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词条 Nickel(II) bromide
释义

  1. Structure

  2. Reactions and Uses

  3. Safety

  4. References

{{chembox
| Verifiedfields = changed
| Watchedfields = changed
| verifiedrevid = 399230547
| ImageFile = Kristallstruktur Cadmiumiodid.png
| ImageSize = 200px
| ImageFile1 = Bromid nikelnatý.PNG
| IUPACName = Nickel(II) bromide
| OtherNames = Nickel dibromide,
Nickel bromide,
Nickelous bromide
|Section1={{Chembox Identifiers
| CASNo = 13462-88-9
| CASNo_Ref = {{cascite|correct|CAS}}
| CASNo_Comment = Anhydrous
| CASNo1_Ref = {{cascite|changed|??}}
| CASNo1 = 13596-19-5
| CASNo1_Comment = dihydrate
| CASNo2_Ref = {{cascite|changed|??}}
| CASNo2 = 7789-49-3
| CASNo2_Comment = trihydrate
| CASNo3_Ref = {{cascite|changed|??}}
| CASNo3 = 18721-96-5
| CASNo3_Comment = hexahydrate
| PubChem = 278492
| ChemSpiderID_Ref = {{chemspidercite|changed|chemspider}}
| ChemSpiderID = 24251
| SMILES = [Ni+2].[Br-].[Br-]
| StdInChI_Ref = {{stdinchicite|changed|chemspider}}
| StdInChI = 1S/2BrH.Ni/h2*1H;/q;;+2/p-2
| StdInChIKey_Ref = {{stdinchicite|changed|chemspider}}
| StdInChIKey = IPLJNQFXJUCRNH-UHFFFAOYSA-L
|Section2={{Chembox Properties
| Formula = NiBr2
| MolarMass = 218.53 g/mol
| Appearance = yellow-brown crystals
| Odor = odorless
| Density = 5.098 g/cm3[1]
| MeltingPtC = 963
| MeltingPt_notes = sublimes
| BoilingPt =
| Solubility = 113 g/100ml (0 °C)
122 g/100ml (10 °C)
134 g/100ml (25 °C)[2]
144 g/100ml (40 °C)
155 g/100ml (100 °C)
| SolubleOther = soluble in ethanol
| MagSus = +5600.0·10−6 cm3/mol
|Section3={{Chembox Hazards
| MainHazards = Irritant, corrosive
| RPhrases =
| SPhrases =
| NFPA-H = 1
| NFPA-F = 0
| NFPA-R = 0
| NFPA-S =
| FlashPt = Non-flammable
|Section8={{Chembox Related
| OtherAnions = nickel(II) fluoride
nickel(II) chloride
nickel(II) iodide
| OtherCations = cobalt(II) bromide
copper(II) bromide
palladium(II) bromide
}}

Nickel(II) bromide is the name for the inorganic compounds with the chemical formula NiBr2(H2O)x. The value of x can be 0 for the anhydrous material, as well as 2, 3, or 6 for the three known hydrate forms. The anhydrous material is a yellow-brown solid which dissolves in water or ethanol to give blue-green hexahydrate (see picture).

Structure

The structure of the nickel bromides varies with the degree of hydration. In all of these cases, the nickel(II) ion adopts an octahedral molecular geometry.

  • Anhydrous NiBr2, adopts the cadmium chloride structure.[3][4] The interatomic distance for Ni-Br is 2.52—2.58 Å.[4]
  • The structure of the trihydrate has not been confirmed by X-ray crystallography. It is assumed to adopt a chain structure.[5]
  • The di- and hexahydrates adopt structures akin to those for the corresponding chlorides. The dihydrate consists of a linear chain, whereas the hexahydrate features isolated trans-[NiBr2(H2O)4] molecules together with two noncoordinated water molecules.

Reactions and Uses

NiBr2 has Lewis acid character. NiBr2 is also used to prepare catalysts for cross-coupling reactions and various carbonylations.[3]

Empirically, NiBr2-glyme has shown increased activity compared to that of NiCl2-glyme for some transformations.[6]

Safety

Nickel(II) is toxic and suspected to be a cancer agent.[3]

References

1. ^http://chemdat.merck.de/documents/sds/emd/deu/de/8181/818174.pdf
2. ^http://chemister.ru/Database/properties-en.php?dbid=1&id=3859
3. ^1 2 {{Cite book|title=Encyclopedia of Reagents for Organic Synthesis|last=Luh|first=Tien-Yau|last2=Kuo|first2=Chi-Hong|date=2001-01-01|publisher=John Wiley & Sons, Ltd|isbn=9780470842898|language=en|doi=10.1002/047084289X.rn009}}
4. ^1 {{Cite journal|last=Wakita|first=Hisanobu|last2=Ichihashi|first2=Mitsuyoshi|last3=Mibuchi|first3=Takeharu|last4=Masuda|first4=Isao|date=1982-03-01|title=The Structure of Nickel(II) Bromide in Highly Concentrated Aqueous Solution by X-Ray Diffraction Analysis|journal=Bulletin of the Chemical Society of Japan|volume=55|issue=3|pages=817–821|doi=10.1246/bcsj.55.817|issn=0009-2673}}
5. ^DeFotis, G. C.; Goodey, J. R.; Narducci, A. A.; Welch, M. H. "NiBr2·3H2O, a lower dimensional antiferromagnet" Journal of Applied Physics (1996), 79(8, Pt. 2A), 4718-4720. {{DOI|10.1063/1.361651}}
6. ^{{Cite journal |last=Konev |first=Mikhail O. |last2=Hanna |first2=Luke E. |last3=Jarvo |first3=Elizabeth R. |date=2016-06-01 |title=Intra- and Intermolecular Nickel-Catalyzed Reductive Cross-Electrophile Coupling Reactions of Benzylic Esters with Aryl Halides |journal=Angewandte Chemie International Edition |language=en |volume=55 |issue=23 |pages=6730–6733 |doi=10.1002/anie.201601206 |pmid=27099968 }}
{{Nickel compounds}}{{bromine compounds}}

3 : Nickel compounds|Bromides|Metal halides
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