This study guide contains over 3 hours of recorded lecture topics and example problems that follow the material covered in chapter 9 of the textbook Chemistry, The Molecular Nature of Matter and Change by Silberberg. The topics covered include: The differences in atomic properties that lead to each of the basic types of bonding. The key features of ionic bonding: electron transfer to form ions and their electrostatic attraction to form an ionic solid. The reasons that lattice energy is responsible for the stability of solid ionic compounds. Ionic compound formation in hypothetical steps (Born-Haber cycle) and how they can be used to calculate lattice energies. How Coulomb’s law accounts for periodic trends in lattice energy. Why ionic compounds are brittle and high melting and conduct electricity only when molten or in aqueous solution. Covalent bonding model: nonmetal atoms share electrons to form a covalent bond. The octet rule: bonding and lone electron pairs fill the valence levels of each atom in a molecule. How covalent bond order, bond length, and bond energy are related. Consideration of bonding and nonbonding forces explains the properties of covalent molecules and network covalent solids. How bond energy differences can account for the heat of reaction; dividing a reaction into bond- breaking and bond-forming steps predicts ΔH of reaction. Electronegativity, its periodic trends and the inverse relationship between EN values and atomic sizes. Predicting bond polarity from differences in the electronegativity of bonded atoms; the direction of bond polarity. Variation of partial ionic character with ΔEN and the change in bonding from ionic to polar covalent to nonpolar covalent across a period. The crucial role of delocalized electrons in metallic bonding. How the sea-of-electrons model explains why metals bend, have very high boiling points, and conduct electricity in solid or liquid form.
