Manganese(II) nitrate
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| Names | |
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| Systematic IUPAC name
Manganese(II) nitrate | |
| Other names
Manganese dinitrate
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| Identifiers | |
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3D model (JSmol)
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| ChemSpider | |
| ECHA InfoCard | 100.030.741 |
| EC Number |
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PubChem CID
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| UNII | |
| UN number | 2724 |
CompTox Dashboard (EPA)
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| 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(10oC) | |
| Related compounds | |
Other anions
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Manganese chloride |
Other cations
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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 is an inorganic compound with formula Mn(NO3)2. Each formula unit is composed of one Mn2+ cation and two NO3− anions and varying amounts of water. Most common 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]
Preparation
Manganese(II) nitrate can be prepared by dissolving manganese(II) carbonate in dilute nitric acid:
- MnCO3 + 2 HNO3 → Mn(NO3)2 + H2O + CO2
It can also be prepared from manganese dioxide and nitrogen dioxide.[1]
Properties
On heating to 300°C, aqueous solutions of manganese(II) nitrate thermally decompose to form MnO2 and NO2 as products. Upon further heating, the MnO2 loses oxygen to form Mn2O3 and eventually Mn3O4.
References
- ^ a b Arno H. Reidies, "Manganese Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, 2002, Wiley-VCH, Weinheim. doi:10.1002/14356007.a16_123
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