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In nature, radium is found in uranium and (to a lesser extent) thorium ores in trace amounts as small as a seventh of a gram per ton of uraninite.
Radium is not necessary for living organisms, and adverse health effects are likely when it is incorporated into biochemical processes because of its radioactivity and chemical reactivity.
It becomes yellow after some time due to self-damage by the alpha radiation given off by radium when it decays.
Radium was isolated in its metallic state by Marie Curie and André-Louis Debierne through the electrolysis of radium chloride in 1911.
One ton of pitchblende typically yields about one seventh of a gram of radium.
Uranium had no large scale application in the late 19th century and therefore no large uranium mines existed.
Its immediate decay product is the dense radioactive noble gas radon, which is responsible for much of the danger of environmental radium.
A sample of radium metal maintains itself at a higher temperature than its surroundings because of the radiation it emits – alpha particles, beta particles, and gamma rays.
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More specifically, natural radium (which is mostly All isotopes of radium have half-lives much shorter than the age of the Earth, so that any primordial radium would have decayed long ago.