Journal
CHEMISTRY-A EUROPEAN JOURNAL
Volume 14, Issue 23, Pages 6901-6911Publisher
WILEY-V C H VERLAG GMBH
DOI: 10.1002/chem.200800013
Keywords
bond theory; carbon; density functional calculations; hypervalent compounds; noble gases
Categories
Funding
- Netherlands Organization of Scientific Research (NWO-CW)
- A Marie Curie fellowship
- Department d'Universitats
- Receerca i Societat de la Informacio (DURSI) of the Generalitat de Catalunya [2004BE00028]
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Silicon in [Cl-SiH3-Cl] is hypervalent, whereas carbon in [Cl-CH3-Cl] is not. We have recently shown how this can be understood in terms of the ball-in-a-box model. according to which silicon fits perfectly into the box that is constituted by the five substituents, whereas carbon is too small and, in a sense, drops to the bottom of the box. But how does carbon acquire hypervalency in the isostructural and isoelectronic not) le gas (Ng)/methyl cation complexes [Ng-CH3-Ng](+) (Ng = He and Ne), which feature a delocalized D-3-symmetric Structure with two equivalent C-Ng bonds? From Ng=Ar onwards, the [Ng-CH3-Ng](+) complex again acquired a propensity to localize one of its axial C-Ng bonds and to largely break the other one, and this propensity increases ill the order Ng = Ar < Kr < Xe < Rn. The behavior of the helium and neon complexes violates the ball-in-a-box principle. Why does this happen? The purpose of this stuck, is to answer these questions and to understand why carbon can become truly hypervalent under certain conditions. To this end, we have Carefully analyzed the structure and bonding in NgCH(3)Ng(+) and, for comparison. CH(3)Ng(+), NgHNg(+), and NgH(+). It appears that, at variance with [Cl-CH3-Cl](-), the carbon atom in [Ng-CH3-Ng](+) call no longer be considered as a ball in a box of the five substituents.
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