1. Review:

2. Review:
(b.) 5 grams of magnesium metal is dropped 20 mL of 3 M hydrochloric acid, HCl, producing hydrogen gas and magnesium chloride.
If the hydrogen gas is collected under standard conditions, what volume is produced?
If the experiment is performed, but only 0.5 L of H2 gas is collected at STP, what is the % yield?

6. Net Ionic Equations:
Sol’n stoich. can be tricky when aqueous ionic compounds are involved …
Remember how ionic things dissociate?
MgCl2 (aq) 
Al(NO3)3 (aq) 

7. Pb(NO3)2 (aq) + NaI (aq)  PbI2 (s) + NaNO3 (aq)
Net Ionic Equations:
Sol’n stoich. can be tricky when aqueous ionic compounds are involved …
Pb(NO3)2 (aq) + NaI (aq)  PbI2 (s) + NaNO3 (aq)
Reactions where 2 aqueous solutions produce an insoluble product are called precipitation reactions.
Ionic equation:
Net Ionic equation:
DOUBLE REPLACEMENT REACTIONS:
AB + CD  AD + CB

8. Remember Solubility Rules:
1). All common salts of the nitrate ion (NO3-) are soluble in water.
2). All common salts of the Na+, K+, and NH4+ cations are soluble in water.
3). Most common salts of the Cl-, Br-, and I- anions are soluble in water EXCEPT when the accompanying cation is Ag+, Pb2+, and Hg22+.
4). All common salts of the sulfate ion (SO42-) are soluble in water EXCEPT when the accompanying cation is Ba2+, Sr2+, and Pb2+.
5). Salts of the S2- ion are insoluble in water EXCEPT when the accompanying cation is Na+, K+, NH4+, Ba2+, and Ca2+.
6). Most of the transition metal cations (Ag+, Cu2+, Ni2+, etc.) form complexes with aqueous ammonia. Sometimes, ammonia is used to "dissolve" otherwise insoluble precipitates of these metal cations.
***The new AP Chemistry Guidelines suggest that you don’t really have to know most of these, just the common ones that are most useful.

9. Net Ionic Equations:
Sol’n stoich. can be tricky when aqueous ionic compounds are involved …
Predict the products and write the net ionic equation for the following precipitation reaction:
Na2SO4 (aq) + BaCl2 (aq) 

10. Single Replacement Reactions:
A + BC --> BA + C (single anion replaces anion in compound) or A + BC --> AC + B (single cation replaces cation in compound) 
*Free metal “A” needs t be above combined metal “B”
Metal Activity Series

11. Net Ionic Equations:
Sol’n stoich. can be tricky when aqueous ionic compounds are involved …
Predict the products and write the net ionic equation for the following aqueous reaction:
Zn (s) + HCl (aq) 

12. Net Ionic Equations:
Practice by writing complete net ionic equations for each of the following:
AgNO3(aq) + K2CO3(aq) 
Al(s) + HCl (aq) 
Ca (s) + H2O (l)  Ca(OH)2 + H2

13. 2Ag+ (aq) + CO3-2 (aq)  Ag2CO3 (s)
Net Ionic Equations:
Practice by writing complete net ionic equations for each of the following:
2Ag+ (aq) + CO3-2 (aq)  Ag2CO3 (s)
AgNO3(aq) + K2CO3(aq) 
Al(s) + HCl (aq) 
Ca (s) + H2O (l)  Ca(OH)2 + H2

14. 2Ag+ (aq) + CO3-2 (aq)  Ag2CO3 (s)
Net Ionic Equations:
Practice by writing complete net ionic equations for each of the following:
2Ag+ (aq) + CO3-2 (aq)  Ag2CO3 (s)
AgNO3(aq) + K2CO3(aq) 
Al(s) + HCl (aq) 
Ca (s) + H2O (l)  Ca(OH)2 + H2
2Al (s) H+ (aq)  2Al+3 (aq) H2 (g)

15. 2Ag+ (aq) + CO3-2 (aq)  Ag2CO3 (s)
Net Ionic Equations:
Practice by writing complete net ionic equations for each of the following:
2Ag+ (aq) + CO3-2 (aq)  Ag2CO3 (s)
AgNO3(aq) + K2CO3(aq) 
Al(s) + HCl (aq) 
Ca (s) + H2O (l)  Ca(OH)2 + H2
2Al (s) H+ (aq)  2Al+3 (aq) H2 (g)
Ca (s) H2O (l)  Ca(OH)2 (s) H2 (g)