The lightest of the solid elements, lithium (Li) is a member of the alkali metal group, Group 1 (Ia) in the periodic table. The soft, white, and glossy metal itself, as well as a number of its alloys and compounds, is manufactured on an industrial basis.
One kind of metal that is ingested through food is lithium, which is primarily found in grains and vegetables. Small amounts of various kinds are utilized in supplements.
Although there is no solid scientific evidence to support any of these purposes, people use lithium supplements for a variety of diseases, including depression, Alzheimer’s disease, and alcohol use disorder.
in this article we discuss what lithium is, its properties and uses
What is lithium?
The word “lithos,” which means stone in Greek, is the source of the term lithium since it is found in tiny amounts in almost all rocks. By boosting the action of chemical messengers in the brain, it may aid mental illnesses.
Other processes, such as the formation of blood cells, may also require lithium. The U.S. FDA has authorized lithium carbonate and lithium citrate as prescription medications for bipolar illness.
This subject does not address these and other lithium medications. The amounts of lithium in supplements are far smaller than those in medications.
The Swedish chemist Johan August Arfwedson identified lithium as a component of the mineral petalite in 1817, and it was separated from its mineral for the first time by W.T. Brande and Sir Humphry Davy.
The name lithium is derived from the Greek word ‘lithos,’ meaning stone (Bolewski et al., 1976). Having an atomic mass of 6.941 g/mol, which means it contains three protons, three electrons, and four neutrons, lithium is the lightest metal with a density of 0.534 g/cm3.
It is highly reactive and flammable, and it tends to form hydroxides. It reacts with nitrogen, oxygen, and water vapor in the air, and it has never been found in its pure form in nature.
Li is therefore kept in an inert environment, such mineral oil or pure kerosene, or in a vacuum (Szlugaj and Bak, 2022).
Lithium (Li) is the 25th most abundant element in the Earth’s crust, with an average crustal abundance of 25 parts per million (ppm) (Taylor and McLennan, 1985).
Numerous rocks, clays, and brines contain lithium. Fig. 1 shows its place in the periodic table along with other significant characteristics.
Properties
Chemical properties
Lithium shares many of the same qualities as the more widely used alkali metals potassium and sodium. Lithium hydroxide (LiOH) and hydrogen gas are therefore produced when lithium, which floats on water, reacts strongly with it to generate strong hydroxide solutions.
In solution or solid state, lithium is the only alkali metal that does not produce the anion Li−.
Because of its chemical activity, lithium may easily shed one of its three electrons to create compounds that include the Li+ cation. The solubility of several of them varies significantly from that of the analogous compounds of the other alkali metals.
The amazing characteristic of retrograde solubility is exhibited by lithium carbonate (Li₂CO₃), which dissolves less readily in hot water than in cold.
A test for the presence of lithium is based on the fact that it and its compounds give a flame a red color. Because it interacts with the moisture in the air, it is frequently stored in mineral oil.
When creating other organic molecules, organolithium compounds—where the lithium atom is directly bonded to a carbon atom instead of existing as the Li+ ion—are helpful.
Butyl bromide (C4H9Br) reacts with metallic lithium to produce butyllithium (C4H9Li), which is used to make synthetic rubber.
Lithium shares several characteristics with alkaline-earth group elements, particularly magnesium, which has comparable atomic and ionic radii. Oxidation characteristics show this commonality, with monoxide often forming in each instance.
The Grignard reactions of organomagnesium compounds, a common synthetic process in organic chemistry, are comparable to the reactions of organolithium compounds.
There are several useful uses for the lithium compounds. When treated with water, lithium hydride (LiH), a gray crystalline solid created by the direct mixing of its component elements at high temperatures, immediately releases hydrogen.
Lithium aluminum hydride (LiAlH4), which swiftly converts aldehydes, ketones, and carboxylic esters to alcohols, is another product of its utilization.
Lithium salts, or soaps, of stearic and other fatty acids are made from lithium hydroxide (LiOH), which is often produced by reacting lithium carbonate with lime.
These soaps are frequently employed as thickeners in lubricating greases. Lithium hydroxide is also utilized as a carbon dioxide absorber and as an addition in the electrolyte of alkaline storage batteries.
Lithium bromide (LiBr) and lithium chloride (LiCl) are other chemicals of industrial importance. They create concentrated brines that are frequently used in big air conditioning and refrigeration systems because they can collect moisture from the air at a variety of temperatures.
The main application for lithium fluoride (LiF) is as a fluxing agent in glassware and enamels.
Nuclear properties
There are two isotopes of mass number 6 (92.5 percent) and 7 (7.5 percent) in lithium, which does not naturally display radioactivity. The ratio of lithium-7 to lithium-6 ranges from 12 to 13.
In 1932, British physicist John Cockcroft and Irish physicist Ernest Walton utilized lithium as the target metal in their groundbreaking work of transmuting nuclei by artificially accelerated atomic particles.
Each lithium nucleus that received a proton created two helium nuclei. One of the main sources of tritium generation is the slow neutron bombardment of lithium-6, which yields helium and tritium (3H).
Among its many applications, such as producing a radioactive hydrogen isotope for biological study, tritium is used in the production of hydrogen bombs. For high power-density nuclear reactors, lithium has potential as a heat-transfer fluid.
The more common stable isotope, lithium-7, has a low nuclear cross section (i.e., it absorbs neutrons very poorly) and can therefore be used as a primary coolant for nuclear reactors that require coolant temperatures above approximately 800 °C (1,500 °F).
The isotopes lithium-8 (half-life 0.855 second) and lithium-9 (half-life 0.17 second) have been created by nuclear bombardment.
Biological properties
Animals have a broad, although low-level, distribution of lithium due to the ubiquitous presence of lithium in plants. When taken into the body, lithium salts have a variety of complicated consequences.
Even very high concentrations may be lethal, they are not very poisonous. In the late 19th century, lithium salts and mineral water containing them were used to cure gout (ineffectively) and prevent depression (ineffectively).
However, in the early 20th century, they were discredited in the medical community. In 1954, it was scientifically shown that lithium carbonate could be used to treat manic-depression, often referred to as bipolar disorder.
Although lithium’s clearance was long delayed due to concerns about its toxicity, it is now the most widely used medication for treating manic episodes and bipolar patients’ maintenance therapy.
Uses
Lithium is a crucial mineral for the energy transition, used in the production of rechargeable batteries for electronic devices like electric cars and grid storage.
The rising demand for lithium-ion batteries has sparked new lithium projects, with batteries accounting for over 87% of total demand in 2023.
Additionally, lithium enhances the strength, corrosion resistance, and thermal resistance of glass items, reducing energy use and productivity. Achieving net-zero emissions requires increased reliance on lithium for battery production.
The most common industrial uses for lithium metal are in metallurgy, where the active element is utilized as a scavenger (impurity remover) in the refining of metals such as iron, nickel, copper, and zinc, as well as their alloys.
Lithium scavenges a wide range of nonmetallic elements, including as oxygen, hydrogen, nitrogen, carbon, sulfur, and halogens. Lithium is used extensively in organic synthesis, both in laboratory and commercial settings.
n-Butyllithium, C₄H₉Li, is a crucial reagent that is commercially manufactured in huge quantities. It is mostly used commercially as a polymerization initiator, such as in the creation of synthetic rubber.
It is also widely utilized in the manufacture of various organic compounds, particularly medicines.
Because of its light weight and high negative electrochemical potential, lithium metal, whether pure or in the presence of additional elements, is used as the anode (negative electrode) in many nonrechargeable lithium primary batteries.
Since the early 1990s, significant research has been conducted on high-power rechargeable lithium storage batteries for electric cars and power storage.
The most effective of these involves separating the anode and cathode, such as LiCoO2, using a solvent-free conducting polymer that allows the lithium cation, Li+, to migrate.
Smaller rechargeable lithium batteries are widely utilized in cellphones, cameras, and other electronic devices.
Lightweight lithium-magnesium alloys and strong lithium-aluminum alloys, which are tougher than aluminum alone, have structural uses in aircraft and other sectors. Metallic lithium is utilized in the production of chemicals like lithium hydride.
FAQs
What is lithium used for?
One kind of medication called a mood stabilizer is lithium. It is used to treat mood disorders including mania, which is characterized by excessive excitement, hyperactivity, or distraction. Hypo-mania, which is less extreme than mania
What are five uses of lithium?
Medical equipment including cardiac pacemakers, lubricants for machinery, specialized glassware and ceramics, lithium-ion batteries for gadgets and electric cars, and mental health treatments for bipolar illness are just a few of the significant uses for lithium.
Where is lithium found?
With more than half of the world’s lithium production in 2023, Australia was the production leader worldwide. With around 50 million tonnes of lithium, the “lithium triangle” of Bolivia, Chile, and Argentina is thought to possess the biggest deposits.
Is lithium safe for humans?
Long-term use of lithium is usually safe. Most individuals use it without any issues for years at a time. Lithium usage over an extended period of time may result in weight gain. After taking lithium for a time, if you notice that you’re gaining weight, make an effort to eat a balanced, healthful diet.