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: element 42 was the answer. 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.
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 observers would promptly perish.
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.
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.
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--giant stars which have burnt out and collapsed into spheres of pure neutrons--are technically enormous atoms with preposterous atomic weights.
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.