2.  Ionic compounds generally are a non-metal with a metal  e - spend more time around the more electronegative (polyatomic) ion  disproportional sharing of electrons causes a ( + ve) charged ion & ( - ve) charge ion  The ( + ve) & ( - ve) ions form a lattice (a solid structure)

3. Sodium ion Water molecule Chlorine ion

4.  Q: What happens when this gets into water (a polar substance with  + and  - )?  A: The ions are pulled off by the water, with opposite charges attracting

5. Sodium ion Water molecule Chlorine ion

6.  http://www.mhhe.com/physsci/chemistry/es sentialchemistry/flash/molvie1.swf http://www.mhhe.com/physsci/chemistry/es sentialchemistry/flash/molvie1.swf

7.  NaCl (solid) + H 2 O (liquid) NaCl (aqueous)  Is there a simpler method to write this?  Use symbols

8.  NaCl (s) NaCl (aq) Molecular Equation OR NaCl (s) Na + (aq) + Cl - (aq) Ionic Equation H2OH2O H2OH2O

9.  What Occurs if we mix a solution of ◦ Sodium Chloride AND ◦ Silver Nitrate  What do we observe? ◦ The white substance means that a ionic solid has formed that is not dissolved in the water ◦ What is the formula of this solid?  What are the two possibilities? (NaCl) ( AgNO 3 )

10.  Molecular Equation:  NaCl (aq) + AgNO 3(aq) AgCl (s) + NaNO 3(aq)  Ionic Equation:  Na + (aq) + Cl - (aq) + Ag + (aq) + NO 3 - (aq) → AgCl (s) + Na + (aq) + NO 3 - (aq) ◦ What ions exist on both sides of the equation? ◦ These can be cancelled out (Known as spectator ions)  Net Ionic Equation:  Cl - (aq) + Ag + (aq) → AgCl (s) Note: Remember your charges need to be balanced on both sides of the equation!

11.  Why would this solid not dissolve in the water when the ions before were dissolved?  The force of attraction between the two ions (Ag + & Cl - ions) are stronger than the force of attraction between the ions and the polar water molecule

12.  http://www.crescent.edu.sg/crezlab/webpag es/pptreaction4.htm http://www.crescent.edu.sg/crezlab/webpag es/pptreaction4.htm