Mercury(II) bromide
Names | |
---|---|
IUPAC name
Mercury(II) bromide
| |
Other names
Mercuric bromide
| |
Identifiers | |
CAS Number
|
|
ECHA InfoCard | 100.029.245 |
PubChem CID
|
|
RTECS number |
|
UNII | |
CompTox Dashboard (EPA)
|
|
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) |
22 g/100 mL (25°C) | |
Solubility product (Ksp)
|
6.2×10−20[1] |
Solubility | 30 g/100 mL (25°C) ethanol |
Magnetic susceptibility (χ)
|
−94.2·10−6 cm3/mol |
Structure | |
rhombic | |
Hazards | |
EU classification (DSD) (outdated)
|
T+ (T+) N (N) |
R-phrases (outdated) | R26/27/28, R33, R50/53 |
S-phrases (outdated) | (S1/2), S13, S28, S45, S60, S61 |
NFPA 704 (fire diamond) |
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). | |
what is ?) | (|
Infobox references | |
Mercury(II) bromide or mercuric bromide is the inorganic compound with the formula HgBr2. This white solid is a laboratory reagent. Like all mercury salts, it is highly toxic.
Preparation[]
Mercury(II) bromide can be produced by reaction of metallic mercury with bromine.[2]
Reactions[]
Mercury(II) bromide is used as a reagent in the Koenigs–Knorr reaction, which forms glycoside linkages on carbohydrates.[3][4]
It is also used to test for the presence of arsenic, as recommended by the Pharmacopoeia.[5] The arsenic in the sample is first converted to arsine gas by treatment with hydrogen. Arsine reacts with mercury(II) bromide:[6]
- AsH3 + 3HgBr2 → As(HgBr)3 + 3HBr
The white mercury(II) bromide will turn yellow, brown, or black if arsenic is present in the sample.[7]
Mercury(II) bromide reacts violently with elemental indium at high temperatures[8] and, when exposed to potassium, can form shock-sensitive explosive mixtures.[9]
References[]
- ^ John Rumble (June 18, 2018). CRC Handbook of Chemistry and Physics (99 ed.). CRC Press. pp. 5–188. ISBN 1138561630.
- ^ F. Wagenknecht; R. Juza (1963). "Mercury(II) bromide". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. 2. NY, NY: Academic Press. p. 1109.
- ^ Horton, Derek (2004), Advances in Carbohydrate Chemistry and Biochemistry, Amsterdam: Elseveir Academic Press, p. 76, ISBN 0-12-007259-9, retrieved 2008-05-29
- ^ 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
- ^ Pederson, Ole (2006), Pharmaceutical Chemical Analysis, Boca Raton, Florida: CRC Press, p. 107, ISBN 0-8493-1978-1, retrieved 2008-05-29
- ^ Odegaard, Nancy; Sadongei, Alyce (2005), Old Poisons, New Problems, Rowman Altamira, p. 58, ISBN 0-7591-0515-4, retrieved 2008-05-29
- ^ 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
- ^ 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
- ^ 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
- Mercury(II) compounds
- Bromides
- Metal halides