- Principles of Chemistry I: Honors
Fall 2012, Unique 51390
Lecture Summary, 23 October 2012
We are now going to use our atomic orbitals to form
orbitals, which will provide the mechanism of keeping stable
density between two nuclei, which will in turn lower the potential
energy of the system and form a molecular bond. The
that we are going to use to do this is called "linear combination
atomic orbitals to molecular orbitals," LCAO-MO. Our
system will be defined with the internuclear axis lying along the
z-axis. From that simple definition, we spent a lot of time
drawing the structure of s and p orbitals of same and opposite
and figuring out what the resulting structure would look like.
These are also drawn in your book, and you should spend some
getting comfortable with these images.
We also reviewed the naming convention for these orbitals. For each orbital, we need to ask 3 questions about the orbitals shape and phase:
1) Does the MO have cylindrical symmetry around the internuclear (z) axis?
2) Is the MO symmetric with respect to inversion?
yes: g (for "gerade" (even))
no: u (for "ungerade" (uneven))
3) Is there a nodal plane perpendicular to the internuclear (z) axis in the center of the molecule?