Silver difluoride

Silver(II) fluoride
Names

IUPAC name silver(II) fluoride
Other names silver difluoride
Identifiers
CAS Number	7783-95-1^N
3D model (JSmol)	Interactive image
ChemSpider	10802085^Y
ECHA InfoCard	100.029.124
EC Number	232-037-5
PubChem CID	82221
InChI InChI=1S/Ag.2FH/h;21H/q+2;;/p-2^Y Key: KWVVTSALYXIJSS-UHFFFAOYSA-L^Y InChI=1/Ag.2FH/h;21H/q+2;;/p-2 Key: KWVVTSALYXIJSS-NUQVWONBAP
SMILES [Ag+2].[F-].[F-]
Properties
Chemical formula	AgF₂
Molar mass	145.865 g/mol
Appearance	white or grey crystalline powder, hygroscopic
Density	4.58 g/cm³
Melting point	690 °C (1,274 °F; 963 K)
Boiling point	700 °C (1,292 °F; 973 K) (decomposes)
Solubility in water	Decomposes violently
Structure
Crystal structure	orthorhombic
Coordination geometry	tetragonally elongated octahedral coordination
Molecular shape	linear
Hazards
Main hazards	toxic, reacts violently with water, powerful oxidizer
Safety data sheet	MSDS
Related compounds
Other anions	Silver(I,III) oxide
Other cations	Copper(II) fluoride Palladium(II) fluoride Zinc fluoride Cadmium(II) fluoride Mercury(II) fluoride
Related compounds	Silver subfluoride Silver(I) fluoride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N (what is ^YN ?)
Infobox references

Silver(II) fluoride is a chemical compound with the formula AgF₂. It is a rare example of a silver(II) compound. Silver usually exists in its +1 oxidation state. It is used as a fluorinating agent.

AgF₂ can be synthesized by fluorinating Ag₂O with elemental fluorine. Also, at 200 °C (473 K) elemental fluorine will react with AgF or AgCl to produce AgF₂.

As a strong fluorinating agent, AgF₂ should be stored in Teflon or a passivated metal container. It is light sensitive.

AgF₂ can be purchased from various suppliers, the demand being less than 100 kg/year. While laboratory experiments find use for AgF₂, it is too expensive for large scale industry use. In 1993, AgF₂ cost between 1000-1400 US dollars per kg.

AgF₂ is a white crystalline powder, but it is usually black/brown due to impurities. The F/Ag ratio for most samples is < 2, typically approaching 1.75 due to contamination with Ag and oxides and carbon.

For some time, it was doubted silver was actually in the +2 oxidation state rather in some combination of states such as Ag^I[Ag^IIIF₄], which would be similar to silver(I,III) oxide. Neutron diffraction studies, however, confirmed its description as silver(II). The Ag^I[Ag^IIIF₄] was found to be present at high temperatures, but it was unstable with respect to AgF₂.

In the gas phase, AgF₂ is believed to have D_∞hsymmetry.

Approximately 14 kcal/mol (59 kJ/mol) separate the ground and first states. The compound is paramagnetic, but it becomes ferromagnetic at temperatures below −110 °C (163 K).

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