Magnesium sulfide 2202860 221385753 2008-06-24T08:25:05Z Sesshomaru 3753540 [[WP:D#Links to disambiguation pages]] {{Redirect|MgS|other uses|MGS (disambiguation)}} {{Chembox new | Name = Magnesium sulfide | ImageFile = Magnesium-sulfide-3D-ionic.png <!-- | ImageSize = 200px --> | ImageName = Magnesium sulfide crystal structure | OtherNames = mag sulfide (jargon)<br />niningerite | Section1 = {{Chembox Identifiers | CASNo = 12032-36-9 }} | Section2 = {{Chembox Properties | Formula = MgS | MolarMass = 56.5 g/mol | Density = 2680 kg/m<sup>3</sup> | Solvent = other solvents | SolubleOther = decomposes | MeltingPt = >2000 °C | BoilingPt =}} }} '''Magnesium sulfide''' is the [[chemical compound]] with the formula MgS. It is a colorless crystalline material but often is encountered in an impure form that is brown and non-crystalline powder. ==Preparation== MgS forms by the reaction of [[sulfur]] or [[hydrogen sulfide]] with [[magnesium]]. In the BOS steelmaking process, sulfur must be removed, and is the first element to be. Sulfur is removed from the impure blast furnace iron by the addition of several hundred kilograms of magnesium powder by a lance. The magnesium reduces the sulfur to form magnesium sulfide (MgS). The ionic equations are: :Mg → Mg<sup>2+</sup> + 2 e<sup>-</sup> :S + 2e<sup>-</sup> → S<sup>2-</sup><ref>Chemical storylines, Salters advanced chemistry, heinemann educational publishers, 2000</ref> ==General properties== MgS crystallizes in the rock salt structure, although the zinc blende structure might be anticipated.<ref>Guntert, O. J.; Faessler, A. "Lattice constants of the alkaline earth sulfides MgS, CaS, SrS, and BaS" Zeitschrift für Kristallographie, Kristallgeometrie, Kristallphysik, Kristallchemie (1956), volume 107, pages 357-61.</ref> The chemical properties of MgS resemble those of related ionic sulfides such as those of Na, Ba, Ca: 1) MgS reacts readily with oxygen to form the corresponding sulfate, [[magnesium sulfate]]. 2) MgS reacts with water to give hydrogen sulfide and [[magnesium hydroxide]]. ==Applications== *MgS is a wide band-gap direct semiconductor of interest as a blue-green emitter, a property that has been known since the early 1900's.<ref>Tiede, E. "Reindarstellung von Magnesiumsulfid und seine Phosphorescenz. I (Preparation of pure magnesium sulfide and its phosphorescence. I)" Berichte der Deutschen Chemischen Gesellschaft (1916), volume 49, pages 1745-9.</ref> *During the purification of iron, sulfur must be extracted. To achieve this, a "lance" is introduced into the molten metal, and powdered magnesium is poured in. In a violent [[exothermic]] reaction ensues, resulting in MgS, which is then raked off as a component of the [[slag]].<ref>Irons, G. A.; Guthrie, R. I. L. "Kinetic aspects of magnesium desulfurization of blast furnace iron" Ironmaking and Steelmaking (1981), volume 8, pp.114-21.</ref> *MgS is claimed to slow labor (childbirth). ==Safety== MgS evolves [[hydrogen sulfide]] upon contact with moisture. ==References== <references/> [[Category:Sulfides]] [[Category:Magnesium compounds]] {{inorganic-compound-stub}} [[ar:كبريتيد مغنزيوم]] [[ca:Sulfur de magnesi]] [[ja:硫化マグネシウム]] [[sr:Магнезијум сулфид]] [[zh:硫化镁]]