Manganese(II) carbonate

Structure and production

180px|thumb|left|Manganese carbonate crystallizes in the same dense motif as [[calcium carbonate]]. Color code: red = O, green = Mn. MnCO3 adopts a structure like calcite, consisting of manganese(II) ions in an octahedral coordination geometry.

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.

Reactions and uses

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 → MnO1.88 + CO2 This method is sometimes employed in the production of manganese dioxide, which is used in dry-cell batteries and for ferrites.

Manganese carbonate is widely used as an additive within plant fertilizers. It is also used in multivitamins, in ceramics as a glaze colorant and flux, and in concrete stains.

Toxicity

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

References

References

1. {{Sigma-Aldrich
2. "Manganese(II) carbonate".
3. Arno H. Reidies. (2007). "Manganese Compounds". Wiley-VCH.
4. Pertlik, F.. (1986). "Structures of hydrothermally synthesized cobalt(II) carbonate and nickel(II) carbonate". Acta Crystallographica Section C.
5. [http://www.stainedfloor.com/Manganese_Recipes.html "How To Stain Concrete with Manganese"]