Formula For Nickel Iii Sulfide
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| IUPAC proper name Nickel(Two) sulfide | |
| Other names nickel sulfide, nickel monosulfide, nickelous sulfide | |
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| ECHA InfoCard | 100.037.113 |
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| Properties | |
| Chemic formula | NiS |
| Molar mass | ninety.7584 one thousand mol−one |
| Appearance | blackness solid |
| Odor | Odorless |
| Density | 5.87 grand/cmthree |
| Melting point | 797 °C (one,467 °F; 1,070 K) |
| Humid point | 1,388 °C (2,530 °F; 1,661 K) |
| Solubility in water | insoluble |
| Solubility | soluble in nitric acid |
| Magnetic susceptibility (χ) | +190.0·10−vi cmthree/mol |
| Structure | |
| Crystal structure | hexagonal |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
| Main hazards | may cause cancer past inhalation |
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| Pictograms |  |
| Except where otherwise noted, data are given for materials in their standard country (at 25 °C [77 °F], 100 kPa). Infobox references | |
Nickel sulfide is whatsoever inorganic chemical compound with the formula NiSx. All are black solids. The nickel sulfide with simplest stoichiometry is NiS, likewise known equally the mineral millerite. From the economical perspective, Ni9S8, the mineral pentlandite, is the chief source of mined nickel. Other minerals include heazlewoodite (Ni3Southward2) and polydymite (Ni3Sfour).[1] The mineral Vaesite is NiS2.[2] Some nickel sulfides are used commercially as catalysts.
Structure [edit]
Similar many related materials, nickel sulfide adopts the nickel arsenide motif. In this structure, nickel is octahedral and the sulfide centers are in trigonal prismatic sites.[three]
| Nickel | Sulfur |
|---|---|
 |  |
| octahedral | trigonal prismatic |
NiS has 2 polymorphs. The α-phase has a hexagonal unit of measurement jail cell, while the β-phase has a rhombohedral jail cell. The α-phase is stable at temperatures above 379 °C (714 °F), and converts into the β-phase at lower temperatures. That stage transition causes an increase in volume by 2-four%.[4] [5] [half-dozen]
Synthesis and reactions [edit]
The atmospheric precipitation of solid black nickel sulfide is a mainstay of traditional qualitative inorganic analysis schemes, which begins with the separation of metals on the basis of the solubility of their sulfides. Such reactions are written:[seven]
- Ni2+ + H2South → NiS + two H+
Many other more than controlled methods have been developed, including solid state metathesis reactions (from NiCl2 and Na2S) and high temperature reactions of the elements.[8]
The nearly commonly practiced reaction of nickel sulfides involves conversion to nickel oxides. This conversion involves heating the sulfide ores in air:[1]
- NiS + 1.v O2 → NiO + And then2
Occurrence [edit]
Natural [edit]
The mineral millerite is also a nickel sulfide with the molecular formula NiS, although its structure differs from synthetic stoichiometric NiS due to the atmospheric condition under which it forms. It occurs naturally in low temperature hydrothermal systems, in cavities of carbonate rocks, and every bit a byproduct of other nickel minerals.[9]
In glass manufacturing [edit]
Float glass contains a small-scale amount of nickel sulfide, formed from the sulfur in the fining agent Na
ii Then
4 and the nickel contained in metallic alloy contaminants.[10]
Nickel sulfide inclusions are a problem for tempered glass applications. Subsequently the tempering process, nickel sulfide inclusions are in the metastable blastoff phase. The inclusions eventually convert to the beta phase (stable at depression temperature), increasing in book and causing cracks in the glass. In the centre of tempered glass, the material is under tension, which causes the cracks to propagate and leads to spontaneous glass fracture.[eleven] That spontaneous fracture occurs years or decades later on drinking glass manufacturing.[10]
References [edit]
- ^ a b Kerfoot, Derek M. East. (2000). "Nickel". Ullmann'due south Encyclopedia of Industrial Chemical science. Weinheim: Wiley-VCH. doi:10.1002/14356007.a17_157.
- ^ Kerfoot, Derek 1000. E. (2005). "Nickel". Ullmann'due south Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a17_157.
- ^ Wells, A.F. (1984) Structural Inorganic Chemistry, Oxford: Clarendon Press. ISBN 0-19-855370-6.
- ^ Bishop, D.Due west.; Thomas, P.Southward.; Ray, A.S. (1998). "Raman spectra of nickel(II) sulfide". Materials Enquiry Message. 33 (ix): 1303. doi:x.1016/S0025-5408(98)00121-4.
- ^ "NiS and Spontaneous Breakage". Glass on Spider web. Nov 2012. Archived from the original on 2013-06-12.
- ^ Bonati, Antonio; Pisano, Gabriele; Royer Carfagni, Gianni (12 October 2018). "A statistical model for the failure of drinking glass plates due to nickel sulfide inclusions". Journal of the American Ceramic Society. doi:10.1111/jace.16106. S2CID 140055629.
- ^ O.Glemser "Nickel Sulfide" in Handbook of Preparative Inorganic Chemistry, 2d Ed. Edited past One thousand. Brauer, Academic Press, 1963, NY. Vol. 2. p. 1551.
- ^ leading reference can exist found in: Shabnam Virji, Richard B. Kaner, Bruce H. Weiller "Direct Electric Measurement of the Conversion of Metallic Acetates to Metal Sulfides by Hydrogen Sulfide" Inorg. Chem., 2006, 45 (26), pp 10467–10471.doi:10.1021/ic0607585
- ^ Gamsjager H. C., Bugajski J., Gajda T., Lemire R. J., Preis Due west. (2005) Chemical Thermodynamics of Nickel, Amsterdam, Elsevier B.V.
- ^ a b Karlsson, Stefan (xxx Apr 2017). "Spontaneous fracture in thermally strengthened glass - A review & outlook". Ceramics - Silikaty: 188–201. doi:10.13168/cs.2017.0016 . Retrieved 16 August 2019.
- ^ Barry, John (12 January 2006). "The Achille Heel of a Wonderful Material: Toughened Glass". Glass on Web . Retrieved 16 August 2019.
Formula For Nickel Iii Sulfide,
Source: https://en.wikipedia.org/wiki/Nickel_sulfide
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