Plutonium

Plutonium was first synthesized in 1940 by a team of American scientists including Edwin McMillan and Philip H. Abelson at the University of California, Berkeley. They produced plutonium through the bombardment of uranium-238 with deuterons in a cyclotron, resulting in element 94. The naming of plutonium follows the tradition of naming elements after planets; it is named after Pluto, the then-planet beyond Neptune. After its discovery, plutonium-239, one of its isotopes, was quickly recognized for its potential in nuclear fission, leading to significant developments during World War II, particularly in the Manhattan Project. Since its discovery, plutonium has garnered attention for both its military applications in nuclear weapons and its role in nuclear power generation.

Plutonium is not found in significant quantities in nature and is primarily produced synthetically in nuclear reactors. Trace amounts of plutonium-244, a naturally occurring isotope with a half-life of approximately 80 million years, were formed during stellar nucleosynthesis and can occasionally be found in uranium ores. The vast majority of plutonium used today is generated through the neutron bombardment of uranium-238 in research reactors or nuclear reactors where it can accumulate over time. Plutonium-239, the isotope most commonly utilized for energy and weaponry, is produced from neutron capture in uranium-238 and subsequent beta decay.

In terms of biological role, plutonium is highly toxic and poses serious health risks upon exposure. It is not a necessary trace element for any known biological processes and can accumulate in living organisms, primarily affecting the liver and bone marrow. The radiological properties of plutonium make it especially hazardous; external exposure can lead to burns, while internal exposure through inhalation or ingestion can result in increased cancer risk and damage to bodily tissues. Therefore, plutonium is strictly regulated, emphasizing containment and safety protocols in handling and processing.

Plutonium has several noteworthy physical and chemical properties. It has an atomic number of 94 and forms a silvery-gray metal that is highly dense, with a density of about 19.86 grams per cubic centimeter. Plutonium exhibits a complex allotropy, existing in six different crystalline forms depending on the temperature and pressure conditions, which can influence its physical properties. Chemically, plutonium is quite reactive, readily oxidizing in air to form plutonium oxide. It can form a variety of oxides, halides, and complex solutions, demonstrating multiple oxidation states ranging from -3 to +7, which allows it to behave as both an oxidizing and reducing agent. Its radioactivity also complicates its chemistry, giving rise to specific challenges in handling and storage.

Plutonium is primarily used in the nuclear industry, specifically in the manufacturing of nuclear weapons and as a fuel in nuclear reactors. Plutonium-239 is effectively used in nuclear reactors due to its ability to undergo fission, contributing to sustained energy release. Moreover, plutonium is being researched for use in radioisotope thermoelectric generators (RTGs) that provide energy for space missions, exploiting the heat released by its radioactive decay. Though its applications have positive implications for energy and exploration, the risks associated with plutonium handling and environmental contamination continue to restrict its broader use in commercial applications.

• Plutonium glows faintly in the dark due to its radioactivity.
• It was the second transuranium element ever to be synthesized, following neptunium.
• The metal is so dense that it is about 1.5 times more dense than lead.
• Plutonium-239 has a half-life of 24,100 years, which presents long-term waste disposal challenges.