Mercury(IV) fluoride

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Mercury(IV) fluoride
Mercury-tetrafluoride-3D-balls.png
Mercury-tetrafluoride-2D.png
Properties
Molecular formula HgF4
Molar mass 276.58 g/mol
Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
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Infobox references

Mercury(IV) fluoride, HgF4, is the first mercury compound to be discovered with mercury in the oxidation state IV. Mercury, like the other group 12 elements (cadmium and zinc), has an s2d10 electron configuration and generally only forms bonds involving its s orbital. This means that the highest oxidation state mercury normally attains is II, and for this reason it is usually considered a post-transition metal instead of a transition metal.

History[edit]

Speculation about higher oxidation states for mercury had been around since the 1970s, and theoretical calculations in the 1990s predicted that it should be stable in the gas phase, with a square-planar geometry consistent with a formal d8 configuration. However, experimental proof remained elusive until 2007, when HgF4 was first prepared using solid neon and argon for matrix isolation at a temperature of 4 K. The compound was detected using infrared spectroscopy.[1][2] Analysis of density functional theory and coupled cluster calculations showed that the d orbitals are involved in bonding, leading to the suggestion that mercury should be considered a transition metal after all.[3] However, that conclusion has been challenged by W. B. Jensen with the argument that HgF4 only exists under highly atypical non-equilibrium conditions and should best be considered as an exception.[4]

Explanation[edit]

Theoretical studies suggest that mercury is unique among the natural elements of group 12 in forming a tetrafluoride, and attribute this observation to relativistic effects. According to calculations, the tetrafluorides of the "less relativistic" elements cadmium and zinc are unstable and eliminate a fluorine molecule, F2, to form the metal difluoride complex. On the other hand, the tetrafluoride of the "more relativistic" synthetic element 112, copernicium, is predicted to be more stable.[5]

Synthesis and properties[edit]

HgF4 is produced by the reaction of elemental mercury with fluorine:

Hg + 2 F2 → HgF4

HgF4 is only stable in matrix isolation at 4 K; upon heating, or if the HgF4 molecules touch each other, it decomposes to mercury(II) fluoride and fluorine:

HgF4 → HgF2 + F2

HgF4 is a diamagnetic, square planar molecule. The mercury atom has a formal 6s25d86p6 electron configuration, and as such obeys the octet rule but not the 18-electron rule. HgF4 is isoelectronic with the tetrafluoroaurate anion, AuF
4
, and is valence isoelectronic with the tetrachloroaurate (AuCl
4
), tetrabromoaurate (AuBr
4
), and tetrachloroplatinate (PtCl2−
4
) anions.

References[edit]

  1. ^ "High Oxidation States: Mercury tetrafluoride synthesized". 
  2. ^ "Elusive Hg(IV) species has been synthesized under cryogenic conditions". 2007-10-12. 
  3. ^ Xuefang Wang; Lester Andrews; Sebastian Riedel; Martin Kaupp (2007). "Mercury Is a Transition Metal: The First Experimental Evidence for HgF4.". Angew. Chem. Int. Ed. 46 (44): 8371–8375. doi:10.1002/anie.200703710. PMID 17899620. 
  4. ^ William B. Jensen (2008). "Is Mercury Now a Transition Element?". J. Chem. Educ. 85 (9): 1182–1183. doi:10.1021/ed085p1182. 
  5. ^ Haire, Richard G. (2006). "Transactinide elements and future elements". In Morss; Edelstein, Norman M.; Fuger, Jean. The Chemistry of the Actinide and Transactinide Elements (3rd ed.). Dordrecht, The Netherlands: Springer Science+Business Media. p. 1675. ISBN 1-4020-3555-1.