Silver fluoride Chemical Properties

Melting point:

≥300 °C(lit.)

Boiling point:

1150 °C

Density 

5.852 g/mL at 25 °C(lit.)

Flash point:

1150°C

storage temp. 

Keep in dark place,Inert atmosphere,Room temperature

solubility 

Methanol (Slightly), Water (Slightly)

form 

solid

color 

orange to brown

Specific Gravity

5.852

Water Solubility 

182 g/100 mL (15.5 ºC)

Sensitive 

Moisture Sensitive & Hygroscopic

Crystal Structure

NaCl type

crystal system

Cube

Merck 

14,8514

Space group

Fm3m

Lattice constant

a/nm	b/nm	c/nm	α/o	β/o	γ/o	V/nm3
0.493	0.493	0.493	90	90	90	0.1198

Exposure limits

ACGIH: TWA 0.01 mg/m3; TWA 2.5 mg/m3
NIOSH: IDLH 10 mg/m3; IDLH 250 mg/m3; TWA 0.01 mg/m3

Stability:

Stable. Incompatible with strong oxidizing agents, strong acids, reducing agents. Light sensitive. Hygroscopic.

InChIKey

REYHXKZHIMGNSE-UHFFFAOYSA-M

CAS DataBase Reference

7775-41-9(CAS DataBase Reference)

NIST Chemistry Reference

Silver monofluoride(7775-41-9)

EPA Substance Registry System

Silver fluoride (7775-41-9)

Safety Information

Hazard Codes 

C

Risk Statements 

34-23/24/25-35

Safety Statements 

26-36/37/39-45-25-28

RIDADR 

UN 3260 8/PG 2

WGK Germany 

3

RTECS 

VW4250000

F 

3-8-10-21

Hazard Note 

Corrosive

TSCA 

T

HazardClass 

HYGROSCOPIC, CORROSIVE

HazardClass 

8

HS Code 

28432900

MSDS

• Language:English Provider:Silver monofluoride
• Language:English Provider:ACROS
• Language:English Provider:SigmaAldrich
• Language:English Provider:ALFA

Silver fluoride Usage And Synthesis

Chemical Properties

orange to brown solid

Uses

Silver(I) fluoride is used as a fluorination and desilylation reagent in organic synthesis. In medical filed, it is used as topical caries in aqueous form in dentistry. It is employed in organofluorine chemistry for addition of fluoride across multiple bonds, especially to prepare perfluoroalkylsilver(I) by reacting with alkenes. Further, it is involved in the preparation of tetralkylammonium fluorides by the reaction with tetralkylammonium bromide. In addition to this, it is used as a desulfuration-fluorination reagent on thiourea derived substrates.

Uses

1. Silver fluoride is applied to convert organic Br and Cl Compounds to their fluoro analogs; as antiseptic.
2. Preparation of bromoacetylenes from bulky, trialkylsilylacetylenes.
3. Also used in a palladium-catalyzed cross coupling of acetanilides with trialkoxysilanes.
4. Silver(I) fluoride is used as a fluorination and desilylation reagent in organic synthesis. In medical filed, it is used as topical caries in aqueous form in dentistry. It is employed in organofluorine chemistry for addition of fluoride across multiple bonds, especially to prepare perfluoroalkylsilver(I) by reacting with alkenes.
5. Further, it is involved in the preparation of tetralkylammonium fluorides by the reaction with tetralkylammonium bromide. In addition to this, it is used as a desulfuration-fluorination reagent on thiourea derived substrates.

Uses

Definition

ChEBI: Silver monofluoride is a silver salt and a fluoride salt.

Preparation

Silver(I) fluoride was prepared by reacting hydrogen fluoride with the carbonate and with the oxide.

General Description

Odorless yellow to gray solid. Sinks and mixes with water.

Air & Water Reactions

Water soluble.

Reactivity Profile

Boron reacts explosively when ground with Silver fluoride; silicon reacts violently [Bretherick 1979 p, 197]. Dimethyl sulfoxide is violently reactive with fluorinating agents such as Silver fluoride [Chem. Eng. News 44(24):7 1956]. When Silver fluoride is ground with calcium hydride the mass becomes incandescent [Mellor 3:389 1946-1947]. CaH2 reacts incandescently with AgF if subject to friction. (Mellor, 1941, Vol. 3, 389, 651).

Hazard

Strong irritant.

Health Hazard

Inhalation of dust causes irritation of nose and throat. Ingestion may cause vomiting, salty taste, abdominal pain, diarrhea, convulsions, collapse, thirst, disturbed color vision, and acute toxic nephritis. Contact with eyes causes irritation. Skin may be blackened on prolonged exposure.

Purification Methods

The fluoride is a hygroscopic solid with a solubility of 135g/100mL of H2O at 15o, and forms an insoluble basic fluoride in moist air. Purify it by washing with AcOH and dry *C6H6, then keep it in a vacuum desiccator at room temperature to remove *C6H6, and store it in opaque glass bottles. The flaky hygroscopic crystals darken on exposure to light. It attacks bone and teeth. [Sharpe J Chem Soc 4538 1952, Kwasnik in Handbook of Preparative Inorganic Chemistry (Ed. Brauer) Academic Press Vol I p 240 1963.]

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