1. Chem-is-try… Please take out:  Your lab book  Your Metal Activity Lab  A whiteboard, pen, & “eraser”  Your PT (Gold) & Metal Activity Series Chart (Pink)  Pink “Writing Single and Double Replacements WS” Practice writing your name with your non-dominate hand… …just for fun

2. 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) + 2AgNO 3(aq)  ???? Claim: Evidence: (We will make observations to confirm/deny our claim) Reasoning:

3. 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) + 2AgNO 3(aq)  Mg(NO 3 ) 2(s) + 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!

4. Activity Series for Metals 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 Elements at the bottom hold electrons tightly/ less likely to react An element can only kick out the ion if it is the more reactive of the two Example: Al (s) + FeCl 3(aq)  AlCl 3(aq) + Fe (s) Fe (s) + AlCl 3(aq)  No Reaction Al is above Fe on the series

5. Learning Targets

6. Homework Review Team Captain is the person with the biggest hands, they will keep the group on track. 1.Please check your pink worksheet with the answer key and make corrections 2.Log only this worksheet on your HW Sheet 3.Pass your HW sheets forward

7. Homework Review Team Captain, designate a new Captain! Compare your answers to the analysis questions on the back of the lab. I will put up the reactions to #6 in a minute

8. Using CER predict if the following will occur, site evidence from the metal activity series lab Cu (s) + MgCl 2 (aq)  Mg (s) + CuCl 2(aq)  When finished staple to your lab and turn in.

9. Classification Clarification! Oxidation- Reduction “Transfer of Electrons” Single Replacement Combination/Synthesis Decomposition Combustion Double Replacement “Solubility” Precipitation/Solid Forming Acid- Base/Water forming Gas Forming

10. Classify each of these reactions and decide if they are oxidation reduction reactions as well 2 AlN (s)  2 Al (s) + N 2 (g) BaCl 2 (aq) + Na 2 SO 4 (aq)  BaSO 4 (s) + 2 NaCl (aq) 2 Cs (s) + Br 2 (l)  2 CsBr (s) H 2 SO 4 (aq) + Ba(OH) 2 (aq)  BaSO 4 (s) + 2 H 2 O (l) Zn (s) + CuSO 4 (aq)  Cu (s) + ZnSO 4 (aq) Decomposition Double Replacement Combination Single Replacement Oxidation-Reduction (redox) Precipitation Oxidation-Reduction (redox) Precipitation Oxidation-Reduction (redox)

11. Batteries – An example of oxidation reduction Aluminum is more reactive than Zinc

12. Extra Practice Page 2 of your pink Writing Single and Double Replacements worksheet Label the appropriate reactions as Redox (Oxidation-Reduction)

13. For the rest of class… Work on Activity Series (Blue) Packet Challenge your tablemate when you don’t fully understand Work on UT Due 11/25 @ 9PM– DON’T PROCRASTINATE! Ask Ms. Bryce 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 Packet UT “Reactions” Assignment (Due 11/25 @9PM) UNIT TEST WED. 11/25!

14. Exit Task You measure out 2.0g of Na 3 PO 4 and 3.2g of AlCl 3 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. Explain using Claim, Evidence, Reasoning (ClEvR!) Next Class Is Review Day! Claim: NaCl + AlPO 4 would form and the bag would weigh 5.5 grams. Evidence: 2.0g+3.2g+0.3g=5.5g A white solid was formed, and so was a liquid. 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).