1. Chem-is-try… Please take out: Your lab book & HW Sheet
Your 6 Bottle Mystery Lab
5 pieces of paper in the back

2. Warm Up
You measure out 2.0g of Na3PO4 and 3.2g of AlCl3 and mix both chemicals in a bag that weighs 0.3g. You observe a chemical reaction. Predict the formulas and mass of the bag with the chemicals after the reaction has occurred (Think: Double Replacement Reaction). Explain using Claim, Evidence, Reasoning (ClEvR!) Next Class Is Review Day! Claim: The compounds NaCl + AlPO4 would form and the bag would weigh 5.5 grams. Evidence: 2.0g+3.2g+0.3g=5.5g A white solid was formed (AlPO₄), and so was a liquid (NaCl). Reasoning: Since the reaction began with 5.2 grams of chemicals, the bag and chemicals after the reaction occurred would weigh a total of 5.5 grams. This is because of the Law of Conservation of Mass, that states that in chemical reactions mass is conversed (not lost). In double replacement reactions the ions switch places, both Na and Cl are soluble so they would create a liquid and both Al and PO₄ are insoluble so they would create a solid.

3. Homework Review Check with your group first…
Do you have the same chemicals identified?
Log this worksheet on your HW Sheet

4. Homework (Lab) Review
A’s 1A Barium Nitrate 2A Potassium Carbonate 3A Sodium Sulfate
B’s
1B Sodium Phosphate
2B Potassium Chloride
3B Silver Nitrate

5. Learning Targets
Predict stable products of single replacement reactions.
Show the transfer of electrons by identifying what elements are oxidized and reduced.

6. Metal activity series notes!

7. Oxidation and Reduction (REDOX)
When elements form ionic bonds, one element is “oxidized” and one is “reduced”
Oxidation = loss of electrons
Reduction = gain of electrons
LEO = lose electrons oxidized
GER = gain electrons reduced

8. Classification Clarification!
Oxidation-Reduction Reactions
Single Replacement
Combination/Synthesis
Decomposition
Combustion
Double Replacement Reactions
Precipitation/Solid Forming
Acid- Base/Water forming
Gas Forming

9. Classify each of these reactions and decide if they are oxidation reduction reactions as well
2 AlN (s)  2 Al (s) + N2 (g)
BaCl2 (aq) + Na2SO4 (aq)  BaSO4 (s) NaCl (aq)
2 Cs (s) + Br2 (l)  2 CsBr (s) 
H2SO4 (aq) + Ba(OH)2 (aq)  BaSO4 (s) + 2 H2O (l)
Zn (s) + CuSO4 (aq)  Cu (s) + ZnSO4 (aq)
Decomposition
Oxidation-Reduction (redox)
Precipitation
Double Replacement
Combination
Oxidation-Reduction (redox)
Double Replacement
Precipitation OR
Acid/Base!
Single Replacement
Oxidation-Reduction (redox)

10. Metal Activity Series
Where have you seen some of these metals before? Does their placement on the chart make sense?
We see these metals in jewelry like gold, lithium is in batteries. This chart shows the reactivity…remember oxidation is the loss of electron. This chart is showing the loss of electrons. If they lose electrons easily they will be at the top. Although H is not a metal it is included in the metal activity series…sometimes it act more like a metal than a non-metal. Lithium highly reactive to be used in batteries, and gold not very reactive used as jewelry.

11. Metal activity series
We can use the metal activity series to determine if a single replacement reaction will occur or not
The lower on the list, the more likely the metal is to steal e- and become the solid
Ex:
Cu(s) + CaCl No reaction
(calcium is not strong enough to steal Cu’s e- and become a solid)
Ca(s) + CuCl Cu(s) + CaCl2
Cu is a stronger “oxidant”, or e- stealer
Copper is lower on the list than calcium, it is happy to be a solid and not as reactive so no reaction. Calcium is higher on the list and therefore will more easily lose its electrons because copper wants to be a solid with no charge, so it will replace copper.

13. Activity Series for Metals
An element can only kick out the ion if it is the more reactive
of the two
Li K Ba Ca Na Mg Al Zn Fe Co Ni Sn Pb H Cu Ag Au
Elements at the top hold electrons weakly / more likely to react
Example:
Al(s) + FeCl3(aq)  AlCl3(aq) + Fe(s)
Fe(s) + AlCl3(aq)  No Reaction
Al is above Fe on the series, so the Iron will kick out the Aluminum.
Elements at the bottom hold electrons tightly/ less likely to react. These guys want to be a solid.

14. Oxidation and Reduction
Al(s) + FeCl3(aq)  AlCl3(aq) + Fe(s)
Which metal is being oxidized and which is being reduced?
Al: 0+3 is a loss of electrons – oxidation
Fe: +3  0 is a gain of electrons - reduction
Can oxidation happen without reduction? Why?
No, because if one element loses electrons something has to gain them, matter is conserved!

15. Activity Series Pre-Lab
We will do the pre-lab section of the lab on the worksheet together.
On the top of the paper, show the single replacement reaction between magnesium and zinc (II) chloride
Mg + ZnCl2  ??
**Show the transfer of electrons!
We will watch a demo of a reaction between copper and silver nitrate solution.

16. Dump in waste container and rinse well plate thoroughly!
Activity Series Lab
Put away any extra papers or journals.
Wear goggles
You will just need ONE piece of metal for each sample
Mix the solid metal with about .5 ml of metal chloride solution (1/2 a dropper)
Record if a reaction occurred (yes or no)
Dump in waste container and rinse well plate thoroughly!
Move on to analysis
Cross out “Something Extra”

17. Copper metal reacted with aq Silver, so Ag is less reactive than Cu
Activity Series Lab
Solutions
(Charges!)
Zn+2
Sn+2
Mg+2
Al+3
Cu+2 Cu No Al
Yes Mg Sn Zn
Solids
(No charge)
Most Reactive
Mg  4 reactions
Copper metal reacted with aq Silver, so
Ag is less reactive than Cu
Al  3 reactions
Zn  2 reactions
Sn  1 reaction
Least Reactive
Cu  0 reactions

18. For the rest of class…until our exit task.
Work on Lab & Activity Series (Blue) Packet
Challenge your tablemate when you don’t fully understand
Ask Ms. Jarvis questions
Check Skyward/HW Sheet and see if you are missing any homework assignments
Tutor a peer on a learning target/concept they are struggling with
Homework:
Activity Series Lab
Activity Series Packet
UNIT TEST Tuesday/Wedensday 12/19 and 12/20!

19. Exit Task
If I put a strip of magnesium metal in a solution of silver nitrate, should I observe a reaction? Why or why not? Mg(s) + 2AgNO3(aq)  ???? Claim: Evidence: (We will make observations to confirm/deny our claim) Reasoning:

20. Warm-Up
If I put a strip of magnesium metal in a solution of silver nitrate, should I observe a reaction? Why or why not? Mg(s) + 2AgNO3(aq)  Mg(NO3)2(aq) + 2Ag(s) Claim: Yes, I should observe a reaction. Evidence: Silver starts to form on the outside, and the magnesium goes into solution. Reasoning: Since magnesium is more easily oxidized (lower ionization energy), magnesium will lose its electrons (oxidation) to silver who will gain electrons (reduction). WHAT WOULD THIS MOLECULAR DRAWING LOOK LIKE!