Radon in Periodic Table
Radon (Rn), a chemical element or noble gas of Group 18 of the periodic table discovered by Ernest Rutherford and Soddy in 1899 from the decay of radioactive substances. It is a colorless, odorless, tasteless, and heavy radioactive noble gas obtained from radium-226 by alpha particle emission. Naturally, a small quantity of radon is formed during the radioactive decay or chain reaction of uranium and thorium. The longest-lived radioactive isotope of radon-222 has a half-life of 3.8 days. Due to the very short-lived, the study of the element is extremely difficult. It has no stable isotopes but it formed thirty-nine radioactive isotopes with atomic mass 193 to 231.
The radioactive rare gas, radon has the chemical symbol Rn, atomic number 86, atomic weight 222 (for most stable isotope), melting point -71 °C, boiling point -61.7 °C, valence shell electron configuration [Xe] 4f14 5d10 6s2 6p6. It is colorless at ambient temperature but when cooled below its melting point, it emits brilliant yellow phosphorescence. The color changes to orange-red when cooled with liquid nitrogen. At room temperature, the density and solubility of radon in water are highest among all noble gases like helium, neon, argon, krypton, and xenon.
Occurrence and Properties
Radon-222 is the longest-lived isotope of the element with a half-life of 3.8 days. It is a member of all three natural radioactive series. Radon is produced directly by alpha-ray decay of an aqueous solution of radium chloride (88Ra226 → 86Rn222 + 2He4). The gas is largely diluted by ozone, hydrogen, and oxygen produced from the alpha-irradiation of water. The mixture of gases passed over heated copper and copper (II) oxide and finally dried with phosphorus pentoxide to obtained pure radon.
Like other noble gases, it is also a member of zero valence elements which make it chemically inert. The ionization energy of radon is slightly lower than xenon. The fact suggests that the chemical element Ra is more reactive than Xe. Due to the small half-life, the study of the chemical properties of radon is very difficult. It is naturally used as a natural tracer for chemical analysis.
Chemistry of Radon
Inspired by the development of xenon chemistry, it is logical to form rich chemistry of radon from energy consideration. But due to the very short life and small availability of the element in the earth’s atmosphere, making its study very difficult in science. One gram of Ra-226 produces only 1g of Ra. Therefore, the study of radon chemistry is restricted to tracer studies. It may be easily detected by its radioactivity which causes lung cancer by breathing. According to the United State Environmental pollution agency, it is the second material that caused lung cancer after cigarette smoking. It is volatile above -80 °C but the compounds are not volatile at the same condition.
Radon reacts with fluorine gas at room temperature or liquid fluorine at -196 °C, the reaction vessel retains some gamma-activity after the volatile substance is pumped out. This suggests that ionic chemical bond might be formed in ionic fluoride like Rn+F– or (RnF+)F–. The fluorine molecule is reduced by hydrogen gas at 500 °C to set free the element from the fluoride compound. It is also oxidized by several interhalogen cations to give Rn+ or RnF+ which may be retained by cation exchange resin. Similar oxidation may be carried out in liquid chlorine trifluoride (ClF3) or bromine trifluoride (BrF3). On electrolysis, the radon is found to move to a positive electrode or cathode, which suggests that it formed cationic species on electrolysis.
Uses and Effect of Radon
The electromagnetic spectrum radiation from radioactive radon is used in testing metal casting, industrial radiography, and radiation therapy in medicine to damage the carcinogenic cancer cell. Changes in the concentration of radon in groundwater are the symbol to predict the Earthquake of our environment. It is prepared commercially for use in radiation therapy but most of the materials used as a nucleotide in the reactor of the nuclear power plants. Radon occurs in nature as a gas that affects human health to causes lung cancer due to the formation of free radicals. Radon is a known pollutant when it is emitted from renewable energy sources like geothermal power stations but it does not more impact on our earth’s environment or human health.