Nickel(II) chromate

Last updated
Nickel chromate
Nickel chromate.JPG
Nickel chromate formula.svg
Names
IUPAC name
Nickel(II) chromate
Other names
nickelous chromate
nickel chromate
nickel(II) chromium(VI) oxide
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.035.227 OOjs UI icon edit-ltr-progressive.svg
EC Number
  • 238-766-5
PubChem CID
  • InChI=1S/Cr.Ni.4O/q;+2;;;2*-1
    Key: QGAXAFUJMMYEPE-UHFFFAOYSA-N
  • [O-][Cr](=O)(=O)[O-].[Ni+2]
Properties
NiCrO4
Molar mass 174.71 g/mol
Appearancedark maroon-colored powder
very slightly soluble in water [1]
Solubility soluble in hydrochloric acid
Hazards
GHS labelling: [2]
GHS-pictogram-silhouette.svg GHS-pictogram-pollu.svg
Danger
H317, H334, H350i, H372, H410
P203, P233, P260, P264, P270, P271, P272, P273, P280, P284, P302+P352, P304+P340, P318, P319, P321, P333+P317, P342+P316, P362+P364, P391, P403, P405, P501
Flash point Non-flammable
Related compounds
Other anions
nickel(II) molybdate
nickel(II) tungstate
Other cations
magnesium chromate
cadmium chromate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
X mark.svgN  verify  (what is  Yes check.svgYX mark.svgN ?)

Nickel(II) chromate is an inorganic compound with the chemical formula (NiCrO4). It is red-brown in color and has a high heat tolerance. It is very slightly soluble in water and soluble in acid. It and the ions that compose it (nickel(II) and chromate) have been linked to tumor formation and gene mutation, particularly to wildlife. [3]

Contents

Synthesis

Nickel(II) chromate can be formed in the lab by heating a mixture of chromium(III) oxide and nickel oxide at between 700 °C and 800 °C under oxygen at 1000 atm pressure. It can be produced at 535 °C and 7.3 bar oxygen, but the reaction takes days to complete. [4] If the pressure is too low or temperature too high but above 660 °C, then the nickel chromium spinel NiCr2O4 forms instead. [4]

It is claimed it can be made using a hydrothermal technique. [5] [6]

Precipitates of Ni2+ ions with chromate produce a brown substance that contains water. [7]

Properties

The structure of nickel chromate is the same as for chromium vanadate, CrVO4. Crystals have an orthorhombic structure with unit cell sizes a = 5.482 Å, b = 8.237 Å, c = 6.147 Å. The cell volume is 277.6 Å3 with four formula per unit cell. [6] [8]

Nickel chromate is dark in color, unlike most other chromates which are yellow. [4] The infrared spectrum of nickel chromate show two sets of absorption bands. The first includes lines at 925, 825, and 800 cm−1 due to Cr-O stretching, and the second has lines at 430, 395, 365 (very weak) due to Cr-O rock and bend and 310 cm−1 produced from Ni-O stretching. [9]

Reactions

When heated at lower oxygen pressure around 600 °C, nickel chromate decomposes to the nickel chromite spinel, nickel oxide and oxygen. [4]

4 NiCrO4→ 2 NiCr2O4 + 2 NiO + 3 O2 (gas)

Nickel chromates can also crystallize with ligands. For instance, with 1,10-phenanthroline it can form: [7]

References

  1. ↑ Perry, Dale L. (19 April 2016). Handbook of Inorganic Compounds, Second Edition. CRC Press. p. 290. ISBN   9781439814628.
  2. ↑ PubChem. "Nickel chromate". pubchem.ncbi.nlm.nih.gov. Retrieved 2026-01-24.
  3. ↑ Eisler, R. (1998). Nickel Hazards to Fish, Wildlife, and Invertebrates: a Synoptic Review. Laurel: U.S. Geological Survey
  4. 1 2 3 4 Muller, Olaf; Roy, Rustum; White, William B. (December 1968). "Phase Equilibria in the Systems NiO-Cr2,O3,-O2, MgO-Cr2O3-O2, and CdO-Cr2,O3,-O2, at High Oxygen Pressures". Journal of the American Ceramic Society. 51 (12): 693–699. doi:10.1111/j.1151-2916.1968.tb15930.x.
  5. ↑ Brandt, Karin (1943). "X-Ray Analysis of CrVO4 and isomorphous compounds". Arkiv för Kemi, Mineralogi och Geologi. 17A (6): 1–13. (not consulted)
  6. 1 2 Muller, Olaf; White, William B.; Roy, Rustum (September 1969). "X-ray diffraction study of the chromates of nickel, magnesium and cadmium". Zeitschrift für Kristallographie. 130 (1–6): 112–120. Bibcode:1969ZK....130..112M. doi:10.1524/zkri.1969.130.1-6.112.
  7. 1 2 Bronowska, W; Staszak, Z; Daszkiewicz, M; Cieślak-Golonka, M; Wojciechowska, A (May 2002). "Systematic investigation of the [Ni2+–phen–CrO42−] system; dichromate species isolated from alkaline solutions". Polyhedron. 21 (9–10): 997–1003. doi:10.1016/S0277-5387(02)00912-9.
  8. ↑ Baran, E. J (May 1998). "Materials belonging to the CrVO4 structure type: preparation, crystal chemistry and physicochemical properties". Journal of Materials Science. 33 (10): 2479–2497. Bibcode:1998JMatS..33.2479B. doi:10.1023/A:1004380530309. S2CID   97516785.
  9. ↑ Muller, Olaf; White, William B.; Roy, Rustum (August 1969). "Infrared spectra of the chromates of magnesium, nickel and cadmium". Spectrochimica Acta Part A: Molecular Spectroscopy. 25 (8): 1491–1499. Bibcode:1969AcSpA..25.1491M. doi:10.1016/0584-8539(69)80133-9.
This page is based on this Wikipedia article
Text is available under the CC BY-SA 4.0 license; additional terms may apply.
Images, videos and audio are available under their respective licenses.