iodine pentafluoride (IF5) is a colorless to pale yellow fuming liquid with a pungent odor. The highly reactive IF5 (melting point 9.4 °C) is distillable at 100.5 °C without any decomposition. Decomposition commences at temperatures above 400 °C. IF5 is not as popular as p-TolIF2 because F2 gas is used in its preparation and it decomposes in air by moisture emitting corrosive HF.
Iodine pentafluoride has good thermal stability and is the most stable halogen compound. The reactivity of IF5 is much weaker than that of other halogen compounds, and it does not interact with silicon, magnesium, copper, iron, and chromium at room temperature, and only interacts with molybdenum, tungsten, phosphorus, arsenic, antimony, boron, etc. The corresponding fluorides are generated, such as:
2 IF5 + 2 Sb → 2 SbF5 + I2
6 IF5 + 10 B → 10 BF3 + 15 I2
It is the least reactive of the halogen fluorides and classified as a soft fluorinating reagent. It is used as a mildest, selective fluorinating reagent in the fluorination of organic molecules.
Black crystalline solid; exists in two modifications: stable black needlesknown as alpha form that produces ruby-red color in transmitted light, and alabile, metastable beta modification consisting of black platelets which appearbrownish-red in transmitted light; density of alpha form 3.86 g/cm3at 0°C;density of beta form 3.66 g/cm3at 0°C; alpha form melts at 27.3°C, vapor pressure being 28 torr at 25°C; beta form melts at 13.9°C; liquid iodine monochloride has bromine-like reddishbrown color; liquid density 3.10 g/mL at 29°C;viscosity 1.21 centipoise at 35°C; decomposes around 100°C; supercools belowits melting point; polar solvent; as a liquid it dissolves iodine, ammoniumchloride and alkali metal chlorides; liquid ICl also miscible with carbon tetrachloride, acetic acid and bromine; the solid crystals dissolve in ethanol, ether,acetic acid and carbon disulfide; solid ICl also dissolves in conc. HCl butdecomposes in water or dilute HCl.
Iodine pentafluoride is a fluorinating agent and strong oxidant, which plays an important role in organic synthesis. It can be used to prepare pentafluoroiodoethane:
5 CF2=CF2 + IF5 + 2 I2 → 5 C2F5I
In addition, iodine pentafluoride can also react with isothiocyanato to generate fluorinated hydrocarbon derivatives, and to synthesize other fluorine-containing compounds.
Iodine pentafluoride (IF5) is rarely used to fluoride common organic compounds due to the difficulty in controlling their reactivity.
Iodine pentafluoride(IF5) is produced by the action of elemental fluorine on iodine which has a low melting point. The reaction is performed either in solvent or heating iodine to maintain its liquid state. In a commercial preparation about one percent iodine is dissolved in IF5 and brought into fluorination chamber where iodine reacts with fluorine and produces more IF5 which is returned to the receiving vessel. Only a small portion of IF5 is withdrawn from the receiving vessel as product, while the major portion of IF5 is used for dissolving more iodine. This process goes on and on until all iodine is converted into IF5.
In another industrial process, iodine is heated above its melting point (113℃) and reacted with elemental fluorine under three atmosphere of pressure. A precaution is taken not to heat iodine above 150℃ to avoid the formation of another product, IF7. Fluorine is added continuously until all iodine has reacted and converted to IF5.
Iodine pentafluoride appears as a toxic colorless fuming liquid (m.p. 9° C). Decomposed by water to iodine and hydrofluoric acid. Contact with organic materials may cause their ignition. Corrosive to metals and tissue. Prolonged exposure of the container to fire or heat may result in their violent rupturing and rocketing. Prolonged exposure to low concentrations or short term exposure to high concentrations may result in adverse health effects.
Fumes in air. Reaction with water or water-containing materials is violent, [Mellor 2, Supp. 1:176, 1956].
A powerful oxidizer. Attack glass. Reacts violently with water or strong bases (potassium hydroxide, sodium hydroxide). Pentalfluoroiodide chars and usually ignites organic matter. Contact with boron, silicon, red phosphorus, sulfur, arsenic, antimony, bismuth, molybdenum and tungsten causes incandescence. Contact with potassium or sodium leads to explosions. Causes aluminum (foil, powder) to ignite. Explosive reactions with tetraiodoethylene, diethylaminotrimethylsilane. Violent reactions wilh benzene, dimethyl sulfoxide, tetraiodoethylene [Bretherick, 5th ed., 1995, p. 1434]. IF5 reacts explosively with diethylaminotrimethylsilane even at low temperature. (Oates, G. et al., J. Chem. Soc., Dalton Trans., 1974, 1383).
Toxic by ingestion and inhalation, corrosive to skin and mucous membranes. Iodinepentafluoride is highly corrosive. Contactwith the skin can cause severe burns. Thevapors are highly irritating to the skin, eyes,and mucous membranes.
Dangerous fire risk, May ignite combustibles (wood, paper, oil, clothing, etc.). React vigorously and/or explosively with water. Produce toxic and/or corrosive substances on contact with water. Flammable/toxic gases may accumulate in tanks and hopper cars. Some may produce flammable hydrogen gas upon contact with metals. Containers may explode when heated. Runoff may create fire or explosion hazard.
Flammability and Explosibility
Non flammable
The iodine pentafluoride was purified by trap-to-trap distillation over preheated sodium fluoride in order to remove hydrogen fluoride. The iodine pentafluoride was then transferred by vacuum distillation to a vessel containing a dry mercury metal. The mixture was shaken mechanically for 5 minutes at room temperature to remove iodine. Once the mercury metal treatement was finished, iodine pentafluoride was stored over sodium fluoride in a sealed Pyrex glass vessel cooled to -196 °C . The purified iodine pentafluoride was colourless.
