Manganese(II) nitrate

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Manganese(II) nitrate
Manganese(II) nitrate tetrahydrate
Names
Systematic IUPAC name
Manganese(II) nitrate
Other names
Manganese dinitrate
Identifiers
3D model (
JSmol
)
ChemSpider
ECHA InfoCard
100.030.741 Edit this at Wikidata
EC Number
  • 233-828-8
UNII
UN number 2724
  • InChI=1S/Mn.2NO3/c;2*2-1(3)4/q+2;2*-1 ☒N
    Key: MIVBAHRSNUNMPP-UHFFFAOYSA-N ☒N
  • InChI=1/Mn.2NO3/c;2*2-1(3)4/q+2;2*-1
    Key: MIVBAHRSNUNMPP-UHFFFAOYAV
  • [N+](=O)([O-])[O-].[N+](=O)([O-])[O-].[Mn+2]
Properties
Mn(NO3)2
Molar mass 178.95 g/mol
Appearance white powder
Density 1.536 g/cm3
Melting point 37 °C (99 °F; 310 K)
Boiling point 100 °C (212 °F; 373 K)
118 g/100 ml(10°C)
Related compounds
Other anions
Manganese chloride
Other cations
Magnesium nitrate
Calcium nitrate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Manganese(II) nitrate refers to the inorganic compounds with formula Mn(NO3)2·(H2O)n. These compounds are nitrate salts containing varying amounts of water. A common derivative is the tetrahydrate, Mn(NO3)2·4H2O, 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.[1] Typical of a manganese(II) compound, it is a paramagnetic pale pink solid.

Structure

Manganese(II) compounds, especially with oxygenated ligands, are typically octahedral. Following this trend, the tetrahydrate features four

aquo ligands bound to Mn as well as two mutually cis, unidentate nitrate ligands.[2] The hexaaquo salt features octahedral [Mn(H2O)6]2+.[3]

Preparation, reactions, uses

Manganese(II) nitrate is prepared from manganese dioxide and nitrogen dioxide:[1]

MnO2 + 2 NO2 + 4 H2O → Mn(H2O)4(NO3)2

Heating the tetrahydrate to 110 °C gives the pale yellow monohydrate.[4] The reaction is reversible in the sense that heating the dinitrate to 450 °C gives a slightly nonstoichiometric dioxide.[5]

Manganese(II) nitrate is the precursor to manganese(II) carbonate, which is used in fertilizers and as a colorant. The advantage of this method, use of ammonia and carbon dioxide, being that the side product ammonium nitrate is also useful as a fertilizer.[1]

References

  1. ^ .
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  5. ^ H. Lux (1963). "Manganeses(II) Oxide". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 2pages=1455. NY, NY: Academic Press.