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Erbium, 68Er
Erbium
Pronunciation/ˈɜːrbiəm/ ​(UR-bee-əm)
Appearancesilvery white
Standard atomic weight Ar°(Er)
Erbium 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
–
↑
Er
↓
Fm
holmium ← erbium → thulium
Atomic number (Z)68
Groupf-block groups (no number)
Periodperiod 6
Block  f-block
Electron configuration[Xe] 4f12 6s2
Electrons per shell2, 8, 18, 30, 8, 2
Physical properties
Phase at STPsolid
Melting point1802 K ​(1529 °C, ​2784 °F)
Boiling point3141 K ​(2868 °C, ​5194 °F)
Density (at 20° C)9.065 g/cm3 [3]
when liquid (at m.p.)8.86 g/cm3
Heat of fusion19.90 kJ/mol
Heat of vaporization280 kJ/mol
Molar heat capacity28.12 J/(mol·K)
Vapor pressure
P (Pa) 1 10 100 1 k 10 k 100 k
at T (K) 1504 1663 (1885) (2163) (2552) (3132)
Atomic properties
Oxidation statescommon: +3
0,[4] +2[5]
ElectronegativityPauling scale: 1.24
Ionization energies
  • 1st: 589.3 kJ/mol
  • 2nd: 1150 kJ/mol
  • 3rd: 2194 kJ/mol
Atomic radiusempirical: 176 pm
Covalent radius189±6 pm
Color lines in a spectral range
Spectral lines of erbium
Other properties
Natural occurrenceprimordial
Crystal structure ​hexagonal close-packed (hcp) (hP2)
Lattice constants
Hexagonal close packed crystal structure for erbium
a = 355.93 pm
c = 558.49 pm (at 20 °C)[3]
Thermal expansionpoly: 12.2 µm/(m⋅K) (r.t.)
Thermal conductivity14.5 W/(m⋅K)
Electrical resistivitypoly: 0.860 µΩ⋅m (r.t.)
Magnetic orderingparamagnetic at 300 K
Molar magnetic susceptibility+44300.00×10−6 cm3/mol[6]
Young's modulus69.9 GPa
Shear modulus28.3 GPa
Bulk modulus44.4 GPa
Speed of sound thin rod2830 m/s (at 20 °C)
Poisson ratio0.237
Vickers hardness430–700 MPa
Brinell hardness600–1070 MPa
CAS Number7440-52-0
History
Namingafter Ytterby (Sweden), where it was mined
DiscoveryCarl Gustaf Mosander (1843)
Isotopes of erbium
Main isotopes[7] Decay
abun­dance half-life (t1/2) mode pro­duct
160Er synth 28.58 h ε 160Ho
162Er 0.139% stable
164Er 1.60% stable
165Er synth 10.36 h ε 165Ho
166Er 33.5% stable
167Er 22.9% stable
168Er 27.0% stable
169Er synth 9.4 d β− 169Tm
170Er 14.9% stable
171Er synth 7.516 h β− 171Tm
172Er synth 49.3 h β− 172Tm
 Category: Erbium
| references

Erbium is a chemical element; it has symbol Er and atomic number 68. A silvery-white solid metal when artificially isolated, natural erbium is always found in chemical combination with other elements. It is a lanthanide, a rare-earth element, originally found in the gadolinite mine in Ytterby, Sweden, which is the source of the element's name.

Erbium's principal uses involve its pink-colored Er3+ ions, which have optical fluorescent properties particularly useful in certain laser applications. Erbium-doped glasses or crystals can be used as optical amplification media, where Er3+ ions are optically pumped at around 980 or 1480 nm and then radiate light at 1530 nm in stimulated emission. This process results in an unusually mechanically simple laser optical amplifier for signals transmitted by fiber optics. The 1550 nm wavelength is especially important for optical communications because standard single mode optical fibers have minimal loss at this particular wavelength.

In addition to optical fiber amplifier-lasers, a large variety of medical applications (e.g. dermatology, dentistry) rely on the erbium ion's 2940 nm emission (see Er:YAG laser) when lit at another wavelength, which is highly absorbed in water in tissues, making its effect very superficial. Such shallow tissue deposition of laser energy is helpful in laser surgery, and for the efficient production of steam which produces enamel ablation by common types of dental laser.

Characteristics

[edit]

Physical properties

[edit]
Erbium(III) chloride in sunlight, showing some pink fluorescence of Er+3 from natural ultraviolet.

A trivalent element, pure erbium metal is malleable (or easily shaped), soft yet stable in air, and does not oxidize as quickly as some other rare-earth metals. Its salts are rose-colored, and the element has characteristic sharp absorption spectra bands in visible light, ultraviolet, and near infrared.[8] Otherwise it looks much like the other rare earths. Its sesquioxide is called erbia. Erbium's properties are to a degree dictated by the kind and amount of impurities present. Erbium does not play any known biological role, but is thought to be able to stimulate metabolism.[9]

Erbium is ferromagnetic below 19 K, antiferromagnetic between 19 and 80 K and paramagnetic above 80 K.[10]

Erbium can form propeller-shaped atomic clusters Er3N, where the distance between the erbium atoms is 0.35 nm. Those clusters can be isolated by encapsulating them into fullerene molecules, as confirmed by transmission electron microscopy.[11]

Like most rare-earth elements, erbium is usually found in the +3 oxidation state. However, it is possible for erbium to also be found in the 0, +1 and +2[12] oxidation states.

Chemical properties

[edit]

Erbium metal retains its luster in dry air, however will tarnish slowly in moist air and burns readily to form erbium(III) oxide:[9]

4 Er + 3 O2 → 2 Er2O3

Erbium is quite electropositive and reacts slowly with cold water and quite quickly with hot water to form erbium hydroxide:[13]

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

Erbium metal reacts with all the halogens:[14]

2 Er (s) + 3 F2 (g) → 2 ErF3 (s) [pink]
2 Er (s) + 3 Cl2 (g) → 2 ErCl3 (s) [violet]
2 Er (s) + 3 Br2 (g) → 2 ErBr3 (s) [violet]
2 Er (s) + 3 I2 (g) → 2 ErI3 (s) [violet]

Erbium dissolves readily in dilute sulfuric acid to form solutions containing hydrated Er(III) ions, which exist as rose red [Er(OH2)9]3+ hydration complexes:[14]

2 Er (s) + 3 H2SO4 (aq) → 2 Er3+ (aq) + 3 SO2−
4 (aq) + 3 H2 (g)

Isotopes

[edit]
Main article: Isotopes of erbium

Naturally occurring erbium is composed of 6 stable isotopes, 162Er, 164Er, 166Er, 167Er, 168Er, and 170Er, with 166Er being the most abundant (33.503% natural abundance). 32 radioisotopes have been characterized, with the most stable being 169Er with a half-life of 9.392 d, 172Er with a half-life of 49.3 h, 160Er with a half-life of 28.58 h, 165Er with a half-life of 10.36 h, and 171Er with a half-life of 7.516 h. All of the remaining radioactive isotopes have half-lives that are less than 3.5 h, and the majority of these have half-lives that are less than 4 minutes. This element also has 26 meta states, with the most stable being 149mEr with a half-life of 8.9 s.[7]

The isotopes of erbium range in 143Er to 180Er. The primary decay mode before the most abundant stable isotope, 166Er, is electron capture, and the primary mode after is beta decay. The primary decay products before 166Er are element 67 (holmium) isotopes, and the primary products after are element 69 (thulium) isotopes.[7]

165Er has been identified as useful for use in Auger therapy, as it decays via electron capture and emits no gamma radiation. It can also be used as a radioactive tracer to label antibodies and peptides, though it cannot be detected by any kind of imaging for the study of its biological distribution. The isotope can be produced via the bombardment of 166Er with 165Tm or 165Er with 165Ho, the latter of which is more convenient due to 165Ho being a stable primordial isotope, though it requires an initial supply of 165Er.[15]

Compounds

[edit]
Main article: Erbium compounds

Oxides

[edit]
Erbium(III) oxide powder
Main article: Erbium(III) oxide

Erbium(III) oxide (also known as erbia) is the only known oxide of erbium, first isolated by Carl Gustaf Mosander in 1843, and first obtained in pure form in 1905 by Georges Urbain and Charles James.[16] It has a cubic structure resembling the bixbyite motif. The Er3+ centers are octahedral.[17] The formation of erbium oxide is accomplished by burning erbium metal,[9] erbium oxalate or other oxyacid salts of erbium.[18] Erbium oxide is insoluble in water and slightly soluble in heated mineral acids. The pink-colored compound is used as a phosphor activator and to produce infrared-absorbing glass.[18]

Halides

[edit]

Erbium(III) fluoride is a pinkish powder[19] that can be produced by reacting erbium(III) nitrate and ammonium fluoride.[20] It can be used to make infrared light-transmitting materials[21] and up-converting luminescent materials,[22] and is an intermediate in the production of erbium metal prior to its reduction with calcium.[18] Erbium(III) chloride is a violet compounds that can be formed by first heating erbium(III) oxide and ammonium chloride to produce the ammonium salt of the pentachloride ([NH4]2ErCl5) then heating it in a vacuum at 350-400 °C.[23][24][25] It forms crystals of the AlCl3 type, with monoclinic crystals and the point group C2/m.[26] Erbium(III) chloride hexahydrate also forms monoclinic crystals with the point group of P2/n (P2/c) - C42h. In this compound, erbium is octa-coordinated to form [Er(H2O)6Cl2]+ ions with the isolated Cl− completing the structure.[27]

Erbium(III) bromide is a violet solid. It is used, like other metal bromide compounds, in water treatment, chemical analysis and for certain crystal growth applications.[28] Erbium(III) iodide[29] is a slightly pink compound that is insoluble in water. It can be prepared by directly reacting erbium with iodine.[30]

Organoerbium compounds

[edit]
See also: Organolanthanide chemistry

Organoerbium compounds are very similar to those of the other lanthanides, as they all share an inability to undergo π backbonding. They are thus mostly restricted to the mostly ionic cyclopentadienides (isostructural with those of lanthanum) and the σ-bonded simple alkyls and aryls, some of which may be polymeric.[31]

History

[edit]
Carl Gustaf Mosander, the scientist who discovered erbium, lanthanum and terbium

Erbium (for Ytterby, a village in Sweden) was discovered by Carl Gustaf Mosander in 1843.[32] Mosander was working with a sample of what was thought to be the single metal oxide yttria, derived from the mineral gadolinite. He discovered that the sample contained at least two metal oxides in addition to pure yttria, which he named "erbia" and "terbia" after the village of Ytterby where the gadolinite had been found. Mosander was not certain of the purity of the oxides and later tests confirmed his uncertainty. Not only did the "yttria" contain yttrium, erbium, and terbium; in the ensuing years, chemists, geologists and spectroscopists discovered five additional elements: ytterbium, scandium, thulium, holmium, and gadolinium.[33]: 701 [34][35][36][37][38]

Erbia and terbia, however, were confused at this time. Marc Delafontaine, a Swiss spectroscopist, mistakenly switched the names of the two elements in his work separating the oxides erbia and terbia. After 1860, terbia was renamed erbia and after 1877 what had been known as erbia was renamed terbia.[39] Fairly pure Er2O3 was independently isolated in 1905 by Georges Urbain and Charles James. Reasonably pure erbium metal was not produced until 1934 when Wilhelm Klemm and Heinrich Bommer reduced the anhydrous chloride with potassium vapor.[40][9]

Occurrence

[edit]
Monazite sand

The concentration of erbium in the Earth crust is about 2.8 mg/kg and in seawater 0.9 ng/L.[41] (Concentration of less abundant elements may vary with location by several orders of magnitude[42] making the relative abundance unreliable). Like other rare earths, this element is never found as a free element in nature but is found in monazite and bastnäsite ores.[9] It has historically been very difficult and expensive to separate rare earths from each other in their ores but ion-exchange chromatography methods[43] developed in the late 20th century have greatly reduced the cost of production of all rare-earth metals and their chemical compounds.[citation needed]

The principal commercial sources of erbium are from the minerals xenotime and euxenite, and most recently, the ion adsorption clays of southern China. Consequently, China has now become the principal global supplier of this element.[44] In the high-yttrium versions of these ore concentrates, yttrium is about two-thirds of the total by weight, and erbia is about 4–5%. When the concentrate is dissolved in acid, the erbia liberates enough erbium ion to impart a distinct and characteristic pink color to the solution. This color behavior is similar to what Mosander and the other early workers in the lanthanides saw in their extracts from the gadolinite minerals of Ytterby.[citation needed]

Production

[edit]

Crushed minerals are attacked by hydrochloric or sulfuric acid that transforms insoluble rare-earth oxides into soluble chlorides or sulfates. The acidic filtrates are partially neutralized with caustic soda (sodium hydroxide) to pH 3–4. Thorium precipitates out of solution as hydroxide and is removed. After that the solution is treated with ammonium oxalate to convert rare earths into their insoluble oxalates. The oxalates are converted to oxides by annealing. The oxides are dissolved in nitric acid that excludes one of the main components, cerium, whose oxide is insoluble in HNO3. The solution is treated with magnesium nitrate to produce a crystallized mixture of double salts of rare-earth metals. The salts are separated by ion exchange. In this process, rare-earth ions are sorbed onto suitable ion-exchange resin by exchange with hydrogen, ammonium or cupric ions present in the resin. The rare earth ions are then selectively washed out by suitable complexing agent.[41] Erbium metal is obtained from its oxide or salts by heating with calcium at 1450 °C under argon atmosphere.[41]

Applications

[edit]
Erbium-colored glass

Lasers and optics

[edit]

A large variety of medical applications (i.e., dermatology, dentistry) utilize erbium ion's 2940 nm emission (see Er:YAG laser), which is highly absorbed in water (absorption coefficient about 12000/cm). Such shallow tissue deposition of laser energy is necessary for laser surgery, and the efficient production of steam for laser enamel ablation in dentistry.[45] Common applications of erbium lasers in dentistry include ceramic cosmetic dentistry and removal of brackets in orthodontic braces; such laser applications have been noted as more time-efficient than performing the same procedures with rotary dental instruments.[46]

Erbium-doped optical silica-glass fibers are the active element in erbium-doped fiber amplifiers (EDFAs), which are widely used in optical communications.[47] The same fibers can be used to create fiber lasers. In order to work efficiently, erbium-doped fiber is usually co-doped with glass modifiers/homogenizers, often aluminium or phosphorus. These dopants help prevent clustering of Er ions and transfer the energy more efficiently between excitation light (also known as optical pump) and the signal. Co-doping of optical fiber with Er and Yb is used in high-power Er/Yb fiber lasers. Erbium can also be used in erbium-doped waveguide amplifiers.[9]

Other applications

[edit]

When added to vanadium as an alloy, erbium lowers hardness and improves workability.[48] An erbium-nickel alloy Er3Ni has an unusually high specific heat capacity at liquid-helium temperatures and is used in cryocoolers; a mixture of 65% Er3Co and 35% Er0.9Yb0.1Ni by volume improves the specific heat capacity even more.[49][50]

Erbium oxide has a pink color, and is sometimes used as a colorant for glass, cubic zirconia and porcelain. The glass is then often used in sunglasses and jewellery,[9][48][51] or where infrared absorption is needed.[18]

Erbium is used in nuclear technology in neutron-absorbing control rods.[9][52] or as a burnable poison in nuclear fuel design.[53]

Biological role and precautions

[edit]

Erbium does not have a biological role, but erbium salts can stimulate metabolism. Humans consume 1 milligram of erbium a year on average. The highest concentration of erbium in humans is in the bones, but there is also erbium in the human kidneys and liver.[9]

Erbium is slightly toxic if ingested, but erbium compounds are generally not toxic.[9] Ionic erbium behaves similar to ionic calcium, and can potentially bind to proteins such as calmodulin. When introduced into the body, nitrates of erbium, similar to other rare earth nitrates, increase triglyceride levels in the liver and cause leakage of hepatic (liver-related) enzymes to the blood, though they uniquely (along with gadolinium and dysprosium nitrates) increase RNA polymerase II activity.[54] Ingestion[55] and inhalation[56] are the main routes of exposure to erbium and other rare earths, as they do not diffuse through unbroken skin.[54]

Metallic erbium in dust form presents a fire and explosion hazard.[57][58][59]

References

[edit]
  1. ^ "Standard Atomic Weights: Erbium". CIAAW. 1999.
  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. ^ All the lanthanides, except Pm, in the +2 oxidation state have been observed in organometallic molecular complexes, see Lanthanides Topple Assumptions and Meyer, G. (2014). "All the Lanthanides Do It and Even Uranium Does Oxidation State +2". Angewandte Chemie International Edition. 53 (14): 3550–51. doi:10.1002/anie.201311325. PMID 24616202.. Additionally, all the lanthanides (La–Lu) form dihydrides (LnH2), dicarbides (LnC2), monosulfides (LnS), monoselenides (LnSe), and monotellurides (LnTe), but for most elements these compounds have Ln3+ ions with electrons delocalized into conduction bands, e. g. Ln3+(H−)2(e−).
  6. ^ Weast, Robert (1984). CRC, Handbook of Chemistry and Physics. Boca Raton, Florida: Chemical Rubber Company Publishing. pp. E110. ISBN 0-8493-0464-4.
  7. ^ a b c 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.
  8. ^ Humpidge, J. S.; Burney, W. (1879-01-01). "XIV.—On erbium and yttrium". Journal of the Chemical Society, Transactions. 35: 111–117. doi:10.1039/CT8793500111. ISSN 0368-1645.
  9. ^ a b c d e f g h i j Emsley, John (2001). "Erbium". Nature's Building Blocks: An A-Z Guide to the Elements. Oxford, England, UK: Oxford University Press. pp. 136–139. ISBN 978-0-19-850340-8.
  10. ^ Jackson, M. (2000). "Magnetism of Rare Earth" (PDF). The IRM Quarterly. 10 (3): 1. Archived from the original (PDF) on 2017-07-12. Retrieved 2009-05-03.
  11. ^ Sato, Yuta; Suenaga, Kazu; Okubo, Shingo; Okazaki, Toshiya; Iijima, Sumio (2007). "Structures of D5d-C80 and Ih-Er3N@C80 Fullerenes and Their Rotation Inside Carbon Nanotubes Demonstrated by Aberration-Corrected Electron Microscopy". Nano Letters. 7 (12): 3704. Bibcode:2007NanoL...7.3704S. doi:10.1021/nl0720152.
  12. ^ MacDonald, Matthew R.; Bates, Jefferson E.; Fieser, Megan E.; Ziller, Joseph W.; Furche, Filipp; Evans, William J. (2012-05-23). "Expanding Rare-Earth Oxidation State Chemistry to Molecular Complexes of Holmium(II) and Erbium(II)". Journal of the American Chemical Society. 134 (20): 8420–8423. Bibcode:2012JAChS.134.8420M. doi:10.1021/ja303357w. ISSN 0002-7863. PMID 22583320.
  13. ^ Assaaoudi, H.; Fang, Z.; Butler, I. S.; Kozinski, J. A. (2008). "Synthesis of erbium hydroxide microflowers and nanostructures in subcritical water". Nanotechnology. 19 (18): 185606. Bibcode:2008Nanot..19r5606A. doi:10.1088/0957-4484/19/18/185606. PMID 21825694. S2CID 24755693.
  14. ^ a b "Chemical reactions of Erbium". Webelements. Retrieved 2009-06-06.
  15. ^ IAEA (2021). "4.11. Erbium-165". Alternative Radionuclide Production with a Cyclotron. International Atomic Energy Agency. ISBN 9789201032218. OCLC 1317842424.
  16. ^ Aaron John Ihde (1984). The development of modern chemistry. Courier Dover Publications. pp. 378–379. ISBN 978-0-486-64235-2.
  17. ^ Adachi, Gin-ya; Imanaka, Nobuhito (1998). "The Binary Rare Earth Oxides". Chemical Reviews. 98 (4): 1479–1514. doi:10.1021/cr940055h. PMID 11848940.
  18. ^ a b c d Larrañaga, Michael D.; Lewis, Richard J.; Lewis, Robert A. (September 2016). Hawley's Condensed Chemical Dictionary, Sixteenth Edition (16th ed.). Wiley. p. 564. doi:10.1002/9781119312468. ISBN 978-1-118-13515-0.
  19. ^ "Erbium Fluoride".
  20. ^ Linna Guo, Yuhua Wang, Zehua Zou, Bing Wang, Xiaoxia Guo, Lili Han, Wei Zeng (2014). "Facile synthesis and enhancement upconversion luminescence of ErF3 nano/microstructures via Li+ doping". Journal of Materials Chemistry C. 2 (15): 2765. doi:10.1039/c3tc32540g. ISSN 2050-7526. Retrieved 2019-03-26.{{cite journal}}: CS1 maint: multiple names: authors list (link)
  21. ^ Su, W. T.; Li, B.; Yin, L.; Yang, L.; Liu, D. Q.; Zhang, F. S. (2007-05-15). "Crystallization and surface morphology evolution of erbium fluoride films on different substrates". Applied Surface Science. 253 (14): 6259–6263. Bibcode:2007ApSS..253.6259S. doi:10.1016/j.apsusc.2007.01.087. ISSN 0169-4332.
  22. ^ Yingxin Hao, Shichao Lv, Zhijun Ma, Jianrong Qiu (2018). "Understanding differences in Er 3+ –Yb 3+ codoped glass and glass ceramic based on upconversion luminescence for optical thermometry". RSC Advances. 8 (22): 12165–12172. Bibcode:2018RSCAd...812165H. doi:10.1039/C8RA01245H. ISSN 2046-2069. PMC 9079277. PMID 35539388.{{cite journal}}: CS1 maint: multiple names: authors list (link)
  23. ^ Brauer, G., ed. (1963). Handbook of Preparative Inorganic Chemistry (2nd ed.). New York: Academic Press.
  24. ^ Meyer, G. (1989). "The Ammonium Chloride Route to Anhydrous Rare Earth Chlorides—The Example of Ycl 3". The Ammonium Chloride Route to Anhydrous Rare Earth Chlorides-The Example of YCl3. Inorganic Syntheses. Vol. 25. pp. 146–150. doi:10.1002/9780470132562.ch35. ISBN 978-0-470-13256-2.
  25. ^ Edelmann, F. T.; Poremba, P. (1997). Herrmann, W. A. (ed.). Synthetic Methods of Organometallic and Inorganic Chemistry. Vol. VI. Stuttgart: Georg Thieme Verlag. ISBN 978-3-13-103021-4.
  26. ^ Tempelton DH, Carter GF (1954). "The Crystal Structure of Yttrium Trichloride and Similar Compounds". J Phys Chem. 58 (11): 940–943. doi:10.1021/j150521a002.
  27. ^ Graebner EJ, Conrad GH, Duliere SF (1966). "Crystallographic data for solvated rare earth chlorides". Acta Crystallographica. 21 (6): 1012–1013. Bibcode:1966AcCry..21.1012G. doi:10.1107/S0365110X66004420.
  28. ^ Elements, American. "Erbium Bromide". American Elements. Retrieved 2020-11-16.
  29. ^ Perry, Dale L (2011). Handbook of Inorganic Compounds (2 ed.). Taylor & Francis. p. 163. ISBN 9781439814628. Retrieved 14 December 2013.
  30. ^ Elements, American. "Erbium Iodide". American Elements. Retrieved 2020-11-16.
  31. ^ Greenwood and Earnshaw, pp. 1248–9
  32. ^ Mosander, C. G. (1843). "On the new metals, Lanthanium and Didymium, which are associated with Cerium; and on Erbium and Terbium, new metals associated with Yttria". Philosophical Magazine. 23 (152): 241–254. doi:10.1080/14786444308644728. Note: The first part of this article, which does NOT concern erbium, is a translation of: C. G. Mosander (1842) "Något om Cer och Lanthan" [Some (news) about cerium and lanthanum], Förhandlingar vid de Skandinaviske naturforskarnes tredje möte (Stockholm) [Transactions of the Third Scandinavian Scientist Conference (Stockholm)], vol. 3, pp. 387–398.
  33. ^ Weeks, Mary Elvira (1956). The discovery of the elements (6th ed.). Easton, PA: Journal of Chemical Education.
  34. ^ 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.
  35. ^ Marshall, James L. Marshall; Marshall, Virginia R. Marshall (2015). "Rediscovery of the elements: The Rare Earths–The Beginnings" (PDF). The Hexagon: 41–45. Retrieved 30 December 2019.
  36. ^ 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.
  37. ^ Piguet, Claude (2014). "Extricating erbium". Nature Chemistry. 6 (4): 370. Bibcode:2014NatCh...6..370P. doi:10.1038/nchem.1908. PMID 24651207.
  38. ^ "Erbium". Royal Society of Chemistry. 2020. Retrieved 4 January 2020.
  39. ^ Voncken, J.H.L. (2016). The Rare Earth Elements: An Introduction. SpringerBriefs in Earth Sciences (1st ed.). Cham : Springer International Publishing. pp. 10–11. doi:10.1007/978-3-319-26809-5. ISBN 978-3-319-26809-5.
  40. ^ "Facts About Erbium". Live Science. July 23, 2013. Retrieved 22 October 2018.
  41. ^ a b c Patnaik, Pradyot (2003). Handbook of Inorganic Chemical Compounds. McGraw-Hill. pp. 293–295. ISBN 978-0-07-049439-8. Retrieved 2009-06-06.
  42. ^ 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
  43. ^ Early paper on the use of displacement ion-exchange chromatography to separate rare earths: Spedding, F. H.; Powell, J. E. (1954). "A practical separation of yttrium group rare earths from gadolinite by ion-exchange". Chemical Engineering Progress. 50: 7–15.
  44. ^ Asad, F. M. M. (2010). Optical Properties of Dye Sensitized Zinc Oxide Thin Film Deposited by Sol-gel Method (Doctoral dissertation, Universiti Teknologi Malaysia).
  45. ^ Šulc, J.; Jelínková, H. (2013-01-01), Jelínková, Helena (ed.), "5 - Solid-state lasers for medical applications", Lasers for Medical Applications, Woodhead Publishing Series in Electronic and Optical Materials, Woodhead Publishing, pp. 127–176, doi:10.1533/9780857097545.2.127, ISBN 978-0-85709-237-3, retrieved 2022-04-28
  46. ^ Deeb, Janina Golob; Grzech-Leśniak, Kinga; Brody, Erica R.; Matys, Jacek; Bencharit, Sompop (December 2022). "Erbium laser-assisted ceramic debonding: a scoping review". Journal of Prosthodontics. 31 (9): e100 – e124. doi:10.1111/jopr.13613. ISSN 1059-941X. PMC 10099628. PMID 36269672.
  47. ^ Becker, P. C.; Olsson, N. A.; Simpson, J. R. (1999). Erbium-doped fiber amplifiers fundamentals and technology. San Diego: Academic Press. ISBN 978-0-12-084590-3.
  48. ^ a b Hammond, C. R. (2000). The Elements, in Handbook of Chemistry and Physics (81st ed.). CRC press. ISBN 978-0-8493-0481-1.
  49. ^ Kittel, Peter (ed.). Advances in Cryogenic Engineering. Vol. 39a.
  50. ^ Ackermann, Robert A. (1997). Cryogenic Regenerative Heat Exchangers. Springer. p. 58. ISBN 978-0-306-45449-3.
  51. ^ Stwertka, Albert. A Guide to the Elements, Oxford University Press, 1996, p. 162. ISBN 0-19-508083-1
  52. ^ Parish, Theodore A.; Khromov, Vyacheslav V.; Carron, Igor, eds. (1999). "Use of UraniumErbium and PlutoniumErbium Fuel in RBMK Reactors". Safety issues associated with Plutonium involvement in the nuclear fuel cycle. CBoston: Kluwer. pp. 121–125. ISBN 978-0-7923-5593-9.
  53. ^ Grossbeck, Renier, and Bigelow (September 2003). "Development of improved burnable poisons for commercial nuclear power reactors" (PDF). University of North Texas (UNT) digital library.{{cite web}}: CS1 maint: multiple names: authors list (link)
  54. ^ a b Hirano, S.; Suzuki, K. T. (March 1996). "Exposure, metabolism, and toxicity of rare earths and related compounds". Environmental Health Perspectives. 104 Suppl 1 (Suppl 1): 85–95. Bibcode:1996EnvHP.104S..85H. doi:10.1289/ehp.96104s185. ISSN 0091-6765. PMC 1469566. PMID 8722113.
  55. ^ Yang, Daoyuan; Sui, Haixia; Mao, Weifeng; Wang, Yibaina; Yang, Dajin; Zhang, Lei; Liu, Zhaoping; Yong, Ling; Song, Yan (2022-11-24). "Dietary Exposure Assessment of Rare Earth Elements in the Chinese Population". International Journal of Environmental Research and Public Health. 19 (23): 15583. doi:10.3390/ijerph192315583. ISSN 1660-4601. PMC 9738814. PMID 36497658.
  56. ^ Pagano, Giovanni; Thomas, Philippe J.; Di Nunzio, Aldo; Trifuoggi, Marco (2019-04-01). "Human exposures to rare earth elements: Present knowledge and research prospects". Environmental Research. 171: 493–500. Bibcode:2019ER....171..493P. doi:10.1016/j.envres.2019.02.004. ISSN 0013-9351. PMID 30743241.
  57. ^ Haley, T. J.; Koste, L.; Komesu, N.; Efros, M.; Upham, H. C. (1966). "Pharmacology and toxicology of dysprosium, holmium, and erbium chlorides". Toxicology and Applied Pharmacology. 8 (1): 37–43. Bibcode:1966ToxAP...8...37H. doi:10.1016/0041-008x(66)90098-6. PMID 5921895.
  58. ^ Haley, T. J. (1965). "Pharmacology and toxicology of the rare earth elements". Journal of Pharmaceutical Sciences. 54 (5): 663–70. doi:10.1002/jps.2600540502. PMID 5321124.
  59. ^ Bruce, D. W.; Hietbrink, B. E.; Dubois, K. P. (1963). "The acute mammalian toxicity of rare earth nitrates and oxides". Toxicology and Applied Pharmacology. 5 (6): 750–9. Bibcode:1963ToxAP...5..750B. doi:10.1016/0041-008X(63)90067-X. PMID 14082480.

Further reading

[edit]
  • Guide to the Elements – Revised Edition, Albert Stwertka (Oxford University Press; 1998), ISBN 0-19-508083-1.
[edit]
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