Study Guide: Chemical Bonding
Vocabulary
Bond Energy
Chemical Bond
Chemical Formula
Covalent Bonding
Ductility
Electron Dot Notation
Formula Unit
Hybrid Orbitals
Hybridization
Ionic Bonding
Ionic Compound
Lattice Energy
Lewis Structure
Malleability
Metallic Bonding
Molecular Compound
Molecule
Multiple Bond
Nonpolar Covalent Bond
Nonpolar Molecule
Polar Covalent Bond
Polar Molecule
Polyatomic ion
Resonance
Single Bond
VSEPR theory
1. When drawing Lewis structures, which atom is usually in the central atom? What are the
exceptions?
2. Distinguish between single, double, and triple covalent bonds. Give an example of each.
3. In writing Lewis structures, how is the need for multiple bonds generally determined?
4. What is lattice energy?
5. What is the relationship between lattice energy and ionic strength of ionic bonding?
6. What properties of metals contribute to their tendency to form metallic bonds?
7. How is VSEPR theory used to classify molecules?
8. Draw a Lewis structure for O, C, S, and Al.
9. Why do atoms of elements chemical bond?
10. What types of atoms will form the following types of bond? (ionic, covalent , and metallic)
Review textbook pages in Chapter 6 pp. 175- 203 (top of page). Look over Chapter summaries on
page 208. Review lab, video questions, Pogils, notes, activities, and practice problems.
Be able to write electron dot notations, molecular geometry, and shape identity. Also, be able
to determine type of bonds and molecules represented in various compounds.
Remember this is just a guide! We have practiced, read, discussed, and covered all concepts on
test in a variety of ways in and out of class.