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–Fockrelativistic 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] and has a tetrahedral (Td) structure with an equilibrium distance between lead and hydrogen of 1.73 Å.[9] By weight, 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 hydrides 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]
^Porritt, C. J. (1975). Chem. Ind-London. 9: 398. {{cite journal}}: Missing or empty |title= (help)
^ abHein, 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. hdl:11858/00-001M-0000-0028-1862-2.
^Cotton, F. A.; Wilkinson, G.; Murillo, C. A.; Bochman, M. Advanced Inorganic Chemistry. Wiley: New York, 1999
^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.
^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. Bibcode:1974CPL....29..534D. doi:10.1016/0009-2614(74)85085-2.
^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. S2CID97874625.
^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.
^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. PMID16395924.
^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. PMID12785799.
