This is sort of a list of questions that pertain to one subject in general:
I've noticed that molecular orbital theory relies less on the concept of hybridization than valence bond theory. A note on page 122 of the textbook mentioned that "molecular orbitals are built from all the available [i]unhybridized[i] atomic orbitals by noting whether or not they have the right shape to overlap with one another". Why is it that in most of our examples in class, the atomic orbitals were considered unhybridized when we were using molecular orbital theory to describe the bonds when they would otherwise be considered hybridized when we were using valence bond theory? And also, what does the last part of the quote mean when it says "whether or not they have the right shape"?
In one of the review sessions, the TA pointed out that it is possible for hybridized atomic orbitals to take part in a molecular orbital diagram. If this is so, then how does one know whether the atomic orbitals should be hybridized or not? And will we be asked to draw molecular orbital diagrams for such complicated structures with hybridized atomic orbitals?
Molecular Orbitals and Hybridization
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Re: Molecular Orbitals and Hybridization
Postby Chem_Mod » Tue Nov 19, 2013 8:09 pm
As discussed in class molecular orbital theory is uses a linear combination of atomic orbitals.
Molecular orbital theory does not use hybridized orbitals.
The last part of the textbook quote is referring to the mathematical process of the linear combination of all atomic orbitals.
Molecular orbital theory does not use hybridized orbitals.
The last part of the textbook quote is referring to the mathematical process of the linear combination of all atomic orbitals.
Return to “*Molecular Orbital Theory (Bond Order, Diamagnetism, Paramagnetism)”
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