Nickel(II) perchlorate

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]

Nickel(II) perchlorate

Nickel perchlorate hexahydrate 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) Y 13520-61-1 (hexahydrate) Y
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/c2*2-1(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] 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[2]
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

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]

Further reading

• D. Nicholls (2013), The Chemistry of Iron, Cobalt and Nickel Comprehensive Inorganic Chemistry, Elsevier, p. 1131, ISBN 978-1-4831-4643-0

See also

• Nickel
• Perchloric acid

References

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.
2. Sigma-Aldrich Co., product no. {{{id}}}.
3. Daniela Sustac Roman (2013), "Nickel (II) perchlorate hexahydrate", Encyclopedia of Reagents for Organic Synthesis, John Wiley & Sons, Ltd, doi:10.1002/047084289X.rn01550, ISBN 978-0-471-93623-7
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.
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 – . 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.
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.