Lithium was discovered in 1817 by Johan August Arfwedson, a young Swedish chemist working in the Stockholm laboratory of the renowned Jöns Jacob Berzelius. Arfwedson identified the new element while analyzing a mineral called petalite, which had been collected from a mine on the island of Utö in the Stockholm archipelago. The story of lithium’s discovery, though, extends well beyond that single moment in a Swedish lab. It winds through 19th-century mineral springs, a makeshift psychiatric ward in Australia, Cold War nuclear programs, and eventually the rechargeable batteries that power modern life.
Arfwedson, Berzelius, and the Petalite Mineral
In the early 19th century, Berzelius was one of the most influential chemists alive. His laboratory attracted talented young scientists, and Arfwedson was among them. When Arfwedson began analyzing petalite, a mineral first identified by the Brazilian naturalist José Bonifácio de Andrada e Silva, he noticed something unusual. After accounting for the known components of the mineral, a residue remained that did not match the behavior of sodium or potassium, the two alkali metals known at the time. Through a series of chemical tests, Arfwedson determined that this residue contained a previously unknown alkali element. Berzelius confirmed the finding and helped publicize it to the broader scientific community.
Arfwedson was only 25 years old at the time of his discovery. He went on to identify lithium in other minerals as well, including spodumene and lepidolite, showing that the element was not confined to a single geological source. Despite his pivotal contribution, Arfwedson never managed to isolate the pure metal. The technology of the day could separate lithium compounds from minerals but could not strip the element down to its metallic form.
Why It Was Named After Stone
The name “lithium” comes from the Greek word lithos, meaning stone. The choice was deliberate and tells you something about how chemists of the era thought about classification. Sodium had been found in plant ashes (its older name, “natrium,” reflects vegetable sources), and potassium had been obtained from potash, also derived from plant material. Lithium was different. It was the first alkali element to come directly from the mineral kingdom rather than from organic material.1JAMA. Notes on Lithium Naming it after stone emphasized that distinction and signaled to other chemists that the periodic table’s alkali metals had a broader geological range than anyone had assumed.
Isolating the Pure Metal
Getting lithium out of a mineral compound was one thing. Producing the actual metal was another challenge entirely. In 1821, William Thomas Brande, a British chemist, is generally credited with the first isolation of lithium metal through electrolysis of lithium oxide, though the amount he produced was tiny and impure. Humphry Davy, the legendary electrochemist who had already isolated sodium and potassium by similar methods, also produced small quantities around the same time. Neither achieved a practical yield.
Larger-scale isolation came decades later. In 1855, Robert Bunsen (of Bunsen burner fame) and Augustus Matthiessen independently used electrolysis of molten lithium chloride to produce more substantial quantities of the metal. This method, electrolysis of lithium chloride, remained the fundamental industrial process for well over a century. The metal they produced was soft, silver-white, and startlingly light. Lithium is the lightest solid element and the least dense metal, about half the density of water. If you dropped a chunk of it into a lake, it would float briefly before reacting violently with the water.
Lithium Water and 19th-Century Medicine
Almost as soon as lithium was identified, people began finding it in natural mineral springs. By the mid-1800s, physicians in Europe and North America were prescribing lithium-containing waters for a grab bag of ailments: gout, kidney stones, rheumatism, and various “nervous” conditions. The logic was partly chemical, since lithium could dissolve uric acid in a test tube, doctors reasoned it might do the same inside the body, breaking up the urate crystals responsible for gout. The reasoning was plausible but largely wrong. The concentrations of lithium in natural spring water were far too low to have meaningful therapeutic effects for most of these conditions.
That did not stop the marketing. “Lithia water” became enormously popular in the late 19th and early 20th centuries, sold under brand names at pharmacies and promoted by resorts built around lithium-containing springs. Some of these products survived well into the 20th century. The soft drink 7 Up originally contained lithium citrate when it was introduced in 1929, marketed as a mood-lifting beverage. The lithium was removed from the formula in 1948, shortly before the U.S. Food and Drug Administration began restricting its use in consumer products. By then, the lithia water craze had largely faded, dismissed as quackery. But the kernel of truth in the old claims, that lithium affects mood, was about to be rediscovered in a far more rigorous way.
John Cade and the Psychiatric Breakthrough
The most dramatic chapter in lithium’s story began in an underfunded psychiatric hospital in Bundoora, Australia. John Cade, an Australian psychiatrist, had spent years as a prisoner of war during World War II and returned to civilian medicine with a hypothesis: perhaps manic illness was caused by some excess metabolic substance circulating in the body, and perhaps depressive illness was caused by a deficiency of the same substance. He began injecting guinea pigs with urine from manic patients to see if it was more toxic than urine from other patients.
To test whether uric acid was the toxic factor, Cade needed to make it more soluble for injection. He chose lithium urate because lithium is the most soluble cation for urate salts. When he injected the guinea pigs with lithium urate, he noticed something unexpected: instead of becoming more agitated, the animals became calm and placid. Intrigued, he tested lithium carbonate alone and got the same sedating effect. The calming agent was the lithium, not the urate.
Cade then took the remarkable step of trying lithium on human patients. In 1949, he published his results, describing how lithium dramatically reduced manic symptoms in a small group of patients.2PubMed Central. The history of lithium therapy His discovery came from a logical chain of reasoning, moving from a hypothesis about metabolism to animal experiments to clinical trials, even if the original hypothesis turned out to be wrong.3PubMed. Cade’s observation of the antimanic effect of lithium and early Australian research The effect was real and reproducible: lithium worked against mania. It remains one of the most important medications in psychiatry today, used to treat bipolar disorder and reduce the risk of suicide in mood disorders.
Cade’s work was initially met with limited enthusiasm outside Australia, partly because lithium had recently been linked to several deaths in the United States. In the late 1940s, lithium chloride had been marketed as a salt substitute for patients with heart disease on sodium-restricted diets. Without proper dosing guidelines, some patients accumulated toxic levels of lithium and died. The resulting bad press made the American medical establishment wary. It took until the 1960s and 1970s, after extensive clinical research by the Danish psychiatrist Mogens Schou and others, before lithium gained widespread acceptance and regulatory approval in the U.S. and Europe.
The Cosmological Lithium Problem
Lithium has a cosmic origin story that is genuinely strange. Along with hydrogen and helium, lithium is one of only three elements created during the Big Bang. In the first few minutes after the universe began, nuclear reactions fused protons and neutrons into light nuclei, and a trace amount of lithium-7 was produced alongside vast quantities of hydrogen and helium. This makes lithium one of the oldest elements in existence.
The trouble is that theoretical models of Big Bang nucleosynthesis predict about three times as much primordial lithium as astronomers actually observe in the oldest stars. This discrepancy, known as the cosmological lithium problem, has persisted for decades. It is not a small rounding error or a matter of measurement uncertainty. The gap is large enough that physicists have spent years trying to explain it through nuclear physics corrections, stellar processes that might destroy lithium, or even new particle physics beyond the standard model.4PubMed. Cosmological Lithium Solution from Discrete Gauged B-L No consensus explanation has emerged. The cosmological lithium problem remains one of the open questions in fundamental physics, a reminder that even for an element discovered over 200 years ago, basic mysteries persist.
Two Isotopes and the Nuclear Age
Lithium exists in nature as two stable isotopes: lithium-6 and lithium-7. They occur in a lopsided ratio, with lithium-7 making up about 92% and lithium-6 about 8% of natural lithium.5ECS Meeting Abstracts. Effect of Applied Voltage Value on Lithium 6 Isotope Enrichment By Intermittent Voltage Application Electrodialysis Method This distinction became profoundly important during the Cold War, because lithium-6 turned out to be a critical ingredient in thermonuclear weapons.
When lithium-6 absorbs a neutron, it produces tritium, the hydrogen isotope needed for nuclear fusion. The first deployable hydrogen bombs used lithium-6 deuteride as their fusion fuel. The U.S. government embarked on a massive isotope separation program at Oak Ridge, Tennessee, during the 1950s, using mercury-based processes to enrich lithium-6. That program produced enormous quantities of enriched lithium and, as a byproduct, one of the worst mercury contamination legacies in American industrial history. The same isotope remains essential for proposed civilian fusion power: future fusion reactors would need lithium-6 to breed the tritium fuel for deuterium-tritium reactions.6Brazilian Journal of Radiation Sciences. Isotopic Enrichment of Lithium-6 for Thermoluminescent Dosimeter Application Meanwhile, lithium-7 has its own niche in the nuclear industry, used as a pH stabilizer in the primary coolant of pressurized water reactors.
From Grease to Batteries
Before lithium became synonymous with batteries, its biggest industrial use was far less glamorous. In the 1940s, Clarence Earle developed a lithium-based grease that outperformed existing lubricants in high-temperature and wet conditions. Lithium hydroxide stearate greases became the global standard for general-purpose lubrication, and by the 2010s lithium-thickened greases still accounted for roughly 70% of total grease production worldwide.7Elsevier. Modern advancements in lubricating grease technology Automotive wheel bearings, industrial machinery, and aircraft components all relied on lithium grease long before anyone was talking about electric vehicles.
The battery revolution started in 1976, when M. Stanley Whittingham, working at Exxon Research, demonstrated that lithium ions could be reversibly inserted into the layered crystal structure of titanium disulfide.8PubMed. Electrical energy storage and intercalation chemistry This intercalation reaction, where lithium ions slip between the atomic layers of a host material without destroying its structure, was the conceptual foundation for rechargeable lithium batteries. Whittingham’s work showed that a battery based on this principle could operate at room temperature and be recharged many times, a radical improvement over existing technologies.
The path from that early prototype to a commercial product took another two decades. John Goodenough identified lithium cobalt oxide as a superior cathode material in 1980, and Akira Yoshino built the first practical lithium-ion battery using a carbon anode in 1985. Sony commercialized the technology in 1991. All three scientists shared the 2019 Nobel Prize in Chemistry. Today, lithium-ion batteries power smartphones, laptops, electric cars, and grid-scale energy storage. Global demand for lithium has surged so dramatically that the element, once considered an obscure curiosity of the periodic table, is now sometimes called “white gold.”
Finding Lithium in the Earth
For most of lithium’s history, its primary geological sources were hard-rock minerals like spodumene, the same family of minerals Arfwedson originally analyzed. Mining these deposits is energy-intensive and expensive, requiring conventional rock extraction and chemical processing. The economics of lithium production shifted dramatically after a 1969 geological survey in Chile’s Salar de Atacama identified massive concentrations of lithium dissolved in underground brines.9Ore Geology Reviews. Lithium brine production, reserves, resources and exploration in Chile: An updated review
Brine extraction works differently from hard-rock mining. Lithium-rich saltwater is pumped to the surface and spread in large evaporation ponds. Over months, solar energy evaporates the water, progressively concentrating the lithium until it can be chemically separated. The process is cheaper than rock mining but slow and water-intensive, a significant concern in the arid regions where the best brine deposits happen to be located. Chile, Argentina, and Bolivia sit atop the “lithium triangle,” the region with the world’s largest known brine reserves. Australia remains the top producer by volume, relying primarily on hard-rock spodumene mining.
The tension between surging demand and limited supply has sparked exploration of unconventional sources: geothermal brines beneath the Salton Sea in California, lithium-rich clays in Nevada, and even direct extraction from seawater, where lithium is present at extremely low concentrations. None of these alternatives has yet achieved the scale needed to challenge traditional brine and hard-rock operations, but the search itself reflects how thoroughly lithium has moved from the periphery of chemistry to the center of global industrial strategy.
Lithium’s Peculiar Chemistry
Part of what makes lithium useful in so many contexts is its unusual position on the periodic table. It is the lightest metal, with an atomic number of just 3, meaning each atom has only three protons. That small size gives lithium ions an exceptionally high charge density, which is why they interact so strongly with other materials and why lithium compounds tend to have distinctive properties compared to other alkali metals.
Lithium behaves oddly for its group. Chemists sometimes say it has a “diagonal relationship” with magnesium, meaning its chemistry resembles that of the element one row down and one column to the right more than it resembles its immediate neighbor sodium. Lithium carbonate, for instance, is only sparingly soluble in water, much like magnesium carbonate but quite unlike the highly soluble sodium carbonate. Lithium also forms stable organometallic compounds that are workhorses in organic chemistry, used to build complex molecules in pharmaceutical synthesis and materials science. Butyllithium, one of the most common, is a powerful base and initiator for polymerization reactions.
The element’s reactivity with water and air means it never occurs free in nature. Every bit of lithium used in industry must be extracted from minerals or brines and refined. When exposed to moist air, lithium metal tarnishes quickly, forming a dull oxide coating. In contact with water, it reacts to produce lithium hydroxide and hydrogen gas, though less violently than sodium or potassium. You can handle a small piece of lithium briefly with dry hands, something you would never attempt with its heavier alkali cousins.
Trace Lithium in Drinking Water
An intriguing footnote to lithium’s medical story involves its natural presence in drinking water. Lithium occurs at trace levels in virtually all groundwater, though concentrations vary enormously by geography. Starting in the 1990s, a series of ecological studies noticed that regions with higher natural lithium levels in their tap water tended to have lower rates of suicide and violent crime. The effect sizes were small, and the study designs could not prove causation, since many confounding factors differ between regions. But the pattern has been replicated across studies in Japan, Austria, Greece, Texas, and several other locations.
This research has prompted occasional proposals to add lithium to public water supplies, analogous to water fluoridation for dental health. The idea remains highly controversial. The therapeutic dose of lithium for bipolar disorder is hundreds of times higher than the trace amounts found in drinking water, so the mechanism by which such tiny concentrations could affect population-level mental health is unclear. Skeptics point out that ecological correlations are notoriously unreliable for drawing causal conclusions. Proponents argue that even subtherapeutic doses of lithium might have neuroprotective effects that accumulate over a lifetime. No public health authority has endorsed water lithiation, and it is unlikely to happen without far stronger evidence, but the question keeps resurfacing in psychiatric and public health literature.