Editing Magnesium (section)

==Safety precautions==
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[[File:Burning Magnesium Block!.ogv|thumb|right|Magnesium block heated with blow torch to self-combustion, emitting intense white light|start=2:40|thumbtime=4:00]]

Magnesium metal and its alloys can be explosive hazards; they are highly flammable in their pure form when molten or in powder or ribbon form. Burning or molten magnesium reacts violently with water. When working with powdered magnesium, [[safety glasses]] with [[eye protection]] and UV filters (such as welders use) are employed because burning magnesium produces [[ultraviolet]] light that can permanently damage the [[retina]] of a human eye.<ref>{{cite web |url=http://www.edu.gov.mb.ca/k12/docs/support/scisafe/chapter8.html |title=Science Safety: Chapter 8 |publisher=Government of Manitoba |access-date=21 August 2007}}</ref>

Magnesium is capable of reducing [[water (molecule)|water]] and releasing highly flammable [[hydrogen]] gas:<ref>{{cite web| url=http://www.webelements.com/webelements/elements/text/Mg/chem.html| title=Chemistry : Periodic Table : magnesium : chemical reaction data| access-date=26 June 2006| publisher=webelements.com}}</ref>

:Mg(s) + 2 {{chem|H|2|O}}(l) → [[Magnesium hydroxide|{{chem|Mg(OH)|2}}]](s) + {{chem|H|2}}(g)

Therefore, water cannot extinguish magnesium fires. The hydrogen gas produced intensifies the fire. Dry sand is an effective smothering agent, but only on relatively level and flat surfaces.

Magnesium reacts with [[carbon dioxide]] exothermically to form [[magnesium oxide]] and [[carbon]]:<ref name=CO2>{{multiref|{{cite web |url=http://chemed.chem.purdue.edu/demos/main_pages/9.8.html |title=The Reaction Between Magnesium and CO<sub>2</sub>|publisher=Purdue University|access-date=2016-06-15}}|{{cite video|first1=David|last1=Whisnant|first2=David|last2=Phillips|first3=Kelly|last3=Houston&nbsp;Jetzer|orig-date=6 Mar 2012|year=2022|title=Reaction of magnesium with carbon dioxide|url=https://www.chemedx.org/video/reaction-magnesium-carbon-dioxide|type=web video|publisher=American Chemical Society, Division of Chemical Education|via=ChemEdX}}}}</ref>

:2 Mg(s) + {{chem|CO|2}}(g) → 2 MgO(s) + C(s)

Hence, carbon dioxide fuels rather than extinguishes magnesium fires.

Burning magnesium can be quenched by using a [[Fire extinguisher#Class D dry powder and other agents for metal fires|Class D]] dry chemical fire extinguisher, or by covering the fire with [[sand]] or magnesium foundry flux to remove its air source.<ref>{{cite book |last=Cote |first=Arthur E. |date=2003 |title=Operation of Fire Protection Systems |publisher= Jones & Bartlett Learning |page=667 |isbn= 978-0877655848}}</ref>