Samarium
Samarium is a moderately hard, silvery lanthanide that was among the first rare-earth elements separated out of the mineral mixtures early chemists were untangling in the 1800s. It's best known today for its very strong permanent magnets and for a radioactive isotope used to ease pain from cancer that has spread to bone.
- Group · Period
- — · 6
- At room temp
- solid
- Melts at
- 1347 K
- Density
- 7.52 g/cm³
- Discovered
- 1879
Uses
Samarium’s most valuable role is in samarium-cobalt magnets, a class of rare-earth permanent magnets developed before the now-more-common neodymium magnets. They’re not as strong at room temperature, but they resist demagnetizing at high temperatures and resist corrosion, which is why they turn up in aerospace components, precision motors, and headphones or microphones that need a small, heat-tolerant magnet. Samarium compounds are also reasonably good at absorbing neutrons, so they’re used in some nuclear reactor control rods alongside elements like europium and gadolinium.
Medicine is samarium’s other notable application: a radioactive isotope, samarium-153, is bonded to a compound that seeks out bone tissue and used to relieve pain in patients whose cancer has spread into their bones. This lets clinicians deliver targeted radiation to affected areas rather than treating the whole body.
History
Samarium was identified in 1879 by French chemist Paul-Émile Lecoq de Boisbaudran, who detected its distinctive spectral lines in a sample derived from the mineral samarskite. Like several other lanthanides, it took more work over the following years to confirm it as a genuinely separate element and eventually isolate it in a purer form, since minerals like samarskite contain a tangle of closely related rare earths. Its name traces back to the mineral it was found in, which had earlier been named after Vasili Samarsky-Bykhovets, a Russian mining official — making samarium one of the first elements named, indirectly, after a real person.
Fun facts
- Samarium-cobalt magnets keep working at much higher temperatures than most other rare-earth magnets, which is why they're chosen for demanding aerospace and military hardware.
- Samarium was named after the mineral samarskite, making it one of the first elements indirectly named after a real person — Russian mine official Vasili Samarsky-Bykhovets.
- A radioactive form of samarium, samarium-153, is used in hospitals to relieve pain caused by cancer that has spread into bone.
Frequently asked questions
What is samarium actually used for?
Its biggest role is in samarium-cobalt magnets, a class of powerful permanent magnets that resist losing their strength even at high temperatures, useful in motors, headphones, and aerospace instruments. Samarium compounds also absorb neutrons well, so they're used in some nuclear reactor control rods, and a radioactive isotope of samarium is used medically to treat bone pain from cancer.
Is samarium radioactive?
Natural samarium is very weakly radioactive — one of its natural isotopes, samarium-147, decays extremely slowly over billions of years, similar to background radiation from many rocks. It's not a health concern in normal use. A different, deliberately produced radioactive isotope, samarium-153, is used in medicine specifically because of its radioactivity.
Why is samarium named after a mineral instead of a place or its properties?
Chemist Paul-Émile Lecoq de Boisbaudran isolated it from a mineral called samarskite, which itself had been named after a Russian mining official, Vasili Samarsky-Bykhovets. That makes samarium one of the earliest elements to carry a person's name, even though the connection is indirect.
Compounds
3 notable compounds containing Sm
- SmI2reagent
Samarium(II) iodide
A deep blue-green solution reagent in which samarium sits in its unusual +2 oxidation state, making it a powerful single-electron reductant.
Used for: Widely used as Kagan's reagent for radical cyclizations in organic synthesis
- SmCl3halide
Samarium(III) chloride
An ionic samarium(III) salt that forms hygroscopic hydrated crystals in air and is the usual starting point for making other samarium compounds.
Used for: Precursor for synthesizing organosamarium and catalytic samarium compounds
- Sm2O3oxide
Samarium(III) oxide
A pale yellow rare-earth oxide formed when samarium metal is burned or its salts are calcined; like other lanthanide sesquioxides it adopts an ionic Sm3+/O2- lattice.
Used for: Infrared-absorbing optical glass and ceramic capacitor additives
Isotopes
40 known isotopes
Swipe to see all columns →
| Isotope | Natural abundance | Half-life | Decay mode | Mass excess | Binding energy / nucleon | Decay width |
|---|---|---|---|---|---|---|
| Sm-144 stable | 3.08% | Stable | — | -81,965.63 keV | 8,303.68 keV | — |
| Sm-147 | 15% | 1.073E11 Y | Alpha decay (100%) | -79,266.05 keV | 8,280.57 keV | 1.35 × 10-34 eV |
| Sm-148 | 11.25% | 7E+15 Y | Alpha decay (100%) | -79,336.07 keV | 8,279.63 keV | 2.07 × 10-39 eV |
| Sm-149 stable | 13.82% | Stable | — | -77,135.9 keV | 8,263.47 keV | — |
| Sm-150 stable | 7.37% | Stable | — | -77,051.34 keV | 8,261.62 keV | — |
| Sm-152 stable | 26.74% | Stable | — | -74,762.98 keV | 8,244.06 keV | — |
| Sm-154 stable | 22.74% | Stable | — | -72,455.56 keV | 8,226.84 keV | — |
Show all 40 isotopes
| Sm-129 | — | 0.55 s | Electron capture / beta-plus decay (100%), ECP (0%) | -42,330 keV | 8,023 keV | 8.30 × 10-16 eV |
| Sm-130 | — | — | Electron capture / beta-plus decay | -47,700 keV | 8,065 keV | — |
| Sm-131 | — | 1.2 s | Electron capture / beta-plus decay (100%), ECP (0%) | -50,280 keV | 8,085 keV | 3.80 × 10-16 eV |
| Sm-132 | — | 4.0 s | Electron capture / beta-plus decay (100%), ECP | -55,140 keV | 8,122 keV | 1.14 × 10-16 eV |
| Sm-133 | — | 2.89 s | Electron capture / beta-plus decay (100%), ECP (0%) | -57,231 keV | 8,137 keV | 1.58 × 10-16 eV |
| Sm-134 | — | 9.5 s | Electron capture / beta-plus decay (100%) | -61,376 keV | 8,167 keV | 4.80 × 10-17 eV |
| Sm-135 | — | 10.3 s | Electron capture / beta-plus decay (100%), ECP (0.02%) | -62,857.22 keV | 8,177.63 keV | 4.43 × 10-17 eV |
| Sm-136 | — | 47 s | Electron capture / beta-plus decay (100%) | -66,810.9 keV | 8,205.92 keV | 9.71 × 10-18 eV |
| Sm-137 | — | 45 s | Electron capture / beta-plus decay (100%) | -67,991.66 keV | 8,213.55 keV | 1.01 × 10-17 eV |
| Sm-138 | — | 3.1 m | Electron capture / beta-plus decay (100%) | -71,497.77 keV | 8,237.93 keV | 2.45 × 10-18 eV |
| Sm-139 | — | 2.57 m | Electron capture / beta-plus decay (100%) | -72,380.23 keV | 8,243.08 keV | 2.96 × 10-18 eV |
| Sm-140 | — | 14.82 m | Electron capture / beta-plus decay (100%) | -75,455.95 keV | 8,263.82 keV | 5.13 × 10-19 eV |
| Sm-141 | — | 10.2 m | Electron capture / beta-plus decay (100%) | -75,933.96 keV | 8,265.85 keV | 7.45 × 10-19 eV |
| Sm-142 | — | 72.49 m | Electron capture / beta-plus decay (100%) | -78,981.93 keV | 8,285.94 keV | 1.05 × 10-19 eV |
| Sm-143 | — | 8.75 m | Electron capture / beta-plus decay (100%) | -79,517.14 keV | 8,288.18 keV | 8.69 × 10-19 eV |
| Sm-145 | — | 340 d | Electron capture (100%) | -80,651.41 keV | 8,293.01 keV | 1.55 × 10-23 eV |
| Sm-146 | — | 6.8E+7 Y | Alpha decay (100%) | -80,996.36 keV | 8,293.86 keV | 2.13 × 10-31 eV |
| Sm-151 | — | 90 Y | Beta-minus decay (100%) | -74,576.48 keV | 8,243.97 keV | 1.61 × 10-25 eV |
| Sm-153 | — | 46.284 h | Beta-minus decay (100%) | -72,560.06 keV | 8,228.54 keV | 2.74 × 10-21 eV |
| Sm-155 | — | 22.18 m | Beta-minus decay (100%) | -70,191.21 keV | 8,211.23 keV | 3.43 × 10-19 eV |
| Sm-156 | — | 9.4 h | Beta-minus decay (100%) | -69,360.74 keV | 8,205.01 keV | 1.35 × 10-20 eV |
| Sm-157 | — | 8.03 m | Beta-minus decay (100%) | -66,677.65 keV | 8,187.06 keV | 9.47 × 10-19 eV |
| Sm-158 | — | 5.30 m | Beta-minus decay (100%) | -65,251.85 keV | 8,177.31 keV | 1.43 × 10-18 eV |
| Sm-159 | — | 11.37 s | Beta-minus decay (100%) | -62,207.85 keV | 8,157.5 keV | 4.01 × 10-17 eV |
| Sm-160 | — | 9.6 s | Beta-minus decay (100%) | -60,233.17 keV | 8,144.62 keV | 4.75 × 10-17 eV |
| Sm-161 | — | 4.8 s | Beta-minus decay (100%) | -56,672.04 keV | 8,122.04 keV | 9.50 × 10-17 eV |
| Sm-162 | — | 2.4 s | Beta-minus decay (100%) | -54,379.05 keV | 8,107.57 keV | 1.90 × 10-16 eV |
| Sm-163 | — | 1.23 s | Beta-minus decay (100%), Beta-minus, neutron emission | -50,599.61 keV | 8,084.17 keV | 3.71 × 10-16 eV |
| Sm-164 | — | 1.43 s | Beta-minus decay (100%), Beta-minus, neutron emission | -47,925.31 keV | 8,067.78 keV | 3.19 × 10-16 eV |
| Sm-165 | — | 0.98 s | Beta-minus decay (100%), Beta-minus, neutron emission | -43,510 keV | 8,041 keV | 4.66 × 10-16 eV |
| Sm-166 | — | 0.80 s | Beta-minus decay (100%), Beta-minus, neutron emission | -40,450 keV | 8,023 keV | 5.70 × 10-16 eV |
| Sm-167 | — | — | Beta-minus decay (100%), Beta-minus, neutron emission | -35,330 keV | 7,992 keV | — |
| Sm-168 | — | — | Beta-minus decay (100%), Beta-minus, neutron emission | -31,640 keV | 7,971 keV | — |