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Iodine pentafluoride is an interhalogen compound with chemical formula IF 5. It is one of the fluorides of iodine. It is a colorless liquid, although impure samples appear yellow. It is used as a fluorination reagent and even a solvent in specialized syntheses. [3]
Liquid iodine trichloride conducts electricity, possibly indicating dissociation to ICl + 2 and ICl − 4 ions. [9] Iodine pentafluoride (IF 5), a colourless, volatile liquid, is the most thermodynamically stable iodine fluoride, and can be made by reacting iodine with fluorine gas at room temperature. It is a fluorinating agent, but is mild ...
Iodosyl pentafluoride is an inorganic compound of iodine, fluorine, ... Reaction of iodine heptafluoride with silicon dioxide: [3] [4] 2 IF 7 + SiO 2 → 2 IOF 5 + SiF 4.
Iodine pentafluoride (IF 5) is a colourless liquid, made by reacting iodine pentoxide with fluorine, or iodine with silver(II) fluoride. It is highly reactive, even slowly with glass. It reacts with water to form hydrofluoric acid and with fluorine gas to form iodine heptafluoride. The molecule has the form of a tetragonal pyramid.
[1] [2] [3] Introduced by Gilbert N. Lewis in his 1916 article The Atom and the Molecule, a Lewis structure can be drawn for any covalently bonded molecule, as well as coordination compounds. [4] Lewis structures extend the concept of the electron dot diagram by adding lines between atoms to represent shared pairs in a chemical bond.
The compounds are weak Lewis bases, with NF 3 again being an exception. [84] The pentafluorides of phosphorus [ 85 ] and arsenic [ 86 ] are much more reactive than their trifluorides; antimony pentafluoride is such a strong acid that it holds the title of the strongest Lewis acid. [ 86 ]
It is a chocolate-brown solid that decomposes at 0 °C, [1] disproportionating to elemental iodine and iodine pentafluoride: 5 IF → 2 I 2 + IF 5. However, its molecular properties can still be precisely determined by spectroscopy: the iodine-fluorine distance is 190.9 pm and the I−F bond dissociation energy is around 277 kJ mol −1.
Synthesis of iodosyl trifluoride can be done by a reaction of iodine pentoxide with iodine pentafluoride. [2] I 2 O 5 + 3IF 5 → 5IOF 3. Synthesis can be by a reaction of gases: [3] I 2 + O 2 + 3F 2 → 2IOF 3. Or alternately by reaction of iodine pentafluoride with water: IF 5 + H 2 O → IOF 3 + 2HF