MIT OpenCourseWare
http://ocw.mit.edu
5.111 Principles of Chemical Science
Fall
2008
For information about citing these materials or our Terms of Use, visit:
http://ocw.mit.edu/terms
.
This
preview
has intentionally blurred sections.
Sign up to view the full version.
1
_______________________________________________________________________________
________________________________________________________________________________
5.111 Lecture Summary #14
Readings for today:
Section 3.8 (3.9 in
3
rd
ed
) – The Limitations of Lewis’s Theory,
Section 3.9 (3.10 in
3
rd
ed
) – Molecular Orbitals, Section 3.10 (3.11 in
3
rd
ed
) – The
Electron Configuration of Diatomic Molecules, Section 3.11 (3.12 in
3
rd
ed
) –
Bonding in Heteronuclear Diatomic Molecules.
Read for Lecture #15:
Sections 3.4, 3.5, 3.6 and 3.7 (Sections 3.4, 3.5, 3.6, 3.7, and 3.8 in
3
rd
ed
) – Valence Bond Theory.
Topics:
Molecular orbital theory
I.
Bonding and antibonding orbitals
II.
Homonuclear diatomic molecules
A.
Molecules with MO’s originating from s orbitals
B.
Molecules with MO’s originating from s and p orbitals
III.
Heteronuclear diatomic molecules
MOLECULAR ORBITAL (MO) THEORY
In MO theory, valence electrons are _________________ over the entire molecule, not
confined to individual atoms or bonds, as in Lewis and valence-bond models.
I. BONDING AND ANTIBONDING ORBITALS
Molecular orbitals (____________________) of diatomic molecules arise from adding
together (
superimposing
) atomic orbitals:
linear combination of atomic orbitals (LCAO) to create a molecular orbital.
This is the end of the preview.
Sign up
to
access the rest of the document.
- Spring '03
- RogerD.Kamm
- Atom, Electron, Chemical bond
-
Click to edit the document details
