| Revision as of 10:43, 16 February 2012 editBeetstra (talk | contribs)Edit filter managers, Administrators172,031 edits Saving copy of the {{chembox}} taken from revid 477121697 of page Sodium_hydroxide for the Chem/Drugbox validation project (updated: ''). |
Latest revision as of 13:49, 27 August 2024 edit Utopes (talk | contribs)Extended confirmed users, Page movers, IP block exemptions, New page reviewers, Pending changes reviewers, Rollbackers38,741 edits the immediate examples use both |
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{{redirects here|NiS2|the European regulation|Cyber-security regulation#The NIS Directive II}} |
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{{ambox | text = This page contains a copy of the infobox ({{tl|chembox}}) taken from revid of page ] with values updated to verified values.}} |
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{{Chembox |
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{{Chembox |
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| Name = |
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| verifiedrevid = 476999826 |
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| ImageFile = Nickel-sulfide-xtal-unit-cell-3D-bs-17.png |
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| ImageFile1 = SodiumHydroxide.jpg |
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| verifiedrevid = 477162765 |
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| ImageFile1_Ref = {{Chemboximage|correct|??}} |
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| IUPACName = Nickel(II) sulfide |
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| ImageName1 = Sample of sodium hydroxide as pellets in a watchglass |
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| OtherNames = nickel sulfide, nickel monosulfide, nickelous sulfide |
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| ImageFile = Sodium-hydroxide-crystal-3D-vdW.png |
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| Section2 = {{Chembox Identifiers |
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| ImageFile_Ref = {{Chemboximage|correct|??}} |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| ImageName = Unit cell, spacefill model of sodium hydroxide |
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| CASNo = 11113-75-0 |
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| PIN = Sodium hydroxide{{Citation needed|date = October 2011}} |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| SystematicName = Sodium oxidanide{{Citation needed|date = October 2011}} |
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| UNII = I6929D52YQ |
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| OtherNames = Caustic soda{{Citation needed|date = October 2011}}<br /> |
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| ChemSpiderID = 26134 |
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Lye{{Citation needed|date = October 2011}} |
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| EINECS = 234-349-7 |
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| Section1 = {{Chembox Identifiers |
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| CASNo = 1310-73-2 |
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| PubChem = 28094 |
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| RTECS = QR9705000 |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| PubChem = 14798 |
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| SMILES = =S |
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| SMILES1 = . |
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| PubChem_Ref = {{Pubchemcite|correct|Pubchem}} |
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| ChemSpiderID = 14114 |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| UNII = 55X04QC32I |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| EINECS = 215-185-5 |
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| UNNumber = 1823 |
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| KEGG = D01169 |
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| KEGG_Ref = {{keggcite|correct|kegg}} |
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| MeSHName = Sodium+Hydroxide |
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| ChEBI = 32145 |
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| ChEBI_Ref = {{ebicite|correct|EBI}} |
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| RTECS = WB4900000 |
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| Gmelin = 68430 |
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| SMILES = O |
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| StdInChI = 1S/Na.H2O/h;1H2/q+1;/p-1 |
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| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
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| InChI = 1/Na.H2O/h;1H2/q+1;/p-1 |
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| StdInChIKey = HEMHJVSKTPXQMS-UHFFFAOYSA-M |
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| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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| InChIKey = HEMHJVSKTPXQMS-REWHXWOFAM |
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}} |
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}} |
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| Section2 = {{Chembox Properties |
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| Section3 = {{Chembox Properties |
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| Formula = {{Chem|NaOH}} |
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| Formula = {{Chem|NiS}} |
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| MolarMass = 39.9971 g mol<sup>-1</sup> |
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| MolarMass = 90.7584 g mol<sup>−1</sup> |
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| Appearance = black solid |
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| ExactMass = 39.992509329 g mol<sup>−1</sup> |
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| Odor = Odorless |
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| Appearance = White, waxy, opaque crystals |
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| Density = 2.13 g cm<sup>−3</sup> |
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| Density = 5.87 g/cm<sup>3</sup> |
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| MeltingPtC = 318 |
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| MeltingPtC = 797 |
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| BoilingPtC = 1388 |
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| BoilingPtC = 1388 |
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| Solubility = 1110 g/L (at 20 °C) |
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| Solubility = insoluble |
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| SolubleOther = degraded by ] |
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| Solvent1 = methanol |
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| Solubility1 = 238 g/L |
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| VaporPressure = |
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| Solvent2 = ethanol |
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| pKa = |
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| MagSus = +190.0·10<sup>−6</sup> cm<sup>3</sup>/mol |
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| Solubility2 = <<139 g/L |
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| VaporPressure = <2.4 kPa (at 20 °C) |
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| pKa = 13 |
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| RefractIndex = 1.412 |
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| Section4 = {{Chembox Thermochemistry |
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| Section4 = {{Chembox Structure |
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| CrystalStruct = hexagonal |
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| DeltaHf = −427 kJ·mol<sup>−1</sup><ref name=b1>{{cite book| author = Zumdahl, Steven S.|title =Chemical Principles 6th Ed.| publisher = Houghton Mifflin Company| year = 2009| isbn = 061894690X|page=A23}}</ref> |
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| Entropy = 64 J·mol<sup>−1</sup>·K<sup>−1</sup><ref name=b1/> |
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}} |
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| Section4 = {{Chembox Hazards |
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| ExternalMSDS = |
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| GHSPictograms = {{GHS corrosion}} |
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| EUIndex = 011-002-00-6 |
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| EUClass = {{Hazchem C}} |
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| RPhrases = {{R35}} |
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| SPhrases = {{S1/2}}, {{S26}}, {{S37/39}}, {{S45}} |
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| NFPA-H = 3 |
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| NFPA-F = 0 |
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| NFPA-R = 1 |
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| NFPA-O = COR |
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}} |
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}} |
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| Section5 = {{Chembox Related |
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| Section7 = {{Chembox Hazards |
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| GHSPictograms = {{GHS exclamation mark}} |
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| OtherAnions = ] |
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| MainHazards = may cause cancer by inhalation |
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| OtherCations = ]<br /> |
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]<br /> |
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] |
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'''Nickel sulfide''' is any ] with the formula Ni<sub>x</sub>S<sub>y</sub>. These compounds range in color from bronze (Ni<sub>3</sub>S<sub>2</sub>) to black (NiS<sub>2</sub>). The nickel sulfide with simplest stoichiometry is NiS, also known as the mineral ]. From the economic perspective, Ni<sub>9</sub>S<sub>8</sub>, the mineral ], is the chief source of mined nickel. Other minerals include ] (Ni<sub>3</sub>S<sub>2</sub>) and ] (Ni<sub>3</sub>S<sub>4</sub>), and the mineral ] (NiS<sub>2</sub>).<ref name="ullmann-1">{{Ullmann|author=Kerfoot, Derek G. E. |title=Nickel|doi=10.1002/14356007.a17_157|year=2005}}</ref> Some nickel sulfides are used commercially as catalysts. |
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==Structure== |
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Like many related materials, nickel sulfide adopts the ] motif. In this structure, nickel is octahedral and the sulfide centers are in trigonal prismatic sites.<ref>Wells, A.F. (1984) Structural Inorganic Chemistry, Oxford: Clarendon Press. {{ISBN|0-19-855370-6}}.</ref> |
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{| class="wikitable" style="text-align:center;" |
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|+Coordination environments in nickel sulfide |
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! Nickel |
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! Sulfur |
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| ] |
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| ] |
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| ] |
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NiS has two ]. The α-phase has a hexagonal unit cell, while the β-phase has a rhombohedral cell. The α-phase is stable at temperatures above {{convert|379|C|F}}, and converts into the β-phase at lower temperatures. That ] causes an increase in volume by 2–4%.<ref name= "NiS in glass">{{cite journal | doi = 10.1016/S0025-5408(98)00121-4 | title = Raman spectra of nickel(II) sulfide | year = 1998 | last1 = Bishop | first1 = D.W. | last2 = Thomas | first2 = P.S. | last3 = Ray | first3 = A.S. | journal = Materials Research Bulletin | volume = 33 | issue = 9 | pages = 1303}}</ref><ref>{{cite web | title = NiS and Spontaneous Breakage | url = http://www.glassonweb.com/articles/article/96/ | publisher = Glass on Web | date = Nov 2012 | url-status = dead | archive-url = https://web.archive.org/web/20130612022942/http://www.glassonweb.com/articles/article/96 | archive-date = 2013-06-12 }}</ref><ref>{{cite journal |last1=Bonati |first1=Antonio |last2=Pisano |first2=Gabriele |last3=Royer Carfagni |first3=Gianni |title=A statistical model for the failure of glass plates due to nickel sulfide inclusions |journal=Journal of the American Ceramic Society |date=12 October 2018 |volume=102 |issue=5 |pages=2506–2521 |doi=10.1111/jace.16106 |s2cid=140055629 }}</ref> |
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==Synthesis and reactions== |
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The precipitation of solid black nickel sulfide is a mainstay of traditional ] schemes, which begins with the separation of metals on the basis of the solubility of their sulfides. Such reactions are written:<ref>O.Glemser "Nickel Sulfide" in Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 2. p. 1551.</ref> |
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:Ni<sup>2+</sup> + H<sub>2</sub>S → NiS + 2 H<sup>+</sup> |
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Many other more controlled methods have been developed, including ] reactions (from NiCl<sub>2</sub> and Na<sub>2</sub>S) and high temperature reactions of the elements.<ref>leading reference can be found in: Shabnam Virji, Richard B. Kaner, Bruce H. Weiller "Direct Electrical Measurement of the Conversion of Metal Acetates to Metal Sulfides by Hydrogen Sulfide" Inorg. Chem., 2006, 45 (26), pp 10467–10471.{{doi|10.1021/ic0607585}}</ref> |
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The most commonly practiced reaction of nickel sulfides involves conversion to nickel oxides. This conversion involves heating the sulfide ores in air:<ref name="ullmann-1"/> |
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:{{Chem2|NiS + 1.5 O2 -> NiO + SO2}} |
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==Occurrence== |
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===Natural=== |
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The mineral ] is also a nickel sulfide with the molecular formula NiS, although its structure differs from synthetic stoichiometric NiS due to the conditions under which it forms. It occurs naturally in low temperature hydrothermal systems, in cavities of carbonate rocks, and as a byproduct of other nickel minerals.<ref>Gamsjager H. C., Bugajski J., Gajda T., Lemire R. J., Preis W. (2005) Chemical Thermodynamics of Nickel, Amsterdam, Elsevier B.V.</ref> |
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] crystals]] |
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In nature, nickel sulfides commonly occur as solid solutions with iron sulfides in minerals such as ] and ]. These minerals have the formula Fe<sub>9-x</sub>Ni<sub>x</sub>S<sub>8</sub> and Fe<sub>7-x</sub>Ni<sub>x</sub>S<sub>6</sub>, respectively. In some cases they are high in nickel (larger values of x). |
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===In glass manufacturing=== |
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] contains a small amount of nickel sulfide, formed from the sulfur in the fining agent {{chem|Na|2|S|O|4}} and the nickel contained in metallic alloy contaminants.<ref name="karlsson2017">{{cite journal |last1=Karlsson |first1=Stefan |title=Spontaneous fracture in thermally strengthened glass – A review & outlook |journal=Ceramics – Silikaty |date=30 April 2017 |pages=188–201 |doi=10.13168/cs.2017.0016 |url=https://www.researchgate.net/publication/316596288 |access-date=16 August 2019|doi-access=free }}</ref> |
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Nickel sulfide inclusions are a problem for ] applications. After the tempering process, nickel sulfide inclusions are in the metastable alpha phase. The inclusions eventually convert to the beta phase (stable at low temperature), increasing in volume and causing cracks in the glass. In the middle of tempered glass, the material is under ], which causes the cracks to propagate and leads to spontaneous glass fracture.<ref name="barry2006">{{cite web |last1=Barry |first1=John |title=The Achille Heel of a Wonderful Material: Toughened Glass |url=https://www.glassonweb.com/article/achille-heel-wonderful-material-toughened-glass |website=Glass on Web |access-date=16 August 2019 |date=12 January 2006}}</ref> That spontaneous fracture occurs years or decades after glass manufacturing.<ref name="karlsson2017" /> |
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==References== |
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{{Reflist|colwidth=30em}} |
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{{Nickel compounds}} |
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{{Sulfides}} |
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] |
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] |
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] |