Contents

Manganese(II) nitrate

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
ECHA InfoCard	100.030.741
EC Number	233-828-8
PubChem CID	61511
UNII	I389H78514 Y 03M0G68R5F (tetrahydrate) Y W5UG18WBJA (hexahydrate) Y
UN number	2724
CompTox Dashboard (EPA)	DTXSID90890659
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

Chemical compound

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[edit]

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[edit]

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 electrontoMnO₂ (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[edit]