"Front Matter". In: Organosilanes in Radical Chemistry - Index of
"Front Matter". In: Organosilanes in Radical Chemistry - Index of "Front Matter". In: Organosilanes in Radical Chemistry - Index of
Theoretical Approaches 45 studies in the gas phase and a number of theoretical investigations. For attacking species such as H, Cl and Br atoms, the room temperature rate constant corrected for reaction path degeneracy, k/n, is higher for Me3SiH than H4Si by a factor of around 4 [36]. However, the interplay of activation energy and preexponential factor is complex and is not fully understood. The reaction of H: atoms is reported in Table 3.7 in detail, for a better understanding of the reactivity trend in this case [36]. Indeed, the methyl substitution leads to an increase in the Si w H bond reactivity when the statistical number of abstracted hydrogens is taken into account. Theory reproduced very well the experimental rate constants at 25 8C (values in parenthesis) [37]. However, the experimental activation energies and A factors are difficult to rationalize because the changes are small and may be also masked by experimental errors. Theoretical calculations suggest that the activation energies for the three reactions are nearly the same (i.e., unaffected by methylation), whereas the increase of reactivity along the series reflects a parallel change in the preexponential factors. The increase in A factor with methylation has been explained in terms of an increase in the entropy of the transition state associated either with the introduction of soft skeletal vibrations, or the freeing of the hindered internal rotation of the methyl groups [38]. 3.7 THEORETICAL APPROACHES A number of theoretical methodologies, spanning from high-level ab initio to empirical calculations have been applied to obtain information on the factors that influence the reactivity of Si w H bond towards radicals and atoms. High-level computational methods are limited, for obvious reasons, to very simple systems. In the previous section we showed the contribution of the theory for a better understanding of the entropic and enthalpic factors that influence the reactions of hydrogen atom with the simplest series of silanes Me4 nSiHn, where n ¼ 1–3. Calculated energy barriers for the forward and reverse hydrogen atom abstraction reactions of Me:, Et:, i-Pr: and t-Bu: radicals with Me4-nSiHn, where n ¼ 0–3, and (H3Si) 3SiH have been obtained at Table 3.7 The substituent effect on the reactivity of silanes towards H: atoms a (in parenthesis theoretical data) b Silane n(Si w H bonds) kn 1 =10 7 M 1 s 1c An 1 =10 10 M 1 s 1 Ea=kJ mol 1 MeSiH3 3 7.8 (7.7) 1.7 (1.5) 13.2 (13.4) Me2SiH2 2 11.9 (11.4) 2.4 (2.1) 13.2 (13.1) Me3SiH 1 16.7 (15.4) 2.0 (3.0) 11.7 (13.2) a From [36]. b ** Using saddle-point structure at the BHLYP/6-311þG level and single-point ab initio at the PMP4/6- 311þG(3df,2p)//BHLYP level [37]. c At 25 8C.
46 Hydrogen Donor Abilities of Silicon Hydrides level of theory as high as QCISD/DZP//MP2/DZP [39]. Transition states in these reactions were found to prefer a collinear arrangement of groups at the hydrogen atom undergoing transfer. These barriers are calculated to decrease, on moving from methyl to primary, secondary and tertiary alkyl radicals, in agreement with the available experimental observations, but their absolute values are overestimated. A nonparametric method that is related to the original London equation has been used to calculate energies of activation for hydrogen abstraction, which agrees with experiment generally to within 4 kJ/mol [40,41]. Indeed, the activation energies calculated for the hydrogen abstraction from Me3SiH and (Me3Si) 3SiH by CH3CH2: and from Me3SiH by CH3O: are 36.8, 22.6 and 10.5 kJ/mol, respectively, and compare very nicely with the experimental values of 33.5, 18.8 and 8.9 kJ/mol reported in this chapter [40]. In addition to the reaction enthalpy, this method demonstrates the importance of triplet repulsion between the terminal atoms of the reacting three-electron system. An empirical algorithm that relates the activation energy to four molecules involved in the reaction (an extended form of Evans–Polanyi equation) predicts activation energies with a good accuracy [42]. The Ea for the reactions of t-BuO: and Cl3C: radicals with Et3SiH are calculated to be 12.6 and 33.9 kJ/ mol, respectively, that match well with the values of 8.8 and 33.9 kJ/mol reported in this chapter. Activation energies for the reaction of a large variety of silanes with different type of radicals have been obtained by applying a semiempirical method using intersecting parabolas [22,43]. 3.8 REFERENCES 1. Chatgilialoglu, C., and Newcomb, M., Adv. Organomet. Chem., 1999, 44, 67. 2. Griller, D., and Ingold, K.U., Acc. Chem. Res., 1980, 13, 317. 3. Newcomb, M., Tetrahedron, 1993, 49, 1151. 4. Newcomb, M. In Radicals in Organic Synthesis, P. Renaud and M.P. Sibi (Eds), Vol. 1, Wiley-VCH, Weinheim, 2001, pp. 317–336. 5. Chatgilialoglu, C., Ferreri, C., and Lucarini, M., J. Org. Chem., 1993, 58, 249. 6. Ballestri, M., Chatgilialoglu, C., Guerra, M., Guerrini, A., Lucarini, M., and Seconi, G., J. Chem. Soc., Perkin Trans. 2, 1993, 421. 7. Oba, M., Kawahara, Y., Yamada, R., Mizuta, H., and Nishiyama, K., J. Chem. Soc., Perkin Trans. 2, 1996, 1843. 8. Chatgilialoglu, C., Timokhin, V.I., and Ballestri, M., J. Org. Chem., 1998, 63, 1327. 9. Chatgilialoglu, C., Guerrini, A., and Lucarini, M., J. Org. Chem., 1992, 57, 3405. 10. Chatgilialoglu, C., Dickhaut, J., and Giese, B., J. Org. Chem., 1991, 56, 6399. 11. Curran, D.P., Xu, J., and Lazzarini, E., J. Chem. Soc., Perkin Trans. 1, 1995, 3046. 12. Chatgilialoglu, C., Altieri, A., and Fischer, H., J. Am. Chem. Soc., 2002, 124, 12816. 13. Chatgilialoglu, C., Ferreri, C., Guerra, M., Timokhin, V., Froudakis, G., and Gimisis, T., J. Am. Chem. Soc., 2002, 124, 10765. 14. Newcomb, M., and Park, S. U., J. Am. Chem. Soc., 1986, 108, 4132. 15. Chatgilialoglu, C., Ferreri, C., Lucarini, M., Pedrielli, P., and Pedulli, G.F., Organometallics, 1995, 14, 2672.
- Page 1 and 2: Organosilanes in Radical Chemistry
- Page 3 and 4: DEDICATION To my parents XrZstoB an
- Page 5 and 6: viii Contents 3.6 Hydrogen Atom: An
- Page 7 and 8: PREFACE A large number of papers de
- Page 9 and 10: ACKNOWLEDGEMENTS I thank Keith U. I
- Page 11 and 12: 2 Formation and Structures of Silyl
- Page 13 and 14: 4 Formation and Structures of Silyl
- Page 15 and 16: 6 Formation and Structures of Silyl
- Page 17 and 18: 8 Formation and Structures of Silyl
- Page 19 and 20: 10 Formation and Structures of Sily
- Page 21 and 22: 12 Formation and Structures of Sily
- Page 23 and 24: 14 Formation and Structures of Sily
- Page 25 and 26: 16 Formation and Structures of Sily
- Page 27 and 28: 2 Thermochemistry 2.1 GENERAL CONSI
- Page 29 and 30: Bond Dissociation Enthalpies 21 Tab
- Page 31 and 32: Bond Dissociation Enthalpies 23 2.2
- Page 33 and 34: Ion Thermochemistry 25 Table 2.4 Re
- Page 35 and 36: Ion Thermochemistry 27 Table 2.5 El
- Page 37 and 38: References 29 3. Goumri, A., Yuan,
- Page 39 and 40: 32 Hydrogen Donor Abilities of Sili
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- Page 57 and 58: General Aspects of Radical Chain Re
- Page 59 and 60: Tris(trimethylsilyl)silane 53 Therm
- Page 61 and 62: Tris(trimethylsilyl)silane 55 4.3.1
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- Page 77 and 78: Other Silicon Hydrides 71 The reduc
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Theoretical Approaches 45<br />
studies <strong>in</strong> the gas phase and a number <strong>of</strong> theoretical <strong>in</strong>vestigations. For<br />
attack<strong>in</strong>g species such as H, Cl and Br atoms, the room temperature rate<br />
constant corrected for reaction path degeneracy, k/n, is higher for Me3SiH<br />
than H4Si by a factor <strong>of</strong> around 4 [36]. However, the <strong>in</strong>terplay <strong>of</strong> activation<br />
energy and preexponential factor is complex and is not fully understood. The<br />
reaction <strong>of</strong> H: atoms is reported <strong>in</strong> Table 3.7 <strong>in</strong> detail, for a better understand<strong>in</strong>g<br />
<strong>of</strong> the reactivity trend <strong>in</strong> this case [36]. <strong>In</strong>deed, the methyl substitution leads<br />
to an <strong>in</strong>crease <strong>in</strong> the Si w H bond reactivity when the statistical number <strong>of</strong><br />
abstracted hydrogens is taken <strong>in</strong>to account. Theory reproduced very well the<br />
experimental rate constants at 25 8C (values <strong>in</strong> parenthesis) [37]. However, the<br />
experimental activation energies and A factors are difficult to rationalize because<br />
the changes are small and may be also masked by experimental errors.<br />
Theoretical calculations suggest that the activation energies for the three reactions<br />
are nearly the same (i.e., unaffected by methylation), whereas the <strong>in</strong>crease<br />
<strong>of</strong> reactivity along the series reflects a parallel change <strong>in</strong> the preexponential<br />
factors. The <strong>in</strong>crease <strong>in</strong> A factor with methylation has been expla<strong>in</strong>ed <strong>in</strong> terms<br />
<strong>of</strong> an <strong>in</strong>crease <strong>in</strong> the entropy <strong>of</strong> the transition state associated either with the<br />
<strong>in</strong>troduction <strong>of</strong> s<strong>of</strong>t skeletal vibrations, or the free<strong>in</strong>g <strong>of</strong> the h<strong>in</strong>dered <strong>in</strong>ternal<br />
rotation <strong>of</strong> the methyl groups [38].<br />
3.7 THEORETICAL APPROACHES<br />
A number <strong>of</strong> theoretical methodologies, spann<strong>in</strong>g from high-level ab <strong>in</strong>itio to<br />
empirical calculations have been applied to obta<strong>in</strong> <strong>in</strong>formation on the factors<br />
that <strong>in</strong>fluence the reactivity <strong>of</strong> Si w H bond towards radicals and atoms.<br />
High-level computational methods are limited, for obvious reasons, to very<br />
simple systems. <strong>In</strong> the previous section we showed the contribution <strong>of</strong> the<br />
theory for a better understand<strong>in</strong>g <strong>of</strong> the entropic and enthalpic factors that<br />
<strong>in</strong>fluence the reactions <strong>of</strong> hydrogen atom with the simplest series <strong>of</strong> silanes<br />
Me4 nSiHn, where n ¼ 1–3. Calculated energy barriers for the forward and<br />
reverse hydrogen atom abstraction reactions <strong>of</strong> Me:, Et:, i-Pr: and t-Bu:<br />
radicals with Me4-nSiHn, where n ¼ 0–3, and (H3Si) 3SiH have been obta<strong>in</strong>ed at<br />
Table 3.7 The substituent effect on the reactivity <strong>of</strong> silanes towards H: atoms a (<strong>in</strong><br />
parenthesis theoretical data) b<br />
Silane n(Si w H bonds) kn 1 =10 7 M 1 s 1c An 1 =10 10 M 1 s 1 Ea=kJ mol 1<br />
MeSiH3 3 7.8 (7.7) 1.7 (1.5) 13.2 (13.4)<br />
Me2SiH2 2 11.9 (11.4) 2.4 (2.1) 13.2 (13.1)<br />
Me3SiH 1 16.7 (15.4) 2.0 (3.0) 11.7 (13.2)<br />
a<br />
From [36].<br />
b **<br />
Us<strong>in</strong>g saddle-po<strong>in</strong>t structure at the BHLYP/6-311þG level and s<strong>in</strong>gle-po<strong>in</strong>t ab <strong>in</strong>itio at the PMP4/6-<br />
311þG(3df,2p)//BHLYP level [37].<br />
c<br />
At 25 8C.