Thulium

Not to be confused with Thallium.

Thulium, 69Tm
Thulium
Pronunciation/ˈθjuːliəm/ ​(THEW-lee-əm)
Appearancesilvery gray
Standard atomic weight Ar°(Tm)
Thulium in the periodic table
Hydrogen Helium
Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon
Sodium Magnesium Aluminium Silicon Phosphorus Sulfur Chlorine Argon
Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton
Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon
Caesium Barium Lanthanum Cerium Praseodymium Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium Erbium Thulium Ytterbium Lutetium Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury (element) Thallium Lead Bismuth Polonium Astatine Radon
Francium Radium Actinium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium Darmstadtium Roentgenium Copernicium Nihonium Flerovium Moscovium Livermorium Tennessine Oganesson
–
↑
Tm
↓
Md
erbium ← thulium → ytterbium
Atomic number (Z)69
Groupf-block groups (no number)
Periodperiod 6
Block  f-block
Electron configuration[Xe] 4f13 6s2
Electrons per shell2, 8, 18, 31, 8, 2
Physical properties
Phase at STPsolid
Melting point1818 K ​(1545 °C, ​2813 °F)
Boiling point2223 K ​(1950 °C, ​3542 °F)
Density (at 20° C)9.320 g/cm3 [3]
when liquid (at m.p.)8.56 g/cm3
Heat of fusion16.84 kJ/mol
Heat of vaporization191 kJ/mol
Molar heat capacity27.03 J/(mol·K)
Vapor pressure
P (Pa) 1 10 100 1 k 10 k 100 k
at T (K) 1117 1235 1381 1570 (1821) (2217)
Atomic properties
Oxidation statescommon: +3
0,[4] +1,[5] +2[6]
ElectronegativityPauling scale: 1.25
Ionization energies
  • 1st: 596.7 kJ/mol
  • 2nd: 1160 kJ/mol
  • 3rd: 2285 kJ/mol
Atomic radiusempirical: 176 pm
Covalent radius190±10 pm
Color lines in a spectral range
Spectral lines of thulium
Other properties
Natural occurrenceprimordial
Crystal structure ​hexagonal close-packed (hcp) (hP2)
Lattice constants
Hexagonal close packed crystal structure for thulium
a = 353.77 pm
c = 555.39 pm (at 20 °C)[3]
Thermal expansionpoly: 13.3 µm/(m⋅K) (at r.t.)
Thermal conductivity16.9 W/(m⋅K)
Electrical resistivitypoly: 676 nΩ⋅m (at r.t.)
Magnetic orderingparamagnetic (at 300 K)
Molar magnetic susceptibility+25500×10−6 cm3/mol (291 K)[7]
Young's modulus74.0 GPa
Shear modulus30.5 GPa
Bulk modulus44.5 GPa
Poisson ratio0.213
Vickers hardness470–650 MPa
Brinell hardness470–900 MPa
CAS Number7440-30-4
History
Namingafter Thule, a mythical region in Scandinavia
Discovery and first isolationPer Teodor Cleve (1879)
Isotopes of thulium
Main isotopes[8] Decay
abun­dance half-life (t1/2) mode pro­duct
167Tm synth 9.25 d ε 167Er
168Tm synth 93.1 d β+ 168Er
169Tm 100% stable
170Tm synth 128.6 d β− 170Yb
171Tm synth 1.92 y β− 171Yb
 Category: Thulium
| references

Thulium is a chemical element; it has symbol Tm and atomic number 69. It is the thirteenth element in the lanthanide series of metals. It is the second-least abundant lanthanide in the Earth's crust, after radioactively unstable promethium. It is an easily workable metal with a bright silvery-gray luster. It is fairly soft and slowly tarnishes in air. Despite its high price and rarity, thulium is used as a dopant in solid-state lasers, and as the radiation source in some portable X-ray devices. It has no significant biological role and is not particularly toxic.

In 1879, the Swedish chemist Per Teodor Cleve separated two previously unknown components, which he called holmia and thulia, from the rare-earth mineral erbia; these were the oxides of holmium and thulium, respectively. A relatively pure sample of thulium metal was first obtained in 1911.

Like the other lanthanides, its most common oxidation state is +3, seen in its oxide, halides and other compounds. In aqueous solution, like compounds of other late lanthanides, soluble thulium compounds form coordination complexes with nine water molecules.

Properties

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Physical properties

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Pure thulium metal has a bright, silvery luster, which tarnishes on exposure to air. The metal can be cut with a knife,[9] as it has a Mohs hardness of 2 to 3; it is malleable and ductile.[10] Thulium is ferromagnetic below 32 K, antiferromagnetic between 32 and 56 K, and paramagnetic above 56 K.[11]

Thulium has two major allotropes: the tetragonal α-Tm and the more stable hexagonal β-Tm.[10]

Chemical properties

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Thulium tarnishes slowly in air and burns readily at 150 °C to form thulium(III) oxide:[12]

4Tm + 3O2 → 2Tm2O3

Thulium is quite electropositive and reacts slowly with cold water and quite quickly with hot water to form thulium hydroxide:

2Tm(s) + 6 H2O(l) → 2Tm(OH)3(aq) + 3H2(g)

Thulium reacts with all the halogens. Reactions are slow at room temperature, but are vigorous above 200 °C:

2Tm(s) + 3F2(g) → 2TmF3(s) (white)
2Tm(s) + 3Cl2(g) → 2TmCl3(s) (yellow)
2Tm(s) + 3Br2(g) → 2TmBr3(s) (white)
2Tm(s) + 3I2(g) → 2TmI3(s) (yellow)

Thulium dissolves readily in dilute sulfuric acid to form solutions containing the pale green Tm(III) ions, which exist as [Tm(OH2)9]3+ complexes:[13]

2Tm(s) + 3H2SO4(aq) → 2Tm3+(aq) + 3SO2−4(aq) + 3H2(aq)

Thulium reacts with various metallic and non-metallic elements forming a range of binary compounds, including TmN, TmS, TmC2, Tm2C3, TmH2, TmH3, TmSi2, TmGe3, TmB4, TmB6 and TmB12.[citation needed] Like most lanthanides, the +3 state is most common and is the only state observed in thulium solutions.[14] Thulium exists as a Tm3+ ion in solution. In this state, the thulium ion is surrounded by nine molecules of water.[9] Tm3+ ions exhibit a bright blue luminescence.[9] Because it occurs late in the series, the +2 oxidation state can also exist, stabilized by the nearly full 4f electron shell, but occurs only in solids.[citation needed]

Thulium's only known oxide is Tm2O3. This oxide is sometimes called "thulia".[15] Reddish-purple thulium(II) compounds can be made by the reduction of thulium(III) compounds. Examples of thulium(II) compounds include the halides (except the fluoride). Some hydrated thulium compounds, such as TmCl3·7H2O and Tm2(C2O4)3·6H2O are green or greenish-white.[16] Thulium dichloride reacts very vigorously with water. This reaction results in hydrogen gas and Tm(OH)3 exhibiting a fading reddish color.[citation needed] Combination of thulium and chalcogens results in thulium chalcogenides.[17]

Thulium reacts with hydrogen chloride to produce hydrogen gas and thulium chloride. With nitric acid it yields thulium nitrate, or Tm(NO3)3.[18]

Isotopes

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Main article: Isotopes of thulium

The isotopes of thulium range from 144Tm to 183Tm.[8][19] The primary decay mode before the most abundant stable isotope, 169Tm, is electron capture, and the primary mode after is beta emission. The primary decay products before 169Tm are element 68 (erbium) isotopes, and the primary products after are element 70 (ytterbium) isotopes.[20]

Thulium-169 is thulium's only primordial isotope and is the only isotope of thulium that is thought to be stable; it is predicted to undergo alpha decay to holmium-165 with a very long half-life.[9][21] The longest-lived radioisotopes are thulium-171, which has a half-life of 1.92 years, and thulium-170, which has a half-life of 128.6 days. Most other isotopes have half-lives of a few minutes or less.[22] In total, 40 isotopes and 26 nuclear isomers of thulium have been detected.[9] Most isotopes of thulium lighter than 169 atomic mass units decay via electron capture or beta-plus decay, although some exhibit significant alpha decay or proton emission. Heavier isotopes undergo beta-minus decay.[22]

History

[edit]
Per Teodor Cleve, the scientist who discovered thulium as well as holmium.

Thulium was discovered by Swedish chemist Per Teodor Cleve in 1879 by looking for impurities in the oxides of other rare earth elements (this was the same method Carl Gustaf Mosander earlier used to discover some other rare earth elements).[23] Cleve started by removing all of the known contaminants of erbia (Er2O3). Upon additional processing, he obtained two new substances; one brown and one green. The brown substance was the oxide of the element holmium and was named holmia by Cleve, and the green substance was the oxide of an unknown element. Cleve named the oxide thulia and its element thulium after Thule, an Ancient Greek place name associated with Scandinavia or Iceland. Thulium's atomic symbol was initially Tu, but later[when?] changed to Tm.[why?][9][24][25][26][27][28][29]

Thulium was so rare that none of the early workers had enough of it to purify sufficiently to actually see the green color; they had to be content with spectroscopically observing the strengthening of the two characteristic absorption bands, as erbium was progressively removed. The first researcher to obtain nearly pure thulium was Charles James, a British expatriate working on a large scale at New Hampshire College in Durham, USA. In 1911 he reported his results, having used his discovered method of bromate fractional crystallization to do the purification. He famously needed 15,000 purification operations to establish that the material was homogeneous.[30]

High-purity thulium oxide was first offered commercially in the late 1950s, as a result of the adoption of ion-exchange separation technology. Lindsay Chemical Division of American Potash & Chemical Corporation offered it in grades of 99% and 99.9% purity. The price per kilogram oscillated between US$4,600 and $13,300 in the period from 1959 to 1998 for 99.9% purity, and it was the second highest for the lanthanides behind lutetium.[31][32]

Occurrence

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Thulium is found in the mineral monazite

The element is never found in nature in pure form, but it is found in small quantities in minerals with other rare earths. Thulium is often found with minerals containing yttrium and gadolinium. In particular, thulium occurs in the mineral gadolinite.[33] However, like many other lanthanides, thulium also occurs in the minerals monazite, xenotime, and euxenite. Thulium has not been found in prevalence over the other rare earths in any mineral yet.[34] Its abundance in the Earth's crust is 0.5 mg/kg by weight.[35] Thulium makes up approximately 0.5 parts per million of soil, although this value can range from 0.4 to 0.8 parts per million. Thulium makes up 250 parts per quadrillion of seawater.[9] In the Solar System, thulium exists in concentrations of 200 parts per trillion by weight and 1 part per trillion by moles.[18] Thulium ore occurs most commonly in China. However, Australia, Brazil, Greenland, India, Tanzania, and the United States also have large reserves of thulium. Total reserves of thulium are approximately 100,000 tonnes. Thulium is the least abundant lanthanide on Earth except for the radioactive promethium.[9]

Production

[edit]

Thulium is principally extracted from monazite ores (~0.007% thulium) found in river sands, through ion exchange. Newer ion-exchange and solvent-extraction techniques have led to easier separation of the rare earths, which has yielded much lower costs for thulium production. The principal sources today are the ion adsorption clays of southern China. In these, where about two-thirds of the total rare-earth content is yttrium, thulium is about 0.5% (or about tied with lutetium for rarity). The metal can be isolated through reduction of its oxide with lanthanum metal or by calcium reduction in a closed container. None of thulium's natural compounds are commercially important. Approximately 50 tonnes per year of thulium oxide are produced.[9] In 1996, thulium oxide cost US$20 per gram, and in 2005, 99%-pure thulium metal powder cost US$70 per gram.[10]

Applications

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Lasers

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Holmium-chromium-thulium triple-doped yttrium aluminium garnet (Ho:Cr:Tm:YAG, or Ho,Cr,Tm:YAG) is an active laser medium material with high efficiency. It lases at 2080 nm in the infrared and is widely used in military applications, medicine, and meteorology. Single-element thulium-doped YAG (Tm:YAG) lasers operate at 2010 nm.[36] The wavelength of thulium-based lasers is very efficient for superficial ablation of tissue, with minimal coagulation depth in air or in water. This makes thulium lasers attractive for laser-based surgery.[37]

X-ray source

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Despite its high cost, portable X-ray devices use thulium that has been bombarded with neutrons in a nuclear reactor to produce the isotope Thulium-170, having a half-life of 128.6 days and five major emission lines of comparable intensity (at 7.4, 51.354, 52.389, 59.4 and 84.253 keV). These radioactive sources have a useful life of about one year, as tools in medical and dental diagnosis, as well as to detect defects in inaccessible mechanical and electronic components. Such sources do not need extensive radiation protection – only a small cup of lead.[38] They are among the most popular radiation sources for use in industrial radiography.[39] Thulium-170 is gaining popularity as an X-ray source for cancer treatment via brachytherapy (sealed source radiation therapy).[40][41]

Others

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Thulium has been used in high-temperature superconductors similarly to yttrium. Thulium potentially has use in ferrites, ceramic magnetic materials that are used in microwave equipment.[38] Thulium is also similar to scandium in that it is used in arc lighting for its unusual spectrum, in this case, its green emission lines, which are not covered by other elements.[42] Because thulium fluoresces with a blue color when exposed to ultraviolet light, thulium is put into euro banknotes as a measure against counterfeiting.[43] The blue fluorescence of Tm-doped calcium sulfate has been used in personal dosimeters for visual monitoring of radiation.[9] Tm-doped halides in which Tm is in its 2+ oxidation state are luminescent materials that are proposed for electric power generating windows based on the principle of a luminescent solar concentrator.[44]

Biological role and precautions

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Soluble thulium salts are mildly toxic, but insoluble thulium salts are completely nontoxic.[9] When injected, thulium can cause degeneration of the liver and spleen and can also cause hemoglobin concentration to fluctuate. Liver damage from thulium is more prevalent in male mice than female mice. Despite this, thulium has a low level of toxicity.[45][46] In humans, thulium occurs in the highest amounts in the liver, kidneys, and bones. Humans typically consume several micrograms of thulium per year. The roots of plants do not take up thulium, and the dry matter of vegetables usually contains one part per billion of thulium.[9] Thulium is toxic.[47] Thulium dust can cause explosions and fires.[48]

See also

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References

[edit]
  1. ^ "Standard Atomic Weights: Thulium". CIAAW. 2021.
  2. ^ Prohaska, Thomas; Irrgeher, Johanna; Benefield, Jacqueline; Böhlke, John K.; Chesson, Lesley A.; Coplen, Tyler B.; Ding, Tiping; Dunn, Philip J. H.; Gröning, Manfred; Holden, Norman E.; Meijer, Harro A. J. (2022-05-04). "Standard atomic weights of the elements 2021 (IUPAC Technical Report)". Pure and Applied Chemistry. doi:10.1515/pac-2019-0603. ISSN 1365-3075.
  3. ^ a b Arblaster, John W. (2018). Selected Values of the Crystallographic Properties of Elements. Materials Park, Ohio: ASM International. ISBN 978-1-62708-155-9.
  4. ^ Yttrium and all lanthanides except Ce and Pm have been observed in the oxidation state 0 in bis(1,3,5-tri-t-butylbenzene) complexes, see Cloke, F. Geoffrey N. (1993). "Zero Oxidation State Compounds of Scandium, Yttrium, and the Lanthanides". Chem. Soc. Rev. 22: 17–24. doi:10.1039/CS9932200017. and Arnold, Polly L.; Petrukhina, Marina A.; Bochenkov, Vladimir E.; Shabatina, Tatyana I.; Zagorskii, Vyacheslav V.; Cloke (2003-12-15). "Arene complexation of Sm, Eu, Tm and Yb atoms: a variable temperature spectroscopic investigation". Journal of Organometallic Chemistry. 688 (1–2): 49–55. doi:10.1016/j.jorganchem.2003.08.028.
  5. ^ La(I), Pr(I), Tb(I), Tm(I), and Yb(I) have been observed in MB8− clusters; see Li, Wan-Lu; Chen, Teng-Teng; Chen, Wei-Jia; Li, Jun; Wang, Lai-Sheng (2021). "Monovalent lanthanide(I) in borozene complexes". Nature Communications. 12 (1): 6467. doi:10.1038/s41467-021-26785-9. PMC 8578558. PMID 34753931.
  6. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 28. ISBN 978-0-08-037941-8.
  7. ^ Weast, Robert (1984). CRC, Handbook of Chemistry and Physics. Boca Raton, Florida: Chemical Rubber Company Publishing. pp. E110. ISBN 0-8493-0464-4.
  8. ^ a b Kondev, F. G.; Wang, M.; Huang, W. J.; Naimi, S.; Audi, G. (2021). "The NUBASE2020 evaluation of nuclear properties" (PDF). Chinese Physics C. 45 (3): 030001. doi:10.1088/1674-1137/abddae.
  9. ^ a b c d e f g h i j k l Emsley, John (2001). Nature's building blocks: an A-Z guide to the elements. US: Oxford University Press. pp. 442–443. ISBN 0-19-850341-5.
  10. ^ a b c Hammond, C. R. (2000). "The Elements". Handbook of Chemistry and Physics (81st ed.). CRC press. ISBN 0-8493-0481-4.
  11. ^ Jackson, M. (2000). "Magnetism of Rare Earth" (PDF). The IRM Quarterly. 10 (3): 1.
  12. ^ Catherine E. Housecroft; Alan G. Sharpe (2008). "Chapter 25: The f-block metals: lanthanoids and actinoids". Inorganic Chemistry, 3rd Edition. Pearson. p. 864. ISBN 978-0-13-175553-6.
  13. ^ "Chemical reactions of Thulium". Webelements. Retrieved 2009-06-06.
  14. ^ Patnaik, Pradyot (2003). Handbook of Inorganic Chemical Compounds. McGraw-Hill. p. 934. ISBN 0-07-049439-8.
  15. ^ Krebs, Robert E (2006). The History and Use of Our Earth's Chemical Elements: A Reference Guide. Greenwood Publishing. ISBN 978-0-313-33438-2.
  16. ^ Eagleson, Mary (1994). Concise Encyclopedia Chemistry. Walter de Gruyter. p. 1105. ISBN 978-3-11-011451-5.
  17. ^ Emeléus, H. J.; Sharpe, A. G. (1977). Advances in Inorganic Chemistry and Radiochemistry. Academic Press. ISBN 978-0-08-057869-9.
  18. ^ a b "Thulium". www.chemicool.com. Retrieved 2023-03-10.
  19. ^ Tarasov, O. B.; Gade, A.; Fukushima, K.; et al. (2024). "Observation of New Isotopes in the Fragmentation of 198Pt at FRIB". Physical Review Letters. 132 (72501): 072501. Bibcode:2024PhRvL.132g2501T. doi:10.1103/PhysRevLett.132.072501. PMID 38427880.
  20. ^ Lide, David R. (1998). "Section 11, Table of the Isotopes". Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0594-2.
  21. ^ Belli, P.; Bernabei, R.; Danevich, F. A.; et al. (2019). "Experimental searches for rare alpha and beta decays". European Physical Journal A. 55 (8): 140–1–140–7. arXiv:1908.11458. Bibcode:2019EPJA...55..140B. doi:10.1140/epja/i2019-12823-2. ISSN 1434-601X. S2CID 201664098.
  22. ^ a b Sonzogni, Alejandro. "Untitled". National Nuclear Data Center. Archived from the original on 2020-11-21. Retrieved 2013-02-20.
  23. ^ See:
    • Cleve, P. T. (1879). "Sur deux nouveaux éléments dans l'erbine" [Two new elements in the oxide of erbium]. Comptes rendus (in French). 89: 478–480. Cleve named thulium on p. 480: "Pour le radical de l'oxyde placé entre l'ytterbine et l'erbine, qui est caractérisé par la bande x dans la partie rouge du spectre, je propose la nom de thulium, dérivé de Thulé, le plus ancien nom de la Scandinavie." (For the radical of the oxide located between the oxides of ytterbium and erbium, which is characterized by the x band in the red part of the spectrum, I propose the name of "thulium", [which is] derived from Thule, the oldest name of Scandinavia.)
    • Cleve, P. T. (1879). "Sur l'erbine" [On the oxide of erbium]. Comptes rendus (in French). 89: 708–709.
    • Cleve, P. T. (1880). "Sur le thulium" [On thulium]. Comptes rendus (in French). 91: 328–329.
  24. ^ Eagleson, Mary (1994). Concise Encyclopedia Chemistry. Walter de Gruyter. p. 1061. ISBN 978-3-11-011451-5.
  25. ^ Weeks, Mary Elvira (1956). The discovery of the elements (6th ed.). Easton, PA: Journal of Chemical Education.
  26. ^ Weeks, Mary Elvira (1932). "The discovery of the elements: XVI. The rare earth elements". Journal of Chemical Education. 9 (10): 1751–1773. Bibcode:1932JChEd...9.1751W. doi:10.1021/ed009p1751.
  27. ^ Marshall, James L. Marshall; Marshall, Virginia R. Marshall (2015). "Rediscovery of the elements: The Rare Earths–The Confusing Years" (PDF). The Hexagon: 72–77. Retrieved 30 December 2019.
  28. ^ Piguet, Claude (2014). "Extricating erbium". Nature Chemistry. 6 (4): 370. Bibcode:2014NatCh...6..370P. doi:10.1038/nchem.1908. PMID 24651207.
  29. ^ "Thulium". Royal Society of Chemistry. 2020. Retrieved 4 January 2020.
  30. ^ James, Charles (1911). "Thulium I". Journal of the American Chemical Society. 33 (8): 1332–1344. doi:10.1021/ja02221a007.
  31. ^ Hedrick, James B. "Rare-Earth Metals" (PDF). U.S. Geological Survey. Retrieved 2009-06-06.
  32. ^ Castor, Stephen B. & Hedrick, James B. "Rare Earth Elements" (PDF). Retrieved 2009-06-06.
  33. ^ Walker, Perrin & Tarn, William H. (2010). CRC Handbook of Metal Etchants. CRC Press. pp. 1241–. ISBN 978-1-4398-2253-1.
  34. ^ Hudson Institute of Mineralogy (1993–2018). "Mindat.org". www.mindat.org. Retrieved 14 January 2018.
  35. ^ ABUNDANCE OF ELEMENTS IN THE EARTH’S CRUST AND IN THE SEA, CRC Handbook of Chemistry and Physics, 97th edition (2016–2017), p. 14-17
  36. ^ Koechner, Walter (2006). Solid-state laser engineering. Springer. p. 49. ISBN 0-387-29094-X.
  37. ^ Duarte, Frank J. (2008). Tunable laser applications. CRC Press. p. 214. ISBN 978-1-4200-6009-6.
  38. ^ a b Gupta, C. K. & Krishnamurthy, Nagaiyar (2004). Extractive metallurgy of rare earths. CRC Press. p. 32. ISBN 0-415-33340-7.
  39. ^ Raj, Baldev; Venkataraman, Balu (2004). Practical Radiography. Alpha Science Int'l. ISBN 978-1-84265-188-9.
  40. ^ Krishnamurthy, Devan; Vivian Weinberg; J. Adam M. Cunha; I-Chow Hsu; Jean Pouliot (2011). "Comparison of high–dose rate prostate brachytherapy dose distributions with iridium-192, ytterbium-169, and thulium-170 sources". Brachytherapy. 10 (6): 461–465. doi:10.1016/j.brachy.2011.01.012. PMID 21397569.
  41. ^ Ayoub, Amal; Shani, Gad (2009). "Development of New Radioactive Seeds Tm-170 for Brachytherapy". In Dössel, Olaf; Schlegel, Wolfgang C. (eds.). World Congress on Medical Physics and Biomedical Engineering, September 7 - 12, 2009, Munich, Germany. IFMBE Proceedings. Vol. 25/1. Berlin, Heidelberg: Springer Berlin Heidelberg. pp. 1–4. doi:10.1007/978-3-642-03474-9_1. ISBN 978-3-642-03472-5. Retrieved 2023-04-01.
  42. ^ Gray, Theodore W. & Mann, Nick (2009). The Elements: A Visual Exploration of Every Known Atom In The Universe. Black Dog & Leventhal Publishers. p. 159. ISBN 978-1-57912-814-2.
  43. ^ Wardle, Brian (2009-11-06). Principles and Applications of Photochemistry. John Wiley & Sons. p. 75. ISBN 978-0-470-71013-5.
  44. ^ Richards, Bryce S.; Howard, Ian A. (2023). "Luminescent solar concentrators for building integrated photovoltaics: opportunities and challenges". Energy & Environmental Science. 16 (8): 3214–3239. doi:10.1039/D3EE00331K. ISSN 1754-5692.
  45. ^ Ayres, D. C. (15 February 2022). Dictionary of environmentally important chemicals. Desmond Hellier (1st ed.). United States: CRC Press. p. 299. ISBN 978-1-315-14115-2. OCLC 1301431003.
  46. ^ Jha, A. R. (2014). Rare Earth Materials : Properties and Applications. Boca Raton: CRC Press. p. 63. ISBN 978-1-4665-6403-9. OCLC 880825396.
  47. ^ "Thulium". Los Alamos National Laboratory. Triad National Security, LLC. Retrieved 1 June 2024.
  48. ^ Thermo Fisher Scientific Chemicals, Inc. (28 March 2024). "SAFETY DATA SHEET". fisher scientific. Section: 5. Fire-fighting measures. Retrieved 1 June 2024.{{cite web}}: CS1 maint: location (link)
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