Samarium (Sm)
lanthanideSolid
표준 원자량
150.36 u전자 배치
[Xe] 6s2 4f6녹는점
1073.85 °C끓는점
1793.85 °C밀도
7520 kg/m³산화 상태
0, +1, +2, +3전기 음성도(Pauling)
1.17제1 이온화 에너지
5.643722 eV발견 연도
1878원자 반지름
185 pm상세 정보
Samarium is a lanthanide metal with atomic number 62. It is a typical rare-earth element in its trivalent chemistry, but it is also notable for accessible divalent compounds and for the strong neutron-absorbing isotope ¹⁴⁹Sm. The element occurs with other light rare earths in minerals such as monazite and bastnäsite. Its technological importance is concentrated in permanent magnets, neutron control, phosphors, and specialized chemical reducing agents.
Samarium has a bright silver luster and is reasonably stable in air. Three crystal modifications of the metal exist, with transformations at 734 and 922°C. The metal ignites in air at about 150°C. The sulfide has excellent high-temperature stability and good thermoelectric efficiencies up to 1100°C.
The name derives from the mineral samarskite, in which it was found and that had been named for Colonel Samarski, a Russian mine official. Samarium was originally discovered in 1878 by the Swiss chemist Marc Delafontaine, who called it decipium. It was also discovered by the French chemist Paul-Emile Lecoq de Boisbaudran in 1879. In 1881, Delafontaine determined that his decipium could be resolved into two elements, one of which was identical to Boisbaudran's samarium. In 1901, the French chemist Eugène-Anatole Demarçay showed that this samarium earth also contained europium.
Samarium was observed spectroscopically by Jean Charles Galissard de Marignac, a Swiss chemist, in a material known as dydimia in 1853. Paul-Émile Lecoq de Boisbaudran, a French chemist, was the first to isolate samarium from the mineral samarskite ((Y, Ce, U, Fe)3(Nb, Ta, Ti)5O16) in 1879. Today, samarium is primarily obtained through an ion exchange process from monazite sand ((Ce, La, Th, Nd, Y)PO4), a material rich in rare earth elements that can contain as much as 2.8% samarium.
Discovered spectroscopically by its sharp absorption lines in 1879 by Lecoq de Boisbaudran in the mineral samarskite, named in honor of a Russian mine official, Col. Samarski.
Pure samarium is a silvery, moderately hard metal that tarnishes in air as oxide forms on the surface. It has the close-packed metallic character typical of lanthanides and is normally handled as ingots, pieces, powder, or alloy feedstock under conditions that limit oxidation.
The largest distinctive use of samarium is in samarium-cobalt permanent magnets, mainly SmCo₅ and Sm₂Co₁₇, which retain magnetization at higher temperatures and resist corrosion better than many neodymium magnets. ¹⁴⁹Sm is an effective neutron absorber and samarium compounds are used in control materials and reactor physics applications. Samarium-doped materials serve in some phosphors, lasers, and infrared-absorbing glasses. Samarium(II) iodide, SmI₂, is an important one-electron reducing reagent in organic synthesis.
Samarium is one of the rare earth elements used to make carbon arc lights which are used in the motion picture industry for studio lighting and projector lights. Samarium also makes up about 1% of Misch metal, a material that is used to make flints for lighters.
Samarium forms a compound with cobalt (SmCo5) which is a powerful permanent magnet with the highest resistance to demagnetization of any material known. Samarium oxide (Sm2O3) is added to glass to absorb infrared radiation and acts as a catalyst for the dehydration and dehydrogenation of ethanol (C2H6O).
Samarium, along with other rare earths, is used for carbon-arc lighting for the motion picture industry. SmCo5 has been used in making a new permanent magnet material with the highest resistance to demagnetization of any known material. It is said to have an intrinsic coercive force as high as 2200 kA/m. Samarium oxide has been used in optical glass to absorb the infrared. Samarium is used to dope calcium fluoride crystal for use in optical lasers or lasers. Compounds of the metal act as sensitizers for phosphors excited in the infrared; the oxide exhibits catalytic properties in the dehydration and dehydrogenation of ethyl alcohol. It is used in infrared absorbing glass and as a neutron absorber in nuclear reactors.
Isotopes in Earth/Planetary Science
One possible origin for the Moon is from debris ejected by an indirect giant impact of Earth by an astronomical body the size of Mars when the Earth was forming [436] R. M. Canup, E. Asphaug. Nature412, 708 (2001).. The kinetic energy liberated is thought to have melted a large part of the Moon forming a lunar magma ocean. Samarium isotope measurement results [437] A. Brandon. Nature450, 1169 (2007)., along with measurements of isotopes of hafnium, tungsten, and neodymium [438] K. Righter, C. K. Shearer. Geochim. Cosmochim. Acta67, 2497 (2003)., suggest that lunar magma formed about 70×106 years after the Solar System formed and had crystallized by about 215×106 years after formation. 147Sm (with a half-life of 1.06×1011 years) is used to study the formation of potassium, rare earth elements, and phosphorus-rich rocks [439] J. Edmunson, L. E. Borg. “The formation age of KREEP based on the 147Sm-143Nd geochemistry of KREEP-rich rocks: duration of lunar magma ocean crystallization and similarity to early mars”, in Workshop on Early Planetary Differentiation..
Isotopes in Geochronology
147Sm is used for determining formation ages of igneous and metamorphic rocks via analysis of the minerals which compose them, such as those shown in Fig. IUPAC.62.1 [440] T. Iizuka, O. Nebel, M. McCulloch. Early Crustal Evolution Deduced from a Combined U-Pb and Sm-Nd Isotopic Study of Mt. Narryer and Jack Hills Monazites, The Australian National University (2014), Feb. 28; http://rses.anu.edu.au/highlights/view.php?article=191., [441] K. Rankenburg, A. D. Brandon, C. R. Neal. Science312 1369 (2006)., [442] F. F. Hu, H. R. Fan, S. Liu, K. F. Yang, F. Chen. Resour. Geol.59, 407 (2009)..
Isotopes in Medicine
The radioisotope 153Sm (with a half-life of 1.9 days) is used in medicine to treat the severe pain associated with cancer that has spread to bones (Fig. IUPAC.62.2) [443] International Atomic Energy Agency. Optimization of Production and Quality Control of Therapeutic Radionuclides and Radiopharmaceuticals, IAEA-TECDOC-1114, IAEA VIENNA (1999)., [444] C. L. Maini, S. Bergomi, L. Romano, R. Sciuto. Eur. J. Nucl. Med. Mol. Imaging31, S171 (2004)., [445] N. Pandit-Taskar, M. Batraki, C. R. Divgi. J. Nucl. Med.45, 1358 (2004)..
Isotopes Used as a Source of Radioactive Isotope(s)
147Sm bombarded with 40Ca produces the radioisotope 182Pb [446] K. S. Toth, D. M. Moltz, J. M. Nitschke, P. A. Wilmarth, J. D. Robertson. AIP Conference Proc.283, 347 (1991)..
Samarium most commonly forms Sm³⁺ salts and oxides. Samarium(III) oxide, Sm₂O₃, is a stable sesquioxide used as a starting material for many other compounds. Halides such as samarium(III) chloride, SmCl₃, and samarium(III) fluoride, SmF₃, are typical ionic rare-earth salts. The Sm²⁺ state is less common but chemically important; samarium(II) iodide, SmI₂, is a mild, selective reductant, and samarium(II) sulfide, SmS, shows pressure-sensitive electronic behavior. Mixed-valence chemistry is known in some solids.
See more information at the Samarium compound page.
Compact samarium metal has low acute toxicity, but finely divided metal can burn and should be kept from ignition sources. Dusts and soluble samarium salts may irritate tissues and should not be inhaled or ingested. Natural samarium is weakly radioactive because of long-lived isotopes, especially ¹⁴⁷Sm and ¹⁴⁸Sm, but its specific activity is low. Reactor-produced or isotope-enriched materials can present additional radiation hazards depending on isotopic composition.
Little is known of the toxicity of samarium; therefore, it should be handled carefully.
Samarium is dispersed in the crust as a minor component of rare-earth minerals rather than as native metal. In soils and waters it is generally present as Sm³⁺ associated with phosphates, carbonates, oxides, and organic ligands. It is not known to have an essential biological role. Mining and processing can mobilize samarium together with other rare earths and, in monazite deposits, with thorium and uranium by-products.
Samarium is produced as part of rare-earth separation rather than from samarium-specific ores. Concentrates from monazite and bastnäsite are chemically processed, and individual rare earths are separated by solvent extraction or ion-exchange methods before conversion to oxides, metals, or alloys. Demand is much smaller than for cerium, lanthanum, or neodymium, but it is strategically important where high-temperature Sm-Co magnets are required. Recycling is limited compared with primary production, partly because samarium is often present in durable, specialized magnet assemblies.
Samarium is found along with other members of the rare-earth elements in many minerals, including monazite and bastnasite, which are commercial sources. It occurs in monazite to the extent of 2.8%. While misch metal containing about 1% of samarium metal, has long been used, samarium has not been isolated in relatively pure form until recently. Ion-exchange and solvent extraction techniques have recently simplified separation of the rare earths from one another; more recently, electrochemical deposition, using an electrolytic solution of lithium citrate and a mercury electrode, is said to be a simple, fast, and highly specific way to separate the rare earths. Samarium metal can be produced by reducing the oxide with lanthanum.
Samarium is a heavy element made mainly by neutron-capture processes in earlier generations of stars. Its stable and long-lived isotopes reflect contributions from both slow and rapid neutron-capture nucleosynthesis. In planetary materials it is lithophile and follows other rare earths into refractory minerals, making samarium-neodymium isotope systematics useful in geochemistry and cosmochemistry.
- Samarium was named from the mineral samarskite, which was itself named after Vasili Samarsky-Bykhovets.
- ¹⁴⁷Sm decays very slowly to ¹⁴³Nd and is used in Sm-Nd radiometric dating.
- ¹⁴⁹Sm has one of the largest thermal-neutron capture cross sections among naturally occurring nuclides.
- Samarium-cobalt magnets preceded modern neodymium-iron-boron magnets in many high-performance applications.
- SmS can change from a black semiconducting phase toward a golden metallic state under pressure.
이미지
특성
물리적 특성
- 원자 반지름(경험값)
- 185 pm 모든 원소의 원자 반지름(경험값) 비교 →
- 공유 결합 반지름
- 198 pm 모든 원소의 공유 결합 반지름 비교 →
- 반데르발스 반지름
- 229 pm 모든 원소의 반데르발스 반지름 비교 →
- 밀도
- 7520 kg/m³ 모든 원소의 밀도 비교 →
- 몰 부피
- 0.0199 L/mol
- STP에서의 상
- 고체 모든 원소의 STP에서의 상 비교 →
- 녹는점
- 1073.85 °C 모든 원소의 녹는점 비교 →
- 끓는점
- 1793.85 °C 모든 원소의 끓는점 비교 →
- 비열
- 0.197 J/(g·K) 모든 원소의 비열 비교 →
- 몰 열용량
- 29.54 J/(mol·K) 모든 원소의 몰 열용량 비교 →
- 결정 구조
- 능면체 모든 원소의 결정 구조 비교 →
화학적 특성
- 전기 음성도(Pauling)
- 1.17 모든 원소의 전기 음성도(Pauling) 비교 →
- 전자 친화도
- 0.156 eV
- 제1 이온화 에너지
- 5.643722 eV 모든 원소의 제1 이온화 에너지 비교 →
- 제2 이온화 에너지
- 11.078038 eV 모든 원소의 제2 이온화 에너지 비교 →
- 제3 이온화 에너지
- 23.550081 eV 모든 원소의 제3 이온화 에너지 비교 →
- 제4 이온화 에너지
- 41.640143 eV 모든 원소의 제4 이온화 에너지 비교 →
- 제5 이온화 에너지
- 62.700216 eV 모든 원소의 제5 이온화 에너지 비교 →
- 산화 상태
- 0, +1, +2, +3 모든 원소의 산화 상태 비교 →
- 원자가 전자
- 3 모든 원소의 원자가 전자 비교 →
- 전자 배치
- [Xe] 6s2 4f6
열역학적 특성
- 융해열
- 0.08934031 eV 모든 원소의 융해열 비교 →
- 기화열
- 1.71011 eV 모든 원소의 기화열 비교 →
- 승화열
- 2.145411 eV
- 원자화열
- 2.145411 eV
- 원자화 엔탈피
- 2.142302 eV
핵 특성
- 양성자 수
- 62 모든 원소의 양성자 수 비교 →
- 중성자 수
- 90 모든 원소의 중성자 수 비교 →
- 알려진 동위원소 수
- 41 모든 원소의 알려진 동위원소 수 비교 →
- 안정 동위원소 수
- 3 모든 원소의 안정 동위원소 수 비교 →
- 가장 안정한 동위원소
- Sm-152
- 발견 연도
- 1878
존재비
- 존재비(지각)
- 7.05 mg/kg 모든 원소의 존재비(지각) 비교 →
- 존재비(해양)
- 4.5 × 10−7 mg/L 모든 원소의 존재비(해양) 비교 →
결정 구조
- 격자 상수 a
- 900 pm
전자 구조
- 전자껍질별 전자 수
- 2, 8, 18, 24, 8, 2 모든 원소의 전자껍질별 전자 수 비교 →
식별자
- CAS 등록 번호
- 7440-19-9 모든 원소의 CAS 등록 번호 비교 →
- 항 기호
- 7F0
- InChI
- InChI=1S/Sm
- InChI 키
- KZUNJOHGWZRPMI-UHFFFAOYSA-N
전자 배치 측정값
Sm: 4f⁶ 6s²[Xe] 4f⁶ 6s²1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s² 4p⁶ 4d¹⁰ 5s² 5p⁶ 4f⁶ 6s²원자 모형
동위원소에 따라 중성자 수, 질량, 안정성은 달라지지만, 중성 원자의 전자 배치는 달라지지 않습니다.
개략적인 원자 모형이며 실제 비율과 다릅니다.
원자 지문
방출 / 흡수 스펙트럼
동위원소 분포
| 질량수 | 원자 질량(u) | 천연 존재비 | 반감기 |
|---|---|---|---|
| 144 안정 | 143.9120065 ± 0.0000021 | 3.0700% | 안정 |
| 150 안정 | 149.9172829 ± 0.0000018 | 7.3800% | 안정 |
| 152 안정 | 151.9197397 ± 0.0000018 | 26.7500% | 안정 |
상 / 상태
이유: 녹는점(1073.85 °C)보다 1048.8 °C 낮음
개략도이며 실제 비율과 다름
상전이점
전이 에너지
녹는점에서 1 mol을 녹이는 데 필요한 에너지
끓는점에서 1 mol을 기화시키는 데 필요한 에너지
승화점에서 1 mol을 승화시키는 데 필요한 에너지
밀도
표준 조건에서
표준 조건에서
원자 스펙트럼
전체 62개 중 10개를 표시합니다. 이온 전하순으로 정렬되었습니다(오름차순).
보유 에너지 준위 데이터 ?
| 이온 | 전하 | 준위 |
|---|---|---|
| Sm I | 0 | 501 |
| Sm II | +1 | 377 |
| Sm III | +2 | 58 |
| Sm IV | +3 | 24 |
| Sm V | +4 | 2 |
| Sm VI | +5 | 2 |
| Sm VII | +6 | 2 |
| Sm VIII | +7 | 2 |
| Sm IX | +8 | 2 |
| Sm X | +9 | 2 |
결정 구조 데이터 없음
결정 구조: rhombohedral
이온 반지름
| 전하 | 배위 | 스핀 | 반지름 |
|---|---|---|---|
| +2 | 7 | 해당 없음 | 122 pm |
| +2 | 8 | 해당 없음 | 127 pm |
| +2 | 9 | 해당 없음 | 132 pm |
| +3 | 6 | 해당 없음 | 95.8 pm |
| +3 | 7 | 해당 없음 | 102 pm |
| +3 | 8 | 해당 없음 | 107.89999999999999 pm |
| +3 | 9 | 해당 없음 | 113.19999999999999 pm |
| +3 | 12 | 해당 없음 | 124 pm |
화합물
동위원소 (3)
Twenty one isotopes of samarium exist. Natural samarium is a mixture of several isotopes, three of which are unstable with long half-lives.
| 질량수 | 원자 질량(u) | 천연 존재비 | 반감기 | 붕괴 방식 | |
|---|---|---|---|---|---|
| 144 안정 | 143.9120065 ± 0.0000021 | 3.0700% ± 0.0700% | 안정 | stable | |
| 150 안정 | 149.9172829 ± 0.0000018 | 7.3800% ± 0.0100% | 안정 | stable | |
| 152 안정 | 151.9197397 ± 0.0000018 | 26.7500% ± 0.1600% | 안정 | stable |
확장 특성
공유 결합 반지름(확장)
- 공유 결합 반지름(Pyykkö)
- 172 pm
- 공유 결합 반지름(Pyykkö, 이중 결합)
- 134 pm
반데르발스 반지름
- Alvarez
- 290 pm
- UFF
- 352 pm
- MM3
- 271 pm
원자 및 금속 반지름
- 원자 반지름(Rahm)
- 280 pm
번호 척도
- Mendeleev
- 23
- Pettifor
- 28
- Glawe
- 27
전기 음성도 척도
- Ghosh
- 0
- Miedema
- 3
- Gunnarsson–Lundqvist
- 6
- Robles–Bartolotti
- 5
분극률 및 분산
- 쌍극자 분극률
- 192 a.u.
- 쌍극자 분극률(불확도)
- 20 a.u.
- C₆ (Gould–Bučko)
- 3130 Ha·Bohr6
미데마 매개변수
- 미데마 몰 부피
- 20.01 cm3/mol
- 미데마 전자 밀도
- 2
공급 위험 및 경제성
- 생산 집중도
- 97
- 상대적 공급 위험
- 10
- 매장량 분포
- 50
- 정치적 안정성(최대 생산국)
- 24
- 정치적 안정성(최대 매장국)
- 24
상전이 및 동소체
| 녹는점 | 1345.15 K |
| 끓는점 | 2067.15 K |
산화 상태 분류
심화 참고 데이터
차폐 상수 (13)
| n | 오비탈 | σ |
|---|---|---|
| 1 | s | 1.2217 |
| 2 | p | 4.269 |
| 2 | s | 16.2652 |
| 3 | d | 13.7711 |
| 3 | p | 19.5815 |
| 3 | s | 19.9736 |
| 4 | d | 33.7604 |
| 4 | f | 38.4684 |
| 4 | p | 30.912 |
| 4 | s | 29.7076 |
결정 반지름 상세 정보 (8)
| 전하 | CN | 스핀 | rcrystal (pm) | 기원 |
|---|---|---|---|---|
| 2 | VII | 136 | ||
| 2 | VIII | 141 | ||
| 2 | IX | 146 | ||
| 3 | VI | 109.8 | from r^3 vs V plots, | |
| 3 | VII | 116 | estimated, | |
| 3 | VIII | 121.9 | from r^3 vs V plots, | |
| 3 | IX | 127.2 | from r^3 vs V plots, | |
| 3 | XII | 138 | calculated, |
동위원소 붕괴 방식 (52)
| 동위원소 | 모드 | 세기 |
|---|---|---|
| 128 | B+ | — |
| 128 | B+p | — |
| 129 | B+ | 100% |
| 129 | B+p | — |
| 130 | B+ | — |
| 131 | B+ | 100% |
| 131 | B+p | — |
| 132 | B+ | 100% |
| 132 | B+p | — |
| 133 | B+ | 100% |
X선 산란 인자 (508)
| 에너지 (eV) | f₁ | f₂ |
|---|---|---|
| 10 | — | 0.18764 |
| 10.1617 | — | 0.19534 |
| 10.3261 | — | 0.20334 |
| 10.4931 | — | 0.21168 |
| 10.6628 | — | 0.22036 |
| 10.8353 | — | 0.22939 |
| 11.0106 | — | 0.2388 |
| 11.1886 | — | 0.24859 |
| 11.3696 | — | 0.25878 |
| 11.5535 | — | 0.26939 |
추가 데이터
Estimated Crustal Abundance
The estimated element abundance in the earth's crust.
7.05 milligrams per kilogram
참고 문헌 (1)
- [5] Samarium https://education.jlab.org/itselemental/ele062.html
Estimated Oceanic Abundance
The estimated element abundance in the earth's oceans.
4.5×10-7 milligrams per liter
참고 문헌 (1)
- [5] Samarium https://education.jlab.org/itselemental/ele062.html
Sources
Sources of this element.
Samarium is found along with other members of the rare-earth elements in many minerals, including monazite and bastnasite, which are commercial sources. It occurs in monazite to the extent of 2.8%. While misch metal containing about 1% of samarium metal, has long been used, samarium has not been isolated in relatively pure form until recently. Ion-exchange and solvent extraction techniques have recently simplified separation of the rare earths from one another; more recently, electrochemical deposition, using an electrolytic solution of lithium citrate and a mercury electrode, is said to be a simple, fast, and highly specific way to separate the rare earths. Samarium metal can be produced by reducing the oxide with lanthanum.
참고 문헌 (1)
- [6] Samarium https://periodic.lanl.gov/62.shtml
참고 문헌
(9)
Data deposited in or computed by PubChem
The half-life and atomic mass data was provided by the Atomic Mass Data Center at the International Atomic Energy Agency.
Element data are cited from the Atomic weights of the elements (an IUPAC Technical Report). The IUPAC periodic table of elements can be found at https://iupac.org/what-we-do/periodic-table-of-elements/. Additional information can be found within IUPAC publication doi:10.1515/pac-2015-0703 Copyright © 2020 International Union of Pure and Applied Chemistry.
The information are cited from Pure Appl. Chem. 2018; 90(12): 1833-2092, https://doi.org/10.1515/pac-2015-0703.
Thomas Jefferson National Accelerator Facility (Jefferson Lab) is one of 17 national laboratories funded by the U.S. Department of Energy. The lab's primary mission is to conduct basic research of the atom's nucleus using the lab's unique particle accelerator, known as the Continuous Electron Beam Accelerator Facility (CEBAF). For more information visit https://www.jlab.org/
The periodic table at the LANL (Los Alamos National Laboratory) contains basic element information together with the history, source, properties, use, handling and more. The provenance data may be found from the link under the source name.
The periodic table contains NIST's critically-evaluated data on atomic properties of the elements. The provenance data that include data for atomic spectroscopy, X-ray and gamma ray, radiation dosimetry, nuclear physics, and condensed matter physics may be found from the link under the source name. Ref: https://www.nist.gov/pml/atomic-spectra-database
This section provides all form of data related to element Samarium.
The element property data was retrieved from publications.