Lithium chlorate

Structural formula
General
Surname	Lithium chlorate
other names	Lithium chlorate
Molecular formula	LiClO 3
Brief description	colorless long hygroscopic needles
External identifiers / databases
CAS number 13453-71-9 (anhydrate) 36355-96-1 (hydrate) EC number 236-632-0 ECHA InfoCard 100.033.288 PubChem 23682463 Wikidata Q416502
properties
Molar mass	90.39 g mol −1
Physical state	firmly
density	1.119 g cm −3
Melting point	127.6-129 ° C
boiling point	270 ° C (decomposition)
solubility	3135 g l −1 (18 ° C) soluble in ethanol
Refractive index	1.64
safety instructions
GHS hazard labeling no classification available
As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions . Refractive index: Na-D line , 20 ° C

Lithium chlorate is the lithium salt of chloric acid and, like many chlorates, is a strong oxidizing agent at high temperatures .

Manufacturing

Lithium chlorate can be made from chloric acid and lithium carbonate .

${\displaystyle \mathrm {Li_{2}CO_{3}+2\ HClO_{3}\longrightarrow 2\ LiClO_{3}+H_{2}O+CO_{2}\uparrow } }$

The synthesis from barium chlorate and lithium sulfate has also been described.

${\displaystyle \mathrm {Li_{2}SO_{4}+Ba(ClO_{3})_{2}\longrightarrow 2\ LiClO_{3}+BaSO_{4}\downarrow } }$

properties

Lithium chlorate forms three different hydrates: a trihydrate LiClO ₃  · 3 H ₂ O, a monohydrate LiClO ₃  · H ₂ O and a quarter hydrate 4 LiClO ₃  · H ₂ O. The monohydrate changes into the quarter hydrate at 20.5 ° C transforms at 42 ° C in the anhydrate in order. This anhydrate crystallizes in the cubic crystal system .

At 270 ° C, lithium chlorate decomposes into lithium chloride and oxygen, and a side reaction is disproportionation to the next lower and the next higher oxidation level of chlorine .

${\displaystyle \mathrm {2\ LiClO_{3}\ {\xrightarrow {\Delta }}\ 2\ LiCl+3\ O_{2}\uparrow } }$

${\displaystyle \mathrm {4\ LiClO_{3}\ {\xrightarrow {\Delta }}\ LiCl+3\ LiClO_{4}} }$

use

Lithium chlorate is used as an oxidizing agent in rocket fuels .

Individual evidence

1. ↑ ^{a b c d e} Jean D'Ans, Ellen Lax: Paperback for chemists and physicists. 3. Elements, inorganic compounds and materials, minerals, Volume 3. 4. Edition, Gabler Wissenschaftsverlage, 1997, ISBN 978-3-5406-0035-0 , p. 534 ( limited preview in the Google book search).
2. ^ SS Wang, DN Bennion: The Electrochemistry of Molten Lithium Chlorate and Its Possible Use with Lithium in a Batter . In: J. Electrochem. Soc. 1983 , 130 (4), pp. 741-747. doi : 10.1149 / 1.2119796 .
3. ↑ TO Campbell, EM Kartzmark, WB MaryK: The system Sodium Chlorate - Water - Dioxane and lithium chlorate - Water - dioxane, at 25 ° . In: Canadian Journal of Chemistry . 44, 1966, pp. 935-937, doi : 10.1139 / v66-136 .
4. ↑ ^{a b c d e} R. Abegg, F. Auerbach, I. Koppel: Handbuch der inorganic Chemie . Verlag S. Hirzel, 1908, 2nd volume, 1st part, p. 136. Full text
5. ↑ This substance has either not yet been classified with regard to its hazardousness or a reliable and citable source has not yet been found.
6. ^ AN Campbell, JE Griffiths: The System Lithium Chlorate - Lithium Chloride - Water at Various Temperatures . In: Canadian Journal of Chemistry . 34, 1956, pp. 1647-1661, doi : 10.1139 / v56-213 .
7. ↑ E.-C. Koch: Special Materials in Pyrotechnics: III. Application of Lithium and its Compounds in Energetic Systems . In: Propellants, Explosives, Pyrotechnics 2004 , 29 (2). Pp. 67-80. doi : 10.1002 / prep.200400032