Copper(II) fluoride

Unit cell of the anhydrous form

Ball-and-stick model of crystal packing in the anhydrous form

Dihydrate

Names
IUPAC name

Copper difluoride

Other names

Cupric fluoride; Copper fluoride; Copper (2+) Difluoride

Identifiers

CAS Number

* 7789-19-7 Y
* 13454-88-1 (dihydrate) Y

3D model (JSmol)

* Interactive image

ChemSpider |

* 74214 Y

EC Number |

* 232-147-3

PubChem CID

* 82236

UNII |

* ML04XYE5C1 Y
* 3A38PC42E9 (dihydrate) Y

InChI

* InChI=1S/Cu.2FH/h;2*1H/q+2;;/p-2 Y

Key: GWFAVIIMQDUCRA-UHFFFAOYSA-L Y

* InChI=1/Cu.2FH/h;2*1H/q+2;;/p-2

Key: GWFAVIIMQDUCRA-NUQVWONBAF

SMILES

* [Cu+2].[F-].[F-]

Properties

Chemical formula

| CuF2
Molar mass | 101.543 g/mol (anhydrous)
137.573 g/mol (dihydrate)
Appearance  | White crystalline powder
When hydrated: Blue
Density | 4.23 g/cm3 (anhydrous)
2.934 g/cm3 (dihydrate)[1]
Melting point |  836 °C (1,537 °F; 1,109 K) (anhydrous)
130 °C (dihydrate, decomposes)
Boiling point |  1,676 °C (3,049 °F; 1,949 K) (anhydrous)

Magnetic susceptibility (χ)

| +1050.0·10−6 cm3/mol
Hazards
NIOSH (US health exposure limits):

PEL (Permissible)

| TWA 1 mg/m3 (as Cu)[2]

REL (Recommended)

| TWA 1 mg/m3 (as Cu)[2]

IDLH (Immediate danger)

| TWA 100 mg/m3 (as Cu)[2]
Related compounds

Other anions

| Copper(II) bromide
Copper(II) chloride

Other cations

| Silver(II) fluoride
Cobalt(II) fluoride

Related compounds

| Copper(I) 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

Copper(II) fluoride is an inorganic compound with the chemical formula CuF2. The anhydrous form is a white, ionic, crystalline, hygroscopic salt with a distorted rutile-type crystal structure, similar to other fluorides of chemical formulae MF2 (where M is a metal). The dihydrate, CuF
2 * 2H2O, is blue in colour.[3]

## Contents

* 1 Structure
* 2 Uses
* 3 Chemistry
* 4 Solubility
* 5 Toxicity
* 6 Hazards
* 7 References
* 8 External links

## Structure

Copper(II) fluoride has a monoclinic crystal structure[4] and cannot achieve a higher-symmetry structure. It forms rectangular prisms with a parallelogram base.[5] Each copper ion has four neighbouring fluoride ions at 1.93 Å separation and two further away at 2.27 Å.[3] This distorted octahedral [4+2] coordination is a consequence of the Jahn–Teller effect in d9 copper(II),[6] and leads to a distorted rutile structure similar to that of chromium(II) fluoride, CrF
2, which is a d4 compound.[3]

Coordination in copper(II) fluoride[3][4] Copper coordination  | Fluorine coordination

|

## Uses

Cupric fluoride catalyzes the decomposition of nitric oxides in emission control systems.[7]

Copper (II) fluoride can be used to make fluorinated aromatic hydrocarbons by reacting with aromatic hydrocarbons in an oxygen-containing atmosphere at temperatures above 450 °C (842 °F). This reaction is simpler than the Sandmeyer reaction, but is only effective in making compounds that can survive at the temperature used. A coupled reaction using oxygen and 2 HF regenerates the copper(II) fluoride, producing water.[8] This method has been proposed as a "greener" method of producing fluoroaromatics since it avoids producing toxic waste products such as ammonium fluoride.

## Chemistry

Copper(II) fluoride can be synthesized from copper and fluorine at temperatures of 400 °C (752 °F). It occurs as a direct reaction.

Cu + F2 → CuF2

It loses fluorine in the molten stage at temperatures above 950 °C (1742 °F).

2CuF2 → 2CuF + F2

2CuF → CuF2 \+ Cu

The complex anions of CuF3−, CuF42− and CuF64− are formed if CuF2 is exposed to substances containing fluoride ions F−.

## Solubility

Copper(II) fluoride is slightly soluble in water, but starts to decompose when it is in hot water, producing basic F− and Cu(OH) ions.[citation needed]

## Toxicity

There is little specific information on the toxicity of Copper(II) fluoride. However, copper and fluoride can both be toxic individually when consumed.

Copper toxicity can affect the skin, eyes, and respiratory tract. Serious conditions include metal fume fever, and hemolysis of red blood cells. Copper can also cause damage to the liver and other major organs.

Metal fluorides are generally safe at low levels and are added to water in many countries to protect against tooth decay. At higher levels they can cause toxic effects ranging from nausea and vomiting to tremors, breathing problems, serious convulsions and even coma. Brain and kidney damage can result. Chronic exposure can cause losses in bone density, weight loss and anorexia.

## Hazards

Experiments using copper(II) fluoride should be conducted in a fume hood because metal oxide fumes can occur. The combination of acids with copper(II) fluoride may lead to the production of hydrogen fluoride, which is highly toxic and corrosive.

## References

1. ↑ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
2. ↑ 2.0 2.1 2.2 NIOSH Pocket Guide to Chemical Hazards. "#0150". National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/npg/npgd0150.html.
3. ↑ 3.0 3.1 3.2 3.3 Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. pp. 1184–1185. ISBN 978-0-08-037941-8.
4. ↑ 4.0 4.1 Fischer, P.; Hälg, W.; Schwarzenbach, D.; Gamsjäger, H. (1974). "Magnetic and crystal structure of copper(II) fluoride". J. Phys. Chem. Solids 35 (12): 1683–1689. doi:10.1016/S0022-3697(74)80182-4.
5. ↑ C. Billy; H. M. Haendler (1957). "The Crystal Structure of Copper(II) Fluoride". Journal of the American Chemical Society 79 (5): 1049–51. doi:10.1021/ja01562a011.
6. ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. pp. 1190–1191. ISBN 978-0-08-037941-8.
7. ↑ Meshri., Dayal T. (2000), "Fluorine compounds, inorganic, copper", Kirk-Othmer Encyclopedia of Chemical Technology, New York: John Wiley, doi:10.1002/0471238961.0315161613051908.a01, ISBN 9780471238966, http://onlinelibrary.wiley.com/book/10.1002/0471238961
8. ↑ M. A. Subramanian; L. E. Manzer (2002). "A "Greener" Synthetic Route for Fluoroaromatics via Copper (II) Fluoride". Science 297 (5587): 1665. doi:10.1126/science.1076397. PMID 12215637.

* P. C. de Mello; M. Hehenberg; S. Larson; M. Zerner (1980). "Studies of the electronic structure of copper fluorides and copper chlorides". Journal of the American Chemical Society 102 (4): 1278–1288. doi:10.1021/ja00524a010.
* H. M. Haendler; L. H. Towle; E. F. Bennett; W. L. Patterson (1954). "The Reaction of Fluorine with Copper and Some of its Compounds. Some Properties of Copper(II) Fluoride". Journal of the American Chemical Society 76 (8): 2178–2179. doi:10.1021/ja01637a039.
* T. C. Ehlert; J. S. Wang (1977). "Thermochemistry of the copper fluorides". Journal of Physical Chemistry 81 (22): 2069–2073. doi:10.1021/j100537a005.
* Dierks, S. "Copper Fluoride". http://www.espimetals.com/index.php/msds/537-copper-fluoride (accessed October 9).
* Subramanian, M. A.; Manzer, L. E. (2002). "A 'Greener' Synthetic Route for Fluoroaromantics via Copper (II) Fluoride". Science 297 (5587): 1665. doi:10.1126/science.1076397. PMID 12215637.
* Olejniczak, I.; Wolak, J.; Barszcz, B.; Schlueter, J.; Manson, J. (2010). "CuF2 Structural Changes in Two-Dimensional Quantum Magnet (H2O)2(pyz) Under Pressure: Raman Study". AIP Conference Proceedings 1267 (1): 597–598. doi:10.1063/1.3482697. Bibcode: 2010AIPC.1267..597O.
* Kent, R. A.; Mcdonald, J. D.; Margrave, J. L. (1966). "Mass Spectrometric Studies at High Temperatures. IX. The Sublimation Pressure of Copper(II) Fluoride". Journal of Physical Chemistry 70 (3): 874–877. doi:10.1021/j100875a042.
* Shashkin, S. Y.; Goddard III, W. A. (1986). "Electron Correlation effects in ligand field parameters and other properties of copper II fluoride". Journal of Physical Chemistry 90 (2): 250–255. doi:10.1021/j100274a010.

## External links

* National Pollutant Inventory - Copper and compounds fact sheet
* National Pollutant Inventory - Fluoride and compounds fact sheet

* v
* t
* e

Copper compounds

Cu(0,I)|

* Cu5Si

Cu(I)|

* CuBr
* CuCN
* CuCl
* CuF
* CuH
* CuI
* Cu2C2
* Cu2Cr2O5
* Cu2O
* CuOH
* CuNO3
* Cu3P
* Cu2S
* CuSCN

Cu(I,II)|

* Cu3H4O8S2

Cu(II)|

* Cu(BF4)2
* CuBr2
* CuC2
* CuCO3
* Cu(CN)2
* Cu(ClO3)2
* CuCl2
* CuF2
* Cu(NO3)2
* Cu3(PO4)2
* Cu(N3)2
* CuO
* CuO2
* Cu(OH)2
* CuI2
* CuS
* CuSO4
* Cu3(AsO4)2

Cu(III)|

* K3CuF6
* Cu2O3

Cu(IV)|

* Cs2CuF6
* Rb2CuF6

* v
* t
* e

Salts and covalent derivatives of the fluoride ion

HF |  |  |  | He

|
|
|
|

LiF | BeF2 | BF
BF3
B2F4 | CF4
other compounds | NF3
FN3
N2F2
N2F4
NF5§  | F2O
F2O2
other compounds | F2 | Ne
NaF | MgF2 | AlF
AlF3 | SiF4 | P2F4
PF3
PF5 | S2F2
SF2
SF4
SF6 | ClF
ClF3
ClF5 | Ar
KF | CaF
CaF2 | ScF3 | TiF2
TiF3
TiF4 | VF2
VF3
VF4
VF5 | CrF2
CrF3
CrF4
CrF5
CrF6§  | MnF2 | FeF2
FeF3 | CoF2
CoF3 | NiF2 | CuF
CuF2 | ZnF2 | GaF2
GaF3 | GeF2
GeF4 | AsF3
AsF5 | Se2F2
SeF4
SeF6 | BrF
BrF3
BrF5 | KrF2
RbF | SrF
SrF2 | YF3 | ZrF3
ZrF4 | NbF4
NbF5 | MoF2
MoF3
MoF4
MoF5
MoF6 | TcF4
TcF6 | RuF3
RuF5
RuF6 | RhF3
RhF5
RhF6 | PdF2 | AgF | CdF2 | InF
InF2
InF3 | SnF2
SnF4 | SbF3
SbF5 | Te3F2
TeF4
TeF6 | IF
IF3</br>IF5</br>IF7 | XeF2
XeF4
XeF6
CsF | BaF2 |  | HfF4 | TaF5 | WF2
WF3
WF4
WF5
WF6 | Re3F9
ReF4
ReF5
ReF6
ReF7 | OsF4
OsF5
OsF6 | IrF2
IrF3
IrF4
IrF5
IrF6 | PtF2
PtF4
PtF5
PtF6 | AuF
AuF3
Au2F10
AuF5•F2 | Hg2F2
HgF2
HgF4 | TlF | PbF2
PbF4 | BiF3
BiF5 | PoF2
PoF4
PoF6 | AtF  | RnF2
FrF | RaF2 |  | Rf  | Db  | Sg  | Bh  | Hs  | Mt  | Ds  | Rg  | Cn  | Nh  | Fl  | Mc  | Lv  | Ts  | Og
| ↓  |  |
LaF3 | CeF3
CeF4 | PrF3 | NdF2,
NdF3 | PmF3 | SmF2,
SmF3 | EuF2,
EuF3 | GdF3 | TbF3 | DyF2,
DyF3 | HoF3 | ErF3 | TmF2
TmF3 | YbF2
YbF3 | LuF3
AcF3 | ThF4 | PaF5 | UF3
UF4
UF5
UF6 | NpF4
NpF6 | PuF3
PuF6 | AmF2
AmF3 | CmF3 | BkF3 | CfF3 | EsF3 | Fm  | Md  | No  | LrF3

§ means the substance has not been made.

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