Nickel (II) perchlorate
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| General | ||||||||||
| Surname | Nickel (II) perchlorate | |||||||||
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| Molecular formula | Ni (ClO 4 ) 2 | |||||||||
| Brief description |
green odorless solid |
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| properties | ||||||||||
| Molar mass | 257.59 g mol −1 | |||||||||
| Physical state |
firmly |
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| density |
3.4 g cm −3 |
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| Melting point |
140 ° C (hexahydrate) |
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| solubility |
very soluble in water and soluble in many organic solvents |
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| Refractive index |
1.55 (20 ° C) |
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| As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions . Refractive index: Na-D line , 20 ° C | ||||||||||
Nickel (II) perchlorate is an inorganic chemical compound of nickel from the group of perchlorates .
Extraction and presentation
Nickel (II) perchlorate can be obtained by reacting nickel (II) trifluoroacetate and perchloric acid with trifluoroacetic acid at 25 ° C. The hexahydrate can be obtained by reacting nickel (II) hydroxide , nickel (II) chloride or nickel (II) carbonate with perchloric acid.
properties
Nickel (II) perchlorate hexahydrate is a green, odorless, crystalline solid that is very soluble in water and soluble in many organic solvents. It begins to decompose from a temperature of 103 ° C. In addition to the hexahydrate, there is also a nonahydrate and a tetrahydrate. It forms complex compounds with pyridines and other compounds. The hexahydrate has a hexagonal crystal structure with the space group P 6 / mmm (space group no. 191) .
use
Nickel (II) perchlorate hexahydrate is used to make other chemical compounds. For example, it is used as a starting material for homometallic, trinuclear scorpionate complexes in studies of electronic and magnetic properties. It also serves as a detonator in explosives.
Individual evidence
- ↑ a b c d e data sheet Nickel (II) perchlorate hexahydrate, Reagent Grade at AlfaAesar, accessed on July 7, 2016 ( PDF )(JavaScript required) .
- ↑ a b Entry on nickel (II) perchlorate in the GESTIS substance database of the IFA , accessed on July 7, 2016(JavaScript required) .
- ↑ Kurt H. Stern: High Temperature Properties and Thermal Decomposition of Inorganic Salts with Oxyanions . CRC Press, 2000, ISBN 978-1-4200-4234-4 , pp. 200 ( limited preview in Google Book Search).
- ↑ a b c data sheet Nickel (II) perchlorate hexahydrate, purum p. a., crystallized, ≥98.0% (KT) from Sigma-Aldrich , accessed on July 7, 2019 ( PDF ).
- ↑ Entry on Nickel diperchlorate in the Classification and Labeling Inventory of the European Chemicals Agency (ECHA), accessed on August 1, 2016. Manufacturers or distributors can expand the harmonized classification and labeling .
- ↑ D. Nicholls: The Chemistry of Iron, Cobalt and Nickel Comprehensive Inorganic Chemistry . Elsevier, 2013, ISBN 978-1-4831-4643-0 , pp. 1131 ( limited preview in Google Book search).
- ↑ Daniela Sustac novel: Encyclopedia of Reagents for Organic Synthesis . John Wiley & Sons, Ltd, 2001, ISBN 978-0-470-84289-8 , Nickel (II) perchlorate hexahydrate.
- ^ John Newton: Cobalt, Nickel, and the Elements of the Platinum Group, Volume IX . 1922, ISBN 978-1-110-34627-1 ( online [PDF]).
- ^ F. Madaule-Aubry, WR Busing, GM Brown: Crystal structures of complexes of nickel perchlorate with substituted pyridines. II. Tetrakis (3,4-dimethylpyridine) nickel (II) perchlorate. In: Acta Crystallographica Section B Structural Crystallography and Crystal Chemistry. 24, p. 754, doi : 10.1107 / S056774086800316X .
- ↑ Ni (ClO4) 2 · 6H2O (Ni [ClO4] 2 [H2O] 6 ht) Crystal Structure. In: Springer Materials. Retrieved July 7, 2016 .
- ^ Robert D. Morrison, Brian L. Murphy: Environmental Forensics Contaminant Specific Guide . Academic Press, 2010, ISBN 978-0-08-049478-4 , pp. 169 ( limited preview in Google Book search).