Gold hexafluoride

Gold hexafluoride
Names
	Other names Gold(VI) fluoride
Identifiers
3D model (JSmol)	Interactive image;
	InChI InChI=1S/Au.6FH/h;6*1H/q+6;;;;;;/p-6 Key: PNIORJQZAPGWIB-UHFFFAOYSA-H;
	SMILES [Au+6].[F-].[F-].[F-].[F-].[F-].[F-];
Properties
Chemical formula	AuF6
Molar mass	310.956989 g·mol−1
Related compounds
Related compounds	Platinum hexafluoride
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Infobox references

Gold hexafluoride is a binary inorganic chemical compound of gold and fluorine with the chemical formula AuF₆.^[1] As of 2023, it is still a hypothetical compound that has never been prepared or observed.^[2]^[3] In 1999, Neil Bartlett stated, "It should exist, if made at low temperature and kept cold."^[4]

Potential properties

Like PtF₆, AuF₆ should be an extremely powerful oxidizer.^[5] The compound is calculated to be stable.^[6]

References

^ Compton, R. N.; Klots, Cornelius E. (1989). Iones, Molecules, and Energy. Oak Ridge National Laboratory . p. 169. Retrieved 2 May 2023.
^ Groult, Henri; Leroux, Frederic; Tressaud, Alain (4 November 2016). Modern Synthesis Processes and Reactivity of Fluorinated Compounds: Progress in Fluorine Science. Elsevier. p. 563. ISBN 978-0-12-803790-4. Retrieved 2 May 2023.
^ Hargittai, Istvan; Hargittai, Magdolna (21 March 2003). Candid Science Iii: More Conversations With Famous Chemists. World Scientific. p. 47. ISBN 978-1-78326-111-6. Retrieved 2 May 2023.
^ Hargittai, Istvan (13 April 2010). Drive and Curiosity: What Fuels the Passion for Science. Prometheus Books. ISBN 978-1-61614-469-2. Retrieved 2 May 2023.
^ Craciun, Raluca; Picone, Désireé; Long, Rebecca T.; Li, Shenggang; Dixon, David A.; Peterson, Kirk A.; Christe, Karl O. (1 February 2010). "Third Row Transition Metal Hexafluorides, Extraordinary Oxidizers, and Lewis Acids: Electron Affinities, Fluoride Affinities, and Heats of Formation of WF₆, ReFF₆, OsF₆, IrF₆, PtF₆, and AuF₆". Inorganic Chemistry. 49 (3): 1056–1070. doi:10.1021/ic901967h. ISSN 0020-1669. PMID 20052991.
^ Bartlett, Neil (26 October 2001). Oxidation Of Oxygen And Related Chemistry, The: Selected Papers Of Neil Bartlett. World Scientific. p. 201. ISBN 978-981-4498-50-0. Retrieved 2 May 2023.

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[1] Compton, R. N.; Klots, Cornelius E. (1989). Iones, Molecules, and Energy. Oak Ridge National Laboratory . p. 169. Retrieved 2 May 2023.

[2] Groult, Henri; Leroux, Frederic; Tressaud, Alain (4 November 2016). Modern Synthesis Processes and Reactivity of Fluorinated Compounds: Progress in Fluorine Science. Elsevier. p. 563. ISBN 978-0-12-803790-4. Retrieved 2 May 2023.

[3] Hargittai, Istvan; Hargittai, Magdolna (21 March 2003). Candid Science Iii: More Conversations With Famous Chemists. World Scientific. p. 47. ISBN 978-1-78326-111-6. Retrieved 2 May 2023.

[4] Hargittai, Istvan (13 April 2010). Drive and Curiosity: What Fuels the Passion for Science. Prometheus Books. ISBN 978-1-61614-469-2. Retrieved 2 May 2023.

[5] Craciun, Raluca; Picone, Désireé; Long, Rebecca T.; Li, Shenggang; Dixon, David A.; Peterson, Kirk A.; Christe, Karl O. (1 February 2010). "Third Row Transition Metal Hexafluorides, Extraordinary Oxidizers, and Lewis Acids: Electron Affinities, Fluoride Affinities, and Heats of Formation of WF₆, ReFF₆, OsF₆, IrF₆, PtF₆, and AuF₆". Inorganic Chemistry. 49 (3): 1056–1070. doi:10.1021/ic901967h. ISSN 0020-1669. PMID 20052991.

[6] Bartlett, Neil (26 October 2001). Oxidation Of Oxygen And Related Chemistry, The: Selected Papers Of Neil Bartlett. World Scientific. p. 201. ISBN 978-981-4498-50-0. Retrieved 2 May 2023.

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