Chapter 6 Molecular Structure & Bonding
orbitals must first be mixed in a process calle
d hybridization. The r
esulting hybrid orbitals
are used to form the
bonds and hold the lone pairs. The hyσ
bridization of an atom is used
to describe both the bonding and structure around the atom because hybrid orbitals have the geometries required by VSEPR. The orbitals
that are not used to construct the hybrid
orbitals are used to form
bonds. π
In molecular orbital theory, electrons occupy
molecular orbitals just as the electrons in
an atom occupy atomic orbitals. The molecula
r orbitals are constructed by combining the
atomic orbitals of different atoms. Unli
ke the bonds produced in valence bond theory,
molecular orbitals can be delocalized over several atoms, which explains the observations that valence bond theory invokes resonance to explain.
After studying the material presented in this chapter, you should be able to: 1. predict molecular and ionic shapes based on VSEPR theory (Section 6.1); 2. determine whether an atom obeys the octet ru
le or uses an expanded octet (Section 6.2);
- predict the shapes of molecules and ions wi
th atoms using expanded octets (Section 6.2);
- visualize the three-dimensional arrangem
ent of atoms around a central atom in a
complicated molecule (Section 6.3);
- represent the overlap of tw
o atomic orbitals qualitatively with a drawing (Section 6.4);
- define and identify
andσ
π
bonds (Sections 6.4 and 6.5);
- draw the
and σ
components of a multiple bond (Section 6.4); π
- determine an atom’s hybridization, draw pictures of hybrid orbitals, and account for
molecular shapes based on hybridization (Section 6.4);
- construct molecular orbitals of simple syst
ems and explain resonance in terms of molecular
orbitals (Section 6.5);
10.
determine whether an MO is bonding, antibonding, or nonbonding (Section 6.5); and
11.
identify the HOMO and LUMO for a molecule given its MO diagram and the number of electrons that go in it (Section 6.5).
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