1. Aim: How to distinguish between ionic and covalent bonding? Two major categories of compounds are ionic and molecular (covalent) compounds. Metals tend to react with nonmetals to form ionic compounds. Nonmetals tend to react with other nonmetals to form molecular (covalent) compounds. Ionic compounds containing polyatomic ions have both ionic and covalent bonding.

2. Aim: How to distinguish between ionic and covalent bonding? Vocabulary Electronegativity- the tendency of an atom to attract electrons to itself when it is chemically combined with another element. (“attraction for electrons”) Covalent bond- attraction formed by the sharing of electrons. Usually between non- metals. (“SHARING of e-”) Ionic bond- involves transfer of e- (NOT sharing); IONS are formed. Usually between a metal and a non-metal.

3. Aim: How to distinguish between ionic and covalent bonding? Essential questions: Compare and contrast ionic and covalent bond types. Draw Lewis structures (electron dot diagrams) for atoms, ions and compounds. Determine the noble gas configuration an atom will achieve when bonding. Use the electro negativity difference ( EN) to determine bond type (ionic, polar covalent, or non-polar covalent.)

4. Aim: How to distinguish between ionic and covalent bonding? Regents Preparation Try #’s 1, 4, 5, and 6 Regents Preparation Rules for drawing Lewis structures with many atoms: Hydrogen and halogen atoms often bind to only one other atom (why?) and are usually on the outside or end of molecule. The atom with the lowest electronegativity is often the central atom. When placing valence electrons around an atom, place one electron on each side before pairing any electrons.

5. Aim: How to distinguish between ionic and covalent bonding? How to name covalent compounds? Use prefixes to note the number of each type of atom: mono-, di-, tri-, tetra-, penta-, hexa-, hepta-, octa-, nona-, deca-

6. Aim: How to distinguish between ionic and covalent bonding? VSEPR (valence shell electron pair repulsion) theory- a model that can be used to predict shape of a molecule based on repulsion of both bonding and nonbonding electron pairs. Using this theory explain why carbon dioxide has a linear shape while sulfur dioxide is bent.