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nickel(II) perchlorate

{{Short description|Compound of nickel}}

{{Chembox

| ImageFile = Nickel_perchlorate_hexahydrate_1.jpg

| ImageName = Nickel perchlorate hexahydrate

| ImageSize = 250px

| ImageCaption = Some green nickel(II) perchlorate hexahydrate powder.

| OtherNames = Nickel diperchlorate
Nickel perchlorate
Nickel(II) chlorate(VII)
Nickel diperchlorate(VII)
Nickel perchlorate(VII)

| IUPACName = Nickel(II) perchlorate

| Section1 = {{Chembox Identifiers

| CASNo = 13637-71-3

| CASNo_Ref = {{Cascite|correct|CAS}}

| CASNo_Comment = (hydrate)

| CASNo2 = 13520-61-1

| CASNo2_Ref = {{cascite|correct|CAS}}

| CASNo2_Comment = (hexahydrate)

| PubChem = 26158

| EINECS = 237-124-1

| SMILES = [O-]Cl(=O)(=O)=O.[O-]Cl(=O)(=O)=O.[Ni+2]

| InChI = 1S/2ClHO4.Ni/c2*2-1(3,4)5;/h2*(H,2,3,4,5);/q;;+2/p-2

| InChIKey = ZLQBNKOPBDZKDP-UHFFFAOYSA-L

| ChemSpiderID = 24369}}

| Section2 = {{Chembox Properties

| Ni = 1|Cl=2|H=12|O=14

| MolarMass =

| Density = 2.98 g/cm³ (hydrate)[https://books.google.com/books?id=ROEsDwAAQBAJ&pg=PA442 Handbook…] (Pierre Villars, Karin Cenzual, Roman Gladyshevskii; Walter de Gruyter GmbH & Co KG, 24 thg 7, 2017 - 1970 pages), page 442. Retrieved February 8, 2021.
1.508 g/cm³ (hexahydrate)

| MeltingPtC = 140

| MeltingPt_notes = (hexahydrate)
{{convert|149|C|F K}} (partially decomposed pentahydrate) {{convert|103|C|F K}})

| Solubility = 259 g/100 mL (hexahydrate)

| SolubleOther = soluble in alcohol, acetone}}

| Section3 = {{Chembox Hazards

| MainHazards = oxidization

| FlashPt = flammable

| GHSPictograms = {{GHS03}}{{GHS05}}{{GHS07}}{{GHS09}}

| GHSSignalWord = Danger

| HPhrases = {{H-phrases|271|350|341|360|372|314|334|317|410}}

| PPhrases = {{P-phrases|201|260|273|280|303+361+353|304+340+310|305+351+338|308+313|391}}{{Sigma-Aldrich|aldrich|309338|Name=Nickel(II) perchlorate hexahydrate, purum p. a., crystallized, ≥98.0% (KT)|Abruf=2019-07-07}}

}}

| Section8 = {{Chembox Related

| OtherAnions = Nickel perrhenate
Nickel nitrate

| OtherCations = Iron(II) perchlorate
Copper(II) perchlorate}}

}}

Nickel(II) perchlorate is a collection of inorganic compounds with the chemical formula of {{chem2|Ni(ClO4)2(H2O)_{x}|}}. Its colors of these solids vary with the degree of hydration. For example, the hydrate forms cyan crystals, the pentahydrate forms green crystals, but the hexahydrate (Ni(ClO4)2·6H2O) forms blue crystals. Nickel(II) perchlorate hexahydrate is highly soluble in water and soluble in some polar organic solvents.{{citation|surname1=Daniela Sustac Roman|title=Encyclopedia of Reagents for Organic Synthesis|date=2013 |publisher=John Wiley & Sons, Ltd|contribution=Nickel (II) perchlorate hexahydrate|doi=10.1002/047084289X.rn01550|isbn=978-0-471-93623-7 }}

Preparation

Aqueous solutions of nickel(II) perchlorate can be obtained by treating nickel(II) hydroxide, nickel(II) chloride or nickel(II) carbonate with perchloric acid.

:Ni(OH)2 + 2HClO4 + 4H2O → Ni(ClO4)2·6H2O

Two hydrates have been characterized by X-ray crystallography: the hexahydrate{{cite journal|last1=Le Borgne|first1=G.|last2=Weigel|first2=D.|title=Etude Thermogravimetrique et Structurale des Perchlorates de Nickel|journal=Bulletin de la Société Chimique de France|year=1972|page=3081-3085}}{{Cite web |url=https://materials.springer.com/isp/crystallographic/docs/sd_0313618 |title=Ni(ClO4)2·6H2O (Ni[ClO4]2[H2O]6 ht) Crystal Structure |publisher=Springer Materials |date=2016-07-07}} and the octahydrate.{{cite journal |doi=10.1524/ncrs.1998.213.14.257 |title=Crystal Structure of Hexaaquanìckel(II) Perchlorate Dihydrate, [Ni(Н2O)б][СIO4]2 2Н2О |date=1998 |last1=Staples |first1=R. J. |last2=Hatfield |first2=T. L. |last3=Pierce |first3=D. T. |journal=Zeitschrift für Kristallographie - New Crystal Structures |volume=213 |issue=1–4 |pages=257–258 |doi-access=free }} Several other hydrates are mentioned including the pentahydrate, which is claimed to crystallize at room temperature, the nonahydrate, which is claimed to crystallize at −21.3 °C, a tetrahydrate, and a monohydrate.{{Cite book |editor=J. Newton Friend|author=J. Newton Friend|chapter=Cobalt, Nickel, and the Elements of the Platinum Group|volume=IX, part I |date=1922 |isbn=978-1110346271 |url=https://library.sciencemadness.org/library/books/ATBOIC/atboic_ix_i_CoNiPt.pdf|title=Textbook of Inorganic Chemistry}}

The yellow anhydrous product is obtained by treating nickel(II) chloride with chlorine trioxide. As deduced by X-ray crystallography, Ni resides in a distorted octahedral environment and the perchlorate ligands bridge between the Ni(II) centers.{{cite journal |doi=10.1016/S0010-8545(98)00102-7 |title=Inorganic Perchlorato Complexes |date=1998 |last1=Pascal |first1=Jean-Louis |last2=Favier |first2=Frédéric |journal=Coordination Chemistry Reviews |volume=178-180 |pages=865–902 }}

Applications

Nickel(II) perchlorates has few practical uses.

Other compounds

  • Ni(ClO4)2 also forms some compounds with NH3, such as Ni(ClO4)2·6NH3 which is a light purple crystal.A Text-book Of Inorganic Chemistry Vol-x, trang 192 – [https://archive.org/details/in.ernet.dli.2015.164237/page/n210/mode/1up]. Retrieved April 1, 2020.
  • Ni(ClO4)2 also forms some compounds with N2H4, including Ni(ClO4)2·2N2H4 as a light positive solid or Ni(ClO4)2·5N2H4 which are purple crystals.{{Cite journal |last1=Maissen |first1=Bernhard |last2=Schwarzenbach |first2=G. |date=1951 |title=Eine Substanz von äusserster Gefährlichkeit: Hydrazinnickelperchlorat |url=http://onlinelibrary.wiley.com/doi/10.1002/hlca.19510340650/full |journal=Helvetica Chimica Acta |language=German |volume=34 |issue=6 |pages=2084–2085 |doi=10.1002/hlca.19510340650|url-access=subscription }}
  • Ni(ClO4)2 forms compounds with CO(NH2)2, like Ni(ClO4)2·6CO(NH2)2 which is a yellow-green solid.{{Cite journal |last1=Stonestreet |first1=Beverly C. |last2=Bull |first2=William E. |last3=Williams |first3=Randall J. |date=1966 |title=Co-ordination compounds of 1,3-dimethylurea |url=https://linkinghub.elsevier.com/retrieve/pii/0022190266802786 |journal=Journal of Inorganic and Nuclear Chemistry |language=en |volume=28 |issue=9 |pages=1895–1900 |doi=10.1016/0022-1902(66)80278-6|url-access=subscription }}
  • Ni(ClO4)2 forms compounds with CON3H5, for example Ni(ClO4)2·3CON3H5 which is a blue solid.{{Cite journal |url=https://books.google.com/books?id=6bgdAQAAMAAJ |journal=Soviet Journal of Coordination Chemistry |date=1977 |volume=2 |page=944 |issue=2}}
  • Ni(ClO4)2 forms compounds with CON4H6, such as Ni(ClO4)2·3CON4H6 which is an explosive blue crystal with a bulk density of 0.95 g/cm³.M. B. Talawar, A. P. Agrawal, J. S. Chhabra, S. N. Asthana – Studies on lead-free initiators: synthesis, characterization and performance evaluation of transition metal complexes of carbohydrazide. J. Hazard Mater., 113 (1–3), 57–65 (September 10, 2004). {{doi|10.1016/j.jhazmat.2004.07.001}}.
  • Ni(ClO4)2 can also form compounds with CS(NH2)2, such as Ni(ClO4)2·6CS(NH2)2 which is a pale green solid.[https://www.academia.edu/18453698/Complexes_of_some_nickel_II_salts_with_thiourea Complexes of some nickel(II) salts with thiourea – Juan Costamagna]. Retrieved March 4, 2021.
  • Ni(ClO4)2 also forms some compounds with CSN3H5, such as Ni(ClO4)2·2CSN3H5·3H2O which is a blue paramagnetic crystalSirota, A., & Šramko, T. (1974). Square planar NiII complexes of thiosemicarbazide. Inorganica Chimica Acta 8, 289–291. {{doi|10.1016/s0020-1693(00)92630-6}}. or Ni(ClO4)2·3CSN3H5·2H2O which is a dark positive crystal.[https://books.google.com/books?id=C0IcAQAAMAAJ Chemické Zvesti, Tập 30,Trang 1-408] (1976), page 94. Retrieved March 10, 2021.
  • Ni(ClO4)2 also forms some compounds with pyridine.F. Madaule-Aubry, W. R. Busing, G. M. Brown: Crystal structures of complexes of nickel perchlorate with substituted pyridines. II. Tetrakis-(3,4-dimethylpyridine)nickel(II) perchlorate. In: Acta Crystallographica Section B: Structural Crystallography and Crystal Chemistry. 24, S. 754, {{doi|10.1107/S056774086800316X}}.

Further reading

  • {{citation|surname1=D. Nicholls|title=The Chemistry of Iron, Cobalt and Nickel Comprehensive Inorganic Chemistry|publisher=Elsevier|at=p. 1131|isbn=978-1-4831-4643-0|date=2013}}

See also

References

{{Reflist}}

{{Nickel compounds}}

{{Perchlorates}}

Category:Oxidizing agents

Category:Nickel compounds

Category:Perchlorates