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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 |
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| 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(10°C) | |
| 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 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.
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How to Write the Formula for Manganese (II) nitrate
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Molar Mass / Molecular Weight of Mn(NO3)2: Manganese (II) Nitrate
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How to Write the Formula for Manganese (II) nitride
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Complex Ions: Precipitating and oxidising manganese (II) hydroxide
Transcription
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
- ^ 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 978-3527306732.
- ^ "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.
- ^ 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.
- ^ 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.
- ^ 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.
This page was last edited on 5 April 2024, at 10:28