88Ra226.02541
Alkaline earth metal

Radium

Radium is a rare, intensely radioactive alkaline earth metal discovered by Marie and Pierre Curie, whose research into it helped launch the scientific study of radioactivity. It's famous today largely for a cautionary history: its glow-in-the-dark use in paint decades ago caused serious harm to workers before the dangers of radioactivity were properly understood.

Group · Period
2 · 7
At room temp
solid
Melts at
973 K
Density
5 g/cm³
Discovered
1898

Uses

Radium’s most well-known historical use — mixed into luminous paint for watch faces, clock dials, and aircraft instruments so they would glow in the dark — has been completely discontinued since the mid-20th century, once it became clear how dangerous ingesting or inhaling radium particles could be, particularly for the factory workers who painted the dials by hand. Safer luminescent materials replaced it entirely for that purpose decades ago.

Radium does still have a narrow, tightly controlled medical use today: a radioactive isotope called radium-223 is used in an approved treatment for certain prostate cancers that have spread to the bones, where its radiation targets the affected bone tissue directly. Outside of this specific medical application and ongoing scientific research, radium has essentially no other current use, given how hazardous it is to handle.

History

Radium was discovered in 1898 by Marie and Pierre Curie, working in Paris, as they investigated the intense radioactivity coming from uranium ore that couldn’t be explained by its uranium content alone. Painstakingly processing tons of pitchblende ore, they isolated tiny amounts of a new, strongly radioactive element and named it radium, from the Latin word for “ray.” The discovery, made in the same year as their discovery of polonium, was a major milestone in early radioactivity research, though it would take decades longer for scientists and the public to fully grasp how dangerous the element the Curies had found really was.

Fun facts

  • Radium naturally glows a faint blue-green in the dark, a genuine physical effect caused by its intense radioactivity exciting the air and any surrounding material.
  • Marie and Pierre Curie discovered radium in 1898, the same year as polonium, after processing tons of uranium ore to isolate just a tiny amount of it.
  • Radium's name comes from the Latin word radius, meaning 'ray,' a direct reference to the radiation it constantly emits.

Frequently asked questions

Why was radium once used in watch dials?

Mixed into paint, radium makes it glow continuously in the dark because its radioactivity excites certain chemicals, called phosphors, without needing an external light source to "charge" them first. Watch and instrument dials painted with radium paint stayed readable at night for years, which seemed like a wonderful property before the health risks of ingesting or inhaling radium were understood.

What happened to the workers who painted radium dials?

Many dial-painting factory workers, most of them young women, were instructed to shape their paintbrush tips with their lips, ingesting small amounts of radium-laced paint repeatedly over time. This led to severe radiation-related illnesses in many of them, a tragedy that became a landmark case in the history of workplace safety and led to much stricter regulation of radioactive materials.

Is radium used for anything today?

Its glow-in-the-dark paint use has been completely discontinued due to the danger it poses. However, a specific radioactive form of radium, radium-223, is approved as a targeted medical treatment for certain cancers that have spread to bone, where its radiation is used in carefully controlled, tiny doses under strict medical supervision.

Compounds

3 notable compounds containing Ra

  • RaBr2salt

    Radium bromide

    A white, radioluminescent salt that the Curies used in painstaking fractional crystallizations alongside barium bromide to concentrate radium and determine its atomic weight.

    Used for: Used historically to isolate and characterize radium from pitchblende ore

  • RaCl2salt

    Radium chloride

    A white salt that was the first radium compound ever isolated in pure form, by Marie and Pierre Curie in 1898, and one that visibly glows faintly in the dark from its own intense radioactivity.

    Used for: Historic first isolated radium compound, later used in early radiotherapy sources

  • RaSO4mineral

    Radium sulfate

    An extremely insoluble salt that closely mirrors barium sulfate in structure and behavior, which is why trace radium co-precipitates with barite and other barium sulfate minerals in nature.

    Used for: Explains radium's natural association with barium-bearing ores

Isotopes

34 known isotopes

Swipe to see all columns →

IsotopeNatural abundanceHalf-lifeDecay modeMass excessBinding energy / nucleonDecay width
Ra-225 14.9 d Beta-minus decay (100%), Alpha decay (0.026%) 21,993.04 keV 7,667.59 keV 3.54 × 10-22 eV
Ra-226 1600 Y Alpha decay (100%), 14C (3.2e-9%) 23,667.58 keV 7,661.96 keV 9.04 × 10-27 eV
Ra-228 5.75 Y Beta-minus decay (100%) 28,940.19 keV 7,642.43 keV 2.51 × 10-24 eV
Show all 34 isotopes
Ra-201 8 ms Alpha decay (100%) 11,936.82 keV 7,669.41 keV 5.70 × 10-14 eV
Ra-202 16 ms Alpha decay (100%) 9,074.9 keV 7,685.57 keV 2.85 × 10-14 eV
Ra-203 31 ms Alpha decay (100%) 8,601.33 keV 7,689.8 keV 1.47 × 10-14 eV
Ra-204 57 ms Alpha decay (100%) 6,061.1 keV 7,704.12 keV 8.00 × 10-15 eV
Ra-205 210 ms Alpha decay (100%) 5,803.85 keV 7,707.17 keV 2.17 × 10-15 eV
Ra-206 0.24 s Alpha decay (100%) 3,565.61 keV 7,719.8 keV 1.90 × 10-15 eV
Ra-207 1.35 s Alpha decay (86%), Electron capture / beta-plus decay (14%) 3,513.99 keV 7,721.75 keV 3.38 × 10-16 eV
Ra-208 1.3 s Alpha decay (95%), Electron capture / beta-plus decay (5%) 1,727.93 keV 7,732.02 keV 3.51 × 10-16 eV
Ra-209 4.8 s Alpha decay (100%) 1,858.24 keV 7,733.02 keV 9.50 × 10-17 eV
Ra-210 3.7 s Alpha decay (96%), Electron capture / beta-plus decay (4%) 442.84 keV 7,741.37 keV 1.23 × 10-16 eV
Ra-211 13 s Alpha decay (93%), Electron capture / beta-plus decay (7%) 831.87 keV 7,741.09 keV 3.51 × 10-17 eV
Ra-212 13.0 s Alpha decay (85%), Electron capture / beta-plus decay (15%) -198.76 keV 7,747.51 keV 3.51 × 10-17 eV
Ra-213 2.73 m Alpha decay (86%), Electron capture / beta-plus decay (14%) 345.56 keV 7,746.47 keV 2.79 × 10-18 eV
Ra-214 2.438 s Alpha decay (99.941%), Electron capture (0.059%) 92.74 keV 7,749.17 keV 1.87 × 10-16 eV
Ra-215 1.66 ms Alpha decay (100%) 2,532 keV 7,739.32 keV 2.75 × 10-13 eV
Ra-216 182 ns Alpha decay (100%), Electron capture (1e-8%) 3,291.47 keV 7,737.35 keV 2.51 × 10-9 eV
Ra-217 1.6 us Alpha decay (100%) 5,889.54 keV 7,726.91 keV 2.85 × 10-10 eV
Ra-218 25.91 us Alpha decay (100%) 6,645.56 keV 7,725.02 keV 1.76 × 10-11 eV
Ra-219 9 ms Alpha decay (100%) 9,393.85 keV 7,714.06 keV 5.07 × 10-14 eV
Ra-220 18 ms Alpha decay (100%) 10,272.09 keV 7,711.69 keV 2.53 × 10-14 eV
Ra-221 28 s Alpha decay (100%) 12,963.88 keV 7,701.14 keV 1.63 × 10-17 eV
Ra-222 38.0 s Alpha decay (100%), 14C (3e-8%) 14,320.21 keV 7,696.69 keV 1.20 × 10-17 eV
Ra-223 11.43 d Alpha decay (100%), 14C (8.9e-8%), 14C (7.7e-8%) 17,233.25 keV 7,685.31 keV 4.62 × 10-22 eV
Ra-224 3.6316 d Alpha decay (100%), 14C (4e-9%) 18,825.83 keV 7,679.92 keV 1.45 × 10-21 eV
Ra-227 42.2 m Beta-minus decay (100%) 27,177.46 keV 7,648.3 keV 1.80 × 10-19 eV
Ra-229 4.0 m Beta-minus decay (100%), Alpha decay (100%) 32,561.96 keV 7,628.49 keV 1.90 × 10-18 eV
Ra-230 93 m Beta-minus decay (100%) 34,516.31 keV 7,621.91 keV 8.18 × 10-20 eV
Ra-231 103.9 s Beta-minus decay (100%) 38,216.49 keV 7,607.84 keV 4.39 × 10-18 eV
Ra-232 4.2 m Beta-minus decay (100%) 40,496.96 keV 7,600.01 keV 1.81 × 10-18 eV
Ra-233 30 s Beta-minus decay (100%) 44,334.06 keV 7,585.56 keV 1.52 × 10-17 eV
Ra-234 30 s Beta-minus decay (100%) 46,930.63 keV 7,576.54 keV 1.52 × 10-17 eV