86Rn222.01758
Noble gas

Radon

Radon is a colorless, odorless, radioactive noble gas that forms naturally as certain rocks and soils slowly release it during the radioactive decay of uranium and radium. Because it's completely undetectable by human senses yet radioactive, it's taken seriously today as an indoor air quality hazard, especially when it seeps into basements and accumulates in poorly ventilated buildings.

Group · Period
18 · 6
At room temp
gas
Melts at
202 K
Density
0.00973 g/cm³
Discovered
1900

Uses

Radon has very few practical uses today, largely because its radioactivity makes it more of a hazard to manage than a resource to exploit. In the early-to-mid 20th century, small sealed capsules of radon gas, called radon seeds, were occasionally used in a form of radiotherapy to treat tumors, since the radiation it emits can damage cancerous tissue; this practice has almost entirely been replaced by safer, more precisely controlled radiation sources. Radon is also occasionally used in scientific research, for instance as a natural tracer that helps geologists study fault lines, groundwater movement, or soil permeability, since its concentration in air or water reflects underlying geological activity.

By far radon’s most significant modern relevance is as something to be monitored and reduced rather than used — building codes and health agencies in many countries recommend testing homes for radon and installing ventilation systems to keep indoor concentrations low.

History

Radon was discovered in 1900 by German physicist Friedrich Ernst Dorn, who noticed that samples of radium continually released a radioactive gas as part of their natural decay process. He referred to it as “radium emanation,” and other researchers around the same period identified similar emanations from thorium and actinium, which were later understood to be different isotopes of the same element. It eventually took the name radon to reflect its connection to radium and its place as a member of the noble gas group, once chemists confirmed that all these “emanations” were really the same chemical element.

Fun facts

  • Radon is the only naturally occurring element that is a gas at room temperature and also radioactive.
  • Radon exposure in homes is considered a leading cause of lung cancer in non-smokers, which is why many countries recommend testing basements and ground-floor rooms for it.
  • Being a noble gas, radon barely reacts chemically with anything, so it simply seeps up through soil and rock and diffuses into the air rather than binding into stable compounds.

Frequently asked questions

Why is radon dangerous if it's chemically unreactive like other noble gases?

Radon's danger has nothing to do with chemical reactivity — it comes from radioactivity. When inhaled, radon and the radioactive particles it decays into can damage lung tissue over time, which is why long-term exposure, especially in enclosed spaces like basements, is linked to an increased risk of lung cancer.

How does radon get into homes if it comes from rock and soil?

Radon gas seeps up naturally from uranium- and radium-bearing rock and soil beneath and around buildings, and it can enter through cracks in foundations, gaps around pipes, or sump pits. It tends to build up most in basements and ground-floor spaces with limited airflow, which is why testing and ventilation matter most there.

Who discovered radon and how?

German scientist Friedrich Ernst Dorn discovered radon in 1900 while studying radium, noticing that radium samples continuously gave off a radioactive gas as they decayed. He initially called it "radium emanation," and it was only later given the name radon, tying it to its place among the other noble gases.

Compounds

1 notable compound containing Rn

  • RnF2halide

    Radon difluoride

    A compound inferred from radiotracer experiments in which radon gas reacts with fluorine to form a nonvolatile solid; because radon decays so quickly, it has never been produced or observed in a visible, weighable amount, so its properties remain only partly established.

    Used for: No practical use — studied only to probe the chemistry of a normally 'inert' gas

Isotopes

39 known isotopes

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IsotopeNatural abundanceHalf-lifeDecay modeMass excessBinding energy / nucleonDecay width
Rn-210 2.4 h Alpha decay (96%), Electron capture / beta-plus decay (4%) -9,604.76 keV 7,796.67 keV 5.28 × 10-20 eV
Rn-211 14.6 h Electron capture (72.6%), Alpha decay (27.4%) -8,755.33 keV 7,793.94 keV 8.68 × 10-21 eV
Rn-222 3.8235 d Alpha decay (100%) 16,371.96 keV 7,694.5 keV 1.38 × 10-21 eV
Show all 39 isotopes
Rn-193 1.15 ms Alpha decay (100%) 9,042.92 keV 7,675.85 keV 3.97 × 10-13 eV
Rn-194 0.78 ms Alpha decay (100%) 5,724.62 keV 7,695 keV 5.85 × 10-13 eV
Rn-195 6 ms Alpha decay (100%) 5,050.29 keV 7,700.38 keV 7.60 × 10-14 eV
Rn-196 4.4 ms Alpha decay (99.9%), Electron capture / beta-plus decay (0.06%) 1,975.17 keV 7,717.97 keV 1.04 × 10-13 eV
Rn-197 65 ms Alpha decay (100%) 1,510.37 keV 7,722.12 keV 7.02 × 10-15 eV
Rn-198 65 ms Electron capture / beta-plus decay, Alpha decay -1,230.32 keV 7,737.72 keV 7.02 × 10-15 eV
Rn-199 0.59 s Alpha decay (94%), Electron capture / beta-plus decay (6%) -1,559.85 keV 7,741.06 keV 7.73 × 10-16 eV
Rn-200 1.03 s Alpha decay (86%), Electron capture / beta-plus decay (14%) -4,000.45 keV 7,754.91 keV 4.43 × 10-16 eV
Rn-201 7.0 s Electron capture / beta-plus decay, Alpha decay -4,107.41 keV 7,757.02 keV 6.52 × 10-17 eV
Rn-202 9.7 s Alpha decay (78%), Electron capture / beta-plus decay (22%) -6,274.56 keV 7,769.3 keV 4.70 × 10-17 eV
Rn-203 44.2 s Alpha decay (66%), Electron capture / beta-plus decay (34%) -6,184.05 keV 7,770.34 keV 1.03 × 10-17 eV
Rn-204 74.5 s Alpha decay (72.4%), Electron capture / beta-plus decay (27.6%) -7,970.12 keV 7,780.57 keV 6.12 × 10-18 eV
Rn-205 170 s Electron capture / beta-plus decay (75.4%), Alpha decay (24.6%) -7,709.76 keV 7,780.72 keV 2.68 × 10-18 eV
Rn-206 5.67 m Alpha decay (62%), Electron capture / beta-plus decay (38%) -9,132.92 keV 7,789.04 keV 1.34 × 10-18 eV
Rn-207 9.25 m Electron capture / beta-plus decay (79%), Alpha decay (21%) -8,634.74 keV 7,788 keV 8.22 × 10-19 eV
Rn-208 24.35 m Alpha decay (62%), Electron capture / beta-plus decay (38%) -9,655.39 keV 7,794.27 keV 3.12 × 10-19 eV
Rn-209 28.8 m Electron capture / beta-plus decay (83%), Alpha decay (17%) -8,941.05 keV 7,792.18 keV 2.64 × 10-19 eV
Rn-212 23.9 m Alpha decay (100%) -8,659.22 keV 7,794.8 keV 3.18 × 10-19 eV
Rn-213 19.4 ms Alpha decay (100%) -5,695.95 keV 7,782.18 keV 2.35 × 10-14 eV
Rn-214 259 ns Alpha decay (100%) -4,319.66 keV 7,777.1 keV 1.76 × 10-9 eV
Rn-215 2.30 us Alpha decay (100%) -1,168.99 keV 7,763.82 keV 1.98 × 10-10 eV
Rn-216 45 us Alpha decay (100%) 253.31 keV 7,758.66 keV 1.01 × 10-11 eV
Rn-217 0.54 ms Alpha decay (100%) 3,658.57 keV 7,744.4 keV 8.45 × 10-13 eV
Rn-218 33.75 ms Alpha decay (100%) 5,217.41 keV 7,738.75 keV 1.35 × 10-14 eV
Rn-219 3.96 s Alpha decay (100%) 8,829.34 keV 7,723.78 keV 1.15 × 10-16 eV
Rn-220 55.6 s Alpha decay (100%) 10,611.99 keV 7,717.26 keV 8.21 × 10-18 eV
Rn-221 25 m Beta-minus decay (78%), Alpha decay (22%) 14,471.35 keV 7,701.39 keV 3.04 × 10-19 eV
Rn-223 24.3 m Beta-minus decay (100%) 20,389.74 keV 7,678.17 keV 3.13 × 10-19 eV
Rn-224 107 m Beta-minus decay (100%) 22,445.1 keV 7,670.75 keV 7.11 × 10-20 eV
Rn-225 4.66 m Beta-minus decay (100%) 26,534.14 keV 7,654.36 keV 1.63 × 10-18 eV
Rn-226 7.4 m Beta-minus decay (100%) 28,747.19 keV 7,646.41 keV 1.03 × 10-18 eV
Rn-227 20.2 s Beta-minus decay (100%) 32,885.84 keV 7,630.05 keV 2.26 × 10-17 eV
Rn-228 65 s Beta-minus decay (100%) 35,243.47 keV 7,621.65 keV 7.02 × 10-18 eV
Rn-229 12.0 s Beta-minus decay (100%) 39,362.4 keV 7,605.62 keV 3.80 × 10-17 eV
Rn-230 Unknown 42,170 keV 7,595 keV
Rn-231 Beta-minus decay (100%) 46,550 keV 7,579 keV