Browse history interactively

Page 1

Page 1Revision 1

Page 2

Page 2Revision 2

← Previous editContent deleted Content addedVisualWikitext

Revision as of 20:22, 23 August 2011 editZéroBot (talk | contribs)704,777 editsm r2.7.1) (robot Adding: no:Jernsulfid← Previous edit		Latest revision as of 17:20, 25 October 2023 edit undoSadisjayallen (talk | contribs)4 editsm Minor grammatical correction.
(122 intermediate revisions by 85 users not shown)
Line 1:		Line 1:
			{{Redirect|FeS||FES (disambiguation)}}
	{{chembox
			{{Chembox
	| verifiedrevid = 402180648
			| Watchedfields = changed
	| Name = Iron(II) sulfide
			| verifiedrevid = 446376772
	| ImageFile = Ferrous sulfide.jpg
			| Name = Iron(II) sulfide
			| ImageFile = Strukturformel Nickelarsenid.png
	| ImageSize = 250px		| ImageSize = 250px
	| ImageName = Sample of iron(II) sulfide		| ImageName2 = Sample of iron(II) sulfide
			| ImageFile2 = Ferrous sulfide.jpg
	| ImageFile1 = Iron(II)-sulfide-unit-cell-3D-balls.png
	<!-- | ImageSize1 = 150px -->		<!-- | ImageSize1 = 150px -->
	| ImageName1 = Ball-and-stick model of FeS's unit cell		| ImageName1 = Ball-and-stick model of FeS's unit cell
	| OtherNames = Iron sulfide, ferrous sulfide, black iron sulfide		| OtherNames = Iron sulfide, ferrous sulfide, black iron sulfide, protosulphuret of iron
	| Section1 = {{Chembox Identifiers		|Section1={{Chembox Identifiers
	| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}		| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
	| ChemSpiderID = 8466211		| ChemSpiderID = 8466211
	| InChI = 1/Fe.S/q+2;-2		| InChI = 1/Fe.S/q+2;-2
Line 19:		Line 21:
	| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}		| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
	| StdInChIKey = GNVXPFBEZCSHQZ-UHFFFAOYSA-N		| StdInChIKey = GNVXPFBEZCSHQZ-UHFFFAOYSA-N
	| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
	| ChemSpiderID = 8466211
	| CASNo = 1317-37-9		| CASNo = 1317-37-9
	| CASNo_Ref = {{cascite|correct|CAS}}		| CASNo_Ref = {{cascite|correct|CAS}}
			| UNII_Ref = {{fdacite|correct|FDA}}
	| PubChem = 10290742
			| UNII = TH5J4TUX6S
	}}
			| PubChem = 10290742
	| Section2 = {{Chembox Properties
			}}
	| Formula = FeS
			|Section2={{Chembox Properties
	| MolarMass = 87.910 g/mol
			| Formula = FeS
	| Density = 4.84 g/cm<sup>3</sup>
			| MolarMass = 87.910 g/mol
	| Solubility = negligible (insoluble)
			| Density = 4.84 g/cm<sup>3</sup>
	| SolubleOther = reacts in ]
			| Solubility = negligible (insoluble)
	| MeltingPt = 1194 °C
			| SolubleOther = reacts in ]
	| BoilingPt =
			| MeltingPtC = 1194
	| Appearance = black solid
			| MeltingPt_notes =
	}}
			| BoilingPt =
	| Section3 = {{Chembox Hazards
			| Appearance = Grey, sometimes in lumps or powder
	| ExternalMSDS =
			| MagSus = +1074·10<sup>−6</sup> cm<sup>3</sup>/mol
	| EUIndex = Not listed
			}}
	| MainHazards = can be pyrophoric
			|Section3={{Chembox Hazards
	| RPhrases =
	| SPhrases =		| ExternalSDS =
			| MainHazards = Source of ], can be pyrophoric
	| FlashPt =
			| NFPA-F = 2
	| Autoignition = variable
			| NFPA-H = 1
	}}
			| NFPA-R = 2
	| Section8 = {{Chembox Related
			| FlashPt =
	| OtherCpds = ]<br/>]
			| AutoignitionPt = variable
	}}
			}}
			|Section8={{Chembox Related
			| OtherAnions = ]<br>]<br>]
			| OtherCations = ]<br>]
			| OtherFunction = ]
			| OtherFunction_label = ] ]s
			| OtherCompounds =
			}}
	}}		}}
	'''Iron(II) sulfide''' or '''ferrous sulfide''' (Br.E. '''sulphide''') is a ] with the ] {{chem|]]}}. In practice, iron sulfides are often ]. Powdered iron sulfide is ] (i.e. will ignite spontaneously in air).		'''Iron(II) sulfide''' or '''ferrous sulfide''' (Br.E. '''sulphide''') is one of a family of ]s and ]s with the approximate ] {{chem|]]}}. Iron sulfides are often iron-deficient ]. All are black, water-insoluble solids.
			==Preparation and structure==
	==Forms of iron sulfide==
			FeS can be obtained by the heating of iron and ]:<ref>H. Lux "Iron (II) Sulfide" in Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 1502.</ref>
	"Iron sulfide" exists in several distinct forms, which differ in the ] and properties:<ref>{{Citation|first1=Vaughan|last1=D.|first2=Craig|last2=J.| year=1978|title=Mineral chemistry of metal sulfides|publisher=Cambridge University Press|isbn=0-521-21489-0}}</ref>
			:Fe + S → FeS
	*], Fe<sub>1-x</sub>S, a mineral, which displays ] and crystallizes in monoclinic system. Iron metal shows ]; iron sulfides do not.
	*], FeS, a stoichiometric compound that adopts hexagonal symmetry.
	*], Fe<sub>1+x</sub>S the least stable form of iron sulfide; mackinawite has a layered structure.
	*] and ], which are ] minerals, have the formula FeS<sub>2</sub>.
	*] (Fe<sub>3</sub>S<sub>4</sub>) a ferromagnetic species akin to ] (Fe<sub>3</sub>O<sub>4</sub>).
			FeS adopts the ] structure, featuring ] Fe centers and trigonal prismatic sulfide sites.
	==Chemical reactions==
	Iron sulfide reacts with ], releasing the pungent and very toxic ]
			==Reactions==
			Iron sulfide reacts with ], releasing ]:<ref></ref>
	:FeS + 2 HCl → FeCl<sub>2</sub> + H<sub>2</sub>S		:FeS + 2 HCl → FeCl<sub>2</sub> + H<sub>2</sub>S
	FeS can be obtained by the heating of iron and ]:
	:Fe + S → FeS
			:FeS + H<sub>2</sub>SO<sub>4</sub> → FeSO<sub>4</sub> + H<sub>2</sub>S
	==Biology and biochemistry==
	]
	As organic matter decays under low-oxygen (or ]) conditions such as in swamps or ] of lakes and oceans, ] will use the ]s present in the water to oxidize the organic matter, producing ] as waste. Some of the hydrogen sulfide will react with metal ions in the water to produce metal sulfides, which are not water soluble. These metal sulfides, such as iron(II) sulfide, are often black or brown, leading to the color of sludge.
			In moist air, iron sulfides oxidize to hydrated ].
	Pyrrotite is a waste product of the '']'' bacteria, a sulfate reducing bacteria.
			==Biology and biogeochemistry==
	When eggs are cooked for a long time, the ]'s surface may turn green. This is due to iron(II) sulfide which forms as iron from the yolk meets hydrogen sulfide released from the egg white by the heat.<ref>{{citation|url=http://chestofbooks.com/food/science/Experimental-Cookery/The-Formation-Of-Ferrous-Sulfide-In-Cooked-Eggs.html|chapter=The formation of ferrous sulfide in cooked eggs|title=Experimental cookery from the chemical and physical standpoint|author=Belle Lowe|year=1937|publisher=John Wiley & Sons}}</ref> This reaction occurs more rapidly in older eggs as the whites are more alkaline.<ref>{{citation|||title=]|author=]|year=2004|publisher=Hodder and Stoughton}}</ref>
			], showing the distinctive green coating on the yolk caused by the presence of iron(II) sulfide]]
			Iron sulfides occur widely in nature in the form of ]s.
			As organic matter decays under low-oxygen (or ]) conditions such as in swamps or ] of lakes and oceans, ] reduce various ]s present in the water, producing ]. Some of the hydrogen sulfide will react with metal ions in the water or solid to produce iron or metal sulfides, which are not water-soluble. These metal sulfides, such as iron(II) sulfide, are often black or brown, leading to the color of sludge.
			] is a waste product of the '']'' bacteria, a sulfate reducing bacteria.
			When eggs are cooked for a long time, the ]'s surface may turn green. This color change is due to iron(II) sulfide, which forms as iron from the yolk reacts with hydrogen sulfide released from the egg white by the heat.<ref>{{citation|url=http://chestofbooks.com/food/science/Experimental-Cookery/The-Formation-Of-Ferrous-Sulfide-In-Cooked-Eggs.html|chapter=The formation of ferrous sulfide in cooked eggs|title=Experimental cookery from the chemical and physical standpoint|author=Belle Lowe|year=1937|publisher=John Wiley & Sons}}</ref> This reaction occurs more rapidly in older eggs as the whites are more alkaline.<ref>{{citation|title=]|author=]|year=2004|publisher=Hodder and Stoughton}}</ref>
	The presence of ferrous sulfide as a visible black ] in the ] ] can be used to distinguish between ] that produce the ] enzyme ] and those that do not. Peptone iron agar contains the ] ] and a ], ]. The degradation of cysteine releases ] gas that reacts with the ] ] to produce ferrous sulfide.		The presence of ferrous sulfide as a visible black ] in the ] ] can be used to distinguish between ] that produce the ] enzyme ] and those that do not. Peptone iron agar contains the ] ] and a ], ]. The degradation of cysteine releases ] gas that reacts with the ] ] to produce ferrous sulfide.
Line 76:		Line 86:
	==See also==		==See also==
	* ]		* ]
			* ]
			* ]
	* ]		* ]
Line 82:		Line 94:
	{{Iron compounds}}		{{Iron compounds}}
			{{Sulfides}}
	]		]
	]
	]		]
	]		]
	]		]
	]
	]
	]
	]
	]
	]
	]
	]
	]
	]
	]
	]
	]
	]
	]
	]