Mercury(II) Oxide - Wikipedia

Mercury(II) oxide

Names
IUPAC name Mercury(II) oxide
Other names Mercuric oxideMontroyditeRed mercury
Identifiers
CAS Number	21908-53-2 Y
3D model (JSmol)	Interactive image
ChemSpider	28626 Y
ECHA InfoCard	100.040.580
KEGG	C18670 Y
PubChem CID	30856
RTECS number	OW8750000
UNII	IY191986AO Y
UN number	1641
CompTox Dashboard (EPA)	DTXSID4042125
InChI InChI=1S/Hg.O YKey: UKWHYYKOEPRTIC-UHFFFAOYSA-N Y
SMILES [Hg]=O
Properties
Chemical formula	HgO
Molar mass	216.591 g·mol−1
Appearance	Yellow or red solid
Odor	odorless
Density	11.14 g/cm3
Melting point	500 °C (932 °F; 773 K) (decomposes)
Solubility in water	0.0053 g/100 mL (25 °C) 0.0395 g/100 mL (100 °C)
Solubility	insoluble in alcohol, ether, acetone, ammonia
Band gap	2.2 eV[1]
Magnetic susceptibility (χ)	−44.0·10−6 cm3/mol
Refractive index (nD)	2.5 (550 nm)[1]
Thermochemistry
Std molarentropy (S⦵298)	70 J·mol−1·K−1[2]
Std enthalpy offormation (ΔfH⦵298)	−90 kJ·mol−1[2]
Hazards
Occupational safety and health (OHS/OSH):
Main hazards	Extremely toxic, environmental pollutant
GHS labelling:[4]
Pictograms
Signal word	Danger
Hazard statements	H300+H310+H330, H372, H410
Precautionary statements	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
NFPA 704 (fire diamond)	[5] 4 0 1
Flash point	Non-flammable
Lethal dose or concentration (LD, LC):
LD50 (median dose)	18 mg/kg (oral, rat)[3]
Safety data sheet (SDS)	ICSC 0981
Related compounds
Other anions	Mercury sulfideMercury selenideMercury telluride
Other cations	Zinc oxideCadmium oxide
Related compounds	Mercury(I) oxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). N verify (what is YN ?) Infobox references

Chemical compound

Mercury(II) oxide, also called mercuric oxide or simply mercury oxide, is the inorganic compound with the formula HgO. It has a red or orange color. Mercury(II) oxide is a solid at room temperature and pressure. The mineral form montroydite is very rarely found.

History

[edit]

An experiment for the preparation of mercuric oxide was first described by 11th century Arab-Spanish alchemist, Maslama al-Majriti, in Rutbat al-hakim.[6] It was historically called red precipitate (as opposed to white precipitate, mercuric amidochloride).

In 1774, Joseph Priestley discovered that oxygen was released by heating mercuric oxide, although he did not identify the gas as oxygen (rather, Priestley called it "dephlogisticated air," as that was the paradigm that he was working under at the time).[7]

Synthesis and reactions

[edit]

The red form of HgO can be made by heating Hg in oxygen at roughly 350 °C, or by pyrolysis of Hg(NO3)2.[8] The yellow form can be obtained by precipitation of aqueous Hg2+ with alkali.[8] 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°.[8]

HgO is soluble in many conventional strong acids through protonation of the anion.[9] The exceptions include acids which form insoluble mercury(II) salts, like mercury(II) iodide in the case of hydroiodic acid. Dissolution is also possible through complexation of the cation; e.g. cyanide ligands form stable water soluble mercury(II) complexes.

Structure

[edit]

Under atmospheric pressure mercuric oxide has two crystalline forms: one is called montroydite (orthorhombic, 2/m 2/m 2/m, Pnma), and the second is analogous to the sulfide mineral cinnabar (hexagonal, hP6, P3221); both are characterized by Hg-O chains.[10] At pressures above 10 GPa both structures convert to a tetragonal form.[1]

Uses

[edit]

Mercury oxide is sometimes used in the production of mercury as it decomposes quite easily. When it decomposes, oxygen gas is generated.[citation needed]

It is also used as a material for cathodes in mercury batteries.[11]

Health issues

[edit]

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, bioaccumulation takes place, specifically in aquatic organisms. The substance is banned as a pesticide in the EU.[12]

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.[13]

References

[edit]

1. ^ a b c Madelung, O; Rössler, U; Schulz, M, eds. (1999). "Mercury oxide (HgO) crystal structure, physical properties". Semiconductors · II-VI and I-VII Compounds; Semimagnetic Compounds. Landolt-Börnstein - Group III Condensed Matter. Vol. 41B. Springer-Verlag. pp. 1–7. doi:10.1007/b71137. ISBN 978-3-540-64964-9.
2. ^ a b Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A22. ISBN 978-0-618-94690-7.
3. ^ "Mercuric oxide [ISO]". ChemIDPlus Advanced. United States National Library of Medicine. CAS RN: 21908-53-2. Retrieved 2022-04-14.
4. ^ "Laboratory Chemical Safety Summary (LCSS): Mercuric oxide". PubChem. National Center for Biotechnology Information. CID 30856. Retrieved 2022-04-14.
5. ^ "Safety Data Sheet: Mercury(II) oxide" (PDF). Thermo Fisher Scientific. 2021-12-25. Cat No. AC316790000. Retrieved 2022-04-13.
6. ^ Holmyard, E. J. (1931). Inorganic chemistry. Рипол Классик. ISBN 978-5-87636-953-6. {{cite book}}: ISBN / Date incompatibility (help)
7. ^ Almqvist, Ebbe (2003). History of Industrial Gases. Springer. p. 23. ISBN 978-0-306-47277-0.
8. ^ a b c Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. doi:10.1016/C2009-0-30414-6. ISBN 978-0-08-037941-8.
9. ^ "Characteristic Reactions of Mercury Ions (Hg²⁺ and Hg₂²⁺)". LibreTextsChemistry. 3 April 2018. Retrieved 23 July 2024.
10. ^ Aurivillius, Karin; Carlsson, Inga-Britt; Pedersen, Christian; Hartiala, K.; Veige, S.; Diczfalusy, E. (1958). "The Structure of Hexagonal Mercury(II)oxide". Acta Chemica Scandinavica. 12: 1297–1304. doi:10.3891/acta.chem.scand.12-1297. Retrieved November 17, 2010.
11. ^ Moore, John W.; Conrad L. Stanitski; Peter C. Jurs (2005). Chemistry: The Molecular Science. Thomson Brooks/Cole. p. 941. ISBN 978-0-534-42201-1. Mercury(II) oxide anode mercury battery.
12. ^ Chemicals Regulation Directorate. "Banned and Non-Authorised Pesticides in the United Kingdom". Retrieved 1 December 2009.
13. ^ "Mercury (II) oxide". International Occupational Safety and Health Information Centre. Retrieved 2009-06-06.

External links

[edit] Wikimedia Commons has media related to Mercury(II) oxide.

• National Pollutant Inventory – Mercury and compounds fact sheet
• Information at Webelements.

v t e Mercury compounds
Mercury(I)	HgH Hg2H2 Hg2Br2 Hg2Cl2 Hg2F2 Hg2I2 Hg2(NO3)2 Hg2O Hg2SO4 Hg2S (hypothetical)
Mercury(II)	HgH2 HgNH2Cl HgSe HgS HgTe Hg(O2CCH3)2 HgBr2 HgCl2 Hg(CN)2 HgF2 Hg(OH)2 HgI2 Hg(NO3)2 HgO Hg(ClO4)2 HgSO4 Hg(SCN)2 Hg(CNO)2 Hg3N2 Hg(Si(CH3)3)2 K2HgI4 Organomercury compounds Hg(CH3)2 Hg(C2H5)2 Hg(C6H5)2 HgC6H5CH3CO2 HgC6H5OB(OH)2 HgC6H5NO3 HgC6H5CCl3 HgClC6H4CO2H HgOHCH2CHOCH3CH2(NHCO) C36H70HgO4 HgOHCH2CHOCH3CH2NHCOC6H4OCH2CO2H Na2HgOHC6HOBrC6H2OBrOCHC6H4CO2 HgOC6H2CH3NO2 NaHgC2H5SC6H4CO2
Mercury(IV)	HgF4 (hypothetical)
Amalgams	Na(Hg) Al(Hg) K(Hg) Au(Hg) Tl(Hg) Sn(Hg)
Mercury cations	Hg2+ Hg2+2 Hg2+3 Hg2+4 Hg4+3 HgCH+3 HgC2H+5 HgC6H+5

v t e Oxides
Mixed oxidation states	Antimony tetroxide (Sb2O4) Boron suboxide (B12O2) Carbon suboxide (C3O2) Chlorine perchlorate (Cl2O4) Chloryl perchlorate (Cl2O6) Cobalt(II,III) oxide (Co3O4) Dichlorine pentoxide (Cl2O5) Iron(II,III) oxide (Fe3O4) Lead(II,IV) oxide (Pb3O4) Manganese(II,III) oxide (Mn3O4) Mellitic anhydride (C12O9) Praseodymium(III,IV) oxide (Pr6O11) Silver(I,III) oxide (Ag2O2) Terbium(III,IV) oxide (Tb4O7) Tribromine octoxide (Br3O8) Triuranium octoxide (U3O8)
+1 oxidation state	Aluminium(I) oxide (Al2O) Copper(I) oxide (Cu2O) Caesium monoxide (Cs2O) Dibromine monoxide (Br2O) Dicarbon monoxide (C2O) Dichlorine monoxide (Cl2O) Gallium(I) oxide (Ga2O) Iodine(I) oxide (I2O) Lithium oxide (Li2O) Mercury(I) oxide (Hg2O) Nitrous oxide (N2O) Potassium oxide (K2O) Rubidium oxide (Rb2O) Silver oxide (Ag2O) Thallium(I) oxide (Tl2O) Sodium oxide (Na2O) Water (hydrogen oxide) (H2O)
+2 oxidation state	Aluminium(II) oxide (AlO) Barium oxide (BaO) Berkelium monoxide (BkO) Beryllium oxide (BeO) Boron monoxide (BO) Bromine monoxide (BrO) Cadmium oxide (CdO) Calcium oxide (CaO) Carbon monoxide (CO) Chlorine monoxide (ClO) Chromium(II) oxide (CrO) Cobalt(II) oxide (CoO) Copper(II) oxide (CuO) Dinitrogen dioxide (N2O2) Disulfur dioxide (S2O2) Europium(II) oxide (EuO) Germanium monoxide (GeO) Iron(II) oxide (FeO) Iodine monoxide (IO) Lead(II) oxide (PbO) Magnesium oxide (MgO) Manganese(II) oxide (MnO) Mercury(II) oxide (HgO) Nickel(II) oxide (NiO) Nitric oxide (NO) Niobium monoxide (NbO) Palladium(II) oxide (PdO) Phosphorus monoxide (PO) Polonium monoxide (PoO) Protactinium monoxide (PaO) Radium oxide (RaO) Silicon monoxide (SiO) Strontium oxide (SrO) Sulfur monoxide (SO) Thorium monoxide (ThO) Tin(II) oxide (SnO) Titanium(II) oxide (TiO) Vanadium(II) oxide (VO) Yttrium(II) oxide (YO) Zirconium monoxide (ZrO) Zinc oxide (ZnO)
+3 oxidation state	Actinium(III) oxide (Ac2O3) Aluminium oxide (Al2O3) Americium(III) oxide (Am2O3) Antimony trioxide (Sb2O3) Arsenic trioxide (As2O3) Berkelium(III) oxide (Bk2O3) Bismuth(III) oxide (Bi2O3) Boron trioxide (B2O3) Californium(III) oxide (Cf2O3) Cerium(III) oxide (Ce2O3) Chromium(III) oxide (Cr2O3) Cobalt(III) oxide (Co2O3) Curium(III) oxide (Cm2O3) Dinitrogen trioxide (N2O3) Dysprosium(III) oxide (Dy2O3) Einsteinium(III) oxide (Es2O3) Erbium(III) oxide (Er2O3) Europium(III) oxide (Eu2O3) Gadolinium(III) oxide (Gd2O3) Gallium(III) oxide (Ga2O3) Gold(III) oxide (Au2O3) Holmium(III) oxide (Ho2O3) Indium(III) oxide (In2O3) Iron(III) oxide (Fe2O3) Lanthanum oxide (La2O3) Lutetium(III) oxide (Lu2O3) Manganese(III) oxide (Mn2O3) Neodymium(III) oxide (Nd2O3) Nickel(III) oxide (Ni2O3) Phosphorus trioxide (P4O6) Praseodymium(III) oxide (Pr2O3) Promethium(III) oxide (Pm2O3) Rhodium(III) oxide (Rh2O3) Samarium(III) oxide (Sm2O3) Scandium oxide (Sc2O3) Terbium(III) oxide (Tb2O3) Thallium(III) oxide (Tl2O3) Thulium(III) oxide (Tm2O3) Titanium(III) oxide (Ti2O3) Tungsten(III) oxide (W2O3) Vanadium(III) oxide (V2O3) Ytterbium(III) oxide (Yb2O3) Yttrium(III) oxide (Y2O3)
+4 oxidation state	Americium dioxide (AmO2) Berkelium(IV) oxide (BkO2) Bromine dioxide (BrO2) Californium dioxide (CfO2) Carbon dioxide (CO2) Carbon trioxide (CO3) Cerium(IV) oxide (CeO2) Chlorine dioxide (ClO2) Chromium(IV) oxide (CrO2) Curium(IV) oxide (CmO2) Dinitrogen tetroxide (N2O4) Germanium dioxide (GeO2) Iodine dioxide (IO2) Iridium dioxide (IrO2) Hafnium(IV) oxide (HfO2) Lead dioxide (PbO2) Manganese dioxide (MnO2) Molybdenum dioxide (MoO2) Neptunium(IV) oxide (NpO2) Nitrogen dioxide (NO2) Niobium dioxide (NbO2) Osmium dioxide (OsO2) Platinum dioxide (PtO2) Plutonium(IV) oxide (PuO2) Polonium dioxide (PoO2) Praseodymium(IV) oxide (PrO2) Protactinium(IV) oxide (PaO2) Rhenium(IV) oxide (ReO2) Rhodium(IV) oxide (RhO2) Ruthenium(IV) oxide (RuO2) Selenium dioxide (SeO2) Silicon dioxide (SiO2) Sulfur dioxide (SO2) Technetium(IV) oxide (TcO2) Tellurium dioxide (TeO2) Terbium(IV) oxide (TbO2) Thorium dioxide (ThO2) Tin dioxide (SnO2) Titanium dioxide (TiO2) Tungsten(IV) oxide (WO2) Uranium dioxide (UO2) Vanadium(IV) oxide (VO2) Xenon dioxide (XeO2) Zirconium dioxide (ZrO2)
+5 oxidation state	Antimony pentoxide (Sb2O5) Arsenic pentoxide (As2O5) Bismuth pentoxide (Bi2O5) Dinitrogen pentoxide (N2O5) Diuranium pentoxide (U2O5) Neptunium(V) oxide (Np2O5) Niobium pentoxide (Nb2O5) Phosphorus pentoxide (P2O5) Protactinium(V) oxide (Pa2O5) Tantalum pentoxide (Ta2O5) Tungsten pentoxide (W2O5) Vanadium(V) oxide (V2O5)
+6 oxidation state	Chromium trioxide (CrO3) Molybdenum trioxide (MoO3) Neptunium trioxide (NpO3) Polonium trioxide (PoO3) Rhenium trioxide (ReO3) Selenium trioxide (SeO3) Sulfur trioxide (SO3) Tellurium trioxide (TeO3) Tungsten trioxide (WO3) Uranium trioxide (UO3) Xenon trioxide (XeO3)
+7 oxidation state	Dichlorine heptoxide (Cl2O7) Manganese heptoxide (Mn2O7) Rhenium(VII) oxide (Re2O7) Technetium(VII) oxide (Tc2O7)
+8 oxidation state	Iridium tetroxide (IrO4) Osmium tetroxide (OsO4) Ruthenium tetroxide (RuO4) Xenon tetroxide (XeO4) Hassium tetroxide (HsO4)
Related	Oxocarbon Suboxide Oxyanion Ozonide Peroxide Superoxide Oxypnictide
Oxides are sorted by oxidation state. Category:Oxides

v t e Oxygen compounds

Ag4O4 Al2O3 AmO2 Am2O3 As2O3 As2O5 Au2O3 B2O3 BaO BeO Bi2O3 BiO2 Bi2O5 BrO2 Br2O3 Br2O5 Br3O8 CO CO2 C3O2 CaO CaO2 CdO CeO2 Ce3O4 Ce2O3 ClO2 Cl2O Cl2O2 Cl2O3 Cl2O4 Cl2O6 Cl2O7 CoO Co2O3 Co3O4 CrO3 Cr2O3 Cr2O5 Cr5O12 CsO2 Cs2O3 CuO Dy2O3 Er2O3 Eu2O3 FeO Fe2O3 Fe3O4 Ga2O Ga2O3 GeO GeO2 H2O 2H2O 3H2O H218O H2O2 HfO2 HgO Hg2O Ho2O3 IO I2O4 I2O5 I2O6 I4O9 In2O3 IrO2 KO2 K2O2 La2O3 Li2O Li2O2 Lu2O3 MgO Mg2O3 MnO MnO2 Mn2O3 Mn2O7 MoO2 MoO3 Mo2O3 NO NO2 N2O N2O3 N2O4 N2O5 NaO2 Na2O Na2O2 NbO NbO2 Nd2O3 O2F OF OF2 O2F2 O3F2 O4F2 O5F2 O6F2 O2PtF6 more...

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