Manganese(II) carbonate

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Manganese(II) carbonate
Calcium-carbonate-xtal-3D-SF.png
Manganese (II) Carbonate.jpg
Names
IUPAC name
Manganese(II) carbonate
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.009.040
EC Number 209-942-9
UNII
Properties
MnCO3
Appearance White to faint pink solid
Density 3.12 g/cm3
Melting point 200–300 °C (392–572 °F; 473–573 K)
decomposes[1][2]
negligible
2.24 x 10−11
Solubility soluble in dilute acid, CO2
insoluble in alcohol, ammonia
+11,400·10−6 cm3/mol
1.597 (20 °C, 589 nm)
Structure
hexagonal-rhombohedral
Thermochemistry
94.8 J/mol·K[2]
109.5 J/mol·K[2]
-881.7 kJ/mol[2]
-811.4 kJ/mol[2]
Hazards
Flash point Non-flammable
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Manganese carbonate is a compound with the chemical formula MnCO3. Manganese carbonate occurs naturally as the mineral rhodochrosite but it is typically produced industrially. It is a pale pink, water-insoluble solid. Approximately 20,000 metric tonnes were produced in 2005.[3]

Structure and production[edit]

MnCO3 adopts a structure like calcite, consisting of manganese(II) ions in an octahedral coordination geometry.[4]

Treatment of aqueous solutions of manganese(II) nitrate with ammonia and carbon dioxide leads to precipitation of this faintly pink solid. The side product, ammonium nitrate is used as fertilizer.

Pink rhodochrosite, the mineral form of MnCO3, is of practical value as well as sought by collectors.

Reactions and uses[edit]

The carbonate is insoluble in water but, like most carbonates, hydrolyses upon treatment with acids to give water-soluble salts.

Manganese carbonate decomposes with release of carbon dioxide, i.e. calcining, at 200 °C to give MnO1.88:

MnCO3 + 0.44 O2 → MnO1.8 + CO2

This method is sometimes employed in the production of manganese dioxide, which is used in dry-cell batteries and for ferrites.[3]

Manganese carbonate is widely used as an additive to plant fertilizers to cure manganese deficient crops. It is also used in health foods, in ceramics as a glaze colorant and flux, and in concrete stains.[5]

It is used in medicine as a hematinic.

Toxicity[edit]

Manganese poisoning, also known as manganism, may be caused by long-term exposure to manganese dust or fumes.

See also[edit]

References[edit]

  1. ^ Sigma-Aldrich Co., Manganese(II) carbonate. Retrieved on 2014-05-06.
  2. ^ a b c d e http://chemister.ru/Database/properties-en.php?dbid=1&id=3854
  3. ^ a b Arno H. Reidies (2007). "Manganese Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a16_123. 
  4. ^ Pertlik, F. (1986). "Structures of hydrothermally synthesized cobalt(II) carbonate and nickel(II) carbonate". Acta Crystallographica Section C. 42: 4–5. doi:10.1107/S0108270186097524. 
  5. ^ "How To Stain Concrete with Manganese"


Carbonates
H2CO3 He
Li2CO3,
LiHCO3
BeCO3 B C (NH4)2CO3,
NH4HCO3
O F Ne
Na2CO3,
NaHCO3,
Na3H(CO3)2
MgCO3,
Mg(HCO3)2
Al2(CO3)3 Si P S Cl Ar
K2CO3,
KHCO3
CaCO3,
Ca(HCO3)2
Sc Ti V Cr MnCO3 FeCO3 CoCO3 NiCO3 CuCO3 ZnCO3 Ga Ge As Se Br Kr
Rb2CO3 SrCO3 Y Zr Nb Mo Tc Ru Rh Pd Ag2CO3 CdCO3 In Sn Sb Te I Xe
Cs2CO3,
CsHCO3
BaCO3   Hf Ta W Re Os Ir Pt Au Hg Tl2CO3 PbCO3 (BiO)2CO3 Po At Rn
Fr Ra   Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og
La2(CO3)3 Ce2(CO3)3 Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
Ac Th Pa UO2CO3 Np Pu Am Cm Bk Cf Es Fm Md No Lr