Difference between revisions of "Copper(II) perchlorate"

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| Solubility = 146 g/100 ml (30 °C)
 
| Solubility = 146 g/100 ml (30 °C)
 
| SolubleOther = Soluble in [[acetic acid]], [[acetone]], [[diethyl ether]], [[ethanol]], [[methanol]]
 
| SolubleOther = Soluble in [[acetic acid]], [[acetone]], [[diethyl ether]], [[ethanol]], [[methanol]]
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| Solubility1 = 69 g/100 ml (20 °C)<ref>Справочник по растворимости. - Т.1, Кн.1. - М.-Л.: ИАН СССР, 1961 (Solubility Handbook. - T.1, Book.1. - M.-L.: IAN USSR, 1961)</ref>
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| Solubility1 = 69 g/100 ml (20 °C)<ref>Solubility Handbook. - T.1, Book.1. - M.-L.: IAN USSR, 1961 (Справочник по растворимости. - Т.1, Кн.1. - М.-Л.: ИАН СССР, 1961)</ref>
 
| Solvent1 = furfural
 
| Solvent1 = furfural
 
| VaporPressure = ~0 mmHg
 
| VaporPressure = ~0 mmHg
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   }}
 
   }}
 
}}
 
}}
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'''Copper(II) perchlorate''' is an inorganic chemical compound, a salt of [[copper]] and [[perchloric acid]]. It has the formula '''Cu(ClO<sub>4</sub>)<sub>2</sub>''', though it is more commonly encountered as hexahydrate, '''Cu(ClO<sub>4</sub>)<sub>2</sub>·6 H<sub>2</sub>O'''. Besides that a heptahydrate, tetrahydrate and dihydrate are also known.<ref name="gmelincub1">''Gmelins Handbuch der Anorganischen Chemie, Kupfer Teil B 1'', 8th edition '''1958''', p. 337-339</ref>
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'''Copper(II) perchlorate''' is an inorganic chemical compound, a salt of [[copper]] and [[perchloric acid]]. It has the formula '''Cu(ClO<sub>4</sub>)<sub>2</sub>''', though it is more commonly encountered as hexahydrate, '''Cu(ClO<sub>4</sub>)<sub>2</sub>·6 H<sub>2</sub>O'''. Besides the hexahydrate, a heptahydrate, tetrahydrate and dihydrate are also known.<ref name="gmelincub1">''Gmelins Handbuch der Anorganischen Chemie, Kupfer Teil B 1'', 8th edition '''1958''', p. 337-339</ref>
  
 
==Properties==
 
==Properties==
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: CuSO<sub>4</sub> + Ba(ClO<sub>4</sub>)<sub>2</sub> → Cu(ClO<sub>4</sub>)<sub>2</sub> + BaSO<sub>4</sub>
 
: CuSO<sub>4</sub> + Ba(ClO<sub>4</sub>)<sub>2</sub> → Cu(ClO<sub>4</sub>)<sub>2</sub> + BaSO<sub>4</sub>
  
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According to one source in literature, anhydrous copper(II) perchlorate can be prepared by [[silver perchlorate]] in [[diethyl ether]], followed by addition of copper(II)bromide. Silver bromide precipitates out of the solution, while copper(II) perchlorate can be obtained by evaporating the ether.<ref>Monnier, G.; Annales de Chimie (Cachan, France); vol. 2; (1957); p. 14 - 57 ; (from Gmelin)</ref> A different source indicates that [[copper(II) chloride]] can also be used, but no product is given.<ref>Dartiguenave, Michele; Dartiguenave, Yves; Guitard, Andre; Mari, Alain; Beauchamp, Andre L.; Polyhedron; vol. 8; (1989); p. 317 - 324</ref>
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According to one source in literature, anhydrous copper(II) perchlorate can be prepared by [[silver perchlorate]] in [[diethyl ether]], followed by addition of copper(II) bromide. [[Silver bromide]] precipitates out of the solution, while copper(II) perchlorate can be obtained by evaporating the ether.<ref>Monnier, G.; Annales de Chimie (Cachan, France); vol. 2; (1957); p. 14 - 57 ; (from Gmelin)</ref> A different source indicates that [[copper(II) chloride]] can also be used, but no product is given.<ref>Dartiguenave, Michele; Dartiguenave, Yves; Guitard, Andre; Mari, Alain; Beauchamp, Andre L.; Polyhedron; vol. 8; (1989); p. 317 - 324</ref>
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 +
: CuBr<sub>2</sub> + 2 AgClO<sub>4</sub> → Cu(ClO<sub>4</sub>)<sub>2</sub> + 2 AgBr
  
 
The anhydrous salt has also been prepared by treating basic copper carbonate with dichlorine hexoxide. The obtained chloryl salt is then decomposed in vacuum at 70 °C to obtain the anhydrous perchlorate. The product can be sublimed at 160 °C in vacuum. The anhydrous salt is very hygroscopic.<ref>F. Favier, S. Barguès, J. L. Pascal, C. Belin, M. Tillard-Charbonnel, ''J. Chem. Soc., Dalton Trans.'' '''1994''', 3119-3121 [https://doi.org/10.1039/DT9940003119 https://doi.org/10.1039/DT9940003119]</ref> Other copper salts may also be used.<ref>J.-L. Pascal, J. Potier, C. S. Zhang, ''J. Chem. Soc., Dalton Trans.'' '''1985''', 297-305, [https://doi.org/10.1039/DT9850000297 https://doi.org/10.1039/DT9850000297]</ref>
 
The anhydrous salt has also been prepared by treating basic copper carbonate with dichlorine hexoxide. The obtained chloryl salt is then decomposed in vacuum at 70 °C to obtain the anhydrous perchlorate. The product can be sublimed at 160 °C in vacuum. The anhydrous salt is very hygroscopic.<ref>F. Favier, S. Barguès, J. L. Pascal, C. Belin, M. Tillard-Charbonnel, ''J. Chem. Soc., Dalton Trans.'' '''1994''', 3119-3121 [https://doi.org/10.1039/DT9940003119 https://doi.org/10.1039/DT9940003119]</ref> Other copper salts may also be used.<ref>J.-L. Pascal, J. Potier, C. S. Zhang, ''J. Chem. Soc., Dalton Trans.'' '''1985''', 297-305, [https://doi.org/10.1039/DT9850000297 https://doi.org/10.1039/DT9850000297]</ref>
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Reaction of nitrosyl perchlorate with copper metal in dry [[acetonitrile]] is claimed to yield anhydrous copper(II) perchlorate.<ref>Ishiguro, Shin-ichi; Jeliazkova, Bojana G.; Ohtaki, Hitoshi; Bulletin of the Chemical Society of Japan; vol. 58; nb. 6; (1985); p. 1749 - 1754</ref>
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: 2 NOClO<sub>4</sub> + Cu → Cu(ClO<sub>4</sub>)<sub>2</sub> + 2 NO
  
 
==Projects==
 
==Projects==
 
*Make [[Bis(ethylenediamine)copper(II) perchlorate]]
 
*Make [[Bis(ethylenediamine)copper(II) perchlorate]]
 +
*Compound collecting
  
 
==Handling==
 
==Handling==

Latest revision as of 12:37, 18 November 2023

Copper(II) perchlorate
Copper perchlorate by Tiget.jpg
Crystals of copper(II) perchlorate hexahydrate
Names
IUPAC name
Copper(II) perchlorate
Other names
Copper diperchlorate
Cupric perchlorate
Properties
Cu(ClO4)2 (anhydrous)
Cu(ClO4)2·6 H2O (hexahydrate)
Molar mass 262.447 g/mol (anhydrous)
370.539 g/mol (hexahydrate)
Appearance Blue crystalline solid
Odor Odorless
Density 2.225 g/cm3 (25 °C)
Melting point 82 °C (180 °F; 355 K)
Boiling point 100–102 °C (212–216 °F; 373–375 K) (decomposes)
146 g/100 ml (30 °C)
Solubility Soluble in acetic acid, acetone, diethyl ether, ethanol, methanol
Solubility in furfural 69 g/100 ml (20 °C)[1]
Vapor pressure ~0 mmHg
Thermochemistry
-1,915 kJ/mol
Hazards
Safety data sheet Sigma-Aldrich (hexahydrate)
Related compounds
Related compounds
 Silver perchlorate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Copper(II) perchlorate is an inorganic chemical compound, a salt of copper and perchloric acid. It has the formula Cu(ClO4)2, though it is more commonly encountered as hexahydrate, Cu(ClO4)2·6 H2O. Besides the hexahydrate, a heptahydrate, tetrahydrate and dihydrate are also known.[2]

Properties

Chemical

Copper(II) perchlorate decomposes when heated.

Physical

Copper(II) perchlorate is a hygroscopic blueish solid, soluble in water.

Availability

Copper(II) perchlorate is sold by chemical suppliers.

Preparation

Copper(II) perchlorate can be prepared by dissolving copper(II) oxide with perchloric acid.[3]

CuO + 2 HClO4 → Cu(ClO4)2 + H2O

Basic copper carbonate has also been employed.[2] Copper metal must not be used as the reaction is claimed to be dangerous.

Another method involves repeatedly evaporating copper(II) nitrate in excess 60 % perchloric acid:[4]

Cu(NO3)2 + 2 HClO4 → Cu(ClO4)2 + 2 HNO3

If perchloric acid is not available but other perchlorate salts are, addition of aq. copper(II) sulfate to aq. barium perchlorate can work:

CuSO4 + Ba(ClO4)2 → Cu(ClO4)2 + BaSO4

According to one source in literature, anhydrous copper(II) perchlorate can be prepared by silver perchlorate in diethyl ether, followed by addition of copper(II) bromide. Silver bromide precipitates out of the solution, while copper(II) perchlorate can be obtained by evaporating the ether.[5] A different source indicates that copper(II) chloride can also be used, but no product is given.[6]

CuBr2 + 2 AgClO4 → Cu(ClO4)2 + 2 AgBr

The anhydrous salt has also been prepared by treating basic copper carbonate with dichlorine hexoxide. The obtained chloryl salt is then decomposed in vacuum at 70 °C to obtain the anhydrous perchlorate. The product can be sublimed at 160 °C in vacuum. The anhydrous salt is very hygroscopic.[7] Other copper salts may also be used.[8]

Reaction of nitrosyl perchlorate with copper metal in dry acetonitrile is claimed to yield anhydrous copper(II) perchlorate.[9]

2 NOClO4 + Cu → Cu(ClO4)2 + 2 NO

Projects

Handling

Safety

Copper(II) perchlorate is a powerful oxidizer. Perchlorates are toxic.

Storage

Should be kept in a clean bottle, away from any reducing agents or combustible materials.

Disposal

Copper(II) perchlorate should be reduced to chloride and the copper recycled.

References

  1. ↑ Solubility Handbook. - T.1, Book.1. - M.-L.: IAN USSR, 1961 (Справочник по растворимости. - Т.1, Кн.1. - М.-Л.: ИАН СССР, 1961)
  2. ↑ 2.0 2.1 Gmelins Handbuch der Anorganischen Chemie, Kupfer Teil B 1, 8th edition 1958, p. 337-339
  3. ↑ Nagy, L.; Zsikla, L.; Burger, K.; Rockenbauer, A.; Kiss, J. T.; Journal of Crystallographic and Spectroscopic Research; vol. 19; nb. 5; (1989); p. 911 - 918
  4. ↑ R. M. Caven, G. Bryce, J. Chem. Soc. 1934, 515, https://doi.org/10.1039/JR9340000514
  5. ↑ Monnier, G.; Annales de Chimie (Cachan, France); vol. 2; (1957); p. 14 - 57 ; (from Gmelin)
  6. ↑ Dartiguenave, Michele; Dartiguenave, Yves; Guitard, Andre; Mari, Alain; Beauchamp, Andre L.; Polyhedron; vol. 8; (1989); p. 317 - 324
  7. ↑ F. Favier, S. Barguès, J. L. Pascal, C. Belin, M. Tillard-Charbonnel, J. Chem. Soc., Dalton Trans. 1994, 3119-3121 https://doi.org/10.1039/DT9940003119
  8. ↑ J.-L. Pascal, J. Potier, C. S. Zhang, J. Chem. Soc., Dalton Trans. 1985, 297-305, https://doi.org/10.1039/DT9850000297
  9. ↑ Ishiguro, Shin-ichi; Jeliazkova, Bojana G.; Ohtaki, Hitoshi; Bulletin of the Chemical Society of Japan; vol. 58; nb. 6; (1985); p. 1749 - 1754

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