What is our justification when we generally ignore mixing of normal localized bonding orbitals (e.g. σ_CH) with one another? (Consider both molecular energy and electron distribution.)

Why should mixing of normal localized bonding orbitals with certain unshared pairs be somewhat less negligible?

What do you learn about the relative energy of σ_CH, p_F, and p_O, by studying the following orbitals that show OMO-OMO mixing in CH₃F and O=CH₂?

Two CH₃F Orbitals
(left, right pairs are different views of the same orbital, drawn at different contour levels)

Two O=CH₂ Orbitals
(left, right pairs are different views of the same orbital, drawn at different contour levels)

(Do click here to read the answer - AFTER you do the problem)

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copyright 2001 J. M. McBride