1. Disassociation What does it mean in Chemistry?

2. Water is a Polar Molecule O HH + - + Opposite Charges Attract ( + and - ) Like Charges Repel ( + and + or - and - )

3. Bending Water

4. H 2 0 Translates: In a liquid particles flow, slide past one another and rotate

5. Bending Water

6. ELECTOSTATIC FORCE Na + Cl -

7. ELECTOSTATIC FORCE Na + Cl -

8. ELECTOSTATIC FORCE Na + Cl -

9. SALT IN WATER? Na + Cl -

10. SALT IN WATER? Na + Cl -

11. DISASSOCIATION Na + Cl - The separation of molecules or ionic compounds (cations and anions) into smaller parts. This usually happens when ionic compounds are placed in H 2 0 When salt is put in water the water molecules pull apart the sodium and chloride ions.

12. DISASSOCIATION Na + Cl - The separation of cations and anions when the ionic compound is placed in water. When salt is put in water the water molecules pull apart the sodium and chloride ions.

13. DISASSOCIATION The negative side of water (oxygen) surrounds and” traps” the positive Sodium cation and the positive end of water (hydrogen) “traps” the negative Chloride anion.

14. DISASSOCIATION NaCl (s) + H 2 0  Na + (aq) +Cl - (aq) If a solute (salt) is dissolving in water (solvent) then it is called an aqueous solution.

15. Assignment NaCl (s) + H 2 0  Na + (aq) +Cl - (aq) That is what happens when table salt is placed in water. [1] Write the equation for Lithium Fluoride if it was placed in water. [2] Write the equation for Barium Chloride if it was placed in water.

16. Solubility Soluble Salts 1. The Na +, K +, and NH 4 + ions form soluble salts. Thus, NaCl, KNO 3, (NH 4 ) 2 SO 4, Na 2 S, and (NH 4 ) 2 CO 3 are soluble. 2. The nitrate (NO 3 - ) ion forms soluble salts. Thus, Cu(NO 3 ) 2 and Fe(NO 3 ) 3 are soluble. 3. The chloride (Cl - ), bromide (Br - ), and iodide (I - ) ions generally form soluble salts. Exceptions to this rule include salts of the Pb 2+, Hg 2 2+, Ag +, and Cu + ions. ZnCl 2 is soluble, but CuBr is not. 4. The sulfate (SO 4 2- ) ion generally forms soluble salts. Exceptions include BaSO 4, SrSO 4, and PbSO 4, which are insoluble, and Ag 2 SO 4, CaSO 4, and Hg 2 SO 4, which are slightly soluble. Insoluble Salts 1. Sulfides (S 2- ) are usually insoluble. Exceptions include Na 2 S, K 2 S, (NH 4 ) 2 S, MgS, CaS, SrS, and BaS. 2. Oxides (O 2- ) are usually insoluble. Exceptions include Na 2 O, K 2 O, SrO, and BaO, which are soluble, and CaO, which is slightly soluble. 3. Hydroxides (OH - ) are usually insoluble. Exceptions include NaOH, KOH, Sr(OH) 2, and Ba(OH) 2, which are soluble, and Ca(OH) 2, which is slightly soluble. 4. Chromates (CrO 4 2- ) are usually insoluble. Exceptions include Na 2 CrO 4, K 2 CrO 4, (NH 4 ) 2 CrO 4, and MgCrO 4. 5. Phosphates (PO 4 3- ) and carbonates (CO 3 2- ) are usually insoluble. Exceptions include salts of the Na +, K +, and NH 4 + ions.