Manganese(II) carbonate

<h2 id="structure-and-production">Structure and production</h2>

<p>MnCO3 adopts a structure like <a href="/facts/Calcite/gKMHYQJo">calcite</a>, consisting of manganese(II) ions in an <a href="/facts/Octahedral_coordination_geometry/bNXLVvks">octahedral coordination geometry</a>.<a class="footnote-ref" id="fnref:2" href="#fn:2"><sup>2</sup></a>
</p><p>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.  
</p>

<h2 id="reactions-and-uses">Reactions and uses</h2>
<p>The carbonate is insoluble in water but, like most carbonates, hydrolyses upon treatment with acids to give water-soluble salts.
</p><p>Manganese carbonate decomposes with release of <a href="/facts/Carbon_dioxide/xGzpppEp">carbon dioxide</a>, i.e. <a href="/facts/Calcining/hghqlHwo">calcining</a>, at 200 °C to give MnO1.88:
</p>
MnCO3 + 0.44 O2  →   MnO1.88  +  CO2
<p>This method is sometimes employed in the production of <a href="/facts/Manganese_dioxide/HRwgXlUe">manganese dioxide</a>, which is used in dry-cell batteries and for <a href="/facts/Ferrite_(magnet)/kBTM7Dqk">ferrites</a>.<a class="footnote-ref" id="fnref:3" href="#fn:3"><sup>3</sup></a>
</p><p>Manganese carbonate is widely used as an additive within plant fertilizers.  It is also used in <a href="/facts/Multivitamin/IfC33Tm9">multivitamins</a>, in ceramics as a <a href="/facts/Ceramic_glaze/eWJqJTYk">glaze</a> <a href="/facts/Ceramic_colorants/YHhBIn7Y">colorant</a> and flux, and in <a href="/facts/Decorative_concrete/vI0Ecx69">concrete stains</a>.<a class="footnote-ref" id="fnref:4" href="#fn:4"><sup>4</sup></a>
</p>
<h2 id="toxicity">Toxicity</h2>
<p>Manganese poisoning, also known as <a href="/facts/Manganism/G4AtRyFu">manganism</a>, may be caused by long-term exposure to manganese dust or fumes.
</p>
<h2 id="see-also">See also</h2>
<ul><li><a href="/facts/Manganese_deficiency_(medicine)/IjhWYy8z">Manganese deficiency (medicine)</a></li></ul>

<h2 id="references">References</h2>

<ol>
<li id="fn:1"><p>Arno H. Reidies (2007). "Manganese Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a16_123. ISBN 978-3527306732. <a href="978-3527306732" target="_blank">978-3527306732</a> <a href="#fnref:1" class="footnote-back-ref">↩</a></p></li>
<li id="fn:2"><p>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. <a href="/wiki/Doi_(identifier)" target="_blank">/wiki/Doi_(identifier)</a> <a href="#fnref:2" class="footnote-back-ref">↩</a></p></li>
<li id="fn:3"><p>Arno H. Reidies (2007). "Manganese Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a16_123. ISBN 978-3527306732. <a href="978-3527306732" target="_blank">978-3527306732</a> <a href="#fnref:3" class="footnote-back-ref">↩</a></p></li>
<li id="fn:4"><p>"How To Stain Concrete with Manganese" <a href="http://www.stainedfloor.com/Manganese_Recipes.html" target="_blank">http://www.stainedfloor.com/Manganese_Recipes.html</a> <a href="#fnref:4" class="footnote-back-ref">↩</a></p></li>
</ol>

Manganese(II) carbonate open-in-new

Manganese(II) carbonate