Iron(III) fluoride Property

Melting point:

1000 °C

Density 

3,87 g/cm³

solubility 

insoluble in ethanol, ethyl ether, benzene

form 

Powder

color 

Pale green

Specific Gravity

3.87

Water Solubility 

Soluble in dilute hydrofluroic acid. Slightly soluble in water. Insoluble in alcohol, ether and benzene.

Sensitive 

Hygroscopic

Crystal Structure

VF3 type

crystal system

Three sides

Merck 

14,4022

Solubility Product Constant (Ksp)

pKsp: 5.63

Space group

R3c

Lattice constant

a/nm	b/nm	c/nm	α/o	β/o	γ/o	V/nm3
0.519	0.519	1.334	90	90	120	0.3113

Exposure limits

ACGIH: TWA 1 mg/m3; TWA 2.5 mg/m3
NIOSH: IDLH 250 mg/m3; TWA 1 mg/m3

Stability:

hygroscopic

CAS DataBase Reference

7783-50-8(CAS DataBase Reference)

EPA Substance Registry System

Ferric fluoride (7783-50-8)

Safety

Hazard Codes 

C

Risk Statements 

34-20/21/22

Safety Statements 

26-36/37/39-45-27-22

RIDADR 

UN 3260 8/PG 2

WGK Germany 

3

RTECS 

NO6865000

F 

3

Hazard Note 

Corrosive

TSCA 

Yes

HazardClass 

6.1

PackingGroup 

III

HS Code 

2826199090

Hazardous Substances Data

7783-50-8(Hazardous Substances Data)

Hazard and Precautionary Statements (GHS)

Symbol(GHS)

Signal word

Warning

Hazard statements

H315Causes skin irritation

Precautionary statements

P264Wash hands thoroughly after handling.

P264Wash skin thouroughly after handling.

P280Wear protective gloves/protective clothing/eye protection/face protection.

P302+P352IF ON SKIN: wash with plenty of soap and water.

P332+P313IF SKIN irritation occurs: Get medical advice/attention.

Iron(III) fluoride Chemical Properties,Usage,Production

Chemical Properties

green powder

Chemical Properties

Iron(III) fluoride is only sparingly soluble in water and insoluble in alcohol and ether. When heated in hydrogen it is reduced to iron(II) fluoride and thence to the metal. In aqueous solution the hydrolysis appears to be very slight ; in the presence of alkali metal fluorides, complex fluorides of types MFeF4, M2FeF5.xH2O and M3FeF6 can be crystallized. The magnetic behaviour of FeF3 is complicated; between 63° and 293°K the susceptibility is field strength dependent. The trihydrate has a magnetic moment μ = 2-25 B.M. at 300°K.

Uses

Iron(III) fluroide is used in ceramics manufacturing. It is used as a catalyst for certain cross coupling reactions. Further, it is involved in the chemoselective addition of cyanide to aldehyde to prepare cyanohydrins.

Uses

As catalyst in organic reactions.

Preparation

This can be prepared by the action of fluorine on the metal, iron(II), or iron(III) chloride or by dehydration of the hydrate (obtained from aqueous solution) by heating in a current of hydrogen fluoride. A convenient laboratory preparation involves the reaction of hydrogen fluoride with anhydrous iron(III) chloride at room temperature :
FeCl3+3HF→ FeF3+3HCl
When crystallized from aqueous solution (iron(III) "hydroxide" and aqueous hydrofluoric acid) it forms the pale pink 4?-hydrate (room temperature evaporation) and the pink 3-hydrate (evaporation by heating).

General Description

IRON (II) FLUORIDE is a green crystalline solid. IRON (II) FLUORIDE is slightly soluble in water. The primary hazard is the threat to the environment. Immediate steps should be taken to limit its spread to the environment. IRON (II) FLUORIDE is used in ceramics.

Air & Water Reactions

Slightly soluble in water forming acidic solutions.

Reactivity Profile

Acidic salts, such as IRON (II) FLUORIDE, are generally soluble in water. The resulting solutions contain moderate concentrations of hydrogen ions and have pH's of less than 7.0. They react as acids to neutralize bases. These neutralizations generate heat, but less or far less than is generated by neutralization of inorganic acids, inorganic oxoacids, and carboxylic acid. They usually do not react as either oxidizing agents or reducing agents but such behavior is not impossible. IRON (II) FLUORIDE is used to catalyze organic reactions.

Hazard

Strong irritant.

Health Hazard

INHALATION: Inorganic fluorides are generally irritating. INGESTION: Ingestion of iron compounds can cause: lethargy, retching, vomiting, tarry stools, fast and weak pulse, low blood pressure, and coma.

Fire Hazard

Behavior in Fire: May give off fumes or vapors of fluorides; hydrofluoric acid.

Safety Profile

Moderately toxic by intraperitoneal route. Mutation data reported. When heated to decomposition it emits toxic fumes of F-. See also FLUORIDES.