Manganese(II) nitrate

Names
Systematic IUPAC name

Manganese(II) nitrate

Other names

Manganese dinitrate

Identifiers

CAS Number

* 10377-66-9 Y
* 20694-39-7 (tetrahydrate) Y
* 17141-63-8 (hexahydrate) Y

3D model (JSmol)

* Interactive image

ChemSpider |

* 55431 N

EC Number |

* 233-828-8

PubChem CID

* 61511

UNII |

* I389H78514 Y
* 03M0G68R5F (tetrahydrate) Y
* W5UG18WBJA (hexahydrate) Y

UN number | 2724

InChI

* 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

SMILES

* [N+](=O)([O-])[O-].[N+](=O)([O-])[O-].[Mn+2]

Properties

Chemical formula

| 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)

Solubility in water

| 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).

N verify (what is YN ?)
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] 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

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

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

1. ↑ 1.0 1.1 1.2 Reidies, Arno H. (2000). "Ullmann's Encyclopedia of Industrial Chemistry". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a16_123.
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.
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. ↑ H. Lux (1963). "Manganeses(II) Oxide". in G. Brauer. Handbook of Preparative Inorganic Chemistry, 2nd Ed.. 2pages=1455. NY, NY: Academic Press.

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Manganese compounds

* MnO
* Mn3O4
* Mn5O8
* MnS
* MnS2
* MnSO4
* MnSe2
* MnSe
* MnTe
* Mn(NO3)2
* MnCO3
* MnCl2
* MnCl3
* MnCl4
* MnF2
* MnBr2
* MnI2
* MnTiO3
* MnMoO4
* Mn(CH3COO)2
* Mn2O3
* MnF3
* K6Mn2O6
* MnO2
* Mn(OH)2
* MnO3
* K3MnO4
* MnF4
* Na2MnO4
* K2MnO4
* Mn2O7
* NaMnO4
* KMnO4
* NH4MnO4
* AgMnO4
* Ca(MnO4)2
* Ba(MnO4)2
* MnH(CO)5
* Mn2(CO)10

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Salts and covalent derivatives of the nitrate ion

HNO3 |  |  |  | He

|
|
|
|

LiNO3 | Be(NO3)2 | B(NO3)−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(NO3)3 | 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(NO3)3 | Pm  | Sm  | Eu(NO3)3 | Gd(NO3)3 | Tb(NO3)3 | 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

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