It is a chemical element with the symbol Ra, and the atomic number of radium is 88. This is the sixth element in group 2 of the periodic table, also known as alkaline earth metals. Pure radium is silver-white, but it reacts readily with nitrogen (other than oxygen) upon exposure to air, forming a black surface layer of radium nitride (Raw 3N2). All isotopes of radium have high radioactivity, the most stable isotope is radium-226, which has a half-life of 1600 years and decays as radon gas (specifically isotope radon-222). When radium is depleted, ionizing radiation is a product that activates fluorescent chemicals and causes radioluminescence.
Introduction of Radium
Radioactive chemical element Radium, in the form of radium chloride. Discovery of radium? Radium was the discovery of radioactive element radium discovered by Marie and Pierre Curie in 1898. Radium was isolated in its metallic state in 1911 by the electrolysis of radium chloride by Marie Curie and Andr–Louis DeBiern.
In nature, trace amounts of radium uranium and (to some extent) thorium ores are as low as one-seventh to one tonne of uraninite. Radium is not required for organisms, and adverse health effects can occur when incorporated into biochemical processes due to radioactivity and chemical reactivity. Today, these earlier applications are now obsolete because the toxicity of radium is known, and less dangerous isotopes are used in radiosensitive devices.
Properties of radium
Radium is a heavily known alkaline earth metal and is the only radioactive member of its group. Physical and chemical properties radium resemble those of its mild condenser barium.
Pure radium is an unstable silver-white metal, but its lightweight condensers have a slightly yellowish tinge of calcium, strontium and barium. This color disappears rapidly by exposure to air, giving a black layer of radium nitride (Raw 3N2). Radium melting point is 700 ° C and its boiling point is 1,737. Like barium and alkali metals, radium crystallizes at standard temperature and pressure in a body-centered cubic structure: radium-radium bond distance 514.8 picometers. Rath 5.5 g / cm 3, more than barium, periodic trends confirms again, radium-barium density ratio compared to a ratio of the mass of radium-barium atom, the two elements of the same crystal structures.
Occurrence of radium
All isotopes of radium have half-lives beyond the age of the earth so that any primitive radium would have decayed long ago. It also occurs in the atmosphere because isotopes 223Ra, 224Ra, 226Ra, and 228Ra are present in decay chains of natural thorium and uranium isotopes; Because thorium and uranium have very long half-lives, these daughters are constantly being reproduced by their decay of these four isotopes of radium, the longest-lived is radium 226 (half-life of radium is 1600 years), which is the decay product of natural uranium. Because of its relative longevity, Radium 226 is the most common isotope of the element, a fraction of a trillion of Earth’s crust; All Natural Radium 226Ra. Thus, uranium ore is found in uraninite and many other uranium ores, in small quantities in radium and in titanium quantities in thorium ores. One ton of pitchblende usually yields one-seventh of a gram of radium.