| Revision as of 09:23, 10 April 2012 editBeetstra (talk | contribs)Edit filter managers, Administrators172,031 edits Saving copy of the {{chembox}} taken from revid 483835854 of page Mercury(II)_oxide for the Chem/Drugbox validation project (updated: 'StdInChI'). |
Latest revision as of 22:24, 23 July 2024 edit Smokefoot (talk | contribs)Autopatrolled, Extended confirmed users, Pending changes reviewers, Rollbackers74,208 edits →Synthesis: HgO reactions |
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{{Chembox |
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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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|Verifiedfields = changed |
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{{chembox |
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| Verifiedfields = changed |
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|Watchedfields = changed |
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| verifiedrevid = 470455221 |
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|verifiedrevid = 486593291 |
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| ImageFile = HgOpowder.jpg |
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|ImageFile = HgOpowder.jpg |
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| ImageName = Mercury(II) oxide |
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|ImageName = Mercury(II) oxide |
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| ImageFile1 = Montroydite-3D-ionic.png |
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|ImageFile1 = Montroydite-3D-ionic.png |
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| ImageName1 = Mercury(II) oxide |
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|ImageName1 = Mercury(II) oxide |
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| IUPACName = Mercury(II) oxide |
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|IUPACName = Mercury(II) oxide |
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| OtherNames = Mercuric oxide<br />] |
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|OtherNames = Mercuric oxide<br />]<br />] |
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| Section1 = {{Chembox Identifiers |
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|Section1={{Chembox Identifiers |
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| CASNo = 21908-53-2 |
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|CASNo = 21908-53-2 |
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| CASNo_Ref = {{cascite|correct|CAS}} |
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|CASNo_Ref = {{cascite|correct|CAS}} |
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|UNII_Ref = {{fdacite|correct|FDA}} |
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| UNNumber = 1641 |
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|UNII = IY191986AO |
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| RTECS = OW8750000 |
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| PubChen = 30856 |
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|UNNumber = 1641 |
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|RTECS = OW8750000 |
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| KEGG_Ref = {{keggcite|correct|kegg}} |
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|PubChem = 30856 |
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| StdInChI_Ref = {{stdinchicite|changed|chemspider}} |
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|KEGG_Ref = {{keggcite|correct|kegg}} |
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| StdInChI = 1S/Hg.O |
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| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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|StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
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|StdInChI = 1S/Hg.O |
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| StdInChIKey = UKWHYYKOEPRTIC-UHFFFAOYSA-N |
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| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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|StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChIKey = UKWHYYKOEPRTIC-UHFFFAOYSA-N |
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|StdInChIKey = UKWHYYKOEPRTIC-UHFFFAOYSA-N |
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|SMILES = =O |
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| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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|ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} |
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| ChemSpiderID = 28626 |
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|ChemSpiderID = 28626 |
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| KEGG = C18670 |
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|KEGG = C18670 |
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}} |
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| Section2 = {{Chembox Properties |
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| Hg = 1 | O = 1 |
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| Appearance = Yellow or red solid |
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| Odor = odorless |
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| Density = 11.14 g/cm<sup>3</sup> |
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| Solubility = 0.0053 g/100 mL (25 °C) <br> 0.0395 g/100 mL (100 °C) |
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| SolubleOther = insoluble in ], ], ], ] |
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| MeltingPt = 500 °C (decomposes) |
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| BandGap = 2.2 eV<ref name=landolt>{{cite book| chapter = Mercury oxide (HgO) crystal structure, physical properties| volume = 41B| doi = 10.1007/b71137| publisher = Springer-Verlag| year = 1999| pages = 1–7| isbn = 978-3-540-64964-9 | work = Landolt-Börnstein – Group III Condensed Matter}}</ref> |
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| RefractIndex = 2.5 (550 nm)<ref name=landolt/> |
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}} |
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| Section3 = {{Chembox Structure |
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| Coordination = orthorhombic |
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| CrystalStruct = |
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| Dipole = |
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}} |
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| Section4 = {{Chembox Thermochemistry |
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| DeltaHf = −90 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=A22}}</ref> |
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| Entropy = 70 J·mol<sup>−1</sup>·K<sup>−1</sup><ref name=b1/> |
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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 = 3 |
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| NFPA-F = 1 |
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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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| Section8 = {{Chembox Related |
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| OtherAnions = ]<br/>]<br/>] |
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| OtherCations = ]<br/>] |
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| OtherCpds = ] |
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}} |
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}} |
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}} |
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|Section2={{Chembox Properties |
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|Hg=1 | O=1 |
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|Appearance = Yellow or red solid |
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|Odor = odorless |
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|Density = 11.14 g/cm<sup>3</sup> |
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|Solubility = 0.0053 g/100 mL (25 °C) <br /> 0.0395 g/100 mL (100 °C) |
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|SolubleOther = insoluble in ], ], ], ] |
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|MeltingPtC = 500 |
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|MeltingPt_notes = (decomposes) |
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|BandGap = 2.2 eV<ref name=landolt>{{cite book| chapter = Mercury oxide (HgO) crystal structure, physical properties| volume = 41B| doi = 10.1007/b71137| publisher = Springer-Verlag| year = 1999| pages = 1–7| isbn = 978-3-540-64964-9 |title=Semiconductors · II-VI and I-VII Compounds; Semimagnetic Compounds| series = Landolt-Börnstein - Group III Condensed Matter| editor1-last = Madelung| editor1-first = O| editor2-first = U| editor2-last = Rössler| editor3-first = M| editor3-last = Schulz}}</ref> |
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|RefractIndex = 2.5 (550 nm)<ref name=landolt/> |
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|MagSus = −44.0·10<sup>−6</sup> cm<sup>3</sup>/mol |
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}} |
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|Section3={{Chembox Thermochemistry |
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|DeltaHf = −90 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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|Entropy = 70 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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|MainHazards = Extremely toxic, environmental pollutant |
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|ExternalSDS = |
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|GHSPictograms = {{GHS06}} {{GHS08}} {{GHS09}} |
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|GHSSignalWord = Danger |
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|HPhrases = {{H-phrases|H300+H310+H330|H372|H410}} |
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|PPhrases = {{P-phrases|P260|P262|P264|P270|P271|P273|P280|P284|P301+P316|P302+P352|P304+P340|P316|P320|P321|P330|P361+P364|P391|P403+P233|P405|P501}} |
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|GHS_ref = <ref>{{cite web|url=https://pubchem.ncbi.nlm.nih.gov/compound/30856#datasheet=LCSS|title=Laboratory Chemical Safety Summary (LCSS): Mercuric oxide|id=CID 30856|website=]|publisher=]|access-date=2022-04-14}}</ref> |
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|NFPA-H = 4 |
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|NFPA-F = 0 |
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|NFPA-R = 1 |
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|NFPA_ref = <ref>{{cite web|url=https://www.fishersci.com/store/msds?partNumber=AC316791000&countryCode=US&language=en|format=PDF|title=Safety Data Sheet: Mercury(II) oxide|id=Cat No. AC316790000|publisher=]|date=2021-12-25|access-date=2022-04-13}}</ref> |
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|FlashPt = Non-flammable |
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|LD50 = 18 mg/kg (oral, rat)<ref>{{cite web|url=https://chem.nlm.nih.gov/chemidplus/rn/21908-53-2|title=Mercuric oxide |id=CAS RN: 21908-53-2|website=ChemIDPlus Advanced|publisher=]|access-date=2022-04-14}}</ref> |
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}} |
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|Section5={{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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'''Mercury(II) oxide''', also called '''mercuric oxide''' or simply '''mercury oxide''', is the ] with the formula ]]. It has a red or orange color. Mercury(II) oxide is a solid at room temperature and pressure. The mineral form ] is very rarely found. |
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==History== |
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An experiment for the preparation of mercuric oxide was first described by 11th century Arab-Spanish alchemist, ], in ''Rutbat al-hakim.''<ref>{{Cite book|last=Holmyard |first=E. J. |url=https://books.google.com/books?id=uLsOAwAAQBAJ&dq=majriti+mercuric+oxide&pg=PA257 |title=Inorganic chemistry |date=1931 |publisher=Рипол Классик |isbn=978-5-87636-953-6 |language=en}}</ref> It was historically called ] (as opposed to ] being the ]). |
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In 1774, ] discovered that oxygen was released by heating mercuric oxide, although he did not identify the gas as ] (rather, Priestley called it "] air," as that was the ] that he was working under at the time).<ref>{{cite book |last=Almqvist |first=Ebbe |title=History of Industrial Gases |url=https://books.google.com/books?id=OI0fTJhydh4C&dq=Joseph+Priestley+oxygen+mercury&pg=PA23 |year=2003 |publisher=Springer |isbn=978-0-306-47277-0 |page=23}}</ref> |
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==Synthesis and reactions== |
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] |
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] structure]] |
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The red form of HgO can be made by heating Hg in oxygen at roughly 350 °C, or by ] of ].<ref name = "Greenwood">{{Greenwood&Earnshaw}}</ref> The yellow form can be obtained by precipitation of aqueous Hg<sup>2+</sup> with alkali.<ref name = "Greenwood"/> The difference in color is due to particle size; both forms have the same structure consisting of near linear O-Hg-O units linked in zigzag chains with an Hg-O-Hg angle of 108°.<ref name = "Greenwood"/> |
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It is sometimes said that HgO "is soluble in acids",<ref>{{cite web |title=Characteristic Reactions of Mercury Ions (Hg²⁺ and Hg₂²⁺) |url=https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Supplemental_Modules_(Analytical_Chemistry)/Qualitative_Analysis/Characteristic_Reactions_of_Select_Metal_Ions/Characteristic_Reactions_of_Mercury_Ions_(Hg_and_Hg) |website=LibreTextsChemistry |access-date=23 July 2024}}</ref> but in fact it reacts with acids to make mercuric salts. |
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==Structure== |
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Under atmospheric pressure mercuric oxide has two crystalline forms: one is called montroydite (], 2/m 2/m 2/m, Pnma), and the second is analogous to the sulfide mineral ] (], |
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hP6, P3221); both are characterized by Hg-O chains.<ref>{{Cite journal | last1 = Aurivillius | first1 = Karin | last2 = Carlsson | first2 = Inga-Britt | last3 = Pedersen | first3 = Christian | last4 = Hartiala | first4 = K. | last5 = Veige | first5 = S. | last6 = Diczfalusy | first6 = E. | title = The Structure of Hexagonal Mercury(II)oxide | journal = Acta Chemica Scandinavica | volume = 12 | pages = 1297–1304 | year = 1958 | url = http://actachemscand.dk/volume.php?select1=2&vol=12 | doi = 10.3891/acta.chem.scand.12-1297 | access-date = November 17, 2010| doi-access = free}}</ref> At pressures above 10 GPa both structures convert to a ] form.<ref name=landolt/> |
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==Uses== |
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Mercury oxide is sometimes used in the production of mercury as it decomposes quite easily. When it decomposes, oxygen gas is generated.{{citation needed|date=September 2023}} |
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It is also used as a material for ]s in ].<ref>{{cite book |last=Moore |first=John W. |author2=Conrad L. Stanitski |author3=Peter C. Jurs |title=Chemistry: The Molecular Science |url=https://archive.org/details/chemistrymolecul0000moor |url-access=registration |quote=Mercury(II) oxide anode mercury battery. |year=2005 |publisher=Thomson Brooks/Cole |isbn=978-0-534-42201-1 |page=}}</ref> |
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==Health issues== |
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] |
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Mercury oxide is a highly toxic substance which can be absorbed into the body by inhalation of its aerosol, through the skin and by ingestion. The substance is irritating to the eyes, the skin and the respiratory tract and may have effects on the kidneys, resulting in kidney impairment. In the food chain important to humans, ] takes place, specifically in aquatic organisms. The substance is banned as a pesticide in the ].<ref name=bnpuk>{{cite web | last = Chemicals Regulation Directorate | title = Banned and Non-Authorised Pesticides in the United Kingdom | url = http://www.pesticides.gov.uk/approvals.asp?id=55 | access-date = 1 December 2009}}</ref> |
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Evaporation at 20 °C is negligible. HgO decomposes on exposure to light or on heating above 500 °C. Heating produces highly toxic mercury fumes and oxygen, which increases the fire hazard. Mercury(II) oxide reacts violently with reducing agents, chlorine, hydrogen peroxide, magnesium (when heated), disulfur dichloride and hydrogen trisulfide. Shock-sensitive compounds are formed with metals and elements such as sulfur and phosphorus.<ref>{{cite web| url = http://www.inchem.org/documents/icsc/icsc/eics0981.htm| title = Mercury (II) oxide| access-date = 2009-06-06| publisher = International Occupational Safety and Health Information Centre}}</ref> |
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==References== |
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{{Reflist}} |
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==External links== |
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{{Commons category|Mercury(II) oxide}} |
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* . |
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{{Mercury compounds}} |
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{{Oxides}} |
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{{oxygen compounds}} |
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{{Authority control}} |
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] |
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] |
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] |