Names | |
---|---|
IUPAC name
Manganese(III) fluoride
| |
Other names
Manganese trifluoride, manganic fluoride
| |
Identifiers | |
3D model (
JSmol)
|
|
ChemSpider | |
ECHA InfoCard | 100.029.096 |
EC Number |
|
PubChem
CID
|
|
RTECS number |
|
UNII | |
CompTox Dashboard (
EPA)
|
|
| |
| |
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] | |
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).
|
Manganese(III) fluoride (also known as Manganese trifluoride) is the inorganic compound with the formula MnF3. This red/purplish solid is useful for converting hydrocarbons into fluorocarbons, i.e., it is a fluorination agent. [2] It forms a hydrate and many derivatives.
MnF3 can be prepared by treating a solution of MnF2 in hydrogen fluoride with fluorine: [3]
It can also be prepared by the reaction of elemental fluorine with a manganese(II) halide at ~250 °C. [4]
Like vanadium(III) fluoride, MnF3 features octahedral metal centers with the same average M-F bond distances. In the Mn compound, however, is distorted (and hence a monoclinic unit cell vs. a higher symmetry one) due to the 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]
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]
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]
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cite book}}
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ignored (
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Names | |
---|---|
IUPAC name
Manganese(III) fluoride
| |
Other names
Manganese trifluoride, manganic fluoride
| |
Identifiers | |
3D model (
JSmol)
|
|
ChemSpider | |
ECHA InfoCard | 100.029.096 |
EC Number |
|
PubChem
CID
|
|
RTECS number |
|
UNII | |
CompTox Dashboard (
EPA)
|
|
| |
| |
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] | |
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).
|
Manganese(III) fluoride (also known as Manganese trifluoride) is the inorganic compound with the formula MnF3. This red/purplish solid is useful for converting hydrocarbons into fluorocarbons, i.e., it is a fluorination agent. [2] It forms a hydrate and many derivatives.
MnF3 can be prepared by treating a solution of MnF2 in hydrogen fluoride with fluorine: [3]
It can also be prepared by the reaction of elemental fluorine with a manganese(II) halide at ~250 °C. [4]
Like vanadium(III) fluoride, MnF3 features octahedral metal centers with the same average M-F bond distances. In the Mn compound, however, is distorted (and hence a monoclinic unit cell vs. a higher symmetry one) due to the 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]
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]
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]
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cite book}}
: |journal=
ignored (
help)