Praseodymium(III) chloride: Difference between revisions
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| ImageFileR1 = Cerium bromide (space filling) 2.png |
| ImageFileR1 = Cerium bromide (space filling) 2.png |
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| IUPACName = Praseodymium(III) chloride |
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| OtherNames = Praseodymium chloride; praseodymium trichloride |
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|Section1={{Chembox Identifiers |
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| CASNo = 10361-79-2 |
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| UNII_Ref = {{fdacite|changed|FDA}} |
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| UNII = 1JB99PM4G8 |
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| PubChem = 66317 |
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| InChI = 1S/3ClH.Pr/h3*1H;/q;;;+3/p-3 |
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| SMILES = Cl[Pr](Cl)Cl |
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|Section2={{Chembox Properties |
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| Formula = PrCl<sub>3</sub> |
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| MolarMass = 247.24 g/mol (anhydrous)<br/>373.77 g/mol (heptahydrate) |
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| Appearance = blue-green solid (anhydrous)<br/>light green solid (heptahydrate) |
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| Density = 4.02 g/cm<sup>3</sup> (anhydrous)<br/>2.250 g/cm<sup>3</sup> (heptahydrate) |
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| Solubility = 104.0 g/100 ml (13 °C) |
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| MeltingPtC = 786 |
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| BoilingPtC = 1710 |
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| pKa = |
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| MagSus = +44.5·10<sup>−6</sup> cm<sup>3</sup>/mol |
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|Section3={{Chembox Structure |
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| Coordination = Tricapped trigonal prismatic<br />(nine-coordinate) |
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| CrystalStruct = [[Hexagonal crystal system|hexagonal]] ([[Uranium trichloride#Structure|UCl<sub>3</sub> type]]), [[Pearson symbol|hP8]] |
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| SpaceGroup = P6<sub>3</sub>/m, No. 176 |
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|Section7={{Chembox Hazards |
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|Section8={{Chembox Related |
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| OtherAnions = [[Praseodymium(III) oxide]], [[Praseodymium(III) fluoride]]<br/>[[Praseodymium bromide]]<br/>[[praseodymium iodide]] |
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| OtherCations = [[Cerium(III) chloride]]<br/>[[Neodymium(III) chloride]] |
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'''Praseodymium(III) chloride''' is the [[inorganic compound]] with the [[chemical formula|formula]] [[praseodymium|Pr]][[chloride|Cl]]<sub>3</sub>. It is a blue-green solid that rapidly absorbs water on exposure to moist air to form a light green hepta[[water of hydration|hydrate]]. |
'''Praseodymium(III) chloride''' is the [[inorganic compound]] with the [[chemical formula|formula]] [[praseodymium|Pr]][[chloride|Cl]]<sub>3</sub>. Like other [[lanthanide trichloride]]s, it exists both in the anhydrous and hydrated forms. It is a blue-green solid that rapidly absorbs water on exposure to moist air to form a light green hepta[[water of hydration|hydrate]]. |
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==Preparation== |
==Preparation== |
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Praseodymium(III) chloride is prepared by treating praseodymium metal |
Praseodymium(III) chloride is prepared by treating praseodymium metal with [[hydrogen chloride]]:<ref name=ref7 /><ref name=ref6>{{cite journal|url=https://pubs.acs.org/doi/10.1021/ja01472a010|author1=L.F. Druding|author2= J.D. Corbett|title=Lower Oxidation States of the Lanthanides. Neodymium(II) Chloride and Iodide|journal=J. Am. Chem. Soc.|volume=83|issue=11|pages=2462-2467|date=1961-06-01|doi=10.1021/ja01472a010}}</ref> |
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:2 Pr + 6 HCl → 2 PrCl<sub>3</sub> + 3 H<sub>2</sub> |
:2 Pr + 6 HCl → 2 PrCl<sub>3</sub> + 3 H<sub>2</sub> |
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It is usually purified by vacuum sublimation.<ref name=ref1 /> |
It is usually purified by vacuum sublimation.<ref name=ref1 /> |
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Hydrated salts of praseodymium(III) chloride can be |
Hydrated salts of praseodymium(III) chloride can be prepared by treatment of either praseodymium metal or praseodymium(III) carbonate with [[hydrochloric acid]]: |
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:Pr<sub>2</sub>(CO<sub>3</sub>)<sub>3</sub> + 6 HCl + 15 H<sub>2</sub>O → 2 [Pr(H<sub>2</sub>O)<sub>9</sub>]Cl<sub>3</sub> + 3 CO<sub>2</sub> |
:Pr<sub>2</sub>(CO<sub>3</sub>)<sub>3</sub> + 6 HCl + 15 H<sub>2</sub>O → 2 [Pr(H<sub>2</sub>O)<sub>9</sub>]Cl<sub>3</sub> + 3 CO<sub>2</sub> |
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Anhydrous PrCl<sub>3</sub> can be made by thermal dehydration of the hydrate at 400 |
PrCl<sub>3</sub>∙7H<sub>2</sub>O is a hygroscopic substance, that will not crystallize from the [[mother liquor]] unless it is left to dry in a desiccator. Anhydrous PrCl<sub>3</sub> can be made by thermal dehydration of the hydrate at 400 °C in the presence of [[ammonium chloride]], the so-called [[ammonium chloride route]].<ref name=ref1 /><ref name=ref4>{{cite journal|url=https://www.sciencedirect.com/science/article/abs/pii/0022190262800347|author1=M.D. Taylor|author2=P.C. Carter|title= Preparation of anhydrous lanthanide halides, especially iodides|journal=J. Inorg. Nucl. Chem.|volume=24|issue=4|pages=387-391|date=April 1962|doi=10.1016/0022-1902(62)80034-7}}</ref><ref name="Kutscher">{{cite journal|url=https://www.sciencedirect.com/science/article/abs/pii/0020165071802532|author1=J. Kutscher|author2=A. Schneider|title=Notiz zur Präparation von wasserfreien Lanthaniden-Haloge-niden, Insbesondere von Jodiden|journal=Inorg. Nucl. Chem. Lett.|volume=7|issue=9|pages=815-819|date=September 1971|doi=10.1016/0020-1650(71)80253-2|language=de}}</ref> Alternatively the hydrate can be dehydrated using [[thionyl chloride]].<ref name=ref1/><ref name=ref5>{{cite journal|url=https://www.sciencedirect.com/science/article/abs/pii/0022190258800731|author1=J.H. Freeman|author2=M.L. Smith|title=The preparation of anhydrous inorganic chlorides by dehydration with thionyl chloride|journal=J. Inorg. Nucl. Chem.|volume=7|issue=3|pages=224-227|date=October 1958|doi=10.1016/0022-1902(58)80073-1}}</ref> |
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==Reactions== |
==Reactions== |
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Praseodymium(III) chloride is [[Lewis acid]]ic, classified as "hard" according to the [[HSAB concept]]. |
Praseodymium(III) chloride is [[Lewis acid]]ic, classified as "hard" according to the [[HSAB concept]]. Rapid heating of the [[hydrate]] may cause small amounts of [[hydrolysis]].<ref name=ref1>{{cite book|author1=F.T. Edelmann|author2= P. Poremba|title=Synthetic Methods of Organometallic and Inorganic Chemistry|volume=6|publisher= Georg Thieme Verlag|location=Stuttgart|date= 1997|isbn=978-31-319-3921-0}}</ref> PrCl<sub>3</sub> forms a stable Lewis acid-base complex K<sub>2</sub>PrCl<sub>5</sub> by reaction with [[potassium chloride]]; this compound shows interesting [[Luminescence|optical]] and [[Magnetism|magnetic]] properties.<ref name=ref7>{{cite journal|url=https://www.semanticscholar.org/paper/Spectroscopic-and-magnetic-studies-of-the-ternary-Cybi%C5%84ska-Sokolnicki/2af96eacdd78d2ec04ac3c0342ca6d875f76130e|author1=J. Cybinska|author2= J. Sokolnicki|author3= J. Legendziewicz|author4= G. Meyer|title=Spectroscopic and magnetic studies of the ternary praseodymium chloride K<sub>2</sub>PrCl<sub>5</sub>|journal=Journal of Alloys and Compounds|volume=341|pages=115–123|date=2002-07-17|doi=10.1016/S0925-8388(02)00089-0}}</ref> |
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[[Aqueous]] solutions of praseodymium(III) chloride can be used to prepare insoluble praseodymium(III) compounds. For example, praseodymium(III) phosphate and praseodymium(III) fluoride can be prepared by reaction with [[potassium phosphate]] and [[sodium fluoride]], respectively: |
[[Aqueous]] solutions of praseodymium(III) chloride can be used to prepare insoluble praseodymium(III) compounds. For example, praseodymium(III) phosphate and praseodymium(III) fluoride can be prepared by reaction with [[potassium phosphate]] and [[sodium fluoride]], respectively: |
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:PrCl<sub>3</sub> + K<sub>3</sub>PO<sub>4</sub> → PrPO<sub>4</sub> + 3 KCl |
:PrCl<sub>3</sub> + K<sub>3</sub>PO<sub>4</sub> → PrPO<sub>4</sub> + 3 KCl |
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:PrCl<sub>3</sub> + 3 NaF → PrF<sub>3</sub> + 3 NaCl |
:PrCl<sub>3</sub> + 3 NaF → PrF<sub>3</sub> + 3 NaCl |
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:2PrCl<sub>3</sub> + 3 Na<sub>2</sub>CO<sub>3</sub>----> Pr<sub>2</sub>CO<sub>3</sub> + 6NaCl |
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⚫ | When heated with alkali metal chlorides, it forms a series of ternary (compounds containing three different elements) materials with the formulae MPr<sub>2</sub>Cl<sub>7</sub>, M<sub>3</sub>PrCl<sub>6</sub>, M<sub>2</sub>PrCl<sub>5</sub>, and M<sub>3</sub>Pr<sub>2</sub>Cl<sub>9</sub> where M = K, Rb, Cs.<ref>{{cite journal|author=Gerd Meyer|title=Ternary Chlorides and Bromides of the Rare-Earth Elements|journal=Inorganic Syntheses|year=1990|volume=30|pages=72–81|doi=10.1002/9780470132616.ch15}}</ref> |
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[[File:Praseodymium chloride heptahydrate under fluorescent lamp light and halogen lamp light.png|thumb|Praseodymium chloride heptahydrate under different light]] |
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⚫ | When heated with alkali metal chlorides, it forms a series of ternary (compounds containing three different elements) materials with the formulae MPr<sub>2</sub>Cl<sub>7</sub>, M<sub>3</sub>PrCl<sub>6</sub>, M<sub>2</sub>PrCl<sub>5</sub>, and M<sub>3</sub>Pr<sub>2</sub>Cl<sub>9</sub> where M = K, Rb, Cs.<ref>Gerd Meyer |
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==References== |
==References== |
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#<!--old 2--> ''CRC Handbook of Chemistry and Physics'' (58th edition), CRC Press, West Palm Beach, Florida, 1977. |
#<!--old 2--> ''CRC Handbook of Chemistry and Physics'' (58th edition), CRC Press, West Palm Beach, Florida, 1977. |
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#<!--old 3--> N. N. Greenwood, A. Earnshaw, ''Chemistry of the Elements'', Pergamon Press, 1984. |
#<!--old 3--> N. N. Greenwood, A. Earnshaw, ''Chemistry of the Elements'', Pergamon Press, 1984. |
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#<!--old 8--> S. Sugiyama, T. Miyamoto, H. Hayashi, M. Tanaka, J. B. |
#<!--old 8--> S. Sugiyama, T. Miyamoto, H. Hayashi, M. Tanaka, J. B. Moffatt, "Effects of chlorine additives in the gas- and solid-phases on the oxidative dehydrogenation of ethane over praseodymium oxide", ''Journal of Molecular Catalysis A'', '''118''', 129-136 (1997). |
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#<!--old 9--> {{cite journal |
#<!--old 9--> {{cite journal |
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| title = Rare Earth Metal-Metal Halide Systems. VI. Praseodymium Chloride |
| title = Rare Earth Metal-Metal Halide Systems. VI. Praseodymium Chloride |
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|author1=Druding L. F. |author2=Corbett J. D. |author3=Ramsey B. N. | journal = [[Inorganic Chemistry (journal)|Inorganic Chemistry]] |
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| journal = [[Inorganic Chemistry (journal)|Inorganic Chemistry]] |
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| year = 1963 |
| year = 1963 |
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| volume = 2 |
| volume = 2 |
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{{Praseodymium compounds}} |
{{Praseodymium compounds}} |
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{{Chlorides}} |
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{{Lanthanide halides}} |
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[[Category:Chlorides]] |
[[Category:Chlorides]] |
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[[Category:Praseodymium compounds]] |
[[Category:Praseodymium(III) compounds]] |
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[[Category: |
[[Category:Lanthanide halides]] |
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[[fr:Chlorure de praséodyme]] |