1. Conductivity & Chemical Bonding Objective Measure the conductivity of compounds in aqueous solutions. Date: Chemical Background Aqueous (aq) – solution with water as the solvent. Electrolyte – solution that conducts electric current. When an ionic solid dissolves in water, the solid dissociates (splits) into cations & anions. NaCl (aq)  Na + + Cl -

2. Experiment Set up a conductivity circuit as shown. Dissolve a small scoop of each solid in distilled water. Wipe dish and test leads clean for each new solution. Discard all solutions in the drain except the last 2.

3. Solution Formula Conductivity (Strong, Weak, Non) Pure Water Tap Water Sodium Chloride (aq)NaCl Potassium Chloride (aq)KCl Sugar (aq)C 12 H 22 O 11 Epsom Salt (aq)MgSO 4 Urea (aq)CH 4 N 2 O EthanolC 2 H 5 OH VinegarCH 3 COOH

4. Analysis 1.Which substances are most likely to possess ionic bonds? 2.If a certain amount of NaCl was dissolved in water, how would the number of Na + ions compare to the number of Cl - ions? Results Questions 

5. Questions 1.Does this experiment give qualitative or quantitative conductivity results? 2.Explain why some of the solids conduct current when they are dissolved in water. 3.Why was it important to dissolve the solids in distilled water rather than tap water? 4.Pure water is not an electrical conductor. So why should we be careful with electricity around water at home?