Lithium, a light element that originated shortly after the Big Bang and occupies the third position (Atomic Number 3) in the periodic table, is predominantly known for its use in lithium-ion batteries. Yet, this critical metal is utilized across a wide range of industries and is far more pervasive than generally assumed. Understanding its properties is the first step in appreciating its far-reaching impact.
Properties of Lithium
Lithium is an alkali metal belonging to Group 1 (or 1A) of the periodic table, possessing an atomic number of 3. Some of its physical and chemical properties are presented in the table below.
| Period | 2 |
| Block | s |
| Physical State(20 degrees) | Solid |
| Electron Configuration | [He] 2s1 |
| Melting Point | 453.65 K |
| Boiling Point | 1615 K |
| Density | 0.534 g/cm3 |
| Atomic Mass | 6.94 |
| Key Isotope | Li7 |
| Metallic Radius | 152 pm |
Lithium is a soft, silvery-white, and lightweight element. It reacts readily with water and produces a crimson flame when burned. Lithium can form organometallic compounds and differs slightly in character from the other alkali metals, exhibiting a more covalent nature.
Discovery of Lithium
The history of lithium spans over two centuries. In the 1790s, the Brazilian scientist, poet, and statesman José Bonifácio de Andrada e Silva discovered two new minerals—petalite and spodumene—on the island of Utö in Sweden. This finding, made during a European expedition, crucially laid the groundwork for the eventual identification of lithium. The element was officially discovered and named in 1817 by Johan August Arfvedson (1792–1841) in Stockholm. It was during his analysis of petalite that Arfvedson first realized the mineral contained a previously unknown metallic element. He named the element lithium, drawing from the Greek word lithos, meaning ‘stone.’ The following year, in 1818, he formally announced his discovery, classifying lithium as an alkali metal similar to sodium. Shortly thereafter, he identified another lithium-bearing mineral, lepidolite.
Johan August Arfvedson
lepidolite
spodumene
Despite its status as an alkali metal, lithium resisted isolation via the standard electrolytic methods used for sodium and potassium. Even Arfvedson’s colleague, William Brande, was unable to obtain a sufficient quantity to study its physical properties. Although the renowned chemist Humphry Davy managed to isolate a minute quantity, this amount remained insufficient to fully characterize the element’s nature.
The breakthrough did not occur until 1855, when German chemist Robert Bunsen and British scientist Augustus Matthiessen, working independently, finally succeeded in isolating the element by electrolyzing molten lithium chloride.
Following its discovery, lithium was quickly found to occur naturally in mineral springs, often associated with other minerals. By 1859, its widespread presence in nature was further confirmed when it was detected in seawater using a spectroscope.
Applications of Lithium
Lithium is utilized in various industries and in multiple forms, reflecting its remarkable versatility.
- Lithium carbonate is used in the treatment of bipolar disorder (manic depression).
- Lithium stearate serves as a lubricant in the automotive industry.
- Due to its light weight, lithium is incorporated into aircraft wings and spacecraft structures.
- It is employed in glass and ceramics manufacturing.
- It also plays a role in hydrogen gas storage.
- Most importantly, lithium is used in batteries and rechargeable cells. This is due to its low density and exceptionally high electrochemical potential—the highest among all elements. Furthermore, lithium-based reactions are reversible, enabling rechargeable functionality. These properties have made lithium the ideal candidate for modern battery technologies.
The Japanese chemist Akira Yoshino revolutionized energy storage by developing a safe and stable lithium-ion battery, ushering in a new technological era and earning the Nobel Prize for his groundbreaking achievement.
Akira Yoshino Source: Wikipedia
Fun Fact 1: In thermonuclear weapons (hydrogen bombs), lithium is used in the form of the lithium-6 isotope, serving as a deuterium reservoir. The heat generated during detonation converts the lithium-6 into tritium and deuterium (heavy hydrogen), and these isotopes then undergo fusion, releasing immense amounts of energy.
Fun Fact 2: In 1929, Charles Leiper Grigg introduced a lemon-flavored soda containing lithium, claiming the drink could improve the consumer’s mood.
A Cosmic Element
Alongside hydrogen and helium, lithium was formed shortly after the Big Bang. Despite this, it remains relatively rare in the universe. Astronomers use lithium to distinguish between brown dwarfs and red dwarfs: red dwarfs are hot enough to destroy lithium, whereas brown dwarfs are not. Thus, the presence of lithium absorption lines in a star’s spectrum indicates that the object is a brown dwarf rather than a red dwarf.
A red dwarf Source: ThePlanets.org
Production
Lithium can be extracted from minerals such as spodumene, lepidolite, and petalite. In fact, a spodumene ore weighing over ten tons has been discovered in South Dakota.
Additionally, lithium can be found in certain saline waters in the form of dissolved salts, from which it can be obtained through solar evaporation.
Although the main producers of lithium include the United States, Russia, China, Australia, Zimbabwe, and Brazil, a significant portion of the world’s lithium supply is derived from brine deposits in Chile. Today, Chile has become one of the largest producers of lithium globally.
References
- Atkins, P., Overton, T., Rourke, J., Weller, M., & Armstrong, F. (2010). Inorganic chemistry (5th ed.). Oxford University Press.
- Emsley, J. (2011). Nature’s building blocks: An A-Z guide to the elements (2nd ed.). Oxford University Press.
- ILiA, & ILiA. (2024, September 2). A Brief History of Lithium – International Lithium Association. International Lithium Association – THE VOICE OF THE LITHIUM INDUSTRY. https://lithium.org/a-brief-history-of-lithium/
