|Classification:||Radon is a noble gas and a nonmetal|
|Atomic weight:||(222), no stable isotopes|
|Melting point:||-71 oC, 202 K|
|Boiling point:||-62 oC, 211 K|
|Neutrons in most abundant isotope:||136|
|Electron configuration:||[Xe] 4f14 5d10 6s2 6p6|
|Density @ 20oC:||0.00973 g/cm3|
|Atomic volume:||50.5 cm3/mol|
|Specific heat capacity||0.09 J g-1 K-1|
|Heat of fusion||2.890 kJ mol-1|
|Heat of atomization||0 kJ mol-1|
|Heat of vaporization||16.40 kJ mol-1|
|1st ionization energy||1037 kJ mol-1|
|2nd ionization energy||–|
|3rd ionization energy||–|
|Minimum oxidation number||0|
|Min. common oxidation no.||0|
|Maximum oxidation number||0|
|Max. common oxidation no.||0|
|Electronegativity (Pauling Scale)||–|
|Polarizability volume||5.3 Å3|
|Reaction with air||none|
|Reaction with 15 M HNO3||none|
|Reaction with 6 M HCl||none|
|Reaction with 6 M NaOH||none|
|Ionic radius (1+ ion)||–|
|Ionic radius (2+ ion)||–|
|Ionic radius (3+ ion)||–|
|Ionic radius (1- ion)||–|
|Ionic radius (2- ion)||–|
|Ionic radius (3- ion)||–|
|Thermal conductivity||3.61 W m-1 K-1|
|Freezing/Melting point:||-71 oC, 202 K|
Discovery of Radon
Radon gas was discovered in 1900 by Fredrich E. Dorn in Halle, Germany. He described it as radium emanation because it arose from the element radium, which he was working with.
In 1908 William Ramsay and Robert Gray isolated the gas and named it niton.
Since 1923, it has been called radon (after radium, one of its sources).
Appearance and Characteristics
Radon is highly radioactive and a carcinogen. Its decay products are toxic and radioactive. Radon is present in most homes and is the number one cause of lung-cancer in non-smokers in the USA. (See video on left.)
Radon is one of the noble gases; hence it is a chemically inert, monatomic gas.
It is also radioactive, colorless and odorless.
Radon is produced naturally by the decay of uranium’s decay products, such as 226Ra.
Uses of Radon
Radon was used for treating cancer by radiotherapy. Safer treatments are now available.
Abundance and Isotopes
Abundance earth’s crust: 4 x10-13 milligrams per kilogram
Abundance solar system:
Cost, pure: $ per 100g
Cost, bulk: $ per 100g
Source: Radon is produced naturally by the radioactive decay of uranium and other elements, such as radium. For example, 222Rn is produced by the decay of radium (226Ra).
Isotopes: Radon has 33 isotopes whose half-lives are known, with mass numbers 196 to 228. None are stable. The most stable isotope is 222Rn, with a half-life of 3.8 days.
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