Manganese(II) fluoride

Manganese(II) fluoride is the chemical compound composed of manganese and fluoride with the formula MnF₂. It is a light pink solid, the light pink color being characteristic for manganese(II) compounds. It is made by treating manganese and diverse compounds of manganese(II) in hydrofluoric acid. Like some other metal difluorides, MnF₂ crystallizes in the rutile structure, which features octahedral Mn centers.^[3]

Manganese(II) fluoride

Names
IUPAC name Manganese(II) fluoride
Identifiers
CAS Number	7782-64-1 Y
3D model (JSmol)	Interactive image
ChemSpider	22935 N
ECHA InfoCard	100.029.054
EC Number	231-960-0
PubChem CID	24528
RTECS number	OP0875000
UNII	1XRA8Q11QP Y
CompTox Dashboard (EPA)	DTXSID7064811
InChI InChI=1S/2FH.Mn/h2*1H;/q;;+2/p-2 N Key: CTNMMTCXUUFYAP-UHFFFAOYSA-L N InChI=1/2FH.Mn/h2*1H;/q;;+2/p-2 Key: CTNMMTCXUUFYAP-NUQVWONBAJ
SMILES F[Mn]F
Properties
Chemical formula	MnF2
Molar mass	92.934855 g/mol
Appearance	pale pink crystalline
Density	3.98 g/cm3[1]
Melting point	856 °C (1,573 °F; 1,129 K)[1]
Boiling point	1,820 °C (3,310 °F; 2,090 K)
Solubility in water	1.02 g/100 ml
Magnetic susceptibility (χ)	+10,700·10−6 cm3/mol
Hazards[2]
GHS labelling:
Pictograms
Signal word	Warning
Hazard statements	H302, H312, H315, H319, H332, H335
Precautionary statements	P261, P264, P270, P271, P280, P301+P312, P302+P352, P304+P312, P304+P340, P305+P351+P338, P312, P321, P322, P330, P332+P313, P337+P313, P362, P363, P403+P233, P405, P501
Flash point	non-flammable
Related compounds
Other anions	Manganese(II) chloride Manganese(II) bromide Manganese(II) iodide
Other cations	Technetium(VI) fluoride Rhenium(VII) fluoride Manganese(III) fluoride Manganese(IV) fluoride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). N verify (what is YN ?) Infobox references

Uses

MnF₂ is used in the manufacture of special kinds of glass and lasers.^[4] It is a canonical example of uniaxial antiferromagnet (with Neel temperature of 68 K)^[5] which has been experimentally studied since early on.^[6]

References

1. Maurice Griffel; J. W. Stout (1950). "Preparation of Single Crystals of Manganous Fluoride. The Crystal Structure from X-Ray Diffraction. The Melting Point and Density". Journal of the American Chemical Society. 72 (10): 4351–4353. doi:10.1021/ja01166a004.
2. "339288 Manganese(II) fluoride 98%". Sigma-Aldrich. Retrieved 2008-06-18.
3. Stout, J. W.; Reed, Stanley A. (1954). "The Crystal Structure of MnF₂, FeF₂, CoF₂, NiF₂ and ZnF₂". J. Am. Chem. Soc. 76 (21): 5279–5281. doi:10.1021/ja01650a005.
4. Ayres, D. C.; Hellier, Desmond (1997). Dictionary of Environmentally Important Chemicals. CRC Press. p. 195. ISBN 0-7514-0256-7. Retrieved 2008-06-18.
5. Felcher, G. P; Kleb, R (20 November 1996). "Antiferromagnetic domains and the spin-flop transition of MnF 2". Europhysics Letters (EPL). 36 (6): 455–460. Bibcode:1996EL.....36..455F. doi:10.1209/epl/i1996-00251-7. S2CID 250849056.
6. Stout, J. W.; Matarrese, L. M. (1 January 1953). "Magnetic Anisotropy of the Iron-Group Fluorides". Reviews of Modern Physics. 25 (1): 338–343. Bibcode:1953RvMP...25..338S. doi:10.1103/RevModPhys.25.338.