Oxygen difluoride

Oxygen difluoride
Structure and dimensions of the oxygen difluoride molecule
Space-filling model of the oxygen difluoride molecule
Names
Other names
difluorine monoxide
fluorine monoxide
oxygen fluoride
hypofluorous anhydride
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.029.087
RTECS number
  • RS2100000
  • FOF
Properties
OF2
Molar mass 53.9962 g/mol
Appearance colorless gas, pale yellow liquid when condensed
Density 1.9 g/cm3
Melting point −223.8 °C
Boiling point −144.8 °C
Solubility in other solvents 68 mL gaseous OF2 in 1 L (0 °C)[1]
Thermochemistry
Std enthalpy of
formation ΔfHo298 		24.5 kJ mol−1
Related compounds
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Oxygen difluoride is the chemical compound with the formula OF2. It has a V-shaped molecular structure like H2O, but has different properties. It is a strong oxidizer.

Preparation

Oxygen difluoride was first prepared in 1929. It was made by the electrolysis of molten potassium fluoride and hydrofluoric acid. The chemicals had a small amount of moisture. [2][3] Nowadays, it is prepared by the reaction of fluorine with a dilute aqueous solution of sodium hydroxide. Sodium fluoride is left as a side-product:

2 F2 + 2 NaOH → OF2 + 2 NaF + H2O

Reactions

It is a very powerful oxidizing agent. This is proved by the oxidation number of +2 for the oxygen atom. This oxidising number is quite unusual. Above 200 °C, OF2 decomposes to oxygen and fluorine.

OF2 reacts with many metals. It produces oxides and fluorides. Nonmetals also react with it. Phosphorus reacts with OF2 to form PF5 and POF3. Sulfur produces SO2 and SF4 with it. A noble gas, xenon also reacts with it. It produces XeF4 and xenon oxyfluorides.

Oxygen difluoride reacts very slowly with water to form hydrofluoric acid:

OF2 (aq) + H2O (aq) → 2 HF (aq) + O2 (g)

Oxygen difluoride oxidizes sulfur dioxide to sulfur trioxide:

OF2 + SO2 → SO3 + F2

However, in the presence of UV radiation the products are sulfuryl fluoride, SO
2F
2, and pyrosulfuryl fluoride, S
2O
5F
2:

OF2 + 2 SO2 → S
2O
5F
2

Safety

OF2 is a dangerous chemical. This is because it is highly oxidising.

References

  1. ↑ Yost, D. M. "Oxygen Fluoride" Inorganic Syntheses, 1939 volume, 1, pages 109-111.
  2. ↑ Paul Lebeau; Damiens, A. "A New Method for the Preparation of the Fluorine Oxide”Compt. rend. 1929, volume 188, 1253-5.
  3. ↑ Lebeau, P.; Damiens, A. "The Existence of an Oxygen Compound of Fluorine"Compt. rend. 1927, volume 185, pages 652-4.

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