词条 | Iron(II,III) sulfide |
释义 |
| verifiedrevid = 427821486 |ImageFile1= |IUPACName= |OtherNames=Ferrous-ferric sulfide, greigite |Section1 = {{Chembox Identifiers | PubChem = 72720442 | ChemSpiderID = 34999896 | ChEBI = 86238 | CASNo = 12063-39-7 | StdInChI=1S/3Fe.4S/q+2;2*+3;4*-2 | StdInChIKey = UHUWQCGPGPPDDT-UHFFFAOYSA-N | SMILES = [S-2].[S-2].[S-2].[S-2].[Fe+2].[Fe+3].[Fe+3] |Section2 = {{Chembox Properties | Formula=FeS·Fe2S3 | MolarMass= 295.805 | Appearance= Bluish-black, pinkish | Density= 4.049 g/cm3 | MeltingPt= | BoilingPt= | Solubility= }} Iron(II,III) sulfide is a blue-black (sometimes pinkish) chemical compound of iron and sulfur with formula Fe3S4 or FeS·Fe2S3, which is much similar to iron(II,III) oxide. It occurs naturally as the sulfide mineral greigite and is magnetic. It is a bio-mineral produced by and found in magnetotactic bacteria. It is a mixed valence compound, featuring both Fe2+ and Fe3+ centers, in 1:2 ratio. Crystal structureThe crystallographic unit cell is cubic, with space group Fd3m. The S anions form a cubic close-packed lattice, and the Fe cations occupy both tetrahedral and octahedral sites.[1][2] {{Gallery|title=Crystal structure of iron(II,III) sulfide projected along the [110] direction |width=250 |align=center |File:Greigite structure 110 SFe4 tetrahedra.png|Emphasis on the SFe4 tetrahedra. |File:Greigite structure 110 FeS4 tetrahedra.png|Emphasis on the FeS4 tetrahedra |File:Greigite structure 110 FeS6 octahedra.png|Emphasis on the FeS6 octahedra }} Magnetic and electronic propertiesLike the related oxide magnetite (Fe3O4), iron(II,III) sulfide is ferrimagnetic, with the spin magnetic moments of the Fe cations in the tetrahedral sites oriented in the opposite direction as those in the octahedral sites, and a net magnetization. Both metal sites have high spin quantum numbers. The electronic structure of greigite is that of a half metal.[3][4] References1. ^{{cite book|editor1=Anthony, John W. |editor2=Bideaux, Richard A. |editor3=Bladh, Kenneth W. |editor4=Nichols, Monte C. |title= Handbook of Mineralogy|publisher= Mineralogical Society of America|place= Chantilly, VA, US|chapter-url=http://rruff.geo.arizona.edu/doclib/hom/greigite.pdf |chapter=Greigite |accessdate=December 5, 2011|isbn=978-0962209703 |volume=I (Elements, Sulfides, Sulfosalts)|year=1990}} 2. ^Vaughan, D. J.; Craig, J. R. “Mineral Chemistry of Metal Sulfides" Cambridge University Press, Cambridge: 1978. {{ISBN|0-521-21489-0}}. 3. ^{{cite journal|last1=Devey|first1=Anthony|first2=R.|last2=Grau-Crespo|first3=N.H.|last3=De Leeuw|title=Electronic and magnetic structure of Fe3S4: GGA+U investigation|journal=Physical Review B|year=2009|volume=79|pages=195126| doi=10.1103/PhysRevB.79.195126|issue=19|bibcode = 2009PhRvB..79s5126D }} 4. ^{{cite journal| title=The Curie temperature and magnetic exchange energy in half-metallic greigite Fe3S4|doi=10.1088/0031-8949/83/04/045702|year=2011|volume=83|pages=045702| last1=Wang| first1=Jun| last2=Cao| first2=Shi-He| last3=Wu| first3=Wei| last4=Zhao| first4=Guo-Meng| journal=Physica Scripta| issue=4|bibcode = 2011PhyS...83d5702W }} Further reading
2 : Iron(Ⅱ,Ⅲ) compounds|Sulfides |
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