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Radium


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Atomic symbol: Ra
Atomic number: 88
Atomic weight: 226.0254
Atomic volume: 45.20 cm3/mol
Density: 5 g/cm3
Period Number: 7
Group number: 2
Group name: Alkali Earth
Element classification: Metal


States


Phase at room temperature: Solid
Melting Point: 973.2 K
Boiling point: 1973 K
Heat of fusion: ?
Heat of vaporization: ?


Energies


Ionization Energy: 5.279 eV
1st ionization energy: 509.4 kJ/mole
2nd ionization energy: 979.1 kJ/mole
3rd ionization energy: kJ/mole
Electronegativity: 0.9
Electron affinity: kJ/mole
Specific heat: 0.12 J/gK
Heat atomization: 159 kJ/mole atoms


Oxidation & Electrons


Shells: 2,8,18,32,18,8,2
Electron Shell Configuration: [Rn] 7s2
Minimum oxidation number: 0
Maximum oxidation number: 2
Minimum common oxidation number: 0
Maximum common oxidation no: 2


Appearance & Characteristics


Structure:: bcc: body-centered cubic
Color: white
Hardness: mohs
Toxicity: ?
Characteristics: Radioactive, luminescent
Uses: neutron source


Reactions


Reaction with air: vigorous, =>RaO2, Ra3N2
Reaction with 6M HCl: ?
Reaction with 15M HNO3: ?
Reaction with 6M NaOH: ?


Other Forms


Number of isotopes: 4
Oxide(s): ?
Hydride(s): ?
Chloride(s): RaCl2


Radius


Atomic Radius: pm
Ionic radius (1- ion): pm
Ionic radius (1+ ion): pm
Ionic radius (2- ion): pm
Ionic radius (2+ ion): 162 pm
Ionic radius (3+ ion): pm


Conductivity


Thermal conductivity: 18.6 J/m-sec-deg
Electrical conductivity: 1/mohm-cm
Polarizability: 38.3 A^3


Abundance


Source: pitchblende(U-238 decay)
Relative abundance solar system: log
Abundance earth's crust: -6 log
Estimated crustal abundance: 9×10-7 milligrams per kilogram
Estimated oceanic abundance: 8.9×10-11 milligrams per liter
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 
 


History


(L. radius: ray) Radium was discovered in 1898 by Mme. Curie in the pitchblende or uraninite of North Bohemia, where it occurs. There is about 1 g of radium in 7 tons of pitchblende. The element was isolated in 1911 by Mme. Curie and Debierne by the electrolysis of a solution of pure radium chloride employing a mercury cathode; on distillation in an atmosphere of hydrogen, this amalgam yielded the pure metal.


Sources


Originally, radium was obtained from the rich pitchblende ore found in Joachimsthal, Bohemia. The carnotite sands of Colorado furnish some radium, but richer ores are found in the Republic of Zaire and the Great Lake region of Canada. Radium is present in all uranium minerals, and could be extracted, if desired, from the extensive wastes of uranium processing. Large uranium deposits are located in Ontario, New Mexico, Utah, Australia, and elsewhere.


Properties


Radium is obtained commercially as bromide and chloride; it is doubtful if any appreciable stock of the isolated element now exists. The pure metal is brilliant white when freshly prepared, but blackens on exposure to air, probably due to formation of the nitride. It exhibits luminescence, as do its slats; it decomposes in water and is somewhat more volatile than barium. It is a member of the alkaline-earth group of metals. Radium imparts a carmine red color to a flame. Radium emits alpha, beta, and gamma rays and when mixed with beryllium produce neutrons. One gram of 226Ra undergoes 3.7 x 1010 disintegrations per second. The curie is defined as that amount of radioactivity which has the same disintegration rate as 1 g of 226Ra. Twenty five isotopes are now known; radium 226, the common isotope, has a half-life of 1600 years.


Uses


One gram of radium produces about 0.0001 ml (stp) of emanation, or radon gas, per day. This is purged from the radium and sealed in minute tubes, which are used in the treatment of cancer and other diseases. Radium was used in the producing of self-luminous paints, neutron sources, and in medicine for the treatment of disease. Other radioisotopes, such as 60Co, are now being used in place of radium. Some of these sources are much more powerful, and others are safer to use. Radium loses about 1% of its activity in 25 years, being transformed into elements of lower atomic weight. Lead is a final product of disintegration. Stored radium and radium-containing products or minerals should be ventilated to prevent build-up of radon.

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