Manganese(II) nitrate
Names | |
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Systematic IUPAC name
Manganese(II) nitrate | |
Other names
Manganese dinitrate | |
Identifiers | |
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3D model (JSmol) |
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ChemSpider | |
ECHA InfoCard | 100.030.741 |
EC Number | 233-828-8 |
PubChem CID |
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UNII | |
UN number | 2724 |
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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 |
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). | |
Infobox references | |
Manganese(II) nitrate are the inorganic compounds with formula Mn(NO3)2(H2O)n. 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, reactions, uses
Manganese(II) nitrate is prepared by dissolving manganese(II) oxide in nitric acid:
- MnO + 2 HNO3 → Mn(NO3)2 + H2O
It can also be prepared from manganese dioxide and nitrogen dioxide:[1]
- MnO2 + 2 NO2 → Mn(NO3)2
On heating to 300 °C, aqueous solutions of manganese(II) nitrate thermally decompose to form MnO2 and NO2.
Manganese(II) nitrate is the precursor to manganese 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 2 3 Arno H. Reidies, "Manganese Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, 2002, Wiley-VCH, Weinheim. doi:10.1002/14356007.a16_123
Salts and covalent derivatives of the nitrate ion | |||||||||||||||||||
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HNO3 | He | ||||||||||||||||||
LiNO3 | Be(NO3)2 | B(NO 3)− 4 |
C | NO− 3, NH4NO3 |
O | 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)3, Fe(NO3)2 |
Co(NO3)2, Co(NO3)3 |
Ni(NO3)2 | Cu(NO3)2 | Zn(NO3)2 | Ga(NO3)3 | Ge | As | Se | Br | Kr | ||
RbNO3 | Sr(NO3)2 | Y | Zr(NO3)4 | Nb | Mo | Tc | Ru | Rh | Pd(NO3)2 | AgNO3 | Cd(NO3)2 | In | Sn | Sb(NO3)3 | Te | I | Xe(NO3)2 | ||
CsNO3 | Ba(NO3)2 | Hf | Ta | W | Re | Os | Ir | Pt | Au | Hg2(NO3)2, Hg(NO3)2 |
Tl(NO3)3, TlNO3 |
Pb(NO3)2 | Bi(NO3)3 BiO(NO3) |
Po | At | Rn | |||
FrNO3 | Ra(NO3)2 | 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 | Nd | Pm | Sm | Eu(NO3)3 | Gd(NO3)3 | Tb | Dy | Ho | Er | Tm | Yb | Lu | |||||
Ac(NO3)3 | Th(NO3)4 | Pa | UO2(NO3)2 | Np | Pu | Am | Cm | Bk | Cf | Es | Fm | Md | No | Lr |