Nickel(II) perchlorate: Difference between revisions

Nickel(II) perchlorate
	; Some green nickel(II) perchlorate hexahydrate powder.
Names
	IUPAC name Nickel(II) perchlorate
	Other names Nickel diperchlorate; Nickel perchlorate; Nickel(II) chlorate(VII); Nickel diperchlorate(VII); Nickel perchlorate(VII)
Identifiers
CAS Number	13637-71-3 (hydrate) ; 13520-61-1 (hexahydrate) ;
3D model (JSmol)	Interactive image;
ChemSpider	24369;
ECHA InfoCard	100.033.735
EC Number	237-124-1;
PubChem CID	26158;
CompTox Dashboard (EPA)	DTXSID5065566 ;
	InChI InChI=1S/2ClHO4.Ni/c22-1(3,4)5;/h2(H,2,3,4,5);/q;;+2/p-2 Key: ZLQBNKOPBDZKDP-UHFFFAOYSA-L;
	SMILES [O-]Cl(=O)(=O)=O.[O-]Cl(=O)(=O)=O.[Ni+2];
Properties
Chemical formula	Cl2H12NiO14
Molar mass	365.68 g·mol−1
Density	2.98 g/cm³ (hydrate); 1,508 g/cm³ (hexahydrate)
Melting point	140 °C (284 °F; 413 K) (hexahydrate); 149 °C (300 °F; 422 K) (partially decomposed pentahydrate) 103 °C (217 °F; 376 K))
Solubility in water	259 g/100 mL (hexahydrate)
Solubility	soluble in alcohol, acetone
Hazards
	Occupational safety and health (OHS/OSH):
Main hazards	oxidization
	GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H271, H314, H317, H334, H341, H350, H360, H372, H410
Precautionary statements	P201, P260, P273, P280, P303+P361+P353, P304+P340+P310, P305+P351+P338, P308+P313, P391
Flash point	flammable
Related compounds
Other anions	Nickel perrhenate; Nickel nitrate
Other cations	Iron(II) perchlorate; Copper(II) perchlorate
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Infobox references

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Nickel(II) perchlorate is a collection of inorganic compounds with the chemical formula of 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.^[3]

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^[4]^[5] and the octahydrate.^[6] 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.^[7]

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.^[8]

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.^[9]
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.^[10]
Ni(ClO₄)₂ forms compounds with CO(NH₂)₂, like Ni(ClO₄)₂·6CO(NH₂)₂ which is a yellow-green solid.^[11]
Ni(ClO₄)₂ forms compounds with CON₃H₅, for example Ni(ClO₄)₂·3CON₃H₅ which is a blue solid.^[12]
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.^[13]
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.^[14]
Ni(ClO₄)₂ also forms some compounds with CSN₃H₅, such as Ni(ClO₄)₂·2CSN₃H₅·3H₂O which is a blue paramagnetic crystal^[15] or Ni(ClO₄)₂·3CSN₃H₅·2H₂O which is a dark positive crystal.^[16]
Ni(ClO₄)₂ also forms some compounds with pyridine.^[17]

References

^ 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.
^ Sigma-Aldrich Co., product no. {{{id}}}.
^ Daniela Sustac Roman, "Nickel (II) perchlorate hexahydrate", Encyclopedia of Reagents for Organic Synthesis, John Wiley & Sons, Ltd, doi:10.1002/047084289X.rn01550
^ Le Borgne, G.; Weigel, D. (1972). "Etude Thermogravimetrique et Structurale des Perchlorates de Nickel". Bulletin de la Société Chimique de France: 3081-3085.
^ "Ni(ClO4)2·6H2O (Ni[ClO4]2[H2O]6 ht) Crystal Structure". Springer Materials. 2016-07-07.
^ Staples, R. J.; Hatfield, T. L.; Pierce, D. T. (1998). "Crystal Structure of Hexaaquanìckel(II) Perchlorate Dihydrate, [Ni(Н₂O)_б][СIO₄]₂ 2Н₂О". Zeitschrift für Kristallographie - New Crystal Structures. 213 (1–4): 257–258. doi:10.1524/ncrs.1998.213.14.257.
^ J. Newton Friend (1922). "Cobalt, Nickel, and the Elements of the Platinum Group". In J. Newton Friend (ed.). Textbook of Inorganic Chemistry (PDF). Vol. IX, part I. ISBN 978-1110346271.
^ Pascal, Jean-Louis; Favier, Frédéric (1998). "Inorganic Perchlorato Complexes". Coordination Chemistry Reviews. 178–180: 865–902. doi:10.1016/S0010-8545(98)00102-7.
^ A Text-book Of Inorganic Chemistry Vol-x, trang 192 – [1]. Retrieved April 1, 2020.
^ Maissen, Bernhard; Schwarzenbach, G. (1951). "Eine Substanz von äusserster Gefährlichkeit: Hydrazinnickelperchlorat". Helvetica Chimica Acta (in German). 34 (6): 2084–2085. doi:10.1002/hlca.19510340650.
^ Stonestreet, Beverly C.; Bull, William E.; Williams, Randall J. (1966). "Co-ordination compounds of 1,3-dimethylurea". Journal of Inorganic and Nuclear Chemistry. 28 (9): 1895–1900. doi:10.1016/0022-1902(66)80278-6.
^ Soviet Journal of Coordination Chemistry. 2 (2): 944. 1977 https://books.google.com/books?id=6bgdAQAAMAAJ. {{cite journal}}: Missing or empty |title= (help)
^ 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.
^ Complexes of some nickel(II) salts with thiourea – Juan Costamagna. Retrieved March 4, 2021.
^ Sirota, A., & Šramko, T. (1974). Square planar Ni^II complexes of thiosemicarbazide. Inorganica Chimica Acta 8, 289–291. doi:10.1016/s0020-1693(00)92630-6.
^ Chemické Zvesti, Tập 30,Trang 1-408 (1976), page 94. Retrieved March 10, 2021.
^ 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.

[Handbook-1] 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.

[Sigma-2] Sigma-Aldrich Co., product no. {{{id}}}.

[Hexahydrate-3] Daniela Sustac Roman, "Nickel (II) perchlorate hexahydrate", Encyclopedia of Reagents for Organic Synthesis, John Wiley & Sons, Ltd, doi:10.1002/047084289X.rn01550

[4] Le Borgne, G.; Weigel, D. (1972). "Etude Thermogravimetrique et Structurale des Perchlorates de Nickel". Bulletin de la Société Chimique de France: 3081-3085.

[5] "Ni(ClO4)2·6H2O (Ni[ClO4]2[H2O]6 ht) Crystal Structure". Springer Materials. 2016-07-07.

[6] Staples, R. J.; Hatfield, T. L.; Pierce, D. T. (1998). "Crystal Structure of Hexaaquanìckel(II) Perchlorate Dihydrate, [Ni(Н₂O)_б][СIO₄]₂ 2Н₂О". Zeitschrift für Kristallographie - New Crystal Structures. 213 (1–4): 257–258. doi:10.1524/ncrs.1998.213.14.257.

[John_Newton-7] J. Newton Friend (1922). "Cobalt, Nickel, and the Elements of the Platinum Group". In J. Newton Friend (ed.). Textbook of Inorganic Chemistry (PDF). Vol. IX, part I. ISBN 978-1110346271.

[8] Pascal, Jean-Louis; Favier, Frédéric (1998). "Inorganic Perchlorato Complexes". Coordination Chemistry Reviews. 178–180: 865–902. doi:10.1016/S0010-8545(98)00102-7.

[9] A Text-book Of Inorganic Chemistry Vol-x, trang 192 – [1]. Retrieved April 1, 2020.

[10] Maissen, Bernhard; Schwarzenbach, G. (1951). "Eine Substanz von äusserster Gefährlichkeit: Hydrazinnickelperchlorat". Helvetica Chimica Acta (in German). 34 (6): 2084–2085. doi:10.1002/hlca.19510340650.

[11] Stonestreet, Beverly C.; Bull, William E.; Williams, Randall J. (1966). "Co-ordination compounds of 1,3-dimethylurea". Journal of Inorganic and Nuclear Chemistry. 28 (9): 1895–1900. doi:10.1016/0022-1902(66)80278-6.

[12] Soviet Journal of Coordination Chemistry. 2 (2): 944. 1977 https://books.google.com/books?id=6bgdAQAAMAAJ. {{cite journal}}: Missing or empty |title= (help)

[13] 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.

[14] Complexes of some nickel(II) salts with thiourea – Juan Costamagna. Retrieved March 4, 2021.

[15] Sirota, A., & Šramko, T. (1974). Square planar Ni^II complexes of thiosemicarbazide. Inorganica Chimica Acta 8, 289–291. doi:10.1016/s0020-1693(00)92630-6.

[16] Chemické Zvesti, Tập 30,Trang 1-408 (1976), page 94. Retrieved March 10, 2021.

[DOI10.1107/S056774086800316X-17] 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.

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@@ Line 1: / Line 1: @@
+{{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
@@ Line 19: / Line 21: @@
 | ChemSpiderID = 24369}}
 | Section2       = {{Chembox Properties
+| Ni = 1|Cl=2|H=12|O=14
-| Formula = Ni(ClO<sub>4</sub>)<sub>2</sub>
+| MolarMass =
-| 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)
+| 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)
-| 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>blue crystals (hexahydrate)
-| Density = 2.98 g/cm³ (hydrate)<ref name=Handbook>[https://books.google.com.vn/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)
-| Solubility = 259 g/100 mL (6 nước)<ref>'''(zh)''' 谢高阳 等. 无机化学丛书 锰分族 铁系 铂系. 科学出版社, 2011, tr. 290. 镍(II)的卤酸盐和高卤酸盐</ref>
-| SolubleOther = soluble in [[alcohol]], [[aceton]]<br>insoluble in [[chloroform]]<br>forming compounds with [[ammonia]]], [[hydrazine]], [[urea]], [ [semicarbide]], [[carbohydrate]], [[thioure]]}}
+| SolubleOther = soluble in [[Alcohol (chemistry)|alcohol]], [[acetone]]}}
 | Section3       = {{Chembox Hazards
 | MainHazards = oxidization
-| FlashPt = flammable}}
+| 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">{{Sigma-Aldrich|aldrich|309338|Name=Nickel(II) perchlorate hexahydrate, purum p.&nbsp;a., crystallized, ≥98.0% (KT)|Abruf=2019-07-07}}</ref>
+}}
 | Section8       = {{Chembox Related
-| OtherAnions = [[Nickel perrhenate]]<br>[[Nikel nitrate]]
+| OtherAnions = [[Nickel perrhenate]]<br>[[Nickel nitrate]]
-| OtherCations = [[Iron(II) perchlorate]]<br>[[Cobalt(II) perchlorate]]
+| OtherCations = [[Iron(II) perchlorate]]<br>[[Copper(II) perchlorate]]}}
-| OtherCpds = [[Perchloric acid]]}}
 }}
-'''Nikel(II) perchlorate is a inorganic compound with the chemical formula''' '''Ni(ClO<sub>4</sub>)<sub>2</sub>''', and it is a strong [[oxidizing agent]]. The hexahydrate Ni(ClO<sub>4</sub>)<sub>2</sub>·6H<sub>2</sub>O is also known.  Both substances have very good solubility in water.
+'''Nickel(II) perchlorate''' is a collection of [[inorganic compound]]s 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(ClO<sub>4</sub>)<sub>2</sub>·6H<sub>2</sub>O) forms blue crystals. Nickel(II) perchlorate hexahydrate is highly [[solubility|soluble]] in [[water]] and soluble in some polar [[organic solvent]]s.<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|doi=10.1002/047084289X.rn01550}}</ref>
 == Preparation ==
-Nickel(II) perchlorate can be obtained by reacting [[perchloric acid]] with [[nickel(II) hydroxide]] or [[nickel(II) carbonate]]. The resulting salt is a pentahydrate, Ni(ClO<sub>4</sub>)<sub>2</sub>·5H<sub>2</sub>O. At −213 °C (−351.4 °F; 60.1 K), the nonahydrate Ni(ClO<sub>4</sub>)<sub>2</sub>·9H<sub>2</sub>O  will be formed.
+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)<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
+Two hydrates have been characterized by [[X-ray crystallography]]: the hexahydrate<ref>{{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}}</ref><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> and the octahydrate.<ref>{{cite journal |doi=10.1524/ncrs.1998.213.14.257 |title=Crystal Structure of Hexaaquanìckel(II) Perchlorate Dihydrate, &#91;Ni(Н<sub>2</sub>O)<sub>б</sub>&#93;&#91;СIO<sub>4</sub>&#93;<sub>2</sub> 2Н<sub>2</sub>О |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 }}</ref> 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&nbsp;°C, a tetrahydrate, and a monohydrate.<ref name="John Newton">{{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=http://library.sciencemadness.org/library/books/ATBOIC/atboic_ix_i_CoNiPt.pdf|title=Textbook of Inorganic Chemistry}}</ref>
-Nickel(II) perchlorate can also be obtained by adding nickel to 6 mol/L perchloric acid for electrolysis with an alternating current of 50 Hz.
-The [[anhydrous]] product is obtained by adding nickel(II) trifluoroacetate and [[perchloric acid]] in a [[trifluoroacetic acid]] solvent.
+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 [[ligand]]s bridge between the Ni(II) centers.<ref>{{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 }}</ref>
 == Applications ==
-Nickel(II) perchlorate can be used to obtain other nickel compounds.
+Nickel(II) perchlorates has few practical uses.
 == Other compounds ==
+* Ni(ClO<sub>4</sub>)<sub>2</sub> also forms some compounds with [[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 [[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 or Ni(ClO<sub>4</sub>)<sub>2</sub>·5N<sub>2</sub>H<sub>4</sub> which are purple crystals.<ref>{{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}}</ref>
+* Ni(ClO<sub>4</sub>)<sub>2</sub> forms compounds with [[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>{{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}}</ref>
+* Ni(ClO<sub>4</sub>)<sub>2</sub> forms compounds with [[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>{{Cite journal |url=https://books.google.com/books?id=6bgdAQAAMAAJ |journal=Soviet Journal of Coordination Chemistry |date=1977 |volume=2 |page=944 |issue=2}}</ref>
+* Ni(ClO<sub>4</sub>)<sub>2</sub> forms compounds with [[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 [[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 [[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 [[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>
+==Further reading==
-* Ni(ClO<sub>4</sub>)<sub>2</sub> also forms some compounds with [[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.
+*{{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}}
-* Ni(ClO<sub>4</sub>)<sub>2</sub> also forms some compounds with [[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  or Ni(ClO<sub>4</sub>)<sub>2</sub>·5N<sub>2</sub>H<sub>4</sub> which are purple crystals.
-* Ni(ClO<sub>4</sub>)<sub>2</sub> forms compounds with [[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.
+==See also==
-* Ni(ClO<sub>4</sub>)<sub>2</sub> forms compounds with CON<nowiki><sub id="mwXA">3</sub></nowiki>H<nowiki><sub id="mwXQ">5</sub></nowiki>, for example Ni(ClO<sub>4</sub>)<sub>2</sub>·3CON<sub>3</sub>H<sub>5</sub> which is a blue solid.
+* [[Nickel]]
-* Ni(ClO<sub>4</sub>)<sub>2</sub> forms compounds with CON<nowiki><sub id="mwaA">4</sub></nowiki>H<nowiki><sub id="mwaQ">6</sub></nowiki>, 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 (ngày 10 tháng 9 năm 2004). {{Doi|10.1016/j.jhazmat.2004.07.001}}.</ref>
+* [[Perchloric acid]]
-* Ni(ClO<sub>4</sub>)<sub>2</sub> can also form compounds with CS(NH<nowiki><sub id="mwdA">2</sub></nowiki>)<nowiki><sub id="mwdQ">2</sub></nowiki>, such as Ni(ClO<sub>4</sub>)<sub>2</sub>·6CS(NH<sub>2</sub>)<sub>2</sub> which is a pale green solid.
-* Ni(ClO<sub>4</sub>)<sub>2</sub> also forms some compounds with CSN<nowiki><sub id="mwgA">3</sub></nowiki>H<nowiki><sub id="mwgQ">5</sub></nowiki>, 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 positive 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.
 == References ==
+{{Reflist}}
 <references group=""></references>
+{{Nickel compounds}}
+{{Perchlorates}}
 [[Category:Oxidizing agents]]
 [[Category:Nickel compounds]]

v t e Nickel compounds
Nickel(0)	Ni(CO)₄ Ni(COD)₂
Nickel(II)	NiF₂ K₂NiF₄ NiF²⁻ ₄ NiCl₂ NiCl²⁻ ₄ NiBr₂ NiBr²⁻ ₄ NiI₂ NiI²⁻ ₄ Ni(CN)₂ K₂Ni(CN)₄ Ni(SCN)₂ NiO Ni(OH)₂ NiCO₃ NiSO₄ Ni₃(PO₄)₂ NiCrO₄ NiTiO₃ NiSeO₄ NiS NiSe Ni(ClO₄)₂ Ni(NO₃)₂ Ni(NO₂)₂ Ni(NO₂)³⁻ ₅ / Ni(NO₂)⁴⁻ ₆ Ni(CO₂H)₂ C ₂₄H ₄₆NiO ₄ C ₃₆H ₇₀NiO ₄ Ni(acac)₂
Nickel(III)	NiF₃ Ni₂O₃ NiOOH
Nickel(IV)	NiF₄ K₂NiF₆ MNiO_$x$