Chapter 10
Recommended Problems: Brown-Box problems and suggested further problems in the back. Selection of
further problems in back of Chapter as good options. Brown box problems would be a very good start,
including the further suggeseted problems. VERY IMPORTANT: Lewis structures from Lab Exercises (note
that the full answers have been provided, along with geometries, via E-mail attachment sent on or about 7
April-Check FerrisConnect) . Brown-Box problems and further suggested problems. Try also 10.33, 37 41,45,
47,53,57,69,65.
10.1 VSEPR See also lab exercises/notes , handout and the key sent out on or about 7
April
Isomer: page 374 (one type)
This is a large
and important
topic which
builds on and
works with lewis
Strcutures.
Aspects of VSEPR
Lewis structure, Molecular (or special) geometry as derived from the
electronic geometry (= electron “arrangement”) by ignoring lone pairs.
Tip: start with the electronic geometry and see what molecular geometry
results from eliminating zero, 1,2 3, etc. lone pairs of electrons.
Know bond angles and how these may be distorted by lone pairs (vs shared
pairs).
10.2 Dipole Moment
and molecular
geometry
What is dipole moment? How is this related to polarity of covalent bonds?
How is it represented? (partial charge deltas or the arrows)
What is the difference between a bond dipole moment and the [possible]
net dipole moment for a molecule? What molecules have bond dipoles but
no net dipole?
Given a shape (molecular, electronic) or a Lewis structure, which ones
have dipole moments.
From a knowledge of electronegativity trends, rank bonds for polarity (=
dipole moment)
10.3
10.4
Valence Bond
Theory
VB for multiple
bonds.
Molecular
orbital theory
not asked on
this exam
Use orbital diagrams to VB arrangements (pairing up electrons), bond
hybridization by mixing orbitals, and resulting electronic and molecular
geometries. Combinations of s,p, d orbitals would be used.
For multiple bonding, construct pictures of molecules using sigma and pi
bonding (How do sigma and pi bonds differ?)
Orbital diagrams are used to start this process (promotion, of electrons,
mixing of orbitals, resulting of hybridized orbitals and geometry). Pictures of
pi and sigma orbitals in molecules; single double triple bonds. See examples
from class in text as models for others. Ends, pae 399. Note isomers.
