Iron (II) fluoride

Crystal structure
	__ Fe 2+ __ F -
General
Surname	Iron (II) fluoride
other names	Iron difluoride
Ratio formula	FeF 2
Brief description	white solid (anhydrous); brown solid (tetrahydrate);
External identifiers / databases
ECHA InfoCard	100.029.232
PubChem	522690
Wikidata	Q421457
properties
Molar mass	93.84 g mol −1
Physical state	firmly
density	4.09 g cm −3 ; 2.20 g cm −3 (tetrahydrate);
Melting point	1100 ° C (sublimation)
solubility	slightly soluble in water; insoluble in ethanol, diethyl ether and benzene;
safety instructions
GHS labeling of hazardous substances danger
H and P phrases	H: 314
	P: 260-280-303 + 361 + 353-304 + 340 + 310-305 + 351 + 338
	As far as possible and customary, SI units are used. Unless otherwise noted, the data given apply to standard conditions .

Iron (II) fluoride is a chemical compound from the groups of iron compounds and fluorides .

Extraction and presentation

Iron (II) fluoride can be obtained by reacting iron (II) chloride with hydrogen fluoride .

{\ displaystyle \ mathrm {FeCl_ {2} +2 \ HF \ longrightarrow FeF_ {2} +2 \ HCl}}

The product made in this way is amorphous. To get it crystalline, it has to be heated to 1000 ° C. In addition, pure white iron (II) fluoride is only obtained if the work is carried out completely without water . Otherwise the compound will turn gray-brown during the recrystallization process.

properties

In its pure state, iron (II) fluoride is a white solid that is sparingly soluble in water. It has a crystal structure of rutile type, space group P 4 ₂ / mnm (space group no. 136) , lattice parameter a = 4.695 Å , c = 3.310 Å. Template: room group / 136

use

Iron (II) fluoride is used as a starting material for the production of other iron (II) compounds. It is also used in organic chemistry as a catalyst for fluorination .

Individual evidence

↑ ^a ^b ^c ^d David R. Lide (Ed.): CRC Handbook of Chemistry and Physics . 90th edition. CRC Press, 2009, ISBN 978-1-4200-9084-0 .
↑ ^a ^b ^c ^d ^e ^f Entry on iron (II) fluoride in the GESTIS substance database of the IFA , accessed on January 10, 2017(JavaScript required) .
↑ ^a ^b ^c ^d ^e ^f Georg Brauer (Ed.), With the collaboration of Marianne Baudler u. a .: Handbook of Preparative Inorganic Chemistry. 3rd, revised edition. Volume I, Ferdinand Enke, Stuttgart 1975, ISBN 3-432-02328-6 , p. 274.
^ WH Baur, AA Khan: Rutile-type compounds. IV. SiO ₂ , GeO ₂ and a comparison with other rutile-type structures. In: Acta Crystallographica , B27, 1971, pp. 2133-2139, doi: 10.1107 / S0567740871005466 .
^ Catherine E. Housecroft, AG Sharpe: Inorganic chemistry. Prentice Hall, 2004, ISBN 978-0130399137 ( limited preview in Google Book Search).
↑ Egon Wildermuth, Hans Stark, Gabriele Friedrich, Franz Ludwig Ebenhöch, Brigitte Kühborth, Jack Silver, Rafael Rituper: Iron Compounds . In: Ullmann's Encyclopedia of Industrial Chemistry . 2000, doi : 10.1002 / 14356007.a14_591 .

[crc-1] David R. Lide (Ed.): CRC Handbook of Chemistry and Physics . 90th edition. CRC Press, 2009, ISBN 978-1-4200-9084-0 .

[GESTIS-2] ↑ ^a ^b ^c ^d ^e ^f Entry on iron (II) fluoride in the GESTIS substance database of the IFA , accessed on January 10, 2017(JavaScript required) .

[brauer-3] ↑ ^a ^b ^c ^d ^e ^f Georg Brauer (Ed.), With the collaboration of Marianne Baudler u. a .: Handbook of Preparative Inorganic Chemistry. 3rd, revised edition. Volume I, Ferdinand Enke, Stuttgart 1975, ISBN 3-432-02328-6 , p. 274.

[4] WH Baur, AA Khan: Rutile-type compounds. IV. SiO ₂ , GeO ₂ and a comparison with other rutile-type structures. In: Acta Crystallographica , B27, 1971, pp. 2133-2139, doi: 10.1107 / S0567740871005466 .

[ic-5] Catherine E. Housecroft, AG Sharpe: Inorganic chemistry. Prentice Hall, 2004, ISBN 978-0130399137 ( limited preview in Google Book Search).

[6] Egon Wildermuth, Hans Stark, Gabriele Friedrich, Franz Ludwig Ebenhöch, Brigitte Kühborth, Jack Silver, Rafael Rituper: Iron Compounds . In: Ullmann's Encyclopedia of Industrial Chemistry . 2000, doi : 10.1002 / 14356007.a14_591 .