Nickel(II) perchlorate

Last updated
Nickel(II) perchlorate
Nickel perchlorate hexahydrate 1.jpg
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
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.033.735 OOjs UI icon edit-ltr-progressive.svg
EC Number
  • 237-124-1
PubChem CID
  • InChI=1S/2ClHO4.Ni/c2*2-1(3,4)5;/h2*(H,2,3,4,5);/q;;+2/p-2
    Key: ZLQBNKOPBDZKDP-UHFFFAOYSA-L
  • [O-]Cl(=O)(=O)=O.[O-]Cl(=O)(=O)=O.[Ni+2]
Properties
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))
259 g/100 mL (hexahydrate)
Solubility soluble in alcohol, acetone
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
oxidization
GHS labelling:
GHS-pictogram-rondflam.svg GHS-pictogram-acid.svg GHS-pictogram-exclam.svg GHS-pictogram-pollu.svg
Danger
H271, H314, H317, H334, H341, H350, H360, H372, H410
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).

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]

Contents

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

Further reading

See also

Related Research Articles

<span class="mw-page-title-main">Perchloric acid</span> Chemical compound

Perchloric acid is a mineral acid with the formula HClO4. Usually found as an aqueous solution, this colorless compound is a stronger acid than sulfuric acid, nitric acid and hydrochloric acid. It is a powerful oxidizer when hot, but aqueous solutions up to approximately 70% by weight at room temperature are generally safe, only showing strong acid features and no oxidizing properties. Perchloric acid is useful for preparing perchlorate salts, especially ammonium perchlorate, an important rocket fuel component. Perchloric acid is dangerously corrosive and readily forms potentially explosive mixtures.

In chemistry, water(s) of crystallization or water(s) of hydration are water molecules that are present inside crystals. Water is often incorporated in the formation of crystals from aqueous solutions. In some contexts, water of crystallization is the total mass of water in a substance at a given temperature and is mostly present in a definite (stoichiometric) ratio. Classically, "water of crystallization" refers to water that is found in the crystalline framework of a metal complex or a salt, which is not directly bonded to the metal cation.

<span class="mw-page-title-main">Chromium(III) chloride</span> Chemical compound

Chromium(III) chloride (also called chromic chloride) is an inorganic chemical compound with the chemical formula CrCl3. It forms several hydrates with the formula CrCl3·nH2O, among which are hydrates where n can be 5 (chromium(III) chloride pentahydrate CrCl3·5H2O) or 6 (chromium(III) chloride hexahydrate CrCl3·6H2O). The anhydrous compound with the formula CrCl3 are violet crystals, while the most common form of the chromium(III) chloride are the dark green crystals of hexahydrate, CrCl3·6H2O. Chromium chlorides find use as catalysts and as precursors to dyes for wool.

<span class="mw-page-title-main">Nickel(II) chloride</span> Chemical compound

Nickel(II) chloride (or just nickel chloride) is the chemical compound NiCl2. The anhydrous salt is yellow, but the more familiar hydrate NiCl2·6H2O is green. Nickel(II) chloride, in various forms, is the most important source of nickel for chemical synthesis. The nickel chlorides are deliquescent, absorbing moisture from the air to form a solution. Nickel salts have been shown to be carcinogenic to the lungs and nasal passages in cases of long-term inhalation exposure.

<span class="mw-page-title-main">Nickel(II) iodide</span> Chemical compound

Nickel(II) iodide is an inorganic compound with the formula NiI2. This paramagnetic black solid dissolves readily in water to give bluish-green solutions, from which crystallizes the aquo complex [Ni(H2O)6]I2 (image above). This bluish-green colour is typical of hydrated nickel(II) compounds. Nickel iodides find some applications in homogeneous catalysis.

<span class="mw-page-title-main">Nickel(II) carbonate</span> Chemical compound

Nickel(II) carbonate describes one or a mixture of inorganic compounds containing nickel and carbonate. From the industrial perspective, an important nickel carbonate is basic nickel carbonate with the formula Ni4CO3(OH)6(H2O)4. Simpler carbonates, ones more likely encountered in the laboratory, are NiCO3 and its hexahydrate. All are paramagnetic green solids containing Ni2+ cations. The basic carbonate is an intermediate in the hydrometallurgical purification of nickel from its ores and is used in electroplating of nickel.

<span class="mw-page-title-main">Iron(III) nitrate</span> Chemical compound

Iron(III) nitrate, or ferric nitrate, is the name used for a series of inorganic compounds with the formula Fe(NO3)3.(H2O)n. Most common is the nonahydrate Fe(NO3)3.(H2O)9. The hydrates are all pale colored, water-soluble paramagnetic salts.

<span class="mw-page-title-main">Nickel(II) nitrate</span> Chemical compound

Nickel nitrate is the inorganic compound Ni(NO3)2 or any hydrate thereof. In the hexahydrate, the nitrate anions are not bonded to nickel. Other hydrates have also been reported: Ni(NO3)2.9H2O, Ni(NO3)2.4H2O, and Ni(NO3)2.2H2O.

<span class="mw-page-title-main">Nickel(II) sulfate</span> Chemical compound

Nickel(II) sulfate, or just nickel sulfate, usually refers to the inorganic compound with the formula NiSO4(H2O)6. This highly soluble blue green coloured salt is a common source of the Ni2+ ion for electroplating. Approximately 40,000 tonnes were produced in 2005.

<span class="mw-page-title-main">Copper(II) perchlorate</span> Chemical compound

Copper(II) perchlorate is an inorganic compound with the chemical formula Cu(ClO4)2(H2O)x. The anhydrous solid is rarely encountered but several hydrates are known. Most important is the perchlorate salt of the aquo complex copper(II) perchlorate hexahydrate, [Cu(H2O)6]2+.

<span class="mw-page-title-main">Magnesium chlorate</span> Chemical compound

Magnesium chlorate refers to inorganic compounds with the chemical formula Mg(ClO3)2(H2O)x. The anhydrous (x = 0), dihydrate (x = 2), and hexahydrate (x = 6) are known. These are thermally labile white solids. The hexahydrate has been identified on the Martian surface.

Nickel is one of the metals that can form Tutton's salts. The singly charged ion can be any of the full range of potassium, rubidium, cesium, ammonium (), or thallium. As a mineral the ammonium nickel salt, (NH4)2Ni(SO4)2 · 6 H2O, can be called nickelboussingaultite. With sodium, the double sulfate is nickelblödite Na2Ni(SO4)2 · 4 H2O from the blödite family. Nickel can be substituted by other divalent metals of similar sized to make mixtures that crystallise in the same form.

<span class="mw-page-title-main">Nickel oxyacid salts</span>

The Nickel oxyacid salts are a class of chemical compounds of nickel with an oxyacid. The compounds include a number of minerals and industrially important nickel compounds.

<span class="mw-page-title-main">Iron(II) perchlorate</span> Chemical compound

Iron(II) perchlorate is the inorganic compound with the formula Fe(ClO4)2·6H2O. A green, water-soluble solid, it is produced by the reaction of iron metal with dilute perchloric acid followed by evaporation of the solution:

<span class="mw-page-title-main">Rhodium(III) perchlorate</span> Chemical compound

Rhodium(III) perchlorate refers to the inorganic compound with the formula Rh(H2O)6(ClO4)3. It is a hygroscopic yellow solid. It is the perchlorate salt of the tricationic aquo complex [Rh(H2O)6]3+. The compound is prepared by treating hydrated rhodium(III) chloride and perchloric acid at elevated temperatures:

<span class="mw-page-title-main">Chromium(III) perchlorate</span> Chemical compound

Chromium(III) perchlorate is an inorganic compound, a salt with the chemical formula Cr(ClO4)3. It's hexahydrate Cr(ClO4)3·6H2O is a cyan solid that dissolves in water.

<span class="mw-page-title-main">Zinc perchlorate</span> Chemical compound

Zinc perchlorate is the inorganic compound with the chemical formula Zn(ClO4)2 which forms the hexahydrate.

<span class="mw-page-title-main">Cobalt(II) perchlorate</span> Chemical compound

Cobalt(II) perchlorate is an inorganic chemical compound with the formula Co(ClO4)2·nH2O (n = 0,6). The pink anhydrous and red hexahydrate forms are both hygroscopic solids.

Manganese(II) perchlorate is an inorganic chemical compound with the formula Mn(ClO4)2. It forms a white-colored anhydrous and a rose-colored hexahydrate, both of which are hygroscopic. As a perchlorate, it is a strong oxidizing agent.

<span class="mw-page-title-main">Transition metal perchlorate complexes</span> Coordination complexes with perchlorate as ligand

Transition metal perchlorate complexes are coordination complexes with one or more perchlorate ligands. Perchlorate can bind to metals through one, two, three, or all four oxygen atoms. Usually however, perchlorate is a counterion, not a ligand.

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, "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 Societe 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 NiII 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.
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