Manganese(II) nitrate
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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). | |
what is ?) | (|
Infobox references | |
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] As a manganese(II) compound, it is paramagnetic and usually pale pink.
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]
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.[3]
On heating to 300 °C, aqueous solutions of manganese(II) nitrate decompose to form MnO2 and NO2.
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[]
- ^ a b c Reidies, Arno H. (2000). "Manganese Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a16_123.
- ^ "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.
- ^ 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.
HNO3 | He | ||||||||||||||||
LiNO3 | Be(NO3)2 | B(NO 3)− 4 |
RONO2 | NO− 3 NH4NO3 |
HOONO2 | FNO3 | Ne | ||||||||||
NaNO3 | Mg(NO3)2 | Al(NO3)3 | Si | P | S | ClONO2 | Ar | ||||||||||
KNO3 | Ca(NO3)2 | Sc(NO3)3 | Ti(NO3)4 | VO(NO3)3 | Cr(NO3)3 | Mn(NO3)2 | Fe(NO3)2 Fe(NO3)3 |
Co(NO3)2 Co(NO3)3 |
Ni(NO3)2 | CuNO3 Cu(NO3)2 |
Zn(NO3)2 | Ga(NO3)3 | Ge | As | Se | BrNO3 | Kr |
RbNO3 | Sr(NO3)2 | Y(NO3)3 | Zr(NO3)4 | Nb | Mo | Tc | Ru(NO3)3 | Rh(NO3)3 | Pd(NO3)2 |
AgNO3 |
Cd(NO3)2 | In(NO3)3 | Sn(NO3)4 | Sb(NO3)3 | Te | INO3 | Xe(NO3)2 |
CsNO3 | Ba(NO3)2 | Hf(NO3)4 | Ta | W | Re | Os | Ir | Au(NO3)3 | Hg2(NO3)2 Hg(NO3)2 |
Tl(NO3)3 |
Pb(NO3)2 | Bi(NO3)3 BiO(NO3) |
Po(NO3)4 | At | Rn | ||
Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Nh | Fl | Mc | Lv | Ts | Og | |||
↓ | |||||||||||||||||
La(NO3)3 | Ce(NO3)3 Ce(NO3)4 |
Pr(NO3)3 | Nd(NO3)3 | Pm(NO3)3 | Sm(NO3)3 | Eu(NO3)3 | Gd(NO3)3 | Tb(NO3)3 | Dy(NO3)3 | Ho(NO3)3 | Er(NO3)3 | Tm(NO3)3 | Yb(NO3)3 | Lu(NO3)3 | |||
Ac(NO3)3 | Th(NO3)4 | UO2(NO3)2 | Np(NO3)4 | Pu(NO3)4 | Am(NO3)3 | Cm(NO3)3 | Bk | Cf | Es | Fm | Md | No | Lr |
- Manganese(II) compounds
- Nitrates
- Inorganic compound stubs