1. What happens when you put
AgNO3 (aq) + NaCl(aq) AgCl(s) + NaNO3(aq)
What happens when you put
AgNO3 and NaCl in water?

2. NaCl (aq) Na +1 (aq) + Cl -1 (aq) KEY POINT: really means:
“dissociated ions” or
“ions in solution”

3. What is Dissolving ?
When an ionic compound (eg salt) dissolves in water, the compound disassociates. (breaks apart into cations and anions)
Ex: Ca(NO3)2(s) Ca2+(aq) + 2NO3-(aq)
When a covalent compound (eg sugar) dissolves in water, the molecules simply disperse; they do not disassociate. Molecules of the covalent compounds simply disperse due to attraction with polar water molecules.

4. An Ionic Compound Dissolves: A Covalent Compound Dissolves:

5. Mg(NO3)2 (aq) Mg +2 (aq) + (NO3) -1 (aq) 2 KEY POINT: really means:
“dissociated ions” or
“ions in solution”

6. KEY POINT:
AgCl (s)
really means:
Solid Silver (I) Chloride.

7. AgNO3
NaCl

8. NO3-
Na+
Ag+
Cl-

9. Na+
NO3-
Ag+
Cl-

10. Na+
NO3-
AgCl

11. Na+
NO3-
AgCl(s)
precipitate
AgCl

12. NO3- Na+ NO3- NO3- Na+ Na+ Na+ NO3- NO3- Na+ Na+ Na+ NO3- NO3- Na+
AgCl(s)

13. AgNO3 (aq) + NaCl(aq) AgCl(s) + NaNO3(aq)
complete ionic equation

14. Na+
NO3-
AgCl
Reaction

15. No Reaction
Na+
NO3-
AgCl

16. These ions do not participate in the reaction. They are called
SPECTATOR IONS
Na+
NO3-
AgCl

17. The net ionic equation is constructed from the complete ionic equation:

18. NO3- and Na+ are not participating in the reaction

19. net ionic equation

20. net ionic equation

21. Complete molecular equation-
describes double replacement reaction
Complete ionic equation-
more accurately shows the reacting species as ions and the products either as ions or a precipitate
Net ionic equation-
focuses only on the ions REACTING
Spectator ions are those ions that do NOT participate in the reaction

22. PREDICTING THE FORMATION OF A PRECIPITATE
Consider the possibility that a precipitate may form bu using solubility table to decide.
Possible outcomes
No visible reaction (nvr)
Formation of one ppt.
Formation of two ppt. (rare occurrence)

23. Basic Chemical equation AgNO3(aq) + KCl(aq) AgCl(s) + KNO3(aq)
Complete ionic equation shows ions in solution Ag+ (aq) + NO3(aq) + K+ (aq) + Cl-(aq)  AgCl(s) + K+ (aq) + NO3- (aq)
Net ionic equation shows ions in rxn Ag+ (aq) + Cl-(aq)  AgCl(s)
(leave out spectator ions)