligand]]. Each oxygen atom in the OH<sup>−</sup> ion has a "lone pair" (unshared pairs) of electrons in the outermost shell, and it forms bonds by donating this pair of electrons to an appropriate receiving atom. In this manner, a hydroxide ion behaves as a [[Lewis base]]. Examples include the aluminate ion [Al(OH)<sub>4</sub>]<sup>−</sup>, and aurate ion [Au(OH)<sub>4</sub>]<sup>−</sup>.
 ==Uses of hydroxide==
-Hydroxides and hydroxide ions are relatively common. Many useful chemicals and chemical processes involve hydroxides or hydroxide ions. [[Sodium hydroxide]] (lye) is used in industry as a strong base, [[potassium hydroxide]] is used in agriculture, and [[iron hydroxide]] minerals such as [[goethite]] and [[limonite]] have been used as low grade ''brown'' iron [[ore]]. The [[aluminium]] ore [[bauxite]] is composed largely of aluminium hydroxides.
+Hydroxides and hydroxide ions are relatively common. Many useful chemicals and chemical processes involve hydroxides or hydroxide ions. [[Sodium hydroxide]] (lye) is used in industry as a strong base, [[potassium hydroxide]] is used in agriculture, and [[iron hydroxide]] minerals such as [[goethite]] and [[limonite]] have been used as low grade ''brown'' iron [[ore]]. The [[aluminum]] ore [[bauxite]] is composed largely of aluminum hydroxides.
-==Ligand==
-Hydroxide ion is a kind of [[ligand]]. It donates lone pairs of electrons, behaving as a [[Lewis base]].
-Examples include the aluminate ion [Al(OH)<sub>4</sub>]<sup>−</sup> and aurate ion [Au(OH)<sub>4</sub>]<sup>−</sup>.
 ==See also==
-*[[Hydronium]]
-*[[Oxide]]
-*[[Hydroxyl]]
-==Notes==
+* [[Base (chemistry)]]
-<references/>
+* [[Hydronium]]
+* [[Hydroxyl]]
+* [[Oxide]]
+* [[Sodium hydroxide]]
 == References ==
-<<Refs needed>>
+* Chang, Raymond. 2006. ''Chemistry''. 9th ed. New York: McGraw-Hill Science/Engineering/Math. ISBN 0073221031 and ISBN 978-0073221038.
+* Cotton, F. Albert, and Geoffrey Wilkinson. 1980. ''Advanced Inorganic Chemistry''. 4th ed. New York: Wiley. ISBN 0471027758.
+* McMurry, J., and R.C. Fay. 2004. ''Chemistry''. 4th ed. Upper Saddle River, NJ: Prentice Hall. ISBN 0131402080.
 [[Category:Physical sciences]]

Hydroxide

General
Systematic name	hydroxide oxidanide hydridooxygenate(1−)
Molecular formula	O H⁻
Molar mass	19.02 g/mol
CAS number	[14280-30-9]
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references