Sectioning edit
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- physical properties -
- chemical properties - (includes oxidation states)
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- compounds - create
remember to say that test has been copied from Ho2O3 and Ho2S3.
Compounds edit
Oxides and chalcogenides edit
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Holmium(III) oxide is the only oxide of holmium. It changes color changes on the lighting conditions. In daylight, it is a tannish yellow color. Under trichromatic light, it is a fiery orange red, almost indistinguishable from the way erbium oxide looks under this same lighting. This is due to the sharp emission bands of the phosphors.[1]
Other chalcogenides are known for holmium. Holmium(III) sulfide has orange-yellow crystals in the monoclinic crystal system,[2] with the space group P21/m (No. 11).[3] Under high pressure, holmium(III) sulfide can form in the cubic and orthorhombic crystal systems.[4] It can be obtained by the reaction of holmium(III) oxide and hydrogen sulfide at 1325 °C.[5] Holmium(III) selenide is also known. It is antiferromagnetic below 6 K.[6]
Halides edit
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.[7] Holmium(III) chloride can be prepared in a similar way, with ammonium chloride instead of ammonium fluoride.[8] It has the YCl3 layer structure in the solid state.[9] These compounds, as well as holmium(III) bromide and holmium(III) iodide, can be obtained by the direct reaction of the elements:[10]
- 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.[11]
Other compounds edit
- ^ Su, Yiguo; Li, Guangshe; Chen, Xiaobo; Liu, Junjie; Li, Liping (2008). "Hydrothermal Synthesis of GdVO4:Ho3+ Nanorods with a Novel White-light Emission". Chemistry Letters. 37 (7): 762. doi:10.1246/cl.2008.762.
- ^ Cite error: The named reference
CRCwas invoked but never defined (see the help page). - ^ "Ho2S3: crystal structure, physical properties". Non-Tetrahedrally Bonded Binary Compounds II. Landolt-Börnstein - Group III Condensed Matter. Vol. 41D. 2000. pp. 1–3. doi:10.1007/10681735_623. ISBN 3-540-64966-2. Archived from the original on 2018-09-01. Retrieved 2021-06-22.
- ^ Tonkov, E. Yu (1998). Compounds and Alloys Under High Pressure A Handbook. CRC Press. p. 272. ISBN 978-90-5699-047-3.
- ^ G. Meyer; Lester R. Morss, eds. (1991). Synthesis of Lanthanide and Actinide Compounds. Kluwer Academic Publishers. pp. 329–335. ISBN 0792310187.
- ^ Bespyatov, M. A.; Musikhin, A. E.; Naumov, V. N.; Zelenina, L. N.; Chusova, T. P.; Nikolaev, R. E.; Naumov, N. G. (2018-03-01). "Low-temperature thermodynamic properties of holmium selenide (2:3)". The Journal of Chemical Thermodynamics. 118: 21–25. doi:10.1016/j.jct.2017.10.013. ISSN 0021-9614.
- ^ Riedel, moderne anorganische Chemie. Erwin Riedel, Christoph Janiak, Hans-Jürgen Meyer (4. Aufl ed.). Berlin: De Gruyter. 2012. ISBN 978-3-11-024900-2. OCLC 781540844.
{{cite book}}: CS1 maint: others (link) - ^ Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY.
- ^ Wells, A. F. (1984). Structural inorganic chemistry (5th ed ed.). Oxford [Oxfordshire]: Clarendon Press. ISBN 0-19-855370-6. OCLC 8866491.
{{cite book}}:|edition=has extra text (help) - ^ Cite error: The named reference
Webelementswas invoked but never defined (see the help page). - ^ Asprey, L. B.; Keenan, T. K.; Kruse, F. H. (1964). "Preparation and crystal data for lanthanide and actinide triiodides". Inorganic Chemistry. 3 (8): 1137–1141. doi:10.1021/ic50018a015.