View source for Chemistry: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<br>Nickel perchlorate<br>Nickel(II) chlorate(VII)<br>Nickel diperchlorate(VII)<br>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
| Formula = Ni(ClO<sub>4</sub>)<sub>2</sub>
| MolarMass = 257.8636 g/mol (hydrate)<br>329,92472 g/mol (tetrahydrate)<br>347.94 g/mol (pentahydrate)<br>365,95528 g/mol (hexahydrate)<br>420,00112 g/mol (nonahydrate)
| Appearance = cyan crystals (hydrate)<br>long green needle-shaped crystals (pentahydrate)<ref name=atomistry>[http://nickel.atomistry.com/nickel_perchlorate.html Nickel Perchlorate, Ni(ClO<sub>4</sub>)<sub>2</sub>]</ref><br>green crystals (hexahydrate)
| Density = 2.98 g/cm³ (hydrate)<ref name=Handbook>[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.</ref><br>1,508 g/cm³ (hexahydrate)
| MeltingPtC = 140
| MeltingPt_notes = (hexahydrate)<br>{{convert|149|C|F K}} (partially decomposed pentahydrate) {{convert|103|C|F K}})
| Solubility = 259 g/100 mL (hexahydrate)<ref name=wj />
| SolubleOther = soluble in [[Chemistry:Alcohol|alcohol]], aceton<br>insoluble in [[Chemistry:Chloroform|chloroform]]<br>forming compounds with [[Chemistry:Ammonia|ammonia]], [[Chemistry:Hydrazine|hydrazine]], [[Chemistry:Urea|urea]], [[Chemistry:Semicarbazide|semicarbazide]], [[Chemistry:Carbohydrate|carbohydrate]], thioure}}
| 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}}<ref name="Sigma" />
}}
| Section8       = {{Chembox Related
| OtherAnions = Nickel perrhenate<br>Nickel nitrate
| OtherCations = [[Chemistry:Iron(II) perchlorate|Iron(II) perchlorate]]<br>[[Chemistry:Copper(II) perchlorate|Copper(II) perchlorate]]}}
}}

'''Nickel(II) perchlorate''' is a [[Chemistry:Inorganic compound|inorganic compound]] with the [[Chemistry:Chemical formula|chemical formula]] of '''Ni(ClO<sub>4</sub>)<sub>2</sub>''', and it is a strong [[Chemistry:Oxidizing agent|oxidizing agent]]. Its colours are different depending on [[Chemistry:Water|water]]. For example, the hydrate forms cyan crystals, the pentahydrate forms green crystals,<ref name=atomistry /> but the hexahydrate (Ni(ClO<sub>4</sub>)<sub>2</sub>·6H<sub>2</sub>O) forms blue crystals.<ref name=Hexahydrate />

== Preparation ==
The hexahydrate of nickel(II) perchlorate can be obtained by reacting [[Chemistry:Perchloric acid|perchloric acid]] with [[Chemistry:Nickel(II) hydroxide|nickel(II) hydroxide]], [[Chemistry:Nickel(II) chloride|nickel(II) chloride]] or [[Chemistry:Nickel(II) carbonate|nickel(II) carbonate]]:<ref name=Hexahydrate>{{citation|surname1=Daniela Sustac Roman|title=Encyclopedia of Reagents for Organic Synthesis|publisher=John Wiley & Sons, Ltd|contribution=Nickel (II) perchlorate hexahydrate|isbn=978-0-470-84289-8|date=2001-01-01|language=German
}}</ref> The resulting salt is a pentahydrate, Ni(ClO<sub>4</sub>)<sub>2</sub>·5H<sub>2</sub>O. At −21.3&nbsp;°C (251.9 K; -6.3&nbsp;°F), the nonahydrate Ni(ClO<sub>4</sub>)<sub>2</sub>·9H<sub>2</sub>O  will be formed.<ref name="atomistry">[http://nickel.atomistry.com/nickel_perchlorate.html Nickel Perchlorate, Ni(ClO<sub>4</sub>)<sub>2</sub>]</ref>

:Ni(OH)<sub>2</sub> + 2HClO<sub>4</sub> + 4H<sub>2</sub>O → Ni(ClO<sub>4</sub>)<sub>2</sub>•6H<sub>2</sub>O

Nickel(II) perchlorate can also be obtained by adding nickel to 6&nbsp;mol/L perchloric acid for electrolysis with an alternating current of 50&nbsp;Hz.<ref>郭花枝,魏建红,张美月. 交流电解制备高氯酸镍[J]. 化学世界, 1991 (12): 531–533.</ref>

The yellow [[Chemistry:Anhydrous|anhydrous]] product is obtained by adding nickel(II) trifluoroacetate and [[Chemistry:Perchloric acid|perchloric acid]] in a [[Chemistry:Trifluoroacetic acid|trifluoroacetic acid]] solvent.<ref name=wj>谢高阳 等. 无机化学丛书 锰分族 铁系 铂系. 科学出版社, 2011. pp 290. 镍(II)的卤酸盐和高卤酸盐</ref><ref name="D. Nicholls">{{citation|surname1=D. Nicholls|title=The Chemistry of Iron, Cobalt and Nickel Comprehensive Inorganic Chemistry|publisher=Elsevier|at=p.&nbsp;1131|isbn=978-1-4831-4643-0|date=2013|language=German}}</ref><ref>{{cite journal |last1=Pascal |first1=Jean-Louis |last2=Potier |first2=Jacqueline |last3=Zhang |first3=Cheng Shan |title=Chlorine trioxide, Cl2O6, a most efficient perchlorating reagent in new syntheses of anhydrous metal perchlorates, chloryl and nitryl perchloratometalates of cobalt(II), nickel(II), and copper(II). Reactivity of chlorine trioxide with anhydrous or hydrated chlorides and nitrates |journal=Journal of the Chemical Society, Dalton Transactions |date=1985 |issue=2 |pages=297 |doi=10.1039/DT9850000297}}</ref>

== Properties ==

Nickel(II) perchlorate hexahydrate is a green odourless crystalline solid that is highly [[Chemistry:Solubility|soluble]] in [[Chemistry:Water|water]] and soluble in many [[Chemistry:Organic chemistry|organic]] [[Physics:Solvent|solvent]]s.<ref name="Alfa" /> It begins to decompose from a temperature of 103&nbsp;°C. It has the hexagonal crystal structure with space group ''P''6''/mmm'' (No. 191).<ref>{{Cite web |url=http://materials.springer.com/isp/crystallographic/docs/sd_0313618 |title=Ni(ClO4)2·6H2O (Ni&#91;ClO4&#93;2&#91;H2O&#93;6 ht) Crystal Structure |publisher=Springer Materials |date=2016-07-07}}</ref> In addition to the hexahydrate, there is also a nonahydrate,<ref name="John Newton" /> a tetrahydrate,<ref name="John Newton">{{Cite book |author=John Newton |title=Cobalt, Nickel, and the Elements of the Platinum Group, Volume IX |date=1922 |isbn=978-1110346271 |url=http://library.sciencemadness.org/library/books/ATBOIC/atboic_ix_i_CoNiPt.pdf}}</ref> a hydrate<ref name=Handbook /> and a pentahydrate.<ref name=atomistry />

== Applications ==
Nickel(II) perchlorate hexahydrate is used in the manufacture of other chemical compounds.<ref name="Sigma">{{Sigma-Aldrich|aldrich|309338|Name=Nickel(II) perchlorate hexahydrate, purum p.&nbsp;a., crystallized, ≥98.0% (KT)|Abruf=2019-07-07}}</ref> For example, it is used as a starting material for homometallic trinuclear [[Chemistry:Scorpionate ligand|scorpionate]] complexes in studies of electronic and magnetic properties.<ref name="Alfa">{{Alfa|11631|Name=Nickel(II) perchlorate hexahydrate, Reagent Grade|Abruf=2016-07-07}}</ref> It also serves as a detonator in explosives.<ref name="Robert D. Morrison, Brian L. Murphy">{{citation|surname1=Robert D. Morrison, Brian L. Murphy|title=Environmental Forensics Contaminant Specific Guide|publisher=Academic Press|at=p.&nbsp;169|isbn=978-0-08-049478-4|date=2010|language=German
}}</ref>

== Other compounds ==
* Ni(ClO<sub>4</sub>)<sub>2</sub> also forms some compounds with [[Chemistry:Ammonia|NH<sub>3</sub>]], such as Ni(ClO<sub>4</sub>)<sub>2</sub>·6NH<sub>3</sub> which is a light purple crystal.<ref>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.</ref>
* Ni(ClO<sub>4</sub>)<sub>2</sub> also forms some compounds with [[Chemistry:Hydrazine|N<sub>2</sub>H<sub>4</sub>]], including Ni(ClO<sub>4</sub>)<sub>2</sub>·2N<sub>2</sub>H<sub>4</sub> as a light positive solid<ref>[http://www.sciencemadness.org/talk/viewthread.php?tid=1778&page=15 Sciencemadness Discussion Board - Exotic Primaries - Complex Salts]. Retrieved May 30, 2020.</ref> or Ni(ClO<sub>4</sub>)<sub>2</sub>·5N<sub>2</sub>H<sub>4</sub> which are purple crystals.<ref>'''(de)'''Bernhard Maissen, G. Schwarzenbach. [http://onlinelibrary.wiley.com/doi/10.1002/hlca.19510340650/full Eine Substanz von äusserster Gefährlichkeit: Hydrazinnickelperchlorat]. ''HELVETICA CHIMICA ACTA'', 1951. 34 (6): 2084–2085. doi: 10.1002/hlca.19510340650</ref>
* Ni(ClO<sub>4</sub>)<sub>2</sub> forms compounds with [[Chemistry:Urea|CO(NH<sub>2</sub>)<sub>2</sub>]], like Ni(ClO<sub>4</sub>)<sub>2</sub>·6CO(NH<sub>2</sub>)<sub>2</sub> which is a yellow-green solid.<ref>[https://www.sciencedirect.com/science/article/abs/pii/0022190266802786 Co-ordination compounds of 1,3-dimethylurea]. Retrieved May 22, 2020.</ref>
* Ni(ClO<sub>4</sub>)<sub>2</sub> forms compounds with [[Chemistry:Semicarbazide|CON<sub id="mwXA">3</sub>H<sub id="mwXQ">5</sub>]], for example Ni(ClO<sub>4</sub>)<sub>2</sub>·3CON<sub>3</sub>H<sub>5</sub> which is a blue solid.<ref>[https://books.google.com/books?id=6bgdAQAAMAAJ Soviet Journal of Coordination Chemistry, Tập 2,Phần 2] (Consultants Bureau., 1977), page 944. Retrieved November 8, 2020.</ref>
* Ni(ClO<sub>4</sub>)<sub>2</sub> forms compounds with [[Chemistry:Carbohydrazide|CON<sub id="mwaA">4</sub>H<sub id="mwaQ">6</sub>]], such as Ni(ClO<sub>4</sub>)<sub>2</sub>·3CON<sub>4</sub>H<sub>6</sub> which is an explosive blue crystal with a bulk density of 0.95 g/cm³.<ref>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}}.</ref>
* Ni(ClO<sub>4</sub>)<sub>2</sub> can also form compounds with [[Chemistry:Thiourea|CS(NH<sub id="mwdA">2</sub>)<sub id="mwdQ">2</sub>]], such as Ni(ClO<sub>4</sub>)<sub>2</sub>·6CS(NH<sub>2</sub>)<sub>2</sub> which is a pale green solid.<ref>[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.</ref>
* Ni(ClO<sub>4</sub>)<sub>2</sub> also forms some compounds with [[Chemistry:Thiosemicarbazide|CSN<sub id="mwgA">3</sub>H<sub id="mwgQ">5</sub>]], such as Ni(ClO<sub>4</sub>)<sub>2</sub>·2CSN<sub>3</sub>H<sub>5</sub>·3H<sub>2</sub>O which is a blue paramagnetic crystal<ref>Sirota, A., & Šramko, T. (1974). Square planar Ni<sup>II</sup> complexes of thiosemicarbazide. ''Inorganica Chimica Acta'' 8, 289–291. {{doi|10.1016/s0020-1693(00)92630-6}}.</ref> or Ni(ClO<sub>4</sub>)<sub>2</sub>·3CSN<sub>3</sub>H<sub>5</sub>·2H<sub>2</sub>O which is a dark positive crystal.<ref>[https://books.google.com/books?id=C0IcAQAAMAAJ Chemické Zvesti, Tập 30,Trang 1-408] (1976), page 94. Retrieved March 10, 2021.</ref>
* Ni(ClO<sub>4</sub>)<sub>2</sub> also forms some compounds with [[Chemistry:Pyridine|pyridine]].<ref name="DOI10.1107/S056774086800316X">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.&nbsp;754, {{doi|10.1107/S056774086800316X}}.</ref>

==See also==
* [[Chemistry:Nickel|Nickel]]
* [[Chemistry:Perchloric acid|Perchloric acid]]

== References ==
{{Reflist}}
<references group=""></references>
{{Nickel compounds}}

[[Category:Oxidizing agents]]
[[Category:Nickel compounds]]

{{Sourceattribution|Nickel(II) perchlorate}}