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| verifiedrevid = 329242438 |
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| Name = Nickel chromate |
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| verifiedrevid = 405485221 |
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| ImageFileL1 = Nickel chromate.JPG |
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| Name = Nickel chromate |
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| IUPACName = Nickel(II) chromate |
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| ImageFile1 = Nickel chromate.JPG |
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| OtherNames = nickelous chromate<br/>nickel chromate<br/>nickel(II) chromium(VI) oxide<br/> |
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| ImageFile2 = File:Nickel chromate formula.svg |
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| Section1 = {{Chembox Identifiers |
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| IUPACName = Nickel(II) chromate |
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| SMILES = |
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| OtherNames = nickelous chromate<br/>nickel chromate<br/>nickel(II) chromium(VI) oxide |
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| InChIKey = |
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|Section1={{Chembox Identifiers |
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| CASNo = |
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| InChI = 1S/Cr.Ni.4O/q;+2;;;2*-1 |
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| CASNo_Ref = |
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| SMILES = (=O)(=O). |
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| CASOther = |
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| InChIKey = QGAXAFUJMMYEPE-UHFFFAOYSA-N |
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| CASNo_Ref = {{cascite|changed|??}} |
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| CASNo = 14721-18-7 |
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| PubChem = 61767 |
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| EINECS = 238-766-5 |
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| Section2 = {{Chembox Properties |
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| Formula = NiCrO<sub>4</sub> |
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| ChemSpiderID_Ref = {{chemspidercite|changed|chemspider}} |
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| MolarMass = 174.71 g/mol |
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| ChemSpiderID = 55656 |
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| Appearance = rust colored powder |
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|Section2={{Chembox Properties |
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| Solubility = insoluble in water |
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| Formula = NiCrO<sub>4</sub> |
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| SolubleOther = soluble in ] |
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| MolarMass = 174.71 g/mol |
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| Appearance = dark maroon-colored powder |
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| Solubility = very slightly soluble in water<ref>{{cite book|last1=Perry|first1=Dale L.|title=Handbook of Inorganic Compounds, Second Edition|date=19 April 2016|publisher=CRC Press|isbn=9781439814628|page=290|url=https://books.google.com/books?id=SFD30BvPBhoC&pg=PA290|language=en}}</ref> |
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| Section3 = {{Chembox Structure |
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| SolubleOther = soluble in ] |
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| Section7 = {{Chembox Hazards |
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| FlashPt = Non-flammable |
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| FlashPt = Non-flammable |
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|Section8={{Chembox Related |
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| OtherCations = ]<br>] |
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'''Nickel chromate''' (NiCrO<sub>4</sub>) is a ]dish ], or ]-coloured compound. It is basic and has a high ]. It is ] in ] but highly soluble in ], forming a yellow solution. |
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'''Nickel(II) chromate''' (NiCrO<sub>4</sub>) is an acid-soluble compound, red-brown in color, with high tolerances for heat. It and the ions that compose it have been linked to tumor formation and gene mutation, particularly to wildlife.<ref>Eisler, R. (1998). Nickel Hazards to Fish, Wildlife, and Invertebrates: a Synoptic Review. Laurel: U.S. Geological Survey</ref> |
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This compound contains nickel in its +2 oxidation state. It is toxic due to the toxicity of the chromate and the nickel ions, though since it is insoluble the toxicity from both sources are diminished. |
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==Synthesis== |
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It may be formed in the lab by reaction a mixture of ] and ]s with ]: |
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Nickel(II) chromate can be formed in the lab by heating a mixture of ] and ] 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.<ref name="mull68">{{cite journal|last1=Muller|first1=Olaf|last2=Roy|first2=Rustum|last3=White|first3=William B.|title=Phase Equilibria in the Systems NiO-Cr<sub>2</sub>,O<sub>3</sub>,-O<sub>2</sub>, MgO-Cr<sub>2</sub>O<sub>3</sub>-O<sub>2</sub>, and CdO-Cr<sub>2</sub>,O<sub>3</sub>,-O<sub>2</sub>, at High Oxygen Pressures|journal=Journal of the American Ceramic Society|date=December 1968|volume=51|issue=12|pages=693–699|doi=10.1111/j.1151-2916.1968.tb15930.x}}</ref> If the pressure is too low or temperature too high but above 660 °C, then the nickel chromium ] NiCr<sub>2</sub>O<sub>4</sub> forms instead.<ref name="mull68"/> |
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: 2 NiCl<sub>2</sub> + 2 CrCl<sub>3</sub> + 10 NaOH + 3 NaClO → 2 NiCrO<sub>4</sub> + 10 NaCl + 5 H<sub>2</sub>O |
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Karin Brandt also claimed to make nickel chromate using a hydrothermal technique.<ref>{{cite journal|last1=Brandt|first1=Karin|title=X-Ray Analysis of CrVO<sub>4</sub> and isomorphous compounds|journal=Arkiv för Kemi, Mineralogi och Geologi|date=1943|volume=17A|issue=6|pages=1–13}} (not consulted)</ref><ref name=mull69/> |
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Precipitates of Ni<sup>2+</sup> ions with chromate produce a brown substance that contains water.<ref name=bron/> |
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==Properties== |
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The structure of nickel chromate is the same as for chromium vanadate, CrVO<sub>4</sub>. 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 Å<sup>3</sup> with four formula per unit cell.<ref name=mull69>{{cite journal|last1=Muller|first1=Olaf|last2=White|first2=William B.|last3=Roy|first3=Rustum|title=X-ray diffraction study of the chromates of nickel, magnesium and cadmium|journal=Zeitschrift für Kristallographie|date=September 1969|volume=130|issue=1–6|pages=112–120|doi=10.1524/zkri.1969.130.1-6.112|bibcode=1969ZK....130..112M }}</ref><ref>{{cite journal|last1=Baran|first1=E. J|title=Materials belonging to the CrVO<sub>4</sub> structure type: preparation, crystal chemistry and physicochemical properties|journal=Journal of Materials Science|date=May 1998|volume=33|issue=10|pages=2479–2497|doi=10.1023/A:1004380530309|bibcode=1998JMatS..33.2479B |s2cid=97516785|url=http://sedici.unlp.edu.ar/handle/10915/144150 }}</ref> |
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Nickel chromate is dark in colour, unlike most other chromates which are yellow.<ref name="mull68"/> The infrared spectrum of nickel chromate show two sets of absorption bands. The first includes lines at 925, 825, and 800 cm<sup>−1</sup> 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<sup>−1</sup> produced from Ni-O stretching.<ref>{{cite journal|last1=Muller|first1=Olaf|last2=White|first2=William B.|last3=Roy|first3=Rustum|title=Infrared spectra of the chromates of magnesium, nickel and cadmium|journal=Spectrochimica Acta Part A: Molecular Spectroscopy|date=August 1969|volume=25|issue=8|pages=1491–1499|doi=10.1016/0584-8539(69)80133-9|bibcode=1969AcSpA..25.1491M }}</ref> |
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==Reaction== |
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When heated at lower oxygen pressure around 600 °C, nickel chromate decomposes to the nickel chromite spinel, nickel oxide and oxygen.<ref name="mull68"/> |
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:4 NiCrO<sub>4</sub> <big>→</big> 2 NiCr<sub>2</sub>O<sub>4</sub> + 2 NiO + 3 O<sub>2</sub> (gas) |
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==Related== |
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Nickel chromates can also crystallize with ligands. For instance, with ] it can form triclinic olive-colored crystals of •H<sub>2</sub>O, orange crystals of Ni(1,10-phenanthroline)<sub>3</sub>Cr<sub>2</sub>O<sub>7</sub>•3H<sub>2</sub>O, and yellow powdered Ni(1,10-phenanthroline)<sub>3</sub>Cr<sub>2</sub>O<sub>7</sub>•8H<sub>2</sub>O.<ref name=bron>{{cite journal|last1=Bronowska|first1=W|last2=Staszak|first2=Z|last3=Daszkiewicz|first3=M|last4=Cieślak-Golonka|first4=M|last5=Wojciechowska|first5=A|title=Systematic investigation of the system; dichromate species isolated from alkaline solutions|journal=Polyhedron|date=May 2002|volume=21|issue=9–10|pages=997–1003|doi=10.1016/S0277-5387(02)00912-9}}</ref> |
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==References== |
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{{Reflist}} |
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{{Nickel compounds}} |
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{{Nickel compounds}} |
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{{Chromates and dichromates}} |
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{{inorganic-compound-stub}} |
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