Few compounds of californium have been made and studied.[1] The only californium ion that is stable in aqueous solutions is the californium(III) cation.[2] The other two oxidation states are IV (strong oxidizing agents) and II (strong reducing agents).[3] The element forms a water-soluble chloride, nitrate, perchlorate, and sulfate and is precipitated as a fluoride, oxalate or hydroxide.[4] If problems of availability of the element could be overcome, then CfBr2 and CfI2 would likely be stable.[5]
The +3 oxidation state is represented by californium(III) oxide (yellow-green, Cf2O3), californium(III) fluoride (bright green, CfF3) and californium(III) iodide (lemon yellow, CfI3).[3] Other +3 oxidation states include the sulfide and metallocene.[6] Californium(IV) oxide (black brown, CfO2), californium(IV) fluoride (green, CfF4) represent the IV oxidation state. The II state is represented by californium(II) bromide (yellow, CfBr2) and californium(II) iodide (dark violet, CfI2).[3]
YouTube Encyclopedic
-
1/3Views:1 0878751 114
-
Californium Explained in 25 Minutes or Less
-
Californium | Wikipedia audio article
-
Californium | Wikipedia audio article
Transcription
Compounds
Californium(IV) oxide (CfO2) is a black-brown solid that has a cubic crystal structure with a lattice parameter, the distance between unit cells in the crystal, of 531.0 ± 0.2 pm.[7] Crystals of californium(III) oxide normally have a body-centered cubic symmetry. They convert to a monoclinic form upon heating to about 1400 °C and melt at 1750 °C.[7]
Californium(III) chloride (CfCl3) is an emerald green compound with a hexagonal structure that can be prepared by reacting Cf2O3 with hydrochloric acid at 500 °C.[8] CfCl3 is then used as a feeder stock to form the yellow-orange triiodide CfI3, which in turn can be reduced to the lavender-violet diiodide CfI2.[9]
Californium(III) fluoride (CfF3) is a yellow-green solid with a crystal symmetry that gradually changes from orthorhombic to trigonal when heated above room temperature.[10] Californium(IV) fluoride (CfF4) is a bright green solid with a monoclinic crystal structure.[11]
Californium(II) iodide (CfI2) is a deep purple solid with a stable rhombohedral structure at room temperature and an unstable hexagonal structure. Californium(III) iodide (CfI3) is a lemon-yellow solid that has a rhombohedral structure and sublimes at ~800 °C.[12]
Californium(III) oxyfluoride (CfOF) is prepared by hydrolysis of californium(III) fluoride (CfF3) at high temperature.[13] Californium(III) oxychloride (CfOCl) is prepared by hydrolysis of the hydrate of californium(III) chloride at 280–320 °C.[14]
Heating the sulfate in air at about 1200 °C and then reducing with hydrogen at 500 °C produces the sesquioxide (Cf2O3).[8] The hydroxide Cf(OH)3 and the trifluoride CfF3 are slightly soluble.[8]
Californium(III) oxychloride (CfOCl) was the first californium compound to be discovered.[15]
Californium(III) polyborate is unusual in that californium is covalently bound to the borate.[16]
Tris(cyclopentadienyl)californium(III) (Cp3Cf) presents itself as ruby red crystals. This cyclopentadienyl complex has been prepared by the reaction between Cp2Be and CfCl3 on a microgram scale and characterized by X-ray crystallography.[17] Californium is the second-heaviest element for which an organometallic compound is known. A bent californium metallocene has also been isolated and characterized.[18]
See also
References
- ^ Krebs, Robert (2006). The History and Use of our Earth's Chemical Elements: A Reference Guide. Westport, Connecticut: Greenwood Publishing Group. pp. 327–328. ISBN 978-0-313-33438-2.
- ^ CRC 2006, p. 4-8.
- ^ a b c Jakubke 1994, p. 166.
- ^ Seaborg 2004.
- ^ Greenwood 1997, p. 1272.
- ^ Cotton 1999, p. 1163.
- ^ a b Baybarz, R. D.; Haire, R. G.; Fahey, J. A (1972). "On the Californium Oxide System". Inorganic and Nuclear Chemistry. 34 (2): 557–565. doi:10.1016/0022-1902(72)80435-4.
- ^ a b c Cunningham 1968, p. 105.
- ^ Cotton, Simon (2006). Lanthanide and Actinide Chemistry. West Sussex, England: John Wiley & Sons. p. 168. ISBN 978-0-470-01006-8.
- ^ Stevenson, J. N.; Peterson, J. R. (1973). "The Trigonal and Orthorhombic Crystal Structures of CfF3 and their Temperature Relationship". Inorganic and Nuclear Chemistry. 35 (10): 3481–3486. doi:10.1016/0022-1902(73)80356-2.
- ^ Chang, C-T. P.; Haire, R. G.; Nave, S. E. (1990). "Magnetic Susceptibility of Californium Fluorides". Physical Review B. 41 (13): 9045–9048. Bibcode:1990PhRvB..41.9045C. doi:10.1103/PhysRevB.41.9045. PMID 9993248.
- ^ Macintyre, J. E.; Daniel, F. M.; Stirling, V. M. (1992). Dictionary of inorganic compounds. London: Chapman and Hall, CRC Press. p. 2826. ISBN 978-0-412-30120-9.
- ^ Peterson, J. R.; Burns, John H. (1968). "Preparation and Crystal Structure of Californium Oxyfluoride, CfOF". Inorganic and Nuclear Chemistry. 30 (11): 2955–2958. doi:10.1016/0022-1902(68)80155-1.
- ^ Copeland, J. C.; Cunningham, B. B. (1969). "Crystallography of the Compounds of Californium. II. Crystal Structure and Lattice Parameters of Californium Oxychloride and Californium Sesquioxide" (PDF). Inorganic and Nuclear Chemistry. 31 (3): 733–740. doi:10.1016/0022-1902(69)80020-5.
- ^ Seaborg, Glenn T. (1963). Man-Made Transuranium Elements. Prentice-Hall.
- ^ "Unusual structure, bonding, and properties may provide a new possibility for a californium borate". 1 June 2015. Retrieved 29 July 2015.
- ^ Laubereau, Peter G.; Burns, John H. (1970). "Microchemical preparation of tricyclopentadienyl compounds of berkelium, californium, and some lanthanide elements". Inorganic Chemistry. 9 (5): 1091–1095. doi:10.1021/ic50087a018.
- ^ Goodwin, Conrad A. P.; Su, Jing; Stevens, Lauren M.; White, Frankie D.; Anderson, Nickolas H.; Auxier, John D.; Albrecht-Schönzart, Thomas E.; Batista, Enrique R.; Briscoe, Sasha F.; Cross, Justin N.; Evans, William J.; Gaiser, Alyssa N.; Gaunt, Andrew J.; James, Michael R.; Janicke, Michael T.; Jenkins, Tener F.; Jones, Zachary R.; Kozimor, Stosh A.; Scott, Brian L.; Sperling, Joseph. M.; Wedal, Justin C.; Windorff, Cory J.; Yang, Ping; Ziller, Joseph W. (18 November 2021). "Isolation and characterization of a californium metallocene" (PDF). Nature. 599 (7885): 421–424. Bibcode:2021Natur.599..421G. doi:10.1038/s41586-021-04027-8. PMID 34789902. S2CID 244347582.
Bibliography
- Cotton, F. Albert; Wilkinson, Geoffrey; Murillo, Carlos A.; Bochmann, Manfred (1999). Advanced Inorganic Chemistry (6th ed.). New York City: John Wiley & Sons. ISBN 0-471-19957-5.
- CRC contributors (2006). David R. Lide (ed.). Handbook of Chemistry and Physics (87th ed.). Boca Raton, Florida: CRC Press, Taylor & Francis Group. ISBN 0-8493-0487-3.
{{cite book}}:|author=has generic name (help) - Cunningham, B. B. (1968). "Californium". In Clifford A. Hampel (ed.). The Encyclopedia of the Chemical Elements. New York City: Reinhold Book Corporation. LCCN 68-29938.
- Greenwood, N. N.; Earnshaw, A. (1997). Chemistry of the Elements (2nd ed.). Oxford, England: Butterworth-Heinemann. ISBN 0-7506-3365-4.
- Jakubke, Hans-Dieter; Jeschkeit, Hans, eds. (1994). Concise Encyclopedia Chemistry. trans. rev. Eagleson, Mary. Berlin: Walter de Gruyter. ISBN 3-11-011451-8.
- Seaborg, Glenn T. (2004). "Californium". In Geller, Elizabeth (ed.). Concise Encyclopedia of Chemistry. New York City: McGraw-Hill. p. 94. ISBN 0-07-143953-6.
This page was last edited on 3 April 2024, at 09:45