1. Add to table of contents Rules for Lewis Structures Pg. 40 Lewis Structures-Ionic Pg. 41

2. Lewis Structures: Ionic Bonds

3. 3 Lewis Theory Lewis bonding theory emphasizes the importance of valence electrons. Uses dots to represent valence electrons either on or shared by atoms. Arranges bonding between atoms to attain certain sets of stable valence electron arrangements. G.N. Lewis (1875-1946)

4. 4 Lewis Symbols of Atoms Also known as electron dot symbols. Uses symbol of element to represent nucleus and inner electrons. Uses dots around the symbol to represent valence electrons. – Puts one electron on each side first, then pair. Remember that elements in the same group have the same number of valence electrons; therefore, their Lewis dot symbols will look alike. Li Be B C N O: :F: :Ne:

5. 5 Practice—Write the Lewis Symbol for Arsenic.

6. 9.1

7. - atoms will tend to gain, lose, or share electrons until their outer energy level contains eight electrons (or two like Helium) (Noble Gas e- configuration) -maximum stability

8. + sodium metalchlorine gastable salt

9. 9 Lewis Bonding Theory Atoms bond because it results in a more stable electron configuration. Atoms bond together by either transferring or sharing electrons. Usually this results in all atoms obtaining an outer shell with 8 electrons. – Octet rule. – There are some exceptions to this rule—the key to remember is to try to get an electron configuration like a noble gas. Li and Be try to achieve the He electron arrangement.

10. 10 Lewis Symbols of Ions Cations have Lewis symbols without valence electrons. – Lost in the cation formation. – They now have a full “outer” shell that was the previous second highest energy shell. Anions have Lewis symbols with 8 valence electrons. – Electrons gained in the formation of the anion. Li Li + :F: [:F:] −

11. 11 Ionic Bonds Metal to nonmetal. Metal loses electrons to form cation. Nonmetal gains electrons to form anion. Ionic bond results from + to − attraction. Lewis theory allows us to predict the correct formulas of ionic compounds.

12. 12 Example—Using Lewis Theory to Predict Chemical Formulas of Ionic Compounds Predict the formula of the compound that forms between calcium and chlorine. Draw the Lewis dot symbols of the elements. Ca ∙ ∙ Cl ∙ ∙ ∙ ∙∙ ∙∙ Transfer all the valance electrons from the metal to the nonmetal, adding more of each atom as you go, until all electrons are lost from the metal atoms and all nonmetal atoms have 8 electrons. Ca ∙ ∙ Cl ∙ ∙ ∙ ∙∙ ∙∙ ∙ ∙ ∙ ∙∙ ∙∙ Ca 2+ CaCl 2

13. 13 Practice—Use Lewis Symbols to Predict the Formula of an Ionic Compound Made from Reacting a Metal, Mg, that Has 2 Valence Electrons with a Nonmetal, N, that Has 5 Valence Electrons.

14. 14 Practice—Use Lewis Symbols to Predict the Formula of an Ionic Compound Made from Reacting a Metal, M, that Has 2 Valence Electrons with a Nonmetal, X, that Has 5 Valence Electrons, Continued. Mg 3 N 2