Xenon tetrafluoride
Chemical compound From Wikipedia, the free encyclopedia
Xenon tetrafluoride is a chemical compound with chemical formula XeF
4. It was the first discovered binary compound of a noble gas.[3] It is produced by the chemical reaction of xenon with fluorine:[4][5]
- Xe + 2 F
2 → XeF
4
4 crystals. 1962. | |||
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| Names | |||
|---|---|---|---|
| IUPAC name
Xenon tetrafluoride | |||
| Identifiers | |||
3D model (JSmol) |
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| ChemSpider | |||
| ECHA InfoCard | 100.033.858 | ||
PubChem CID |
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| UNII | |||
CompTox Dashboard (EPA) |
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| Properties | |||
| XeF 4 | |||
| Molar mass | 207.2836 g mol−1 | ||
| Appearance | White solid | ||
| Density | 4.040 g cm−3, solid | ||
| Melting point | 117 °C (243 °F; 390 K) sublimes[1] | ||
| Reacts | |||
| Structure | |||
| D4h | |||
| square planar | |||
| 0 D | |||
| Thermochemistry | |||
Std molar entropy (S⦵298) |
146 J·mol−1·K−1[2] | ||
Std enthalpy of formation (ΔfH⦵298) |
−251 kJ·mol−1[2] | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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This reaction is exothermic, releasing an energy of 251 kJ/mol.[3]
Xenon tetrafluoride is a colorless crystalline solid that sublimes at 117 °C. Its structure was determined by both NMR spectroscopy and X-ray crystallography in 1963.[6][7] The structure is square planar, as has been confirmed by neutron diffraction studies.[8] According to VSEPR theory, in addition to four fluoride ligands, the xenon center has two lone pairs of electrons. These lone pairs are mutually trans.
Synthesis
The original synthesis of xenon tetrafluoride occurred through direct 1:5-molar-ratio combination of the elements in a nickel (Monel) vessel at 400 °C.[9] The nickel does not catalyze the reaction,[citation needed] but rather protects the container surfaces against fluoride corrosion. Controlling the process against impurities is difficult, as xenon difluoride (XeF
2), tetrafluoride, and hexafluoride (XeF
6) are all in chemical equilibrium, the difluoride favored at low temperatures and little fluorine and the hexafluoride favored at high temperatures and excess fluorine.[9][10] Fractional sublimation (xenon tetrafluoride is particularly involatile) or other equilibria generally allow purification of the product mixture.[9]
The elements combine more selectively when γ- or UV-irradiated in a nickel container or dissolved in anhydrous hydrogen fluoride with catalytic oxygen. That reaction is believed selective because dioxygen difluoride at standard conditions is too weak an oxidant to generate xenon(VI) species.[9]
Alternatively, fluoroxenonium perfluorometallate salts pyrolyze to XeF4.[9]
Reactions
Summarize
Perspective
Xenon tetrafluoride hydrolyzes at low temperatures to form elemental xenon, oxygen, hydrofluoric acid, and aqueous xenon trioxide:[11]
It is used as a precursor for synthesis of all tetravalent Xe compounds.[9] Reaction with tetramethylammonium fluoride gives tetramethylammonium pentafluoroxenate, which contains the pentagonal XeF−
5 anion. The XeF−
5 anion is also formed by reaction with cesium fluoride:[12]
- CsF + XeF
4 → CsXeF
5
Reaction with bismuth pentafluoride (BiF
5) forms the XeF+
3 cation:[13]
- BiF
5 + XeF
4 → XeF3BiF6
The XeF+
3 cation in the salt XeF3Sb2F11 has been characterized by NMR spectroscopy.[14]
At 400 °C, XeF
4 reacts with xenon to form XeF
2:[10]
- XeF4 + Xe → 2 XeF2
The reaction of xenon tetrafluoride with platinum yields platinum tetrafluoride and xenon:[10]
- XeF4 + Pt → PtF4 + Xe
Applications
Xenon tetrafluoride has few applications. It has been shown to degrade silicone rubber for analyzing trace metal impurities in the rubber. XeF
4 reacts with the silicone to form simple gaseous products, leaving a residue of metal impurities.[15]
References
External links
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