Lithium perchlorate
Crystal structure | |||||||||||||||||||
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__ Li + __ Cl 7+ __ O 2− | |||||||||||||||||||
Crystal system |
orthorhombic |
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Space group |
Pnma (No. 62) |
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Lattice parameters |
a = 8.657 Å, b = 6.912 Å, c = 4.832 Å |
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General | |||||||||||||||||||
Surname | Lithium perchlorate | ||||||||||||||||||
other names |
Perchloric acid lithium |
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Ratio formula | LiClO 4 | ||||||||||||||||||
Brief description |
white solid |
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External identifiers / databases | |||||||||||||||||||
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properties | |||||||||||||||||||
Molar mass | 106.39 g mol −1 | ||||||||||||||||||
Physical state |
firmly |
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density |
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Melting point |
236 ° C |
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boiling point |
Decomposes at 400 ° C |
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solubility | |||||||||||||||||||
safety instructions | |||||||||||||||||||
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As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions . |
Lithium perchlorate is the lithium salt of perchloric acid and, like many perchlorates, is a strong oxidizing agent at high temperatures . It is a colorless solid, easily soluble in water, alcohols and some other solvents.
Manufacturing
Lithium perchlorate can be made from perchloric acid and lithium carbonate .
properties
Lithium perchlorate crystallizes as the trihydrate LiClO 4 · 3 H 2 O in the hexagonal crystal system in the space group P 6 3 mc (space group no. 186) . The lattice parameters are a = 7.719 Å and c = 5.455 Å. At 98-100 ° C, it changes into a monohydrate LiClO 4 · H 2 O with elimination of water . The anhydrate is formed at 130 - 150 ° C, it is hygroscopic and crystallizes in the orthorhombic crystal system in the space group space group Pnma (space group no. 62) and the lattice parameters a = 8.657 Å, b = 6.912 Å and c = 4.832 Å. In the unit cell contains four formula units .
Lithium perchlorate is soluble to very well in water and polar organic solvents.
Solubility in various solvents at 25 ° C solvent water Methanol Ethanol n-propanol acetone Ethyl acetate Diethyl ether solubility in g / 100 g solvent 59.71 182.25 151.76 105.00 136.52 95.12 113.72
At 380 ° C, pure lithium perchlorate first decomposes into lithium chlorate , lithium chloride and oxygen. The lithium chlorate formed decomposes in a subsequent reaction into lithium chloride and oxygen:
The overall reaction is therefore:
Contaminated lithium perchlorate can decompose in a violent reaction below 300 ° C.
handling
Heat, open flames, strong reducing agents and flammable substances should be avoided due to the risk of explosion.
Areas of application
Lithium perchlorate is only used to a limited extent technically because it is expensive and difficult to handle. Since it is relatively soluble in many organic solvents, including ethanol and ether , it is used as an electrolyte , with its application in lithium batteries being particularly important. Another example of its use as an electrolyte in non-aqueous solutions is the production of polypyrrole , which can then also be doped with lithium perchlorate.
Since lithium perchlorate in all previously known perchlorates having the lowest mass-to-volume ratio of oxygen, it is in the air and space travel estimated as an oxygen carrier.
Individual evidence
- ↑ a b c M. S. Wickleder: Crystal Structure of LiClO 4 in Zeitschrift für inorganic und Allgemeine Chemie , 2003 , 629 (9), pp. 1466-1468. doi : 10.1002 / zaac.200300114 .
- ↑ a b c d e data sheet Lithium perchlorate, anhydrous at AlfaAesar, accessed on December 15, 2010 ( PDF )(JavaScript required) .
- ↑ Data sheet Lithium perchlorate trihydrate (PDF) from Strem, accessed on May 14, 2017.
- ↑ Entry on lithium perchlorate. In: Römpp Online . Georg Thieme Verlag, accessed on July 15, 2014.
- ↑ Dimethyl Sulfoxide (DMSO) Solubility Data. Gaylord Chemical Company, LLC; Bulletin 102, June 2014, p. 14. (PDF)
- ↑ a b data sheet Lithium perchlorate from Sigma-Aldrich , accessed on October 22, 2016 ( PDF ).
- ↑ a b c R. Abegg, F. Auerbach, I. Koppel: Handbook of inorganic chemistry . Verlag S. Hirzel, 1908, 2nd volume, 1st part, p. 137. Full text
- ^ A. Sequeira, I. Bernal, ID Brown, R. Faggiani: "The Structure of Lithium Perhclorate Trihydrate Li (H 2 O) 3 ClO 4 - an X-ray and Neutron Diffraction Study" in Acta Cryst. 1975 , B31 , p. 1735. doi : 10.1107 / S0567740875006000 .
- ↑ a b Long, JR: Perchlorate safety: Reconciling inorganic and organic guidelines in Chem. Health Safety 9 (2002) 12-18, doi : 10.1016 / S1074-9098 (02) 00294-0 .
- ↑ Willard, HH; Smith, GF: The Perchlorates of the Alkali and Alkaline Earth Metals and Ammonium. Their Solubility in Water and Other Solvents in J. Am. Chem. Soc. 45 (1923) 286-297, doi : 10.1021 / ja01655a004 .