The elements are the fundamental substances that make up everything you can touch, breathe, or see in the universe. There are 118 confirmed entries on the periodic table, ranging from hydrogen, the lightest and most abundant, to oganesson, a synthetic behemoth that exists for mere fractions of a second in particle accelerators. What makes the story of the elements so compelling is that it spans nearly the entire history of the cosmos: from the first minutes after the Big Bang to the inside of a supernova to the quiet, invisible work that trace metals do inside your cells right now.
Where the Elements Were Forged
Not all elements were born in the same place or at the same time, and tracing their origins requires looking at several distinct cosmic processes. The lightest elements, hydrogen, helium, and small amounts of lithium, were produced in the first few minutes after the Big Bang in a process called Big Bang nucleosynthesis. The abundances of these primordial elements are one of the key pieces of evidence for the Big Bang model itself. Theoretical calculations using nucleosynthesis codes can reproduce the observed amounts of helium and deuterium in the universe with impressive accuracy, though lithium remains a stubborn outlier: models consistently predict about three to four times more primordial lithium than astronomers actually observe, a discrepancy known as the cosmological lithium problem.1The Astrophysical Journal. Big Bang Nucleosynthesis with f(R) Gravity Scalarons and Astrophysical Consequences
Everything heavier than lithium was made inside stars. Low-mass stars like our Sun fuse hydrogen into helium over billions of years. High-mass stars burn through their fuel far faster and fuse progressively heavier nuclei, building up elements like carbon, oxygen, silicon, and iron in layered shells. When these massive stars exhaust their fuel, they explode as supernovae, scattering those elements into the surrounding space.2Science. Populating the periodic table: Nucleosynthesis of the elements Iron is roughly where stellar fusion stops being energetically favorable, so making elements heavier than iron requires a different kind of violence.
That violence comes largely from the rapid neutron-capture process, or r-process, which occurs in environments flooded with free neutrons, most dramatically during the collision of two neutron stars. Neutron star mergers are responsible for creating roughly half of all elements heavier than iron and are the only natural source of elements beyond lead and bismuth.3Annual Review of Nuclear and Particle Science. Neutron Star Mergers and Nucleosynthesis of Heavy Elements When astronomers detected gravitational waves from a neutron star merger in 2017 and simultaneously observed the characteristic glow of freshly made heavy elements in the aftermath, it was one of the most satisfying confirmations in modern astrophysics. The gold in your jewelry and the platinum in a catalytic converter were, in all likelihood, forged in exactly this kind of cataclysm billions of years ago.
How the Elements Sorted Themselves on Earth
Once those elements became part of a young planet, they did not stay evenly mixed. Early in Earth’s history, the planet was largely molten, and elements separated based on their chemical affinities. In the 1920s, the geochemist Victor Goldschmidt devised a classification system still used today, dividing elements into groups based on where they ended up during Earth’s differentiation. He drew evidence from meteorite phases and metallurgical experiments, observing how elements partitioned among coexisting metal, sulfide, and silicate phases.4American Mineralogist. Goldschmidt’s geochemical classification of the elements: The evolution of a nuanced hypothesis
The basic framework looks like this:
- Siderophile elements: iron-loving elements like nickel, cobalt, and the platinum-group metals that sank into Earth’s metallic core.
- Chalcophile elements: sulfur-loving elements like copper, zinc, and lead that concentrated in sulfide minerals.
- Lithophile elements: rock-loving elements like silicon, aluminum, and calcium that bonded with oxygen and built the silicate minerals of the mantle and crust.
- Atmophile elements: gases like nitrogen and the noble gases that accumulated in the atmosphere.
This sorting explains why some elements are frustratingly rare in the crust despite being abundant in the planet as a whole. Iron is the most common element on Earth by mass, but much of it is locked in the core, thousands of kilometers below the surface. Meanwhile, elements like aluminum and silicon dominate the crust because their chemistry favored staying in the rocky outer layers. The practical consequence is that mining for certain metals means finding places where geological processes, such as volcanic activity or hydrothermal circulation, have re-concentrated them into economically viable deposits.
Elements That Keep You Alive
About 99 percent of your body by mass is made of just six elements: oxygen, carbon, hydrogen, nitrogen, calcium, and phosphorus. But life also depends on a suite of trace elements, required in tiny amounts but absolutely essential. These trace elements are needed in quantities ranging from about 50 micrograms to 18 milligrams per day, acting as catalytic or structural components of larger molecules with specific, indispensable functions.5PubMed. The essential trace elements
Iron carries oxygen in your blood. Zinc is involved in hundreds of enzymatic reactions, from wound healing to immune defense. Copper helps build connective tissue. Selenium protects cells from oxidative damage. Iodine is essential for thyroid hormones that regulate metabolism. Cobalt sits at the heart of vitamin B12. Chromium plays a role in insulin signaling. These are not optional extras; a deficiency in any single one of them can produce serious disease. Iron deficiency is the most common nutritional deficiency worldwide, affecting billions of people and causing anemia. Iodine deficiency, before the widespread iodization of salt, was a leading cause of preventable intellectual disability.
What makes the biological story interesting is selectivity. Life uses only about 25 to 30 of the 118 known elements. Some abundant elements are biologically irrelevant (aluminum, for instance, is the third most common element in the crust but has no known biological role in humans), while some rare ones are critical. The reasons trace back to chemistry: the elements life uses tend to be those that dissolve readily in water, form flexible bonds with organic molecules, and were available in Earth’s early oceans when the biochemistry of life was being established.
Same Element, Wildly Different Material
One of the more surprising facts about the elements is that a single element can exist in completely different physical forms, a phenomenon called allotropy. Allotropes arise because the atoms of an element can be arranged in different structural patterns, leading to dramatic differences in properties like density, hardness, and electrical conductivity.6Advanced Materials Science Research. Understanding Allotropy: The Fascinating World of Different Forms of Elements
Carbon is the textbook example. Diamond, one of the hardest known materials, and graphite, the soft, slippery substance in pencil lead, are both pure carbon. The only difference is how the carbon atoms are bonded and arranged. Diamond forms a rigid three-dimensional lattice; graphite consists of loosely stacked sheets that slide over each other easily. Add a third arrangement, the hollow soccer-ball-shaped molecules called fullerenes or the rolled-up tubes called carbon nanotubes, and you have materials with entirely different electrical and mechanical properties, all from the same element.
Carbon gets the most attention, but allotropy shows up across the periodic table. Oxygen exists as the two-atom molecule you breathe (O₂) and as ozone (O₃), which absorbs ultraviolet radiation in the stratosphere. Sulfur can form rings of eight atoms, long polymer chains, or a plastic-like amorphous solid depending on temperature and pressure. Tin undergoes a transformation from a metallic form to a brittle, crumbly grey form in cold temperatures, a property that famously contributed to the failure of solder joints in extreme cold during several historical expeditions. Phosphorus comes in white, red, and black forms, with white phosphorus being dangerously reactive and spontaneously flammable in air, while red phosphorus is stable enough to coat the striking surface of a matchbox.
Making Elements That Nature Cannot
Every element heavier than uranium (element 92) does not occur naturally in any significant amount. These transuranic elements have to be created artificially, typically by smashing lighter atomic nuclei together in particle accelerators and hoping they fuse into something new before flying apart. The challenge grows exponentially as you move to heavier elements because the electrostatic repulsion between the positively charged nuclei becomes enormous.
A key breakthrough came with the use of calcium-48 as a projectile. This particular isotope of calcium is doubly “magic” in nuclear physics terms, meaning both its proton and neutron counts correspond to especially stable configurations. Researchers first produced a calcium-48 ion beam at the JINR heavy-ion cyclotron and showed it had major advantages for synthesizing superheavy elements, because the extreme neutron excess of calcium-48 allowed the formation of compound nuclei with lower excitation energies, sharply increasing the chances of a successful fusion reaction.7Nuclear Physics A. Acceleration of 48Ca ions and new possibilities of synthesizing superheavy elements Experiments using calcium-48 beams have been responsible for the synthesis of elements 113 through 118, the entire bottom row of the modern periodic table.
Early results from these reactions showed decay chains of individual atoms, sequential alpha decays ending in spontaneous fission, with energies and half-lives matching the predictions of theoretical models. These were considered the first experimental evidence for a long-hypothesized region of enhanced nuclear stability among the superheavy elements.8Radiation Physics and Chemistry. Towards the “islands of stability” of superheavy elements
The Island of Stability
The concept behind the island of stability is that certain combinations of protons and neutrons should form unusually long-lived nuclei, even among the superheavy elements that are generally expected to fall apart almost instantly. The idea dates back to theoretical work in the late 1960s, which predicted that the region around 114 protons and 184 neutrons would show enhanced stability against alpha decay, beta decay, and spontaneous fission.9Nuclear Physics A. On the nuclear structure and stability of heavy and superheavy elements
The exact center of the island remains debated. Some calculations favor 114 protons and 184 neutrons as the magic numbers, others point to 120 protons and 184 neutrons, and still others suggest 126 protons and 184 neutrons may give the strongest shell effects.10Journal of Physics G: Nuclear and Particle Physics. Island of stability for superheavy elements and the dynamical cluster-decay model for fusion evaporation residue cross sections: 48Ca+238U→286112* as an example A separate analysis using the same model framework found that 120 protons and 184 neutrons represent the strongest magic numbers for the center of the island.11Journal of Physics G: Nuclear and Particle Physics. Establishing the island of stability for superheavy nuclei via the dynamical cluster-decay model applied to a hot fusion reaction 48Ca + 238U → 286112* The disagreement is not a sign of confusion so much as a reflection of how difficult it is to model nuclear forces at these extremes. Different theoretical approaches weight the competing effects slightly differently, and experimental data in this region is extraordinarily scarce because no one has yet managed to produce nuclei with 184 neutrons.
If the island exists as predicted, some superheavy nuclei might survive for minutes, hours, or conceivably even longer, rather than the milliseconds typical of the superheavy elements produced so far. That would open the door to studying their chemistry, not just their nuclear physics. Right now, chemical experiments on superheavy elements are limited to a handful of atoms produced one at a time, each vanishing before much can be learned. Longer-lived isotopes would change the game entirely.
How Elements Behave Under Extreme Pressure
The periodic table as it appears on classroom walls describes how elements behave at ordinary surface conditions. Squeeze those same elements to millions of atmospheres, the kind of pressures found deep inside planets, and the rules start to bend. Under high pressure, the fundamental chemical properties of atoms, including their tendency to attract or share electrons, change in ways that can make familiar elements behave like completely different substances.12PubMed Central. Electronegativity and chemical hardness of elements under pressure
Sodium, normally a soft, reactive metal, becomes a transparent insulator at very high pressures. Lithium, the lightest metal, is predicted to become a superconductor. Hydrogen itself might form a metallic solid under sufficient compression, a possibility that has tantalized physicists for nearly a century because metallic hydrogen could be a room-temperature superconductor. These are not just quirky laboratory curiosities. Understanding how elements behave under pressure is essential for modeling the interiors of gas giants like Jupiter and Saturn, where hydrogen and helium exist at pressures millions of times higher than anything on Earth’s surface. The researchers studying electronegativity and chemical hardness under pressure have argued that the changes in fundamental atomic properties they observe can provide a unified framework for explaining and predicting many of these unusual chemical phenomena.
The Politics of Naming a New Element
Discovering a new element is hard. Naming it can be almost as contentious. The procedure managed by the International Union of Pure and Applied Chemistry (IUPAC) involves first establishing which research group has priority of discovery, then inviting that group to propose a name. This protocol has not always been accepted without friction. The chemist Friedrich Paneth argued in 1947 that discoverers have the undisputed right to name their elements, a view that clashed with IUPAC’s more consultative approach and came to a head during a workshop convened to name elements 104 through 109, when competing discovery claims led to bitter disputes over who was entitled to do the naming.13Helvetica Chimica Acta. Paneth, IUPAC, and the Naming of Elements
Current IUPAC rules allow new elements to be named after a mythological concept, a mineral, a place, a property, or a scientist. This is why the periodic table reads like a world atlas in places: francium for France, nihonium for Japan, moscovium for Moscow, tennessine for Tennessee. Names honoring scientists include einsteinium, curium, fermium, and mendelevium. The most recent additions, elements 113 through 118, were officially named in 2016. Oganesson, element 118, was named after Yuri Oganessian, a nuclear physicist still alive at the time, one of only two people to have an element named after them during their lifetime.
Critical Elements and the Energy Transition
The periodic table has taken on a new kind of practical urgency in recent decades. The shift away from fossil fuels toward renewable energy and electric vehicles has dramatically increased demand for a specific set of elements that most people had never heard of a generation ago. Lithium for batteries, cobalt for cathodes, rare earth elements like neodymium and dysprosium for wind turbine magnets, indium and gallium for thin-film solar cells, platinum-group metals for fuel cells: the clean energy transition runs on a surprisingly narrow group of materials.
The emerging challenge is sometimes described as trading an emissions problem for a resources problem. Despite ample geological reserves in many cases, ensuring sustainable access to critical raw materials is complicated by concentration of mining and refining in a handful of countries, the environmental and social impacts of extraction, and long lead times for new mining projects.14Mineral Economics. From emissions to resources: mitigating the critical raw material supply chain vulnerability of renewable energy technologies Cobalt, for instance, is predominantly mined in the Democratic Republic of Congo, often under conditions that have drawn serious human rights scrutiny. Rare earth processing is overwhelmingly concentrated in China, which gives that country significant leverage over global supply chains.
Efforts to address these vulnerabilities include recycling spent batteries to recover lithium and cobalt, developing alternative battery chemistries that use more abundant elements like sodium or iron phosphate, diversifying mining sources, and exploring deep-sea mineral deposits. None of these solutions is simple, and each carries its own environmental trade-offs. The periodic table, in a sense, has become a strategic document: which elements you can access, and at what cost, shapes the pace and feasibility of decarbonization.
Isotopic Fingerprints
Every element exists as a mixture of isotopes, atoms with the same number of protons but different numbers of neutrons. Most of the time, isotopes of a given element behave identically in chemical reactions, but subtle differences in mass cause slight variations in how readily they participate in physical and biological processes. Over geological time, these tiny differences accumulate, leaving characteristic isotopic signatures in rocks, water, soils, and living organisms.
The ratios of stable isotopes of elements like strontium, neodymium, and lead in rocks and minerals carry strong regional fingerprints that are reflected in atmospheric components, water, and even agricultural and fishery products. Geologically derived stable isotope ratios can serve as tracers for the source of many kinds of substances.15Proceedings of the Japan Academy, Series B. Potential uses of stable isotope ratios of Sr, Nd, and Pb in geological materials for environmental studies This has practical applications far beyond geology. Forensic scientists use strontium isotope ratios in teeth and bones to determine where a person grew up, because the strontium you ingest through food and water reflects the local geology. Food fraud investigators use isotopic analysis to verify whether high-value products like olive oil, wine, or high-grade rice actually originate from the regions claimed on their labels. Environmental regulators track pollution sources by comparing the lead isotope signatures of contaminated sediments with the signatures of suspected industrial sources.
The precision of modern isotope-ratio mass spectrometry has made these analyses routine enough to use in court. What started as a tool for understanding the deep history of rocks has become a remarkably versatile method for tracing the movement of elements through the modern world, from the water cycle to the food supply to criminal investigations.