Radium

Brilliant-white solid. Luminescent, turns black on exposure to air. Soluble in water with evolution of hydrogen; forms water-soluble compounds. Decays by emis- sion of α-, β-, and γ-radiation. Bone-seeking when taken into the body. Radium (Ra) is a radioactive element, found naturally occurring in the environment. Ra is a silvery- white-metallic solid @ 25℃; it tarnishes black when exposed to air. It is an alkaline earth metal; there are 33 isotopes, all of them are unstable. Radium is common

Radium is a naturally occurring silvery-white radioactive metal that can exist in several forms called isotopes. Radium is formed when uranium and thorium break down in the environment. Uranium and thorium are found in small amounts in most rocks and soil. Two of the main radium isotopes found in the environment are radium-226 and radium-228. Radium undergoes radioactive decay. It divides into two parts-one part is called radiation and the other part is called a daughter. The daughter, like radium, is not stable, and it also divides into radiation and another daughter. The dividing of daughters continues until a stable, nonradioactive daughter is formed. During the decay process, alpha, beta, and gamma radiation are released. Alpha particles can travel only a short distance and cannot travel through your skin. Beta particles can penetrate through your skin, but they cannot go all the way through your body. Gamma radiation can go all the way through your body. Radium has been used as a radiation source for treating cancer, in radiography of metals, and combined with other metals as a neutron source for research and radiation instrument calibration. Until the 1960s, radium was a component of the luminous paints used for watch and clock dials, intrument panels in airplanes, military instruments, and compasses.|Radium atom is an alkaline earth metal atom.|Uranium, radium, and radon are naturally occurring radionuclides found in the environment. No information is available on the acute (short-term) noncancer effects of the radionuclides in humans. Animal studies have reported inflammatory reactions in the nasal passages and kidney damage from acute inhalation exposure to uranium. Chronic (long-term) inhalation exposure to uranium and radon in humans has been linked to respiratory effects, such as chronic lung disease, while radium exposure has resulted in acute leukopenia, anemia, necrosis of the jaw, and other effects. Cancer is the major effect of concern from the radionuclides. Radium, via oral exposure, is known to cause bone, head, and nasal passage tumors in humans, and radon, via inhalation exposure, causes lung cancer in humans. Uranium may cause lung cancer and tumors of the lymphatic and hematopoietic tissues. EPA has not classified uranium, radon or radium for carcinogenicity.|Radium is an element with atomic symbol Ra, atomic number of 88, and atomic weight 226.0|A radioactive element of the alkaline earth series of metals. It has the atomic symbol Ra and atomic number 88. Radium is the product of the disintegration of URANIUM and is present in pitchblende and all ores containing uranium. It is used clinically as a source of beta and gamma-rays in radiotherapy, particularly BRACHYTHERAPY.

Medical treatment for malignant growths, ind- ustrial radiography, source of neutrons and radon. Radium’s most important use is as a source of radiation in industry, medicine, and laboratories. The isotope radium-226, which is the most abundant of all the 25 isotopes and has ahalf-life of 1630 years, is the only useful form of the element. It is used in the medical treatment of malignant cancer growth. It kills cancer cells that have spread throughout the body.Other uses are to produce phosphorescence and fluorescence in organic compounds andfor scintillation screens on instruments used to detect radiation. Radium salts were used in thepast to paint the dials of luminous clock faces that glow in the dark. In 1909, the famous Rutherford experiment used radium as an alpha source to probe the atomic structure of gold. This experiment led to the Rutherford model of the atom and revolutionized the field of nuclear physics. Radium (usually in the form of RaCl2) was used in medicine to produce radon gas which in turn was used as a cancer treatment. For example, several radon sources were used in Canada in the 1920s and 1930s. The isotope
223
Ra is currently under investigation for its use in cancer treatment of bone metastasis. Some of the few practical uses of radium are derived from its radioactive properties. More recently discovered radioisotopes, such as
60
Co and
137
Cs are replacing radium in even these limited uses because several of these isotopes are more powerful emitters, safer to handle, and available in more concentrated form.

Molecular Weight:226.02541
Exact Mass:226.02541
Monoisotopic Mass:226.02541
Heavy Atom Count:1
Covalently-Bonded Unit Count:1
Compound Is Canonicalized:Yes