9.1. Lewis Electron Dot Structures http://www.ck12.org
9.1 Lewis Electron Dot Structures
Lesson Objectives
- Describe how a covalent bond forms, including the energy change involved in the process.
- Use the octet rule to draw Lewis electron dot structures for simple molecules. Know how and when to
incorporate double and triple bonds into the structures. - Understand how a coordinate covalent bond differs from other covalent bonds.
- Be able to draw Lewis structures for polyatomic ions.
- Understand the concept of resonance.
- Know some common exceptions to the octet rule.
- Relate bond energy to the stability and reactivity of molecules.
Lesson Vocabulary
- bond energy
- coordinate covalent bond
- covalent bond
- diatomic molecule
- double covalent bond
- Lewis electron dot structures
- lone pair
- resonance
- single covalent bond
- structural formula
- triple covalent bond
Check Your Understanding
Recalling Prior Knowledge
- What is a molecule?
- What is shown in an electron dot diagram?
- What are polyatomic ions?
In previous chapters, you have learned about several forms that matter can take. Pure metals exist as extended
three-dimensional structures of close packed metal cations with mobile valence electrons. Ionic compounds are also
crystalline in nature, but with alternating cations and anions held together by attractive electrostatic forces called
ionic bonds. The noble gases are monatomic and exist as individual atoms. In this chapter, you will learn about the
structure and bonding that occurs in molecular compounds.