Chapter 10 Chemical Bonding II:

Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory

10.1 Artificial Sweeteners: Fooled by Molecular Shape

10.2 VSEPR Theory: The Five Basic Shapes

Two Electron Groups: Linear Geometry

Three Electron Groups: Trigonal Planar Geometry

Four Electron Groups: Tetrahedral Geometry

Five Electron Groups: Trigonal Bipyramidal Geometry

Six Electron Groups: Octahedral Geometry

10.3 VSEPR Theory: The Effect of Lone Pairs

Four Electron Groups with Lone Pairs

Five Electron Groups with Lone Pairs

Six Electron Groups with Lone Pairs

10.4 VSEPR Theory: Predicting Molecular Geometries

Representing Molecular Geometries on Paper

Predicting the Shapes of Larger Molecules

10.5 Molecular Shape and Polarity

Vector Addition

Chemistry in Your Day: How Soap Works

10.6 Valence Bond Theory: Orbital Overlap as a Chemical Bond

10.7 Valence Bond Theory: Hybridization of Atomic Orbitals

sp[Sup(3)] Hybridization

sp[Sup(2)] Hybridization and Double Bonds

Chemistry in Your Day: The Chemistry of Vision

sp Hybridization and Triple Bonds

sp[Sup(3)]d and sp[Sup(3)]d[Sup(2)] Hybridization

Writing Hybridization and Bonding Schemes

10.8 Molecular Orbital Theory: Electron Delocalization

Linear Combination of Atomic Orbitals (LCAOs)

Period Two Homonuclear Diatomic Molecules

Second-Period Heteronuclear Diatomic Molecules

Polyatomic Molecules

CHAPTER IN REVIEW: Self-Assessment Quiz

Key Terms

Key Concepts

Key Equations and Relationships

Key Learning Outcomes

EXERCISES: Review Questions

Problems by Topic

Cumulative Problems

Challenge Problems

Conceptual Problems

Questions for Group Work

Data Interpretation and Analysis

Answers to Conceptual Connections