I suspect the CO2 LG takes the bonding electrons with it, such that you get a carbocation ( or a carbocation-like transition state ? )-- would that explain why longer-chain COOH's are easier to decarboxylate?
32.
The equations for bonding electrons in multi-electron atoms could not be solved to mathematical perfection ( i . e ., " analytically " ), but approximations for them still gave many good qualitative predictions and results.
33.
The FeH molecule has at least four low energy electronic states caused by the non bonding electron taking up positions in different orbitals : X 4 ?, a 6 ? b 6 ?, and c 6 ? +.
34.
In an SN2 reaction, the positive charge on the SAM sulfur atom pulls the bonding electron from the carbon of the methyl group, which interacts with the arsenic lone pair to form an As " C bond, leaving SAH.
35.
The surface was generated by calculating the energy of interaction of a spherical point positive charge ( e . g ., a proton, H +, ) with the molecule's atoms and bonding electrons, in a series of discrete computational steps.
36.
So in fact, before that carbon converts to sp3, it's like the alkoxy oxygen's lone pair is participating in the pi system and pushing the existing bonding electrons away . ( Okay this might be an unacceptable classical picture though .)
37.
The bond valence is thus equal to three different quantities : the number of electrons each atom contributes to the bond, the number of electron pairs that form the bond, and the electrostatic flux linking each core to the bonding electron pair.
38.
Both the shortened length of the N-C bond and the longer Se = C bond suggest a delocalization of the lone pair on the amines; the Se = C ?-bonding electrons are drawn towards the Se atom, while the N-lone pair is drawn towards the carbonyl carbon.
39.
Good reducing agents tend to consist of atoms with a low electronegativity, the ability of an atom or molecule to attract bonding electrons, and species with relatively small ionization energies serve as good reducing agents too . " The measure of a material to oxidize or lose electrons is known as its oxidation potential ".
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