1. Ionic Bonding Table of Contents Lecture/Lab/Activity Date Pg# 22. The Periodic Table9/24/10 47 23. Periodic Def & Trends9/27/10 49 24. Electron config practice10/4/10 51 25. Ions and Oxidation Numbers10/5/10 53 26. Lewis Dot Diagram10/6/10 54 27. Intro to Chemical Bonding10/7/10 57 28. Covalent Bonding10/12/10 61 29. Ionic Bonding 10/14/10 61 Objective: The student will construct Lewis dot diagrams to illustrate ionic bonds and discuss their properties during lecture. Agenda: Ionic Bonding– Lecture Covalent & Ionic Bonding - Homework

2. Ionic bonds are characterized as: - bonds between metals & non-metals - bonds between cations & anions - bonds involving a transfer of e - (from a metal to a nonmetal)

3. Ionic compounds form crystalline lattice structures which are very strong. High Melting Point Ex. Melting point for NaCl is 800°C

4. NaCl + Na + Cl - + Remember!!! [Ne]3s 1 [Ne]3s 2 3p 5 [Ne][Ne]3s 2 3p 6 Na ClNa + Cl - Anions have larger atomic radii Cations have smaller atomic radii Starting Valence e - = 8 Final Valence e - = 8 End Total Charge = 0 Starting Total Charge = 0

5. When ionic compounds dissolve into solution, their + and – ions separate (electrolyte). H 2 O surrounds ions in solution to prevent cations & anions from recombining (solvation) += Na + (aq) - = Cl - (aq)

6. Good electrolytes, like many ionic compounds are good conductors of electricity. Electrolysis

7. How do ionic compounds with subscripts form? Ex. How does MgCl 2 form? Mg Cl Mg Cl - - 2+

8. Diagram the formation of the ionic compound AlF 3 ! Al F F - FF 3+ F - F -

9. Find the balanced ionic formula for Calcium & Bromine. Ca oxidation # = Br oxidation # = +2 We need a 2 nd Br atom to balance the net charge! CaBr 2 Ca Br Ca 2+ Br - -