Manganese(III) fluoride

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Manganese(III) fluoride
Manganese(III) fluoride
Names
IUPAC name
Manganese(III) fluoride
Other names
Manganese trifluoride, manganic fluoride
Identifiers
3D model (
JSmol
)
ChemSpider
ECHA InfoCard
100.029.096 Edit this at Wikidata
EC Number
  • 232-006-6
RTECS number
  • OP0882600
UNII
  • InChI=1S/3FH.Mn/h3*1H;/q;;;+3/p-3 checkY
    Key: SRVINXWCFNHIQZ-UHFFFAOYSA-K checkY
  • InChI=1/3FH.Mn/h3*1H;/q;;;+3/p-3
    Key: SRVINXWCFNHIQZ-DFZHHIFOAX
  • [Mn+3].[F-].[F-].[F-]
Properties
MnF3
Molar mass 111.938 g/mol
Appearance purple-pink powder
hygroscopic
Density 3.54 g/cm3
Melting point > 600 °C (1,112 °F; 873 K) (decomposes)
hydrolysis
+10,500·10−6 cm3/mol
Structure
Monoclinic, mS48
C2/c, No. 15
distorted octahedral
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
toxic fumes
GHS labelling:[1]
GHS03: OxidizingGHS06: Toxic
Danger
H272, H301, H312, H315, H319, H332, H335
P220, P261, P280, P301+P310, P305+P351+P338
Related compounds
Other anions
manganese(III) oxide, manganese(III) acetate
Other cations
chromium(III) fluoride, iron(III) fluoride. cobalt(III) fluoride
Related compounds
manganese(II) fluoride, manganese(IV) fluoride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Manganese(III) fluoride (also known as Manganese trifluoride) is the

fluorination agent.[2]
It forms a hydrate and many derivatives.

Synthesis, structure and reactions

MnF3 can be prepared by treating a solution of MnF2 in hydrogen fluoride with fluorine:[3]

MnF2 + 0.5 F2 → MnF3

It can also be prepared by the reaction of elemental fluorine with a manganese(II) halide at ~250 °C.[4]

Structure

Like

Jahn-Teller effect, with pairs of Mn-F distances of 1.79, 1.91, 2.09 Å.[5][6][7]

The hydrate MnF3.3H2O is obtained by crystallisation of MnF3 from hydrofluoric acid. The hydrate exists as two polymorphs, with space groups P21/c and P21/a. Each consists of the salt [Mn(H2O)4F2]+[Mn(H2O)2F4] ).[8]

Reactions

MnF3 is Lewis acidic and forms a variety of derivatives. One example is K2MnF3(SO4).[9] MnF3 reacts with sodium fluoride to give the octahedral hexafluoride:[4]

3NaF + MnF3 → Na3MnF6

Related reactions salts of the anions MnF52− or MnF4. These anions adopt chain and layer structures respectively, with bridging fluoride. Manganese remains 6 coordinate, octahedral, and trivalent in all of these materials.[4]

Manganese(III) fluoride fluorinates organic compounds including aromatic hydrocarbons,[10] cyclobutenes,[11] and fullerenes.[12]

On heating, MnF3 decomposes to manganese(II) fluoride.[13][14]

MnF3 is a source of MnCl3 complexes by reaction with bismuth trichloride.[15]

See also

  • CoF3, another fluorinating agent based on a transition metal in an oxidising +3 state.

References

  1. ^ GHS: sigma-aldrich 339296[dead link]
  2. .
  3. .
  4. ^ a b c Inorganic chemistry, Catherine E. Housecroft, A.G. Sharpe, pp.711-712, section Manganese (III) , googlebooks link
  5. .
  6. .
  7. .
  8. .
  9. ISBN 978-0-470-13258-6. {{cite book}}: |journal= ignored (help
    )
  10. ^ Fluorination of p-chlorobenzotrifluoride by manganese trifluoride Archived 2011-08-23 at the Wayback Machine A. Kachanov, V. Kornilov, V.Belogay , Fluorine Notes :Vol. 1 (1) November–December 1998 , via notes.fluorine1.ru
  11. .
  12. .
  13. ^ Chisholm, Hugh, ed. (1911). "Manganese § Manganic Salts" . Encyclopædia Britannica. Vol. 17 (11th ed.). Cambridge University Press. p. 570.
  14. ^ In situ time-resolved X-ray diffraction study of manganese trifluoride thermal decomposition , J.V. Raua, V. Rossi Albertinib, N.S. Chilingarova, S. Colonnab, U. Anselmi Tamburini, Journal of Fluorine Chemistry 4506 (2001) 1–4 , online version
  15. .

Further reading

External links