Mercury(II) bromide

Mercury(II) bromide
Mercury(II) bromide
Names
IUPAC name
Mercury(II) bromide
Other names
Mercuric bromide
Identifiers
CAS Number
  • 7789-47-1 checkY
ECHA InfoCard 100.029.245 Edit this at Wikidata
PubChem CID
  • 24612
RTECS number
  • OV7415000
UNII
  • P986675T8V checkY
CompTox Dashboard (EPA)
  • DTXSID2064864 Edit this at Wikidata
Properties
Chemical formula
 HgBr2
Molar mass 360.41 g/mol
Appearance white solid
Density 6.03 g/cm3, solid
Melting point 237 °C (459 °F; 510 K)
Boiling point 322 °C (612 °F; 595 K)
Solubility in water
 0.6 g/100 mL (25°C)
Solubility 30 g/100 mL (25°C) ethanol
Magnetic susceptibility (χ)
 −94.2·10−6 cm3/mol
Structure
Coordination geometry
 rhombic
Hazards
GHS labelling:[1]
Pictograms
 GHS06: ToxicGHS08: Health hazardGHS09: Environmental hazard
Danger
Hazard statements
 H300, H310, H330, H373, H410
Precautionary statements
 P260, P262, P264, P270, P271, P273, P280, P284, P301+P310, P302+P350, P304+P340, P310, P314, P320, P321, P322, P330, P361, P363, P391, P403+P233, P405, P501
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g. white phosphorusSpecial hazards (white): no code
3
0
2
Flash point Non-flammable
Related compounds
Other anions
 Mercury(II) fluoride
Mercury(II) chloride
Mercury(II) iodide
Other cations
 Zinc bromide
Cadmium bromide
Mercury(I) bromide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references
Chemical compound

Mercury(II) bromide or mercuric bromide is an inorganic compound with the formula HgBr2.[2] This white solid is a laboratory reagent.[3] [2] Like all mercury salts, it is highly toxic.[2]

Preparation

Mercury(II) bromide can be produced by reaction of metallic mercury with bromine.[4]

Reactions

Mercury(II) bromide is used as a reagent in the Koenigs–Knorr reaction, which forms glycoside linkages on carbohydrates.[5][6]

It is also used to test for the presence of arsenic, as recommended by the European Pharmacopoeia.[7] The arsenic in the sample is first converted to arsine gas by treatment with hydrogen. Arsine reacts with mercury(II) bromide:[8]

AsH3 + 3HgBr2 → As(HgBr)3 + 3HBr

The white mercury(II) bromide will turn yellow, brown, or black if arsenic is present in the sample.[9]

Mercury(II) bromide reacts violently with elemental indium at high temperatures[10] and, when exposed to potassium, can form shock-sensitive explosive mixtures.[11]

References

  1. ^ "Mercuric bromide". PubChem. National Center for Biotechnology Information. Retrieved 2021-11-25.
  2. ^ a b c PubChem. "Mercury bromide (Hg2Br2)". pubchem.ncbi.nlm.nih.gov. Retrieved 2022-12-22.
  3. ^ Elements, American. "Mercury Bromide". American Elements. Retrieved 2022-12-22.
  4. ^ F. Wagenknecht; R. Juza (1963). "Mercury(II) bromide". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 2. NY, NY: Academic Press. p. 1109.
  5. ^ Horton, Derek (2004), Advances in Carbohydrate Chemistry and Biochemistry, Amsterdam: Elseveir Academic Press, p. 76, ISBN 0-12-007259-9, retrieved 2008-05-29
  6. ^ Stick, Robert V. (2001), Carbohydrates: The Sweet Molecules of Life, San Diego: Academic Press, p. 125, ISBN 0-12-670960-2, retrieved 2008-05-29
  7. ^ Pederson, Ole (2006), Pharmaceutical Chemical Analysis, Boca Raton, Florida: CRC Press, p. 107, ISBN 0-8493-1978-1, retrieved 2008-05-29
  8. ^ Odegaard, Nancy; Sadongei, Alyce (2005), Old Poisons, New Problems, Rowman Altamira, p. 58, ISBN 0-7591-0515-4, retrieved 2008-05-29
  9. ^ Townsend, Timothy G.; Solo-Gabriele, Helena (2006), Environmental Impacts of Treated Wood, Boca Raton, Florida: CRC Press, p. 339, ISBN 0-8493-6495-7, retrieved 2008-05-29
  10. ^ Bretherick, L.; Urben, P. G.; Pitt, Martin John (1999), Bretherick's Handbook of Reactive Chemical Hazards, Elseveir Academic Press, p. 110, ISBN 0-7506-3605-X
  11. ^ Bretherick, L.; Urben, P. G.; Pitt, Martin John (1999), Bretherick's Handbook of Reactive Chemical Hazards, Elseveir Academic Press, p. 1276, ISBN 0-7506-3605-X
  • v
  • t
  • e
Mercury(I)
  • HgH
  • Hg2H2
  • Hg2Br2
  • Hg2Cl2
  • Hg2F2
  • Hg2I2
  • Hg2(NO3)2
  • Hg2O
  • Hg2CO3
  • 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
  • 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)
  • C
    36    H
    70    HgO
    4
  • HgOHCH2CHOCH3CH2NHCOC6H4OCH2CO2H
  • Na2HgOHC6HOBrC6H2OBrOCHC6H4CO2
  • HgOC6H2CH3NO2
  • NaHgC2H5SC6H4CO2
Mercury(IV)
  • HgF4 (hypothetical)
Amalgams
Mercury cations
  • Hg2+
  • Hg22+
  • Hg32+
  • Hg42+
  • Hg34+
  • HgCH3+
  • HgC2H5+
  • HgC6H5+
  • v
  • t
  • e
Br(−I)
  • Br−
  • CH3Br
  • CH2Br2
  • CHBr3
  • CBr4
  • HBr
  • C3H5Br
Br(−I,I)
  • Br3−
Br(I)
  • BrCl
  • BrF
  • BrN3
  • BrNO3
  • Br2O
  • BrO−
  • NBr3
Br(II)
Br(I,V)
  • Br2O3
Br(III)
  • BrF3
  • BrO2−
Br(IV)
  • BrO2
Br(V)
  • BrF5
  • Br2O5
  • BrO3−
  • BrOF3
  • BrO2F
Br(VII)
  • BrO4−
  • BrO3F
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