The lithium chloride is a chemical compound of formula LiCl to do lighting lithium chloride, although it is difficult because the reaction is violent. In this way the anhydrous form (without water) is produced. Lithium chloride can also be extracted from other alkali metal chlorides with amyl alcohol.
Until the 1990s, the metal and lithium market was dominated by US production from mineral deposits. However, at the beginning of the 21st century, most of the production was derived from non-US sources, with Australia, Chile and Portugal being the world's largest suppliers.
Figure 1: structure of lithium chloride.
As a curiosity to note that, although Bolivia has half of the world's lithium deposits, it is not a large producer.
The most important commercial form is lithium carbonate, Li 2 CO 3, produced from minerals or brines by several different processes.
The addition of hydrochloric acid (HCl) produces lithium chloride. With this method the hydrated compound (water bound to the molecule) is produced. The hydrated form can be dried to the anhydrous form by heating it with hydrogen chloride gas.
Physical and chemical properties of lithium chloride
Lithium chloride is a white solid without a particular aroma and with a salty taste (National Center for Biotechnology Information, 2005). Its appearance is shown in figure 2.
Figure 2: appearance of lithium chloride.
Lithium chloride are highly hygroscopic crystals with octahedral geometry similar to that of sodium chloride. Its crystalline structure is presented in figure 3 (Winter, SF).
Figure 3: crystalline structure of lithium chloride.
Its molecular weight is 42.39 g / mol, its density is 2.068 g / mL, and its melting and boiling points are 605 ºC and 1360 ºC respectively.
The compound is very soluble in water, alcohol, ether, pyridine, and nitrobenzene (Royal Society of Chemistry, 2015).
Lithium chloride has a weak oxidizing or reducing power. However, redox reactions can still occur. Lithium chloride solutions are generally neither strongly acidic nor strongly basic.
Since it is extremely hygroscopic, lithium chloride can also absorb up to four equivalents of ammonia per mole. Aqueous lithium chloride solutions can corrode metals (LITHIUM CHLORIDE, SF).
Reactivity and hazards
Lithium chloride is a stable compound incompatible with strong oxidizing agents, strong acids, bromine trichloride, bromine trifluoride.
It is not toxic if swallowed, but due to its corrosive nature it can be irritating in contact with the skin and eyes, it can also irritate the nasal passages (National Institute for Occupational Safety and Health, 2015).
In case of contact with the eyes, check whether you are wearing contact lenses and remove them immediately.
Eyes should be flushed with running water for at least 15 minutes, keeping the eyelids open. Cold water can be used. Eye ointment should not be used.
If the chemical comes into contact with clothing, remove it as quickly as possible, protecting your own hands and body.
Place the victim under a safety shower. If the chemical accumulates on the victim's exposed skin, such as hands, the contaminated skin is gently and carefully washed with running water and non-abrasive soap.
Cold water can be used. If irritation persists, seek medical attention. Wash the contaminated clothing before using it again.
In case of inhalation, the victim should be allowed to rest in a well-ventilated area. If inhalation is severe, the victim should be evacuated to a safe area as soon as possible.
Loosen tight clothing such as a collar, belt, or tie. If it is difficult for the victim to breathe, oxygen should be administered.
If the victim is not breathing, mouth-to-mouth resuscitation is performed. Always keeping in mind that it can be dangerous for the person providing aid to give mouth-to-mouth resuscitation when the inhaled material is toxic, infectious or corrosive.
In all cases, immediate medical attention should be sought (Material Safety Data Sheet Lithium chloride, 2013).
Applications
Lithium chloride is the compound used to produce lithium metal by electrolysis. Lithium metal is produced by electrolysis of a molten mixture of lithium and potassium chlorides.
The lower melting point of the mixture (400-420 ° C or 750-790 ° F) compared to that of pure lithium chloride (610 ° C or 1130 ° F) allows for lower temperature operation of the electrolysis.
Since the voltage at which lithium chloride decomposes is less than that of potassium chloride, lithium is deposited at a purity level greater than 97 percent (Dye, 2017).
Liquid lithium chloride serves as a desiccant that can reduce humidity levels in the surrounding air by up to 15 percent.
Liquid desiccants that combine lithium chloride and calcium chloride create a substance that is cheaper than lithium chloride, but more stable than calcium chloride.
Lithium chloride cools the air quickly because the chemical contains an enormous amount of water for its weight as a solid. The substance also dries large quantities of industrial gases.
Lithium chloride is a red dye in pyrotechnic displays such as fireworks. Lithium chloride, or any water-soluble lithium-based salt, burns red when turned on.
Special pyrotechnic effects can be ignited by mixing ionic salts with flammable liquids such as methyl alcohol.
In the 1940s, lithium chloride served as a substitute for table salt, but some patients died from toxic levels of lithium.
The compound has pharmacological applications as antimaniacs, which are agents used to treat bipolar disorders or mania associated with other affective disorders.
The human body normally contains approximately 7 milligrams of lithium at any one time.
Lithium occurs naturally in plants as organisms use the substance to stimulate growth.
References
- Dye, JL (2017, January 23). Lithium (Li). Recovered from britannica: britannica.com.
- EMBL-EBI. (2009, November 23). lithium chloride. Recovered from ChEBI: ebi.ac.uk.
- LITHIUM CHLORIDE. (SF). Recovered from CAMEO: cameochemicals.noaa.gov.
- Material Safety Data Sheet Lithium chloride. (2013, May 21). Recovered from sciencelab.com.
- National Center for Biotechnology Information.. (2005, March 26). PubChem Compound Database; CID = 433294. Retrieved from PubChem.
- National Institute for Occupational Safety and Health. (2015, July 22). LITHIUM CHLORIDE. Recovered from cdc.gov.
- Winter, M. (SF). Lithium: lithium chloride. Recovered from webelements.