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It was the summer of 1936 when Ernest Lawrence, the inventor of the atom-smashing cyclotron, received a visit from Emilio Segrè, a scientific colleague from Italy. Segrè explained that he had come all the way to America to ask a very small favor: He wondered whether Lawrence would part with a few strips of thin metal from an old cyclotron unit. Dr. Lawrence was happy to oblige; as far as he was concerned, the stuff Segrè sought was mere radioactive trash. He sealed some scraps of the foil in an envelope and mailed it to Segrè’s lab in Sicily. Unbeknownst to Lawrence, Segrè was on a surreptitious scientific errand.

At that time, the majority of chemical elements had been isolated and added to the periodic table, yet there was an unsightly hole where an element with 43 protons ought to be. Elements with 42 and 44 protons⁠—₄₂molybdenum and ₄₄ruthenium respectively⁠—had been isolated decades earlier, but element 43 was yet to be seen. Considerable accolades awaited whichever scientist could isolate the elusive element, so chemists worldwide were scanning through tons of ores with their spectroscopes, watching for the anticipated pattern.

Upon receiving Dr. Lawrence’s radioactive mail back in Italy, Segrè and his colleague Carlo Perrier subjected the strips of molybdenum foil to a carefully choreographed succession of Bunsen burners, salts, chemicals, and acids. The resulting precipitate confirmed their hypothesis: The radiation in Lawrence’s cyclotron had converted a few ₄₂molybdenum atoms into element 43, and one ten-billionth of a gram of the stuff now sat in the bottom of their beaker. They dubbed their plundered discovery “technetium” for the Greek word technetos, meaning “artificial.” It was considered to be the first element made by man rather than nature, and its “short” half-life⁠—anywhere from a few nanoseconds to a few million years depending on the isotope⁠—was the reason there’s negligible naturally-occurring technetium left on modern Earth.

In the years since this discovery, scientists have employed increasingly sophisticated apparatuses to bang particles together to create and isolate increasingly heavy never-before-seen elements, an effort which continues even today. Most of the obese nuclei beyond ₉₂uranium are too unstable to stay assembled for more than a moment, to the extent that it makes one wonder why researchers expend such time, effort, and expense to fabricate these fickle fragments of matter. But according to our current understanding of quantum mechanics, if we can pack enough protons and neutrons into these husky nuclei we may encounter something astonishing.

In the 1950s and 60s scientists worldwide were employing nuclear reactors, atom smashers, and particle accelerators to combine subatomic particles into heavier and heavier elements. It seemed that all atoms heavier than ₈₂lead or ₈₃bismuth were inherently unstable, and that packing on more protons and neutrons always shortened the atoms’ existence. As these progressively heavier synthesized atoms’ half-lives diminished from years to days to hours to seconds, the prevailing assumption among researchers was that science was approaching the end of the elemental road. Given the poor return on investment, excitement surrounding the synthesis of new elements began to wane. It seemed that the Nobel Foundation had long since given away their last prize for the discovery of a new chemical element; atoms that decompose within milliseconds were just not very useful or interesting.

But in the late 1960s, a comprehensively successful chemist named Glenn T. Seaborg made a bold prediction: despite the predominant view to the contrary, he asserted that there are likely to be some “superheavy” elements with very stable nuclei that had never before been seen by man. He was singularly qualified to make such a deduction, having personally discovered or co-discovered nine elements already. Later he would be credited with his tenth elemental co-discovery, his honorarily eponymous “seaborgium”. He had also worked on the Manhattan Project, advised several US presidents on nuclear policy, and acted as chairman of the United States Atomic Energy Commission from 1961 to 1971.

Seaborg’s insight was based on his thorough understanding of the nuclear shell model, which is one of science’s most accurate models of how the stuff of atomic nuclei might be organized. The model describes a system where the particles of the nucleus organize themselves into structures of progressively larger nested “shells”, each made up entirely of protons or neutrons. At atomic scales the strong nuclear force binds the nucleon particles of the nucleus together while the electrostatic force simultaneously presses them apart.

The strong force easily dominates petite nuclei such as ₃lithium, keeping the nucleons in strict bondage. But in beefier elements on the periodic table such as ₈₅astatine-210 (85 protons and 125 neutrons), the nuclei start to become girthy enough that mere attraction is insufficient to bind the bits together indefinitely. For these unstable atoms, it is only a matter of time until the struggle between attraction and repulsion results in a sudden discharge of nuclear material. This radioactive decay releases considerable energy as radiation, and reduces the original atom to a lighter element. The assorted ejecta may form into other lighter atoms and/or fly off as loose subatomic bits. For instance, when ₈₉actinium decays in nature it can produce the lighter element ₈₇francium. Francium tends to surrender to decay rather rapidly⁠—usually within an hour⁠—to produce atoms of ₈₅astatine, ₈₈radium, or ₈₆radon, each of which further decays into other atoms. Francium’s abbreviated half-life means that only about 30 grams of of the stuff are present in the Earth’s crust at any given time. If one attempted to assemble some francium atoms together to observe the properties of this metal, any sample large enough to see would instantly vaporize due to the heat of spontaneous fission, and all unprotected biological observers would promptly perish.

Owing to atomic decay in heavy nuclei, about the heaviest atom one is likely to encounter here on Earth is ₉₂uranium. Essentially all atoms with heavier nuclei have fallen apart over the past few billion years. This battle between attractive and repelling forces would seem to suggest that the life expectancy of an atom is inversely proportional to its obesity. In general, this is roughly true. Some heavier nuclei, however, deviate from the pattern and outlast their daintier cousins by a considerable margin. The aforementioned nuclear shell model ascribes this to the fact that these atomic outliers have a “magic number” of particles in their nuclei. When a nucleus has all of its proton shells or neutron shells loaded to full capacity, the layers can align so well that each shell can spoon intimately with its attractive neighbors, forming a more compact sphere that fits well within the strong nuclear force’s area of influence. When all shells of both nucleon types have a full complement, the layers snuggle spectacularly, and the tightly bound result is known as “doubly magic”. One example is ₈₂lead-208, which along with other double-magic atoms will loiter around the universe for a very long time indeed.

Seaborg’s stimulating proposition was that the steady decline in cohesion at the end of the periodic table may not be a one-way dive into the stability abyss. There ought to be, he suggested, an “island of stability” where certain superheavy isotopes have enough nucleons of the right types to fill all of their shells and become magic or doubly-magic. These never-before-seen elements would possess sturdy, comparatively long-lasting nuclei. Presumably, some of these exotic isotopes would even be stable. Considering the flighty nature of the heaviest atoms yet wrought by man, Seaborg’s claim was counterintuitive at best, but the subsequent flurry of calculations indicated that he was almost certainly correct.

The obvious challenge to the island of stability hypothesis is to ask why we have not yet encountered any of these stable superheavy atoms in nature. If they indeed exist, they ought to be present on Earth in observable quantities like all of the other long-lived elements. The answer seems to be that the universe’s atom fabricators⁠—stars and supernovae⁠—don’t tend to create the conditions necessary to produce superheavy elements. The immense heat and pressure at the center of a large star is adept at fusing the universe’s primordial hydrogen, helium, and lithium into progressively heavier atoms. But once the star reaches the point in its life where it is producing atoms of ₂₈nickel it begins to spend more energy than it gains from each fusion. Some stars can cook up atoms as heavy as ₈₃bismuth before they are completely exhausted. Once it’s bismuth time, the star clenches rapidly, producing high-pressure internal shock waves that can spawn ₉₂uranium, ₉₄plutonium, and _#%$!pandemonium. The star then explodes, scattering its astronomical atomic abundance into the cosmos. The heaviest natural elements are now known to be the product of neutron stars⁠—giant stars which have burnt out and collapsed into spheres of pure neutrons. When two of these stars collide, some of their mass is ejected, and various heavy nuclei can coalesce from this soup of naked neutrons.

This galactic chemical evolution is the source of all of the natural heavy atoms we humans know and enjoy today. As famed astrophysicist Carl Sagan was fond of saying, “We are made of star stuff.” But despite stars’ best efforts to manufacture heavier atoms, today’s universe is still essentially 90% hydrogen and 10% helium, with the rest of the matter in the universe amounting to a rounding error. Humans, of course, then picked up where stars left off by synthesizing atoms that stellar fusion and supernovae are incapable of producing. As of this writing (January 2013) the heaviest element yet made by man is element 118, known by the temporary name “ununoctium”. In 2005 Russian and American researchers working in tandem produced several atoms of element 118 by colliding ₉₈californium-249 atoms with ₂₀calcium-48 ions. The ₁₁₈ununoctium-294 nuclei had a half-life of less than a millisecond, but this was longer than would be predicted in a non-island theoretical framework, which further reinforces the island of stability hypothesis.

If atomic explorers ever do manage to slosh up the beach onto the island of stability, it is impossible to predict precisely what scientific novelties they will find there. Although chemists can make some guesses regarding the properties of stable and semistable superheavy elements based on the existing patterns in the periodic table, we cannot know whether or not these undiscovered atoms are useful or bizarre until science forges a few. Interestingly, the heaviest isotopes physicists have managed to synthesize so far don’t behave quite like science’s best current models predict, so stable superheavy nuclei are likely to be full of surprises. Chemists cannot even predict with any certainty whether these materials will exist as gases, liquids, or solids at room temperature.

The essence of chemistry⁠—the basic reason that any chemical reacts with any other⁠—is that atoms store their electrons in nested “shells” surrounding the nucleus, each of which can hold a limited quantity of electrons. Atoms desperately want their exposed outermost electron shell to be filled, and as they bump against other atoms they jettison, share, or burgle electrons in an effort to accomplish this. These transactions can be cooperative or competitive, resulting in peaceful or violent reactions. In the early days of elemental chemistry, the atoms in the first few rows of the periodic table were found to fill their outer shells in predictable patterns, producing somewhat predictable chemical reactions. But some oddities emerged as some heavier elements such as the lanthanides began to be discovered, consequently confounding the predictive models and forcing them to be revised. It is quite possible that the exotic island of stability elements will similarly diverge from expectations.

Dr. Seaborg’s original models suggested that we would find magic superheavy semistable nuclei in atoms of ₁₁₄flerovium-298 and ₁₂₀unbinilium-304, and doubly-magic nuclei in ₁₂₆unbihexium-310. Subsequent discoveries in physics, however, show that such enormous nuclei would become deformed, thereby probably shifting the magic and double-magic quantities. Only with further experimentation can science be certain.

It is difficult to predict exactly how heavy nuclei can get even with doubly-magic nucleon shells. Famed physicist Richard Feynman allegedly suggested that element 137 may be the heaviest electromagnetically neutral element that can possibly exist in our universe since an atom with 138 electrons would require that the innermost electrons move faster than the speed of light. For this reason, the yet-to-be-synthesized element 137 is often referred to as “feynmanium.” Modern physicists using more sophisticated computations estimate that this limit may be nearer to element 173. Even in spite of this, physicists are not convinced that element 173 spells the end of the periodic table. Nature, as they say, finds a way. In fact, if one wishes to be particularly pedantic, one could point out that neutron stars are technically enormous atoms with preposterous atomic weights.

By the time he died in 1999, Dr. Seaborg had spent 30 years of his chemistry career attempting to traverse the treacherous channel between the known elements and the elusive island of stability. A year before his death, in 1998, researchers in Russia managed to synthesize atoms of ₁₁₄flerovium-289 by crashing ₉₄plutonium-244 into ions of ₂₀calcium-48. Unfortunately these fused atoms were nine neutrons short of the doubly-magic ₁₁₄flerovium-298, so they decayed rapidly. But Dr. Seaborg lived at least long enough to see atomic explorers get within sight of the shell-strewn “shores” of the island. Cramming in enough neutrons remains as the primary problem to solve in synthesizing stable superheavy elements.

If science ever does succeed in concocting these extraordinary materials, the atoms will certainly be expensive to produce in substantial quantities. If the new elements exhibit profitable properties, science will likely find a way to mass-produce them à la Manhattan Project plutonium. But even if they prove pedestrian, these unusual atoms would still represent a scientific first, and their study would greatly advance our knowledge of the building blocks of the universe. Indeed, perhaps there is a solid ₇₉gold Nobel or two still on the table. Regardless, unless there is some alien civilization more advanced than our own that has beaten us to it, humanity may be on the cusp of creating elements unlike anything the universe has ever seen.

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