Magnesium peroxide
<p >Magnesium peroxide is a stable <a href="http://en.wikipedia.org/wiki/Oxygen" title="Oxygen" >oxygen</a> releasing compound, which is used in <a href="http://en.wikipedia.org/wiki/Agricultural" title="Agricultural" class="mw-redirect" >agricultural</a> and<a href="http://en.wikipedia.org/wiki/Natural_environment" title="Natural environment" >environmental</a> industries. It is used to reduce contaminant levels in <a href="http://en.wikipedia.org/wiki/Groundwater" title="Groundwater" >groundwater</a>. Magnesium peroxide is used in the <a href="http://en.wikipedia.org/wiki/Bioremediation" title="Bioremediation" >bioremediation</a> of contaminated <a href="http://en.wikipedia.org/wiki/Soil" title="Soil" >soil</a> and can improve the soil quality for <a href="http://en.wikipedia.org/wiki/Plant" title="Plant" >plant</a> growth and <a href="http://en.wikipedia.org/wiki/Metabolism" title="Metabolism" >metabolism</a>. It also used in the <a href="http://en.wikipedia.org/wiki/Aquaculture" title="Aquaculture" >aquaculture</a> industry for bioremediation.
For sanitation purposes magnesium peroxide is often used as a source of oxygen for <a href="http://en.wikipedia.org/wiki/Aerobic_organisms" title="Aerobic organisms" class="mw-redirect" >aerobic organisms</a> in the treatment and disposal of biological waste. </p>
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Since the breakdown of <a href="http://en.wikipedia.org/wiki/Hydrocarbons" title="Hydrocarbons" class="mw-redirect" >hydrocarbons</a> in soil is usually quicker in aerobic conditions, MgO<sub >2</sub> can also added to compost piles or in soil to speed up the microbe activities and to reduce the odors produced in the process <sup >[2]</sup>.<sup id="cite_ref-2" class="reference" ><a href="http://en.wikipedia.org/wiki/Magnesium_peroxide#cite_note-2" >[3]</a></sup> Since this process involves adding chemicals into the ground, it is only done in sites where the ground water has already been contaminated.<sup id="cite_ref-3" class="reference" ><a href="http://en.wikipedia.org/wiki/Magnesium_peroxide#cite_note-3" >[4]</a></sup></p>
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In certain circumstances MgO<sub >2</sub> has also been shown to inhibit growth of bacteria. In particular, the growth of <a href="http://en.wikipedia.org/wiki/Sulfate-reducing_bacteria" title="Sulfate-reducing bacteria" >sulfate-reducing bacteria</a> can be inhibited in an environment containing magnesium peroxide. While the oxygen slowly dissociates, it is theorized that it may then act to displace the sulfate that normally acts as the terminal electron acceptor in their electron transport chain.<sup id="cite_ref-4" class="reference" ><a href="http://en.wikipedia.org/wiki/Magnesium_peroxide#cite_note-4" >[5]</a></sup>
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<h2 >Toxicity</h2>
<p >Magnesium peroxide is an irritant that can cause redness, itching, swelling, and may burn the skin and eyes on contact.</p>
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Inhalation can also cause irritation to the lungs, nose, and throat, as well as causing coughing. Long term exposure may lead to lung damage, shortness of breath, and tightening of the chest. Ingestion of MgO<sub >2</sub> can cause numerous adverse effects including: bloating, belching, abdominal pain, irritation of the mouth and throat, nausea, vomiting, and diarrhea.<sup id="cite_ref-5" class="reference" ><a href="http://en.wikipedia.org/wiki/Magnesium_peroxide#cite_note-5" >[6]</a></sup><sup id="cite_ref-6" class="reference" ><a href="http://en.wikipedia.org/wiki/Magnesium_peroxide#cite_note-6" >[7]</a></sup></p>
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Environmentally, Magnesium peroxide is not a naturally occurring compound and is not known to persist in the environment for prolonged times, in its complete state, or to bio-accumulate. The natural degradation of MgO<sub >2</sub> leads to Magnesium hydroxide, O<sub >2</sub>, and H<sub >2</sub>O. If spilled MgO<sub >2</sub> should be contained and isolated from any waterways, sewer drains, and it should be isolated from combustible materials or chemicals including paper, cloth, and wood<sup >[6]</sup>.</p>