1. Chemistry 12/1/14

2.  Fill out Valence Electron Practice on the notes sheet.  HW: ◦ Finish pg. 1, Bonding Practice ◦ pg. 3 #15-22

3.  IWBAT ◦ Create and name a structure for ionic compounds

4.  Drill  Ionic Bonding Notes  Ionic Bonding Practice  Closure

5.  Paired valence electrons ◦ Relatively stable ◦ Resistant to change ◦ Don’t form chemical bonds ◦ Called non- bonding pairs or lone pairs.  Unpaired valence electrons ◦ Have a strong tendency to participate in chemical bonding

6.  Atoms gain or lose valence electrons until the valence shell is filled or empty;  Since valence shells are made of “s” and “p” sublevels, they can hold a maximum of 8 electrons (or 2 electrons for the 1 st energy level)

7.  occurs when the less electronegative element (metal) transfers one or more valence electrons to the more electronegative element (nonmetal)  the metal loses electrons to become a cation (a positively charged ion) while the nonmetal gains an electron to become an anion ( a negatively charged ion)

8.  Transfer of valence electrons  Formed by a Metal & Nonmetal ion ◦ ex. NaCl  The smallest unit of the compound is a formula unit.

9.  Properties of ionic compounds: ◦ Crystalline solids at room temperature ◦ Conduct electric current in molten state, but not solid state (ions not free to move) ◦ High melting and boiling points ◦ Usually water-soluble. Mobile ions in solution conduct electricity -- electrolytes

10.  Use Lewis Structures to show ionic bonding: ◦ Ms. Bloedorn will demonstrate with pg. 1 – Bonding Practice  The charge of any compound MUST be ZERO!!  Criss-Cross Basics ◦ Cross the numbers and drop the charges ◦ Don’t write “1” ◦ Reduce the ratio – 2:2  1:1, 2:4  1:2  Naming basics – Name the CATION, then ANION

11.  Mg and F form a compound. ◦ What is the formula? ◦ Draw the Lewis structure. ◦ Name it!