Praseodymium (III) chloride

Crystal structure
	__ Pr 3+ __ Cl -
Crystal system	hexagonal
Space group	P 6 3 / m (No. 176)
Coordination numbers	Pr [9], Cl [3]
General
Surname	Praseodymium (III) chloride
other names	Praseodymium trichloride
Ratio formula	PrCl 3
Brief description	green-blue odorless solid
External identifiers / databases
ECHA InfoCard	100.030.710
PubChem	66317
Wikidata	Q411333
properties
Molar mass	247.27 g mol −1
Physical state	firmly
density	4.02 g cm −3 ; 2.25 g cm −3 (heptahydrate);
Melting point	786 ° C
boiling point	1710 ° C
solubility	soluble in water (96.1 g / 100 g at 25 ° C) and ethanol
safety instructions
GHS labeling of hazardous substances Caution
H and P phrases	H: 319
	P: 305 + 351 + 338
Toxicological data	1318 mg kg −1 ( LD 50 , rat , ip )
	As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions .

Praseodymium (III) chloride is a chemical compound from the group of chlorides .

Extraction and presentation

Praseodymium (III) chloride can be obtained by reacting praseodymium with hydrogen chloride .

{\ displaystyle \ mathrm {2 \ Pr + 6 \ HCl \ longrightarrow 2 \ PrCl_ {3} +3 \ H_ {2}}}

The hydrates can be obtained by reacting praseodymium or praseodymium (III) carbonate with hydrochloric acid .

{\ displaystyle \ mathrm {2 \ Pr (CO_ {3}) _ {3} +6 \ HCl + 15 \ H_ {2} O \ longrightarrow 2 \ PrCl_ {3} \ cdot 9H_ {2} O + 3 \ CO_ {2}}}

The anhydrous form can be obtained by thermal dehydrogenation at 400 ° C. in the presence of ammonium chloride . As an alternative, thionyl chloride can also be used.

properties

Praseodymium (III) chloride heptahydrate

Praseodymium (III) chloride is a hygroscopic green-blue solid; as a heptahydrate, green solid. The anhydrate quickly converts to the heptahydrate in air. It exists in a hexagonal crystal system with the space group P 6 ₃ / m (No. 176) . Its heptahydrate has a triclinic crystal structure with the space group P 1 (No. 1) . Template: room group / 176Template: room group / 1

use

Praseodymium (III) chloride is used as a laboratory chemical and to make other chemical compounds.

Individual evidence

↑ ^a ^b ^c ^d ^e ^f ^g data sheet Praseodym (III) chloride, anhydrous, powder, 99.99% trace metals basis from Sigma-Aldrich , accessed on April 23, 2012 ( PDF ).
^ ^A ^b ^c Jean D'Ans, Ellen Lax: Pocket book for chemists and physicists . 2007, ISBN 978-3-540-60035-0 ( page 672 in the Google book search).
^ Praseodymium (III) chloride at webelements.com , accessed October 12, 2012.
↑ David R. Lide (Ed.): CRC Handbook of Chemistry and Physics . 89th edition. (Internet version: 2009), CRC Press / Taylor and Francis, Boca Raton, FL, Properties of the Elements and Inorganic Compounds, pp. 4-84.
↑ Leonard F. Druding, John D. Corbett: "Lower Oxidation States of the Lanthanides. Neodymium (II) Chloride and Iodide “, in: J. Am. Chem. Soc. , 1961 , 83 , pp. 2462-2467 ( doi: 10.1021 / ja01472a010 ).
^ JD Corbett: "Reduced Halides of the rare-earth elements", in: Rev. Chim. Minerale , 1973 , 10 , pp. 239-257.
^ MD Taylor, PC Carter: "Preparation of anhydrous lanthanide halides, especially iodides", in: J. Inorg. Nucl. Chem. , 1962 , 24 , pp. 387-391 ( doi: 10.1016 / 0022-1902 (62) 80034-7 ).
↑ J. Kutscher, A. Schneider, “Note on the preparation of anhydrous lanthanide halides, especially from iodides”, in: Inorg. Nucl. Chem. Lett. , 1971 , 7 , pp. 815-819 ( doi: 10.1016 / 0020-1650 (71) 80253-2 ).
↑ JH Freeman, ML Smith: “The preparation of anhydrous inorganic chlorides by dehydration with thionyl chloride”, in: J. Inorg. Nucl. Chem. , 1958 , 7 , pp. 224-227 ( doi: 10.1016 / 0022-1902 (58) 80073-1 ).

[Sigma-1] ↑ ^a ^b ^c ^d ^e ^f ^g data sheet Praseodym (III) chloride, anhydrous, powder, 99.99% trace metals basis from Sigma-Aldrich , accessed on April 23, 2012 ( PDF ).

[Lax-2] A ^b ^c Jean D'Ans, Ellen Lax: Pocket book for chemists and physicists . 2007, ISBN 978-3-540-60035-0 ( page 672 in the Google book search).

[3] Praseodymium (III) chloride at webelements.com , accessed October 12, 2012.

[CRC89-4] David R. Lide (Ed.): CRC Handbook of Chemistry and Physics . 89th edition. (Internet version: 2009), CRC Press / Taylor and Francis, Boca Raton, FL, Properties of the Elements and Inorganic Compounds, pp. 4-84.

[5] Leonard F. Druding, John D. Corbett: "Lower Oxidation States of the Lanthanides. Neodymium (II) Chloride and Iodide “, in: J. Am. Chem. Soc. , 1961 , 83 , pp. 2462-2467 ( doi: 10.1021 / ja01472a010 ).

[6] JD Corbett: "Reduced Halides of the rare-earth elements", in: Rev. Chim. Minerale , 1973 , 10 , pp. 239-257.

[7] MD Taylor, PC Carter: "Preparation of anhydrous lanthanide halides, especially iodides", in: J. Inorg. Nucl. Chem. , 1962 , 24 , pp. 387-391 ( doi: 10.1016 / 0022-1902 (62) 80034-7 ).

[8] J. Kutscher, A. Schneider, “Note on the preparation of anhydrous lanthanide halides, especially from iodides”, in: Inorg. Nucl. Chem. Lett. , 1971 , 7 , pp. 815-819 ( doi: 10.1016 / 0020-1650 (71) 80253-2 ).

[9] JH Freeman, ML Smith: “The preparation of anhydrous inorganic chlorides by dehydration with thionyl chloride”, in: J. Inorg. Nucl. Chem. , 1958 , 7 , pp. 224-227 ( doi: 10.1016 / 0022-1902 (58) 80073-1 ).