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Names | |
---|---|
Systematic IUPAC name
Nickel(2+) diacetate | |
Identifiers | |
3D model (
JSmol)
|
|
ECHA InfoCard | 100.006.147 |
EC Number |
|
PubChem
CID
|
|
UNII |
|
CompTox Dashboard (
EPA)
|
|
| |
| |
Properties | |
C4H6NiO4 | |
Molar mass | 176.781 g·mol−1 |
Appearance | Green Solid |
Odor | slight acetic acid |
Density | 1.798 g/cm3 (anhydrous) 1.744 g/cm3 (tetrahydrate) |
Melting point | decomposes when heated [1] [2] |
Easily soluble in cold water, hot water | |
Solubility | Soluble in
methanol insoluble in diethyl ether, n-octanol |
+4,690.0·10−6 cm3/mol | |
Structure | |
monoclinic | |
P21/c | |
a = 4.764, b = 11.771, c = 8.425 Å α = 90°, β = 93.6°, γ = 90°
[3] tetrahydrate
| |
Lattice volume (V)
|
471.5 |
Formula units (Z)
|
2 |
distorted octahedral | |
Hazards | |
NFPA 704 (fire diamond) | |
Lethal dose or concentration (LD, LC): | |
LD50 (
median dose)
|
350 mg/kg (rat, oral) 410 mg/kg (mouse, oral) [4] |
Except where otherwise noted, data are given for materials in their
standard state (at 25 °C [77 °F], 100 kPa).
|
Nickel(II) acetate is the name for the coordination compounds with the formula Ni(CH3CO2)2·x H2O where x can be 0, 2, and 4. The green tetrahydrate Ni(CH3CO2)2·4 H2O is most common. It is used for electroplating.
The compound can be prepared by treating nickel or nickel(II) carbonate with acetic acid:
The green tetrahydrate has been shown by X-ray crystallography to adopt an octahedral structure, the central nickel centre being coordinated by four water molecules and two acetate ligands. [5] It may be dehydrated in vacuo, by reaction with acetic anhydride [6] or by heat. [7]
Nickel salts are carcinogenic and irritate the skin.
![]() | |
![]() | |
Names | |
---|---|
Systematic IUPAC name
Nickel(2+) diacetate | |
Identifiers | |
3D model (
JSmol)
|
|
ECHA InfoCard | 100.006.147 |
EC Number |
|
PubChem
CID
|
|
UNII |
|
CompTox Dashboard (
EPA)
|
|
| |
| |
Properties | |
C4H6NiO4 | |
Molar mass | 176.781 g·mol−1 |
Appearance | Green Solid |
Odor | slight acetic acid |
Density | 1.798 g/cm3 (anhydrous) 1.744 g/cm3 (tetrahydrate) |
Melting point | decomposes when heated [1] [2] |
Easily soluble in cold water, hot water | |
Solubility | Soluble in
methanol insoluble in diethyl ether, n-octanol |
+4,690.0·10−6 cm3/mol | |
Structure | |
monoclinic | |
P21/c | |
a = 4.764, b = 11.771, c = 8.425 Å α = 90°, β = 93.6°, γ = 90°
[3] tetrahydrate
| |
Lattice volume (V)
|
471.5 |
Formula units (Z)
|
2 |
distorted octahedral | |
Hazards | |
NFPA 704 (fire diamond) | |
Lethal dose or concentration (LD, LC): | |
LD50 (
median dose)
|
350 mg/kg (rat, oral) 410 mg/kg (mouse, oral) [4] |
Except where otherwise noted, data are given for materials in their
standard state (at 25 °C [77 °F], 100 kPa).
|
Nickel(II) acetate is the name for the coordination compounds with the formula Ni(CH3CO2)2·x H2O where x can be 0, 2, and 4. The green tetrahydrate Ni(CH3CO2)2·4 H2O is most common. It is used for electroplating.
The compound can be prepared by treating nickel or nickel(II) carbonate with acetic acid:
The green tetrahydrate has been shown by X-ray crystallography to adopt an octahedral structure, the central nickel centre being coordinated by four water molecules and two acetate ligands. [5] It may be dehydrated in vacuo, by reaction with acetic anhydride [6] or by heat. [7]
Nickel salts are carcinogenic and irritate the skin.