In predicting the bond angle of water, Bent s rule suggests that hybrid orbitals with more s character should be directed towards the very electropositive lone pairs, while that leaves orbitals with more p character directed towards the hydrogens.
32.
The hybrid orbital description of the ground state is therefore " equivalent " to the delocalised orbital description for ground state total energy and electron density, as well as the molecular geometry that corresponds to the minimum total energy value.
33.
The hybrid orbital that carbon contributes to the C-F bond will have relatively less electron density in it than in the C-H case and so the energy of that bond will be less dependent on the carbon's hybridisation.
34.
To form five bonds, the one s, three p and one d orbitals combine to form five sp 3 d hybrid orbitals which each share an electron pair with a halogen atom, for a total of 10 shared electrons, two more than the octet rule predicts.
35.
The fractional character of orbital i is \ frac { \ lambda _ i ^ 2 } { 1 + \ lambda _ i ^ 2 }, and the p character of all the hybrid orbitals sums to the number of p orbitals involved in the formation of hybrids:
36.
To construct hybrid s and p orbitals, let the first hybrid orbital be given by p i " } }, where p i is directed towards a bonding group and " & lambda; i " determines the amount of p character this hybrid orbital has.
37.
To construct hybrid s and p orbitals, let the first hybrid orbital be given by p i " } }, where p i is directed towards a bonding group and " & lambda; i " determines the amount of p character this hybrid orbital has.
38.
Bent's rule, that centrals atoms direct orbitals of greater p character towards more electronegative substituents, is easily applicable to the above by noting that an increase in the " & lambda; i " coefficient increases the p character of the p i " } } hybrid orbital.
39.
Despite the fact that two of the electrons are in s-orbitals and the other two in higher-energy p-orbitals, one electron is " promoted " from an s-orbital to a p-orbital, and then all form four intermediate hybrid orbitals in a process called sp 3 hybridization.
40.
This is what I was told at uni, but I was wondering why some sort of hybridisation ( e . g . sp3 ) would not occur . ( This would affect lone pairs and the exact nature of the sigma bond ? ) If this does not involve hybrid orbitals, what determines when this happens?
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