1. Bell Ringer Please have the following out on your desk
Notes packet p 14
Worksheet picked up
Turn in
Double replacement lab
Complete double replacement equations 1-4 on worksheet picked up.

2. -Notes: single replacement -Lab: single replacement -PPP p 4
Day
Topic HW
Monday
12/1
Test corrections after school
-Notes: single replacement
-Lab: single replacement
-PPP p 4
-Lab SR due 12/3
-Pre-lab double replacement
Tuesday
12/2
Test corrections before school
-Notes: double replacement
-Lab: double replacement
-PPP p 5
-Lab DR due 12/4
-Pre-lab all types in notebook (include data table)
Wednesday
12/3
Tutorials before and after school
SR Lab due
-Notes: combustion
-Lab: all types (in notebook)
-Lab all types due 12/5
-PPP pp 6 & 7
Thursday
12/4
DR Lab due
-Net Ionics
-Redox reactions
-Pre-lab reaction rates
Friday
12/5
Tutorials before school
All Types Lab due
-Notes: reaction rates
-Lab: reaction rates
-Predicting Products Scavenger Hunt
-Lab RR due 12/9
-Comp quiz Monday 12/8
-PPP due 12/9

3. Types of Reactions Type of Reaction Pattern Example Synthesis
X + Y  XY
2Na (s) + Cl2 (g)  2NaCl
Decomposition
AB  A + B
H2O2 (aq)  H2O (l) + O2(g)
Single Replacement
XY + A  AY + X
Mg (s) + 2 HCl (aq)  H2 (g) + MgCl2 (s)
Double Replacement
XY + AB  XB + AY
KI (aq) + Pb(NO3)2  PbI2 (s)+ KNO3 (aq)
Combustion
CxHy + O2  CO2 + H2O
CH4 (l) + O2 (g)  CO2 (g) + H2O (l)

4. T6: Net Ionic Equations
Reactions that are simplified to only show what particles are changing.

5. What type of reaction is happening?
Pb(NO3)2 (aq) + NaI (aq) 

6. What states are the products in?
Pb(NO3)2 (aq) + NaI (aq) 
Pb(NO3)2 (aq) + NaI (aq)  PbI2 + NaNO3

7. Pb(NO3)2 (aq) + NaI (aq) 
Pb(NO3)2 (aq) + NaI (aq)  PbI2 (s) + NaNO3 (aq)
Are there any ions that are not actually undergoing a chemical change?

8. Pb(NO3)2 (aq) + NaI (aq) 
Pb(NO3)2 (aq) + NaI (aq)  PbI2 (s) + NaNO3 (aq)
Are there any ions that are not actually undergoing a chemical change? Na+ (aq) and NO3- (aq)
A net ionic equations does not show the ions that don’t change (ions that stay aqueous)

9. Strong Acids (these acids fully ionize)
Hydrochloric
Hydrobromic
Hydriodic
Sulfuric
Nitric
Chloric
Perchloric
Write these down!

10. Redox – notes pg 12 Redox stands for reduction-oxidation reactions.
Electrons move from one atom to another or from one ion to another.

11. REMEMBER one of these: L losing E electrons O oxidation Says G gaining
R reduction
O oxidation
I is
L losing
R reduction
G gaining

12. Oil Rig Leo Ger
Losing electrons – becoming more positive (more protons than electrons)
Gaining electrons – becoming more negative (more electrons than protons)

13. Oxidation Numbers – notes pg 11
Assigning oxidation numbers:
All single elements are neutral so they have an oxidation # of 0
Oxygen is almost always -2
Hydrogen is almost always +1
The compound should add up to 0 unless it is a polyatomic then it adds up to the charge.

14. Assign Oxidation Numbers to the compounds below:
SO2
SO3
NO2
PCl3
NO3-1
CO3-2
HBrO Al

15. Example: (notes pg 12) 2 Na + Cl2  2 NaCl
Which element is oxidized? _________
Which element is reduced? _________

16. Agents
The element that is oxidized, donates electrons, is the reducing agent.
The element that is reduced, accepts electrons, is the oxidizing agent.
Species – any kind of chemical unit

17. Example:
2 Na + Cl2  2 NaCl
Which element is the reducing agent? ________
Which element is the oxidizing agent? ________

18. Complete, balance, identify element oxidized, element reduced, oxidizing agent and reducing agent.
H2S + Cl2  S + HCl

19. Examples of REDOX Reactions
-Iron rusting.
-Hydrogen peroxide sanitizing wounds.
-Photography development.
-Chlorine bleach whitening laundry.
-Silver tarnishing.