Manganese(II) nitrate

Manganese(II) nitrate
Manganese(II) nitrate tetrahydrate
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

In this redox reaction, two moles of the reductant NO2 (gas) donate each one electron to MnO2 (black solid), the oxidant, which is reduced from its oxidation state (IV) to its lower state (II). Simultaneously, NO2 (IV) is oxidized to form nitrate (NO−3) (V).

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

Manganese(II) nitrate is the precursor to manganese(II) carbonate (MnCO3), which is used in fertilizers and as a colourant. The advantage of this method, based on the use of ammonia (NH3) and carbon dioxide (CO2) as reaction intermediates, being that the side product ammonium nitrate (NH4NO3) is also useful as a fertilizer.[1]

References

  1. ^ a b c Reidies, Arno H. (2000). "Manganese Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a16_123. ISBN 3527306730.
  2. ^ "The Crystal Structure of Manganese Nitrate Tetrahydrate Mn(NO3)2·4H2O". Zeitschrift für Kristallographie - Crystalline Materials. 137 (4): 280–289. 1973. doi:10.1524/zkri.1973.137.4.280.
  3. ^ Petrovič, D.; Ribár, B.; Djurič, S.; Krstanovič, I. (1976). "The Crystal Structure of Hexaquomanganese Nitrate, Mn(OH2)6(NO3)2". Zeitschrift für Kristallographie - Crystalline Materials. 144 (1–6): 334–340. doi:10.1524/zkri.1976.144.16.334. S2CID 97491858.
  4. ^ Milinski, N.; Ribár, B.; Ćulum, Ž.; Djurić, S. (1977). "The Crystal Structure of Manganese Nitrate Monohydrate". Acta Crystallographica Section B: Structural Crystallography and Crystal Chemistry. 33 (6): 1678–1682. doi:10.1107/S056774087700689X.
  5. ^ Lux H. (1963). "Manganeses(II) Oxide". In Brauer G. (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 2. New York: Academic Press. p. 1455.

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