Anhydrous
| |
Hexahydrate
| |
Names | |
---|---|
IUPAC name
Nickel(II) bromide
| |
Other names
Nickel dibromide,
Nickel bromide, Nickelous bromide | |
Identifiers | |
| |
3D model (
JSmol)
|
|
ChemSpider | |
ECHA InfoCard | 100.033.318 |
PubChem
CID
|
|
UNII | |
CompTox Dashboard (
EPA)
|
|
| |
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Properties | |
NiBr2 | |
Molar mass | 218.53 g/mol |
Appearance | yellow-brown crystals |
Odor | odorless |
Density | 5.10 g/cm3 [1] |
Melting point | 963 °C (1,765 °F; 1,236 K) sublimes [1] |
1.13 kg/L (0 °C) 1.22 kg/L (10 °C) 1.31 kg/L (20 °C) [1] 1.44 kg/L (40 °C) 1.55 kg/L (100 °C) [2] | |
Band gap | 2.5 eV [3] |
+5600.0·10−6 cm3/mol [4] | |
Structure [5] | |
hexagonal, hR9 | |
R3m, No. 166 | |
a = 0.36998 nm, c = 1.82796 nm
| |
Formula units (Z)
|
3 |
Thermochemistry [6] | |
Std enthalpy of
formation (ΔfH⦵298) |
−212.1 kJ·mol−1 |
Hazards | |
Occupational safety and health (OHS/OSH): | |
Main hazards
|
Irritant, corrosive |
NFPA 704 (fire diamond) | |
Flash point | Non-flammable |
Related compounds | |
Other
anions
|
nickel(II) fluoride nickel(II) chloride nickel(II) iodide |
Other
cations
|
cobalt(II) bromide copper(II) bromide palladium(II) bromide |
Except where otherwise noted, data are given for materials in their
standard state (at 25 °C [77 °F], 100 kPa).
|
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 to give blue-green hexahydrate (see picture).
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. Similar structures are observed in aqueous solutions of nickel bromide. [7]
NiBr2 has Lewis acid character, as indicated by its tendency to hydrate and form adducts with a variety of other Lewis bases.
NiBr2 is also used to prepare catalysts for cross-coupling reactions and various carbonylations. [8] NiBr2-glyme shows increased activity compared to NiCl2-glyme for some transformations. [10]
This compound is a suspected carcinogen. [11]
Anhydrous
| |
Hexahydrate
| |
Names | |
---|---|
IUPAC name
Nickel(II) bromide
| |
Other names
Nickel dibromide,
Nickel bromide, Nickelous bromide | |
Identifiers | |
| |
3D model (
JSmol)
|
|
ChemSpider | |
ECHA InfoCard | 100.033.318 |
PubChem
CID
|
|
UNII | |
CompTox Dashboard (
EPA)
|
|
| |
| |
Properties | |
NiBr2 | |
Molar mass | 218.53 g/mol |
Appearance | yellow-brown crystals |
Odor | odorless |
Density | 5.10 g/cm3 [1] |
Melting point | 963 °C (1,765 °F; 1,236 K) sublimes [1] |
1.13 kg/L (0 °C) 1.22 kg/L (10 °C) 1.31 kg/L (20 °C) [1] 1.44 kg/L (40 °C) 1.55 kg/L (100 °C) [2] | |
Band gap | 2.5 eV [3] |
+5600.0·10−6 cm3/mol [4] | |
Structure [5] | |
hexagonal, hR9 | |
R3m, No. 166 | |
a = 0.36998 nm, c = 1.82796 nm
| |
Formula units (Z)
|
3 |
Thermochemistry [6] | |
Std enthalpy of
formation (ΔfH⦵298) |
−212.1 kJ·mol−1 |
Hazards | |
Occupational safety and health (OHS/OSH): | |
Main hazards
|
Irritant, corrosive |
NFPA 704 (fire diamond) | |
Flash point | Non-flammable |
Related compounds | |
Other
anions
|
nickel(II) fluoride nickel(II) chloride nickel(II) iodide |
Other
cations
|
cobalt(II) bromide copper(II) bromide palladium(II) bromide |
Except where otherwise noted, data are given for materials in their
standard state (at 25 °C [77 °F], 100 kPa).
|
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 to give blue-green hexahydrate (see picture).
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. Similar structures are observed in aqueous solutions of nickel bromide. [7]
NiBr2 has Lewis acid character, as indicated by its tendency to hydrate and form adducts with a variety of other Lewis bases.
NiBr2 is also used to prepare catalysts for cross-coupling reactions and various carbonylations. [8] NiBr2-glyme shows increased activity compared to NiCl2-glyme for some transformations. [10]
This compound is a suspected carcinogen. [11]