Names | |
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IUPAC name
Zinc bromide
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Other names
Zinc(II) bromide,
Zinc dibromide | |
Identifiers | |
3D model (JSmol)
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ChemSpider | |
ECHA InfoCard | 100.028.836 |
PubChem CID
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RTECS number |
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UNII | |
CompTox Dashboard (EPA)
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Properties | |
ZnBr2 | |
Molar mass | 225.198 g/mol |
Appearance | white crystalline powder hygroscopic |
Density | 4.20 g/cm3 (20 °C) 4.22 g/cm3 (25 °C) |
Melting point | 394 °C (741 °F; 667 K) |
Boiling point | 697 °C (1,287 °F; 970 K) |
388 g/100 mL (0 °C) 675 g/100 mL (100 °C, for the anhydrous material)[1] | |
Solubility | very soluble in alcohol, ether, acetone, tetrahydrofuran |
Refractive index (nD)
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1.5452 |
Hazards | |
NFPA 704 (fire diamond) | |
Flash point | Non-flammable |
Safety data sheet (SDS) | External MSDS |
Related compounds | |
Other anions
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Zinc fluoride, Zinc chloride, Zinc iodide |
Other cations
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Cadmium bromide, Mercury(II) bromide, Calcium 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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Zinc bromide (ZnBr2) is an inorganic compound with the chemical formula ZnBr2. It is a colourless salt that shares many properties with zinc chloride (ZnCl2), namely a high solubility in water forming acidic solutions, and good solubility in organic solvents. It is hygroscopic and forms a dihydrate ZnBr2·2H2O.
ZnBr2 · 2H2O is prepared by treating zinc oxide or zinc metal with hydrobromic acid.[1]
The anhydrous material can be produced by dehydration of the dihydrate with hot CO2 or by reaction of zinc metal and bromine.[2] Sublimation in a stream of hydrogen bromide also gives the anhydrous derivative.[1]
ZnBr2 crystallizes in the same structure as ZnI2: four tetrahedral Zn centers share three vertices to form “super-tetrahedra” of nominal composition {Zn4Br10}2−, which are linked by their vertices to form a three-dimensional structure.[3] The dihydrate ZnBr2 · 2H2O can be described as ([Zn(H2O)6]2+)2([Zn2Br6]2-).[4]
Gaseous ZnBr2 is linear in accordance with VSEPR theory with a Zn-Br bond length of 221 pm.[5]
Zinc bromide is used in the following applications:[2]
Safety considerations are similar to those for zinc chloride, for which the toxic dose for humans is 3–5 g.[2]