Basic Concepts of Chemical Bonding

	8.1	Determine the number of valence electrons for any atom, and write its Lewis symbol.
	8.2	Recognize when the octet rule applies to the arrangement of electrons in the valence shell for an atom.
	8.3	Describe the origin of the energy terms that lead to stabilization of ionic lattices.
	8.4	Predict on the basis of the periodic table the probable formulas of ionic substances formed between common metals and nonmetals.
	8.5	Describe how the radii of ions relate to those of atoms.
	8.6	Explain the concept of an isoelectronic series and the origin of changes in atomic radius within such a series.
	8.7	Describe the general differences in physical properties between substances with ionic bonds and those with covalent bonds.
	8.8	Describe the basis Lewis theory, and predict the valence of common nonmetallic elements from their position in the periodic table.
	8.9	Explain the significance of electronegativity and in a general way relate the electronegativity of an element to its position in the periodic table.
	8.10	Predict the relative polarities of bonds using either the periodic table or electronegativity values.
	8.11	Write the Lewis structure for molecules and ions containing covalent bonds, using the periodic table.
	8.12	Write the resonance forms for molecules or polyatomic ions that are not adequately described by a single Lewis structure.
	8.13	You should be able to write the Lewis structure for molecules and ions containing covalent bonds that have an odd number of electrons, a deficiency of electrons, or an expanded octet.
	8.14	Relate bond enthalpies to bond strengths and use bond enthalpies to estimate delta H for reactions.
	8.15	Assign oxidation numbers to atoms in molecules and ions
	8.16	Assign acceptable names to simple inorganic compounds and ions

You are responsiblefor all material discussed in Lecture and all material
contained in the text (unless otherwise indicated) whether or not it apperas here.

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