| 词条 | Nickel chromate |
| 释义 |
| Verifiedfields = changed | Watchedfields = changed | verifiedrevid = 405485221 | Name = Nickel chromate | ImageFileL1 = Nickel chromate.JPG | ImageSizeL1 = | IUPACName = Nickel(II) chromate | OtherNames = nickelous chromate nickel chromate nickel(II) chromium(VI) oxide |Section1={{Chembox Identifiers | InChI = 1S/Cr.Ni.4O/q;+2;;;2*-1 | SMILES = [O-][Cr](=O)(=O)[O-].[Ni+2] | InChIKey = QGAXAFUJMMYEPE-UHFFFAOYSA-N | CASNo_Ref = {{cascite|changed|??}} | CASNo = 14721-18-7 | CASNoOther = | PubChem = 61767 | EINECS = 238-766-5 | RTECS = | ChemSpiderID_Ref = {{chemspidercite|changed|chemspider}} | ChemSpiderID = 55656 |Section2={{Chembox Properties | Formula = NiCrO4 | MolarMass = 174.71 g/mol | Appearance = dark maroon-colored powder | Density = | Solubility = very slightly soluble in water[1] | SolubleOther = soluble in hydrochloric acid | MeltingPt = | RefractIndex = |Section3={{Chembox Structure | Coordination = | CrystalStruct = |Section5={{Chembox Thermochemistry | Entropy = |Section7={{Chembox Hazards | ExternalSDS = | EUClass = | RPhrases = | SPhrases = | NFPA-H = | NFPA-F = | NFPA-R = | FlashPt = Non-flammable | LD50 = |Section8={{Chembox Related | OtherCations = magnesium chromate cadmium chromate | OtherAnions = nickel(II) moybdate nickel(II) tunstate }}Nickel (II) Chromate (NiCrO4) 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.[2] SynthesisNickel (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 1000 atmosphere's pressure of oxygen. It can be produced at 535°C and 7.3 bar oxygen, but the reaction takes days to complete.[3] If the pressure is too low or temperature too high but above 660° then the nickel chromium spinel NiCr2O4 forms instead.[3] Karin Brandt also claimed to make nickel chromate using a hydrothermal technique.[4][6] Precipitates of Ni2+ ions with chromate produce a brown substance that contains water.[7] PropertiesThe 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.[5][6] Nickel chromate is dark in colour, unlike most other chromates which are yellow.[3] 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.[7] ReactionWhen heated at lower oxygen pressure around 600°C, nickel chromate decomposes to the nickel chromite spinel, nickel oxide and oxygen.[3] 4NiCrO4 → 2NiCr2O4 + 2NiO + 3O2 (gas) RelatedNickel chromates can also crystallize with ligands [Ni(1,10-phenanthroline)CrO4•3H2O]•H2O which forms triclinic olive coloured crystals, and orange crystals of Ni(1,10-phenanthroline)3Cr2O7•3H2O and yellow powdered Ni(1,10-phenanthroline)3Cr2O7•8H2O.[8] References1. ^{{cite book|last1=Perry|first1=Dale L.|title=Handbook of Inorganic Compounds, Second Edition|publisher=CRC Press|isbn=9781439814628|page=290|url=https://books.google.com.au/books?id=SFD30BvPBhoC&pg=PA290|language=en}} {{Nickel compounds}}2. ^Eisler, R. (1998). Nickel Hazards to Fish, Wildlife, and Invertebrates: a Synoptic Review. Laurel: U.S. Geological Survey 3. ^1 2 3 {{cite journal|last1=Muller|first1=Olaf|last2=Roy|first2=Rustum|last3=White|first3=William B.|title=Phase Equilibria in the Systems NiO-Cr2,O3,-O2, MgO-Cr2O3-O2, and CdO-Cr2,O3,-O2, 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}} 4. ^{{cite journal|last1=Brandt|first1=Karin|title=X-Ray Analysis of CrVO4 and isomorphous compounds|journal=Arkiv for Kemi, Mineralogi och Geologi|date=1943|volume=17A|issue=6|pages=1-13}} (not consulted) 5. ^1 {{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}} 6. ^{{cite journal|last1=Baran|first1=E. J|title=Materials belonging to the CrVO4 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}} 7. ^{{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}} 8. ^1 {{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 [Ni2+–phen–CrO42−] 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}} 3 : Nickel compounds|Chromates|Oxidizing agents |
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