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

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

4. 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.

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

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

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

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

9. AgNO3
NaCl

10. NO3-
Na+
Ag+
Cl-

11. Na+
NO3-
Ag+
Cl-

12. Na+
NO3-
AgCl

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

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

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

16. Na+
NO3-
AgCl
Reaction

17. No Reaction
Na+
NO3-
AgCl

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

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

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

21. net ionic equation

22. net ionic equation

23. 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

24. PREDICTING THE FORMATION OF A PRECIPITATE
Consider the possibility that a precipitate may form.
Must use the solubility table on page 227 to decide.
Possible outcomes
No visible reaction (nvr)
Formation of one ppt.
Formation of two ppt. (rare occurrence)

25. 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)
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