Lithium perchlorate

Source: Wikipedia, the free encyclopedia.
Lithium perchlorate
Lithium perchlorate
The orthorhombic unit cell of lithium perchlorate under standard conditions.
__ Li+     __ Cl7+     __ O2−
Unit cell of lithium perchlorate.
Names
IUPAC name
Lithium perchlorate
Other names
Perchloric acid, lithium salt; Lithium Cloricum
Identifiers
3D model (
JSmol
)
ChemSpider
ECHA InfoCard
 100.029.307 Edit this at Wikidata
UNII
  • InChI=1S/ClHO4.Li/c2-1(3,4)5;/h(H,2,3,4,5);/q;+1/p-1 checkY
    Key: MHCFAGZWMAWTNR-UHFFFAOYSA-M checkY
  • InChI=1/ClHO4.Li/c2-1(3,4)5;/h(H,2,3,4,5);/q;+1/p-1
    Key: MHCFAGZWMAWTNR-REWHXWOFAR
  • [Li+].[O-]Cl(=O)(=O)=O
Properties
LiClO
4
Molar mass
  • 106.39 g/mol (anhydrous)
  • 160.44 g/mol (trihydrate)
Appearance White crystals
Odor Odorless
Density 2.42 g/cm3
Melting point 236 °C (457 °F; 509 K)
Boiling point 430 °C (806 °F; 703 K)
decomposes from 400 °C
  • 42.7 g/100 mL (0 °C)
  • 49 g/100 mL (10 °C)
  • 59.8 g/100 mL (25 °C)
  • 71.8 g/100 mL (40 °C)
  • 119.5 g/100 mL (80 °C)
  • 300 g/100 g (120 °C)[1]
Solubility Soluble in
alcohols, ethyl acetate[1]
Solubility in acetone 137 g/100 g[1]
alcohols
Solubility in ethyl acetate 95.2 g/100 g[2]
ethyl ether
 113.7 g/100 g[2]
Structure
Pnma, No. 62
a = 865.7(1) pm, b = 691.29(9) pm, c = 483.23(6) pm[3]
4 formula per cell
tetrahedral
at Cl
Thermochemistry
105 J/mol·K[1]
125.5 J/mol·K[1]
Std enthalpy of
formation
(ΔfH⦵298)
 −380.99 kJ/mol
−254 kJ/mol[1]
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 Oxidizer, irritant
GHS labelling:
GHS03: OxidizingGHS07: Exclamation mark[4]
Danger
H272, H315, H319, H335[4]
P220, P261, P305+P351+P338[4]
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazard OX: Oxidizer. E.g. potassium perchlorate
2
0
0
OX
Safety data sheet (SDS) MSDS
Related compounds
Other anions
 Lithium chloride
Lithium hypochlorite
Lithium chlorate
Other cations
 Sodium perchlorate
Potassium perchlorate
Rubidium perchlorate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

Lithium perchlorate is the inorganic compound with the formula LiClO4. This white or colourless crystalline salt is noteworthy for its high solubility in many solvents. It exists both in anhydrous form and as a trihydrate.

Applications

Inorganic chemistry

Lithium perchlorate is used as a source of oxygen in some chemical oxygen generators. It decomposes at about 400 °C, yielding lithium chloride and oxygen:[5]

LiClO4 → LiCl + 2 O2

Over 60% of the mass of the lithium perchlorate is released as oxygen.[2] It has both the highest oxygen to weight and oxygen to volume ratio of all practical perchlorate salts, and higher oxygen to volume ratio than liquid oxygen.[6]

Lithium perchlorate is used as an

colored flame in pyrotechnic compositions.[2][7]

Organic chemistry

LiClO4 is highly soluble in organic solvents, even diethyl ether. Such solutions are employed in

Lewis acidic Li+ binds to Lewis basic sites on the dienophile, thereby accelerating the reaction.[8]

Lithium perchlorate is also used as a

co-catalyst in the coupling of α,β-unsaturated carbonyls with aldehydes, also known as the Baylis–Hillman reaction.[9]

Solid lithium perchlorate is found to be a mild and efficient Lewis acid for promoting cyanosilylation of carbonyl compounds under neutral conditions.[10]

Batteries

Lithium perchlorate is also used as an

hygroscopicity, and anodic stability properties are of importance to the specific application.[11] However, these beneficial properties are often overshadowed by the electrolyte's strong oxidizing properties, making the electrolyte reactive toward its solvent at high temperatures and/or high current loads. Due to these hazards the battery is often considered unfit for industrial applications.[11]

Biochemistry

Concentrated solutions of lithium perchlorate (4.5 mol/L) are used as a chaotropic agent to denature proteins.

Production

Lithium perchlorate can be manufactured by reaction of sodium perchlorate with lithium chloride. It can be also prepared by electrolysis of lithium chlorate at 200 mA/cm2 at temperatures above 20 °C.[12]

Safety

Perchlorates often give explosive mixtures with organic compounds, finely divided metals, sulfur, and other reducing agents.[12][2]

References

  1. ^ a b c d e f g "Lithium perchlorate". chemister.ru.
  2. ^
    US Army Materiel Command
    . October 1963. pp. 181–182.
  3. doi:10.1002/zaac.200300114
    .
  4. ^ a b c Sigma-Aldrich Co., Lithium perchlorate. Retrieved on 2014-05-09.
  5. doi:10.1021/i360012a016
    .
  6. OL 37082807M
    .
  7. LCCN 61-61759
    .
  8. doi:10.1002/047084289X
    .
  9. ^ [1] Lithium Perchlorate Product Detail Page
  10. doi:10.1016/j.jorganchem.2003.09.014
    .
  11. ^
    PMID 15669157
    . Retrieved 24 February 2014.
  12. ^
    doi:10.1002/14356007.a06_483

External links
Retrieved from "https://en.wikipedia.org/w/index.php?title=Lithium_perchlorate&oldid=1160568545"