Krypton difluoride

Krypton difluoride, KrF₂ is a chemical compound of krypton and fluorine. It was the first compound of krypton discovered. It is a volatile, colourless solid at room temperature. The structure of the KrF₂ molecule is linear, with Kr−F distances of 188.9 pm. It reacts with strong Lewis acids to form salts of the KrF⁺ and Kr cations.

The atomization energy of KrF₂ (KrF_2(g) → Kr_(g) + 2 F_(g)) is 21.9 kcal/mol, giving an average Kr–F bond energy of only 11 kcal/mol, the weakest of any isolable fluoride. In comparison, the dissociation of difluorine to atomic fluorine requires cleaving a F–F bond with a bond dissociation energy of 36 kcal/mol. Consequently, KrF₂ is a good source of the extremely reactive and oxidizing atomic fluorine. It is thermally unstable, with a decomposition rate of 10% per hour at room temperature. The formation of krypton difluoride is endothermic, with a heat of formation (gas) of 14.4 ± 0.8 kcal/mol measured at 93 °C.

Synthesis

Krypton difluoride can be synthesized using many different methods including electrical discharge, photoionization, hot wire, and proton bombardment. The product can be stored at −78 °C without decomposition.

Electrical discharge

Electric discharge was the first method used to make krypton difluoride. It was also used in the only experiment ever reported to produce krypton tetrafluoride, although the identification of krypton tetrafluoride was later shown to be mistaken. The electrical discharge method involves having 1:1 to 2:1 mixtures of F₂ to Kr at a pressure of 40 to 60 torr and then arcing large amounts of energy between it. Rates of almost 0.25 g/h can be achieved. The problem with this method is that it is unreliable with respect to yield.

Proton bombardment

Using proton bombardment for the production of KrF₂ has a maximum production rate of about 1 g/h. This is achieved by bombarding mixtures of Kr and F₂ with a proton beam operating at an energy level of 10 MeV and at a temperature of about 133 K. It is a fast method of producing relatively large amounts of KrF₂, but requires a source of high-energy protons, which usually would come from a cyclotron.

Photochemical

The successful photochemical synthesis of krypton difluoride was first reported by Lucia V. Streng in 1963. It was next reported in 1975 by J. Slivnik. The photochemical process for the production of KrF₂ involves the use of UV light and can produce under ideal circumstances 1.22 g/h. The ideal wavelengths to use are in the range of 303–313 nm. Harder UV radiation is detrimental to the production of KrF₂. Using Pyrex glass, Vycor, or quartz will significantly increase yield because they all block harder UV light. In a series of experiments performed by S. A Kinkead et al., it was shown that a quartz insert (UV cut off of 170 nm) produced on average 158 mg/h, Vycor 7913 (UV cut off of 210 nm) produced on average 204 mg/h and Pyrex 7740 (UV cut off of 280 nm) produced on average 507 mg/h. It is clear from these results that higher-energy ultraviolet light reduces the yield significantly. The ideal circumstances for the production KrF₂ by a photochemical process appear to occur when krypton is a solid and fluorine is a liquid, which occur at 77 K. The biggest problem with this method is that it requires the handling of liquid F₂ and the potential of it being released if it becomes overpressurized.

Hot wire

The hot wire method for the production of KrF₂ uses krypton in a solid state with a hot wire running a few centimeters away from it as fluorine gas is then run past the wire. The wire has a large current, causing it to reach temperatures around 680 °C. This causes the fluorine gas to split into its radicals, which then can react with the solid krypton. Under ideal conditions, it has been known to reach a maximum yield of 6 g/h. In order to achieve optimal yields the gap between the wire and the solid krypton should be 1 cm, giving rise to a temperature gradient of about 900 °C/cm. A major downside to this method is the amount of electricity that has to be passed through the wire. It is dangerous if not properly set up.

Structure

Krypton difluoride can exist in one of two possible crystallographic morphologies: α-phase and β-phase. β-KrF₂ generally exists at above −80 °C, while α-KrF₂ is more stable at lower temperatures. The unit cell of α-KrF₂ is body-centred tetragonal.

Reactions

Krypton difluoride is primarily a powerful oxidising and fluorinating agent, more powerful even than elemental fluorine because Kr–F has less bond energy. It has a redox potential of +3.5 V for the KrF₂/Kr couple, making it the most powerful known oxidising agent. However, the hypothetical could be even stronger and nickel tetrafluoride comes close.

For example, krypton difluoride can oxidise gold to its highest-known oxidation state, +5:
:
KrFAuF decomposes at 60 °C into gold(V) fluoride and krypton and fluorine gases:
:

can also directly oxidise xenon to xenon hexafluoride:
:

is used to synthesize the highly reactive BrF cation. reacts with to form the salt KrFSbF; the KrF cation is capable of oxidising both and to BrF and ClF, respectively.

can also react with elemental silver to produce .

Irradiation of a crystal of KrF₂ at 77 K with γ-rays leads to the formation of the krypton monofluoride radical, KrF•, a violet-colored species that was identified by its ESR spectrum. The radical, trapped in the crystal lattice, is stable indefinitely at 77 K but decomposes at 120 K.

See also

*Krypton fluoride laser

References

General reading

*

External links

NIST Chemistry WebBook: krypton difluoride

{{fluorine compounds

Fluorides
Nonmetal halides
Krypton compounds