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{{About|the mercuric salt|the hypothesized mercurous salt|mercury(I) sulfide}} |
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{{chembox |
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{{Chembox |
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| verifiedrevid = 387279401 |
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| Verifiedfields = changed |
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| Name = Mercury sulfide |
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| Watchedfields = changed |
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| ImageFile1 = HgS-alpha-cinnabar-xtal-1999-looking-down-a-axis-CM-3D-balls.png |
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| verifiedrevid = 441024282 |
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| ImageFile2 = HgS-alpha-cinnabar-xtal-1999-looking-down-c-axis-CM-3D-balls.png |
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| Name = Mercury sulfide |
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| ImageSize2 = 150px |
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| IUPACName = Mercury sulfide |
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| ImageFile = Mercury(II) sulfide.jpg |
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| ImageSize = 150px |
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| OtherNames = ]<br/>] |
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| ImageFile1 = |
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| Section1 = {{Chembox Identifiers |
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| CASNo = 1344-48-5 |
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| ImageFile2 = |
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| CASNo_Ref = {{cascite}} |
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| ImageSize2 = |
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| IUPACName = Mercury sulfide |
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| OtherNames = ]<br>] |
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| SystematicName = |
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| Section1 = {{Chembox Identifiers |
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| CASNo = 1344-48-5 |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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| EC_number = 215-696-3 |
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| UNII_Ref = {{fdacite|correct|FDA}} |
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| UNII = ZI0T668SF1 |
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| PubChem = 62402 |
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| UNNumber = 2025 |
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| SMILES = = |
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| StdInChI=1S/Hg.S |
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| StdInChIKey = QXKXDIKCIPXUPL-UHFFFAOYSA-N |
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}} |
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| Section2 = {{Chembox Properties |
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| Section2 = {{Chembox Properties |
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| Formula = HgS |
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| Formula = HgS |
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| MolarMass = 232.66 g/mol |
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| MolarMass = 232.66 g/mol |
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| Density = 8.10 g/cm<sup>3</sup> |
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| Density = 8.10 g/cm<sup>3</sup> |
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| Solubility = insoluble |
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| Solubility = insoluble |
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| MeltingPt = 580 °C decomp. |
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| MeltingPtC = 580 |
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| MeltingPt_notes = decomposes |
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| BandGap = 2.1 eV (direct, α-HgS) <ref>L. I. Berger, ''Semiconductor Materials'' (1997) CRC Press ISBN 0849389127</ref> |
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| BandGap = 2.1 eV (direct, α-HgS) <ref>L. I. Berger, ''Semiconductor Materials'' (1997) CRC Press {{ISBN|0-8493-8912-7}}</ref> |
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| RefractIndex = w=2.905, e=3.256, bire=0.3510 (α-HgS) <ref></ref> |
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| RefractIndex = w=2.905, e=3.256, bire=0.3510 (α-HgS) <ref></ref> |
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| MagSus = −55.4·10<sup>−6</sup> cm<sup>3</sup>/mol |
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}} |
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| Section7 = {{Chembox Hazards |
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| ExternalMSDS = |
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| EUIndex = 080-002-00-6 |
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| EUClass = Very toxic ('''T+''')<br/>Dangerous for the environment ('''N''') |
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| RPhrases = {{R26/27/28}}, {{R33}}, {{R50/53}} |
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| SPhrases = {{S1/2}}, {{S13}}, {{S28}}, {{S45}}, {{S60}}, {{S61}} |
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| NFPA-H = |
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| NFPA-F = |
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| NFPA-R = |
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| FlashPt = Non-flammable |
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| PEL = |
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}} |
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| Section3 = |
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| Section8 = {{Chembox Related |
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| Section4 = {{Chembox Thermochemistry |
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| OtherAnions = ]<br/>]<br/>] |
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| DeltaHf = −58 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=978-0-618-94690-7 |page=A22}}</ref> |
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| OtherCations = ]<br/>] |
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| Entropy = 78 J·mol<sup>−1</sup>·K<sup>−1</sup><ref name=b1/> |
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| OtherCpds = |
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}} |
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| Section5 = |
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| Section6 = |
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| Section7 = {{Chembox Hazards |
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| ExternalSDS = |
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| GHSPictograms = {{GHS skull and crossbones}}{{GHS exclamation mark}}{{GHS health hazard}}{{GHS environment}} |
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| GHSSignalWord = Danger |
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| HPhrases = {{H-phrases|300|310|317|330|373|410}} |
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| PPhrases = {{P-phrases|261|272|280|302+352|321|333+313|363|501}} |
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| NFPA-H = 4 |
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| NFPA-F = 0 |
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| NFPA-R = 0 |
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| FlashPt = Non-flammable |
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| PEL = |
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}} |
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}} |
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| Section8 = {{Chembox Related |
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| OtherAnions = ]<br>]<br>] |
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| OtherCations = ]<br>] |
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| OtherCompounds = |
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}} |
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}} |
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}} |
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'''Mercury sulfide''', '''mercuric sulfide''', or '''mercury(II) sulfide''' is a chemical compound composed of the ] ] and ]. It is represented by the ] HgS. It is virtually insoluble in water.<ref name = "Greenwood">{{Greenwood&Earnshaw1st|page=1406}}</ref> |
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'''Mercury sulfide''', or '''mercury(II) sulfide''' is a chemical compound composed of the ] ] and ]. It is represented by the ] HgS. It is virtually insoluble in water.<ref name="Greenwood">{{Greenwood&Earnshaw1st|page=1406}}</ref> |
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==Crystal structure== |
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==Crystal structure== |
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] |
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] |
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] |
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HgS is dimorphic with two crystal forms: |
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HgS is dimorphic with two crystal forms: |
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*red ] (α-HgS, ], hP6, P3221), is the form in which mercury is most commonly found in nature. |
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* red ] (α-HgS, ], hP6, P3221) is the form in which mercury is most commonly found in nature. Cinnabar has rhombohedral crystal system. Crystals of red are ]. This is caused by the Hg-S helices in the structure.<ref>{{cite journal |author=A. M. Glazer, K. Stadnicka |year=1986 |title=On the origin of optical activity in crystal structures |journal=J. Appl. Crystallogr. |volume=19 |pages=108–122 |doi=10.1107/S0021889886089823 |issue=2 |s2cid=96545158}}</ref> |
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*black, metacinnabar (β-HgS), is less common in nature and adopts the ] (''T''<sup>2</sup><sub>d</sub>-''F''-4''3m'') ]. |
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* black ] (β-HgS) is less common in nature and adopts the ] (''T''<sup>2</sup><sub>d</sub>-''F''{{overline|4}}''3m''). |
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Crystals of red, α-HgS, are optically active. This is caused by the Hg-S helices in the structure.<ref> |
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{{cite journal |
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|last= Glazer |
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|authorlink= |
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|coauthors= Stadnicka K. |
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|year= 1986 |
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|title= On the origin of optical activity in crystal structures |
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|journal= J. Appl. Cryst. |
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|volume= 19 |
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|pages= 108–122 |
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|doi= 10.1107/S0021889886089823 |
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|first1= A. M. |
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|issue= 2}}</ref> |
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==Preparation and chemistry== |
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==Preparation and chemistry== |
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β-HgS precipitates as a black solid when Hg(II) salts are treated with ]. The reaction is conveniently conducted with an acetic acid solution of ]. With gentle heating of the slurry, the black ] converts to the red form.<ref>{{cite book |doi=10.1002/9780470132326.ch7 |chapter=Red Mercuric Sulfide |year=1939 |last1=Newell |first1=Lyman C. |last2=Maxson |first2=R. N. |last3=Filson |first3=M. H. |title=Inorganic Syntheses |pages=19–20 |volume=1 |isbn=9780470132326}}</ref> β-HgS is unreactive to all but concentrated acids.<ref name="Greenwood"/> |
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β-HgS is precipitated as a black powder when ] is bubbled through solutions of Hg(II) salts.<ref>{{Cotton&Wilkinson6th}}</ref> β-HgS is unreactive to all but concentrated acids.<ref name ="Greenwood"/> <br />Mercury metal is produced from the ] ore by roasting in air and condensing the vapour.<ref name = "Greenwood"/> |
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Mercury is produced from the ] ore by roasting in air and condensing the vapour.<ref name="Greenwood"/> |
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:HgS → Hg + S |
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==Uses== |
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==Uses== |
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] |
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α-HgS is used as a red pigment when it is known as ]. Vermilion is known to darken and this has been ascribed to conversion from red α-HgS to black β-HgS. Investigations at Pompeii where red walls when originally excavated have darkened has been ascribed to the formation of Hg-Cl compounds (e.g., ], ], and ]) and ], gypsum, rather than β-HgS, which was not detected.<ref> |
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When α-HgS is used as a red pigment, it is known as ]. The tendency of cinnabar to darken has been ascribed to conversion from red α-HgS to black β-HgS. However β-HgS was not detected at excavations in Pompeii, where originally red walls darkened, and was attributed to the formation of Hg-Cl compounds (e.g., ], ], and ]) and ], gypsum.<ref> {{cite journal |last1=Cotte |first1=M |author2=Susini J |author3=Metrich N |author4=Moscato A |author5=Gratziu C |author6=Bertagnini A |author7=Pagano M |year=2006 |title=Blackening of Pompeian Cinnabar Paintings: X-ray Microspectroscopy Analysis |journal=Anal. Chem. |volume=78 |issue=21 |pages=7484–7492 |doi=10.1021/ac0612224 |pmid=17073416}}</ref> |
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{{cite journal |
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|last= Cotte |
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As the mercury cell as used in the chlor-alkali industry (]) is being phased out over concerns over mercury emissions, the metallic mercury from these setups is converted into mercury sulfide for underground storage. |
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|authorlink= |
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|coauthors= Susini J, Metrich N, Moscato A, Gratziu C, Bertagnini A, Pagano M |
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With a band gap of 2.1 eV and its stability, it is possible to be used as ].<ref>{{Cite journal |last1=Davidson |first1=R. S. |last2=Willsher |first2=C. J. |date=March 1979 |title=Mercury(II) sulphide: a photo-stable semiconductor |url=https://www.nature.com/articles/278238a0 |journal=Nature |language=en |volume=278 |issue=5701 |pages=238–239 |doi=10.1038/278238a0 |s2cid=4363745 |issn=1476-4687}}</ref> |
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|year= 2006 |
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|month= |
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|title= Blackening of Pompeian Cinnabar Paintings: X-ray Microspectroscopy Analysis |
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|journal= Anal. Chem. |
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|volume= 78 |
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|issue= 21 |
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|pages= 7484–7492 |
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|doi= 10.1021/ac0612224 |
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|id= |
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|url= |
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|accessdate= |
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|quote= |
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|pmid= 17073416 |
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|first1= M |
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|unused_data= DUPLICATE DATA: unused_data= - first= M }}</ref> |
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==See also== |
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==See also== |
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* ] |
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* ] |
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* ] |
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* ] (mercurous sulfide, {{chem|Hg|2|S}}), hypothetical |
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==References== |
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==References== |
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{{Reflist}} |
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<references/> |
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==External links== |
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* |
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{{Mercury compounds}} |
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{{Mercury compounds}} |
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{{Sulfides}} |
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{{DEFAULTSORT:Mercury Sulfide}} |
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