Search results
Radium is a chemical element; it has symbol Ra and atomic number 88. It is the sixth element in group 2 of the periodic table, also known as the alkaline earth metals. Pure radium is silvery-white, but it readily reacts with nitrogen (rather than oxygen) upon exposure to air, forming a black surface layer of radium nitride (Ra 3 N 2).
- Overview
- Occurrence, properties, and uses
- Compounds
radium (Ra), radioactive chemical element, the heaviest of the alkaline-earth metals of Group 2 (IIa) of the periodic table. Radium is a silvery white metal that does not occur free in nature.
(Read Marie Curie’s 1926 Britannica essay on radium.)
Britannica Quiz
118 Names and Symbols of the Periodic Table Quiz
Radium was discovered (1898) by Pierre Curie, Marie Curie, and an assistant, G. Bémont, after Marie Curie observed that the radioactivity of pitchblende was four or five times greater than that of the uranium it contained and was not fully explained on the basis of radioactive polonium, which she had just discovered in pitchblende residues. The new, powerfully radioactive substance could be concentrated with barium, but, because its chloride was slightly more insoluble, it could be precipitated by fractional crystallization. The separation was followed by the increase in intensity of new lines in the ultraviolet spectrum and by a steady increase in the apparent atomic weight of the material until a value of 225.2 was obtained, remarkably close to the currently accepted value of 226.03. By 1902, 0.1 gram of pure radium chloride was prepared by refining several tons of pitchblende residues, and by 1910 Marie Curie and André-Louis Debierne had isolated the metal itself.
Thirty-four isotopes of radium, all radioactive, are known; their half-lives, except for radium-226 (1,600 years) and radium-228 (5.75 years), are less than a few weeks. The long-lived radium-226 is found in nature as a result of its continuous formation from uranium-238 decay. Radium thus occurs in all uranium ores, but it is more widely distributed because it forms water-soluble compounds; Earth’s surface contains an estimated 1.8 × 1013 grams (2 × 107 tons) of radium.
The chemistry of radium is what would be expected of the heaviest of the alkaline earths, but the intense radioactivity is its most characteristic property. Its compounds display a faint bluish glow in the dark, a result of their radioactivity in which emitted alpha particles excite electrons in the other elements in the compound and the electrons release their energy as light when they are de-excited. One gram of radium-226 undergoes 3.7 × 1010 disintegrations per second, a level of activity that defined the curie (Ci), an early unit of radioactivity. This is an energy release equivalent to about 6.8 × 10−3 calorie per second, sufficient to raise the temperature of a well-insulated 25-gram sample of water at the rate of 1 °C every hour. The practical energy release is even greater than this (by four to five times), because of the production of a large number of short-lived radioactive decay products. The alpha particles emitted by radium may be used to initiate nuclear reactions.
Are you a student? Get Britannica Premium for only 24.95 - a 67% discount!
Learn More
Radium’s uses all stem from its radioactivity. The most important use of radium was formerly in medicine, principally for the treatment of cancer by subjecting tumours to the gamma radiation of its daughter isotopes. Radium-223, an alpha emitter with a half-life of 11.43 days, has been studied for use in cell-directed cancer therapy, in which a monoclonal antibody or related targeting protein with high specificity is attached to the radium. In most therapeutic applications, however, radium has been superseded by the less costly and more powerful artificial radioisotopes cobalt-60 and cesium-137. An intimate mixture of radium and beryllium is a moderately intense source of neutrons and has been used for scientific research and for well logging in geophysical prospecting for petroleum. For these uses, however, substitutes have become available. One of the products of radium decay is radon, the heaviest noble gas; this decay process is the chief source of that element. A gram of radium-226 will emit 1 × 10−4 millilitre of radon per day.
When a radium salt is mixed with a paste of zinc sulfide, the alpha radiation causes the zinc sulfide to glow, yielding a self-luminescent paint for watch, clock, and instrument dials. From about 1913 up until the 1970s, several million radium dials, coated with a mixture of radium-226 and zinc sulfide, were manufactured. By the early 1930s it was found, however, that exposure to radium posed a serious hazard to health: a number of women who had worked with the radium-containing luminescent paint during the 1910s and ’20s subsequently died. They had ingested considerable amounts of radium through the technique called “lip-pointing,” which meant using their lips and tongues to shape their paintbrushes to a fine tip. Like calcium and strontium, radium tends to concentrate in bones, where its alpha radiation interferes with red corpuscle production, and some of those women developed anemia and bone cancer. The practice of employing radium in luminescent coatings was curtailed in the early 1960s after the high toxicity of the material was recognized. Phosphorescent paints that absorb light and later release it have replaced radium. (The detection of exhaled radon provides a very sensitive test for radium absorption.)
Radium metal may be prepared by electrolytic reduction of its salts, and it displays high chemical reactivity. It is attacked by water with vigorous evolution of hydrogen and by air with the formation of the nitride. It occurs exclusively as the Ra2+ ion in all its compounds. The sulfate, RaSO4, is the most insoluble sulfate known, and the hydroxide, Ra(OH)2, is the most soluble of the alkaline-earth hydroxides. The gradual buildup of helium within crystals of radium bromide, RaBr2, weakens them, and they occasionally explode. In general, the compounds of radium are very similar to their barium counterparts, making separation of the two elements difficult.
Element Radium (Ra), Group 2, Atomic Number 88, s-block, Mass [226]. Sources, facts, uses, scarcity (SRI), podcasts, alchemical symbols, videos and images. Jump to main content
Oct 14, 2016 · Radium is the heaviest alkaline earth metal, according to Encyclopedia. The other alkali earth metals include beryllium, magnesium, calcium, strontium and barium. Radium changes from a...
Dec 19, 2018 · Among a slew of papers that the Curies published in the years after its discovery, one showed that radium could treat cancer by killing cancer cells more quickly than healthy cells. It became...
- Stephen Mansell
Oct 9, 2012 · 9 Ways People Used Radium Before We Understood the Risks. Radium was discovered by Marie Curie and her husband Pierre in 1898. In 1903, the Royal Academy of Sciences awarded Marie and Pierre...
Jul 6, 2023 · Radium is a radioactive substance found in nature. Radium is produced by the radioactive decay of uranium. The intensity of radiation from radioactive materials decreases over time. The time required for the intensity to decrease by one-half is referred to as the half-life. The half-life of radium is approximately 1,600 years. How is radium used?
People also ask
Is radium free?
Is radium a metal?
What is the half life of radium?
Why is radium important?
