Zinc bromide
Crystal structure | ||||||||||
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__ Zn 2+ __ Br - | ||||||||||
General | ||||||||||
Surname | Zinc bromide | |||||||||
other names |
Zinc (II) bromide |
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Ratio formula | ZnBr 2 | |||||||||
Brief description |
white, almost odorless solid |
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External identifiers / databases | ||||||||||
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properties | ||||||||||
Molar mass | 225.18 g · mol -1 | |||||||||
Physical state |
firmly |
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density |
4.2 g cm −3 (20 ° C) |
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Melting point |
394 ° C |
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boiling point |
697 ° C |
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solubility |
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safety instructions | ||||||||||
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As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions . |
Zinc bromide is a chemical compound that is mainly used in electrolysis and in the oil industry. It is the bromide of zinc .
Extraction and presentation
Zinc bromide can be obtained by reacting zinc with bromine .
Further possibilities are the reaction of barium bromide with zinc sulphate (which also forms barium sulphate ) or the reaction of hydrogen bromide with zinc:
Chemical properties
Zinc bromide is a white, almost odorless, very hygroscopic solid and a Lewis acid . The dihydrate ZnBr 2 · 2H 2 O crystallizes out from aqueous solution below 37 ° C. The real structure of the dihydrate is Zn (H 2 O) 6 Zn 2 Br 6 , with the two zinc atoms in the Zn 2 Br 6 2− anion being linked via bromine atoms.
use
Zinc bromide is often used in school experiments to demonstrate the chemical principles of electrolysis or of batteries or accumulators . It is also used as an additive in fluxes for soldering and for the production of zinc organic compounds ( zinc organyls ) by electrolysis. In medicine it can be used as a sedative .
Most of the zinc bromide produced is used in deep-sea oil drilling as a component of the displacement and reaction fluid.
safety instructions
Zinc bromide has a caustic and corrosive effect on metals.
Individual evidence
- ↑ a b c d e f g Zinc bromide data sheet (PDF) from Merck , accessed April 25, 2011.
- ↑ a b Georg Brauer (Ed.), With the collaboration of Marianne Baudler u a .: Handbook of Preparative Inorganic Chemistry. 3rd, revised edition. Volume II, Ferdinand Enke, Stuttgart 1978, ISBN 3-432-87813-3 , p. 1025.
- ↑ a b Entry on zinc bromide in the GESTIS substance database of the IFA , accessed on July 23, 2016(JavaScript required) .
- ↑ Pradyot Patnaik, 2003, Handbook of Inorganic Chemicals, McGraw-Hill Professional, ISBN 0070494398 .
- ↑ Yoffe, D .; Frim, R .; Ukeles, SD; Dagani, MJ; Barda, HJ; Benya, TJ; Sanders, DC: Bromine Compounds. In: Ullmanns Enzyklopädie der Technischen Chemie , Wiley-VCH Verlag GmbH & Co. KGaA, Weinheim 2013; doi : 10.1002 / 14356007.a04_405.pub2 .
- ↑ Duhlev, R .; Brown, ID; Faggiani, R .: Zinc bromide dihydrate ZnBr 2 · 2H 2 O: a double-salt structure in Acta Cryst. C, Cryst. Struct. Commun. 44 (1988), 1696-1698, doi : 10.1107 / S0108270188005876 , pdf .
- ↑ Martin Winter, Jürgen 0. Besenhard: Rechargeable batteries ( Memento of the original from May 17, 2013 in the Internet Archive ) Info: The archive link was inserted automatically and has not yet been checked. Please check the original and archive link according to the instructions and then remove this notice. (PDF file; 8.4 MB) . Chemistry in Our Time, 33 (5), 1999.
- ↑ data sheet at chemicalland21.com
- ↑ Viktorija Rjabova: Influence of the structure of CH-acidic nitriles on the electrochemical synthesis of organometallic complexes of copper and zinc . Dissertation, 2001.