Holmium
Holmium | |||||||||||||||||||||||||||||||||||||||||||
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Pronunciation | /ˈhoʊlmiəm/ | ||||||||||||||||||||||||||||||||||||||||||
Appearance | silvery white | ||||||||||||||||||||||||||||||||||||||||||
Standard atomic weight Ar°(Ho) | |||||||||||||||||||||||||||||||||||||||||||
Holmium in the periodic table | |||||||||||||||||||||||||||||||||||||||||||
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kJ/mol | |||||||||||||||||||||||||||||||||||||||||||
Heat of vaporization | 251 kJ/mol | ||||||||||||||||||||||||||||||||||||||||||
Molar heat capacity | 27.15 J/(mol·K) | ||||||||||||||||||||||||||||||||||||||||||
Vapor pressure
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Atomic properties | |||||||||||||||||||||||||||||||||||||||||||
Isotopes of holmium | |||||||||||||||||||||||||||||||||||||||||||
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Holmium is a
In nature, holmium occurs together with the other rare-earth metals (like
Like many other
Holmium has the highest
Properties
Holmium is the eleventh member of the
Physical properties
With a boiling point of 3,000 K (2,730 °C), holmium is the sixth most
Holmium, like all of the lanthanides, at
Chemical properties
Holmium metal tarnishes slowly in air, forming a yellowish oxide layer that has an appearance similar to that of iron rust. It burns readily to form holmium(III) oxide:[14]
- 4 Ho + 3 O2 → 2 Ho2O3
It is a relatively soft and
Holmium is quite electropositive: on the Pauling electronegativity scale, it has an electronegativity of 1.23.[16] It is generally trivalent. It reacts slowly with cold water and quickly with hot water to form holmium(III) hydroxide:[17]
- 2 Ho (s) + 6 H2O (l) → 2 Ho(OH)3 (aq) + 3 H2 (g)
Holmium metal reacts with all the stable halogens:[18]
- 2 Ho (s) + 3 F2 (g) → 2 HoF3 (s) [pink]
- 2 Ho (s) + 3 Cl2 (g) → 2 HoCl3 (s) [yellow]
- 2 Ho (s) + 3 Br2 (g) → 2 HoBr3 (s) [yellow]
- 2 Ho (s) + 3 I2 (g) → 2 HoI3 (s) [yellow]
Holmium dissolves readily in dilute sulfuric acid to form solutions containing the yellow Ho(III) ions, which exist as a [Ho(OH2)9]3+ complexes:[18]
- 2 Ho (s) + 3 H2SO4 (aq) → 2 Ho3+ (aq) + 3 SO2−
4 (aq) + 3 H2 (g)
Oxidation states
As with many lanthanides, holmium is usually found in the +3 oxidation state, forming compounds such as holmium(III) fluoride (HoF3) and holmium(III) chloride (HoCl3). Holmium in solution is in the form of Ho3+ surrounded by nine molecules of water. Holmium dissolves in acids.[12] However, holmium is also found to exist in the +2, +1 and 0 oxidation states.[citation needed]
Isotopes
The isotopes of holmium range from 140Ho to 175Ho. The primary
Natural holmium consists of one
166m1Ho has a half-life of around 1200 years.
Compounds
Oxides and chalcogenides
Holmium(III) oxide is the only oxide of holmium. It changes its color depending on the lighting conditions. In daylight, it has a yellowish color. Under trichromatic light, it appears orange red, almost indistinguishable from the appearance of erbium oxide under the same lighting conditions.[25] The color change is related to the sharp emission lines of trivalent holmium ions acting as red phosphors.[26] Holmium(III) oxide appears pink under a cold-cathode fluorescent lamp.
Other chalcogenides are known for holmium. Holmium(III) sulfide has orange-yellow crystals in the monoclinic crystal system,[19] with the space group P21/m (No. 11).[27] Under high pressure, holmium(III) sulfide can form in the cubic and orthorhombic crystal systems.[28] It can be obtained by the reaction of holmium(III) oxide and hydrogen sulfide at 1,598 K (1,325 °C; 2,417 °F).[29] Holmium(III) selenide is also known. It is antiferromagnetic below 6 K.[30]
Halides
All four trihalides of holmium are known. Holmium(III) fluoride is a yellowish powder that can be produced by reacting holmium(III) oxide and ammonium fluoride, then crystallising it from the ammonium salt formed in solution.[31] Holmium(III) chloride can be prepared in a similar way, with ammonium chloride instead of ammonium fluoride.[32] It has the YCl3 layer structure in the solid state.[33] These compounds, as well as holmium(III) bromide and holmium(III) iodide, can be obtained by the direct reaction of the elements:[18]
- 2 Ho + 3 X2 → 2 HoX3
In addition, holmium(III) iodide can be obtained by the direct reaction of holmium and mercury(II) iodide, then removing the mercury by distillation.[34]
Organoholmium compounds
Organoholmium compounds are very similar to
History
Holmium (Holmia,
The Swedish chemist
In the English physicist Henry Moseley's classic paper on atomic numbers, holmium was assigned the value 66. The holmium preparation he had been given to investigate had been impure, dominated by neighboring (at the time undiscovered) dysprosium. He would have seen x-ray emission lines for both elements, but assumed that the dominant ones belonged to holmium, instead of the dysprosium impurity.[40]
Occurrence and production
Like all the other rare-earth elements, holmium is not naturally found as a free element. It occurs combined with other elements in gadolinite, monazite and other rare-earth minerals. No holmium-dominant mineral has yet been found. The main mining areas are China, United States, Brazil, India, Sri Lanka, and Australia with reserves of holmium estimated as 400,000 tonnes.[39] The annual production of holmium metal is of about 10 tonnes per year.[41]
Holmium makes up 1.3 parts per million of the
Holmium is commercially extracted by
Applications
Glass containing holmium oxide and holmium oxide solutions (usually in perchloric acid) have sharp optical absorption peaks in the spectral range 200 to 900 nm. They are therefore used as a calibration standard for optical spectrophotometers.[46][47][48] The radioactive but long-lived 166m1Ho is used in calibration of gamma-ray spectrometers.[49]
Holmium is used to create the strongest artificially generated
Holmium-doped
Since holmium can absorb
Biological role and precautions
Holmium plays no
See also
References
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- ^ ISBN 978-1-62708-155-9.
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- ^ a b 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.
- ^ a b "Holmium". Royal Society of Chemistry. 2020. Retrieved 4 January 2020.
- ^ Stwertka, Albert (1998). A guide to the elements (2nd ed.). p. 161.
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- ^ Cullity, B. D.; Graham, C. D. (2005). Introduction to Magnetic Materials. p. 172.
- ^ Jiles, David (1998). Introduction to magnetism and magnetic materials. p. 228.
- ^ a b c Emsley, John (2011). Nature's Building Blocks. p. 226.
- ^ ISBN 0-415-33340-7.
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- ^ Winter, Mark J. "Holmium - 67Ho: electronegativity". WebElements. University of Sheffield. Retrieved 4 August 2023.
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- ^ a b c "Chemical reactions of Holmium". Webelements. Retrieved 2009-06-06.
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- ^ Oliveira, Bernardes, Estela Maria de (2001-01-01). "Holmium-166m: multi-gamma standard to determine the activity of radionuclides in semiconductor detectors" (in Portuguese).
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: CS1 maint: multiple names: authors list (link) - ^ Ganjali, Mohammad Reza; Gupta, Vinod Kumar; Faridbod, Farnoush; Norouzi, Parviz (2016-02-25). Lanthanides Series Determination by Various Analytical Methods. p. 27.
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- ISBN 3-540-64966-2. Archivedfrom the original on 2018-09-01. Retrieved 2021-06-22.
- ^ Tonkov, E. Yu (1998). Compounds and Alloys Under High Pressure A Handbook. p. 272.
- ^ G. Meyer; Lester R. Morss, eds. (1991). Synthesis of Lanthanide and Actinide Compounds. p. 329.
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- ^ Riedel, moderne anorganische Chemie. Erwin Riedel, Christoph Janiak, Hans-Jürgen Meyer. De Gruyter. 2012.
{{cite book}}
: CS1 maint: others (link) - ^ "Holmium chloride | 10138-62-2". ChemicalBook. Retrieved 2023-08-09.
- ^ Wells, A. F. Structural inorganic chemistry. p. 421.
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- ^ Greenwood and Earnshaw, pp. 1248–1249
- ^ Jacques-Louis Soret (1878). "Sur les spectres d'absorption ultra-violets des terres de la gadolinite". Comptes rendus de l'Académie des sciences. 87: 1062.
- ^ Jacques-Louis Soret (1879). "Sur le spectre des terres faisant partie du groupe de l'yttria". Comptes rendus de l'Académie des sciences. 89: 521.
- ^ Weeks, Mary Elvira (1956). The discovery of the elements. Journal of Chemical Education. p. 710.
- ^ a b c d Emsley, John (2011). Nature's Building Blocks. p. 225.
- ^ Moseley, H.G.J. (1913). "The high-frequency spectra of the elements". Philosophical Magazine. 6th series. 26: 1024–1034.
- ^ "Ho - Holmium". MMTA. Retrieved 5 December 2022.
- ^ 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
- ^ Ltd, Mark Winter, University of Sheffield and WebElements. "WebElements Periodic Table » Periodicity » Abundance in the universe » periodicity". www.webelements.com. Archived from the original on 2017-09-29. Retrieved 27 March 2018.
{{cite web}}
: CS1 maint: multiple names: authors list (link) - ISBN 0-07-049439-8. Archived from the originalon 2023-06-14. Retrieved 2009-06-06.
- ^ James B. Hedrick. "Rare-Earth Metals" (PDF). USGS. Retrieved 2009-06-06.
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- ^ "Holmium: Biological Action". 2011-04-15. Archived from the original on 2011-04-15. Retrieved 2023-03-05.
Bibliography
- ISBN 978-0-19-960563-7.
- Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
- Stwertka, Albert (1998). A guide to the elements (2nd ed.). Oxford University Press. ISBN 0-19-508083-1.
- Cullity, B. D.; Graham, C. D. (2005). Introduction to Magnetic Materials. ISBN 978-1-118-21149-6.
- Jiles, David (1998). Introduction to magnetism and magnetic materials. CRC Press. ISBN 0-412-79860-3.
- Ganjali, Mohammad Reza; Gupta, Vinod Kumar; Faridbod, Farnoush; Norouzi, Parviz (2016-02-25). Lanthanides Series Determination by Various Analytical Methods. Elsevier. ISBN 978-0-12-420095-1.
- Tonkov, E. Yu (1998). Compounds and Alloys Under High Pressure A Handbook. CRC Press. ISBN 978-90-5699-047-3.
- G. Meyer; Lester R. Morss, eds. (1991). Synthesis of Lanthanide and Actinide Compounds. Kluwer Academic Publishers. ISBN 0792310187.
- Riedel, moderne anorganische Chemie (in German). Erwin Riedel, Christoph Janiak, Hans-Jürgen Meyer (4. Aufl ed.). Berlin: De Gruyter. 2012. )
- Wells, A. F. (1984). Structural inorganic chemistry (5th ed.). Oxford [Oxfordshire]: Clarendon Press. OCLC 8866491.
- Weeks, Mary Elvira (1956). The discovery of the elements (6th ed.). Easton, PA: Journal of Chemical Education.
Further reading
- R. J. Callow, The Industrial Chemistry of the Lanthanons, Yttrium, Thorium, and Uranium, Pergamon Press, 1967.
External links
- Holmium at The Periodic Table of Videos(University of Nottingham)