Plumbane

From Handwiki
Plumbane
Skeletal formula of plumbane
Spacefill model of plumbane
  Lead, Pb
  Hydrogen, H
Names
IUPAC name
Plumbane
Other names
lead tetrahydride, tetrahydridolead, lead(IV) hydride, hydrogen plumbide
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
Properties
PbH4
Molar mass 211.23 g/mol
Appearance Colorless gas
Boiling point −13 °C (9 °F; 260 K)
Structure
Tetrahedral at the Pb atom
Related compounds
Related tetrahydride 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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Plumbane is an inorganic chemical compound with the chemical formula PbH4. It is a colorless gas. It is a metal hydride and group 14 hydride composed of lead and hydrogen.[1] Plumbane is not well characterized or well known, and it is thermodynamically unstable with respect to the loss of a hydrogen atom.[2] Derivatives of plumbane include lead tetrafluoride, PbF4, and tetraethyllead, (CH3CH2)4Pb.

History

Until recently, it was uncertain whether plumbane had ever actually been synthesized,[3] although the first reports date back to the 1920s[4] and in 1963, Saalfeld and Svec reported the observation of PbH+4 by mass spectrometry.[5] Plumbane has repeatedly been the subject of Dirac–Hartree–Fock relativistic calculation studies, which investigate the stabilities, geometries, and relative energies of hydrides of the formula MH4 or MH2.[2][6][7]

Properties

Plumbane is an unstable colorless gas and is the heaviest group IV hydride.[8] Furthermore, plumbane has a tetrahedral (Td) structure with an equilibrium distance between lead and hydrogen of 1.73 Å.[9] By weight percent, the composition of plumbane is 1.91% hydrogen and 98.09% lead. In plumbane, the formal oxidation states of hydrogen and lead are +1 and -4, respectively, because the electronegativity of lead(IV) is higher than that of hydrogen. The stability of metal hydrides with the formula MH4 (M = C–Pb) decreases as the atomic number of M increases.

Preparation

Early studies of PbH4 revealed that the molecule is unstable as compared to its lighter congeners (silane, germane, and stannane).[10] It cannot be made by methods used to synthesize GeH4 or SnH4.

In 1999, plumbane was synthesized from lead(II) nitrate, Pb(NO3)2, and sodium borohydride, NaBH4.[11] A non-nascent mechanism for plumbane synthesis was reported in 2005.[12]

In 2003, Wang and Andrews carefully studied the preparation of PbH4 by laser ablation and additionally identified the infrared (IR) bands.[13]

Congeners

Congeners of plumbane include:

References

  1. ↑ Porritt, C. J. (1975). Chem. Ind-London 9: 398. 
  2. ↑ 2.0 2.1 Hein, Thomas A.; Thiel, Walter; Lee, Timothy J. (1993). "Ab initio study of the stability and vibrational spectra of plumbane, methylplumbane, and homologous compounds". The Journal of Physical Chemistry 97 (17): 4381–4385. doi:10.1021/j100119a021. 
  3. ↑ Cotton, F. A.; Wilkinson, G.; Murillo, C. A.; Bochman, M. Advanced Inorganic Chemistry. Wiley: New York, 1999
  4. ↑ Paneth, Fritz; Nörring, Otto (1920). "Über Bleiwasserstoff". Berichte der Deutschen Chemischen Gesellschaft (A and B Series) 53 (9): 1693–1710. doi:10.1002/cber.19200530915. https://zenodo.org/record/1426681. 
  5. ↑ Saalfeld, Fred E.; Svec, Harry J. (1963). "The Mass Spectra of Volatile Hydrides. I. The Monoelemental Hydrides of the Group IVB and VB Elements". Inorganic Chemistry 2: 46–50. doi:10.1021/ic50005a014. 
  6. ↑ Desclaux, J. P.; Pyykko, P. (1974). "Relativistic and non-relativistic Hartree-Fock one-centre expansion calculations for the series CH4 to PbH4 within the spherical approximation". Chemical Physics Letters 29 (4): 534–539. doi:10.1016/0009-2614(74)85085-2. Bibcode: 1974CPL....29..534D. 
  7. ↑ Pyykkö, P.; Desclaux, J. P. (1977). "Dirac–Fock one-centre calculations show (114)H4 to resemble PbH4". Nature 266 (5600): 336–337. doi:10.1038/266336a0. Bibcode: 1977Natur.266..336P. 
  8. ↑ CRC Handbook of Chemistry and Physics Online Edition.
  9. ↑ Visser, O.; Visscher, L.; Aerts, P. J. C.; Nieuwpoort, W. C. (1992). "Relativistic all-electron molecular Hartree-Fock-Dirac-(Breit) calculations on CH4, SiH4, GeH4, SnH4, PbH4". Theoretica Chimica Acta 81 (6): 405–416. doi:10.1007/BF01134864. 
  10. ↑ Malli, Gulzari L.; Siegert, Martin; Turner, David P. (2004). "Relativistic and electron correlation effects for molecules of heavy elements: Ab initio fully relativistic coupled-cluster calculations for PbH4". International Journal of Quantum Chemistry 99 (6): 940–949. doi:10.1002/qua.20142. 
  11. ↑ Krivtsun, V. M.; Kuritsyn, Y. A.; Snegirev, E. P. (1999). "Observation of IR absorption spectra of the unstable PbH4 molecule". Opt. Spectrosc 86 (5): 686–691. Bibcode: 1999OptSp..86..686K. http://www.isan.troitsk.ru/dms/tdl/publ/1999os_en.pdf. Retrieved 2012-12-31. 
  12. ↑ Zou, Y; Jin, FX; Chen, ZJ; Qiu, DR; Yang, PY (2005). "Non-nascent hydrogen mechanism of plumbane generation". Guang Pu Xue Yu Guang Pu Fen Xi = Guang Pu 25 (10): 1720–3. PMID 16395924. 
  13. ↑ Wang, Xuefeng; Andrews, Lester (2003). "Infrared Spectra of Group 14 Hydrides in Solid Hydrogen: Experimental Observation of PbH4, Pb2H2, and Pb2H4". Journal of the American Chemical Society 125 (21): 6581–6587. doi:10.1021/ja029862l. PMID 12785799. 



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Categories: [Metal hydrides] [Lead compounds]

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