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Updating {{chembox}} (no changed fields - added verified revid - updated 'DrugBank_Ref', 'UNII_Ref', 'ChEMBL_Ref', 'ChEBI_Ref', 'StdInChI_Ref', 'StdInChIKey_Ref') per Chem/Drugbox validation (report [[Wikipedia_talk:WikiProject_Chemi
→‎Preparation, reactions, uses: Description of the redox reaction + minor copyedit elsewhere + wikilinks
 
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{{Chembox
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| InChI = 1/Mn.2NO3/c;2*2-1(3)4/q+2;2*-1
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| Formula = Mn(NO<sub>3</sub>)<sub>2</sub>
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| MolarMass = 178.95 g/mol
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| Solubility = 118 g/100 ml(10°C)
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'''Manganese(II) nitrate''' is an [[inorganic compound]] with [[Chemical formula|formula]] [[Manganese|Mn]]([[Nitrate|NO<sub>3</sub>]])<sub>2</sub>. Each [[formula unit]] is composed of one Mn<sup>2+</sup> [[cation]] and two [[Nitrate|NO<sub>3</sub><sup>-</sup>]] [[anion]]s and varying amounts of water. Most common is the tetrahydrate Mn(NO<sub>3</sub>)<sub>2</sub>·4H<sub>2</sub>O, but mono- and hexahydrates are also known as well as the [[anhydrous]] compound. Some of these compounds are useful precursors to the oxides of manganese.<ref name=Ullmann>Arno H. Reidies, “Manganese Compounds” in ''Ullmann's Encyclopedia of Industrial Chemistry'', 2002, Wiley-VCH, Weinheim. {{DOI|10.1002/14356007.a16_123}}</ref>
'''Manganese(II) nitrate''' refers to the [[inorganic compound]]s with [[Chemical formula|formula]] [[Manganese|Mn]]([[Nitrate|NO<sub>3</sub>]])<sub>2</sub>·(H<sub>2</sub>O)<sub>n</sub>. These compounds are nitrate salts containing varying amounts of water. A common derivative is the tetrahydrate, Mn(NO<sub>3</sub>)<sub>2</sub>·4H<sub>2</sub>O, but mono- and hexahydrates are also known as well as the [[anhydrous]] compound. Some of these compounds are useful precursors to the oxides of manganese.<ref name=Ullmann>{{Ullmann|doi=10.1002/14356007.a16_123|title=Manganese Compounds|year=2000|last1=Reidies|first1=Arno H.|isbn=3527306730}}</ref> Typical of a manganese(II) compound, it is a paramagnetic pale pink solid.


== Preparation ==
==Structure==
Manganese(II) compounds, especially with oxygenated ligands, are typically octahedral. Following this trend, the tetrahydrate features four [[aquo ligand]]s bound to Mn as well as two mutually cis, unidentate nitrate [[ligand]]s.<ref>{{cite journal |doi=10.1524/zkri.1973.137.4.280|title=The Crystal Structure of Manganese Nitrate Tetrahydrate Mn(NO<sub>3</sub>)<sub>2</sub>·4H<sub>2</sub>O|journal=Zeitschrift für Kristallographie - Crystalline Materials|year=1973|volume=137|issue=4|pages=280–289}}</ref> The hexaaquo salt features octahedral [Mn(H<sub>2</sub>O)<sub>6</sub>]<sup>2+</sup>.<ref>{{cite journal |doi=10.1524/zkri.1976.144.16.334| title=The Crystal Structure of Hexaquomanganese Nitrate, Mn(OH<sub>2</sub>)<sub>6</sub>(NO<sub>3</sub>)<sub>2</sub> | year=1976 | last1=Petrovič | first1=D. | last2=Ribár | first2=B. | last3=Djurič | first3=S. | last4=Krstanovič | first4=I. | journal=Zeitschrift für Kristallographie - Crystalline Materials | volume=144 | issue=1–6 | pages=334–340 | s2cid=97491858 }}</ref>
Manganese(II) nitrate can be prepared by dissolving [[manganese(II) carbonate]] in dilute [[nitric acid]]:
:MnCO<sub>3</sub> + 2 HNO<sub>3</sub> → Mn(NO<sub>3</sub>)<sub>2</sub> + H<sub>2</sub>O + CO<sub>2</sub>
It can also be prepared from MnO<sub>2</sub> and nitrogen dioxide.<ref name=Ullmann/>


== Preparation, reactions, uses ==
== References ==
Manganese(II) nitrate is prepared from [[manganese dioxide]] and [[nitrogen dioxide]]:<ref name=Ullmann/>
{{reflist}}


: {{chem2|MnO2 + 2 NO2 + 4 H2O -> Mn(H2O)4(NO3)2}}


In this [[redox]] reaction, two [[Mole (unit)|moles]] of the [[Reducing agent|reductant]] {{chem2|NO2}} (gas) donate each one [[electron]] to {{chem2|MnO2}} (black solid), the [[Oxidizing agent|oxidant]], which is reduced from its [[oxidation state]] (IV) to its lower state (II). Simultaneously, {{chem2|NO2}} (IV) is oxidized to form [[nitrate]] ({{chem2|NO3-}}) (V).

Heating the tetrahydrate to 110&nbsp;°C gives the pale yellow monohydrate.<ref>{{cite journal |doi=10.1107/S056774087700689X|title=The Crystal Structure of Manganese Nitrate Monohydrate|year=1977|last1=Milinski|first1=N.|last2=Ribár|first2=B.|last3=Ćulum|first3=Ž.|last4=Djurić|first4=S.|journal=Acta Crystallographica Section B: Structural Crystallography and Crystal Chemistry|volume=33|issue=6|pages=1678–1682}}</ref>
The reaction is reversible in the sense that heating the Mn(II) dinitrate to 450{{nbsp}}°C gives a slightly [[Stoichiometry|nonstoichiometric]] Mn(IV) dioxide.<ref>{{cite book|author1= Lux H.|chapter=Manganeses(II) Oxide|title=Handbook of Preparative Inorganic Chemistry, 2nd Ed. |editor= Brauer G.|publisher=Academic Press|year=1963|place=New York|volume=2|pages=1455}}</ref>

Manganese(II) nitrate is the precursor to [[manganese(II) carbonate]] ({{chem2|MnCO3}}), which is used in [[fertilizer]]s and as a [[colourant]]. The advantage of this method, based on the use of [[ammonia]] ({{chem2|NH3}}) and [[carbon dioxide]] ({{CO2}}) as reaction intermediates, being that the side product [[ammonium nitrate]] ({{chem2|NH4NO3}}) is also useful as a fertilizer.<ref name=Ullmann/>

== References ==
{{reflist}}


{{Manganese compounds}}
{{Manganese compounds}}
{{nitrates}}


[[Category:Manganese compounds]]
[[Category:Manganese(II) compounds]]
[[Category:Salts]]
[[Category:Nitrates]]
[[Category:Nitrates]]
{{inorganic-compound-stub}}

[[de:Mangan(II)-nitrat]]
[[pl:Azotan(V) manganu(II)]]
[[zh:硝酸锰]]
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