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

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) ????Claim:Evidence: (We will make observations to confirm/deny our claim)

Reasoning:

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(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!

Activity Series for MetalsLiK

BaCaNa MgAlZnFeCoNiSnPbHCuAgAu

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 reactiveof the two

Example:Al(s) + FeCl3(aq) AlCl3(aq)

+ Fe(s)

Fe(s) + AlCl3(aq) No Reaction

Al is above Fe on the series

Learning Targets

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 corrections2. Log only this worksheet on your HW Sheet3. Pass your HW sheets forward

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

Using CER predict if the following will occur, site evidence from the metal activity series lab

•Cu(s) + MgCl2 (aq)

•Mg(s) + CuCl2(aq)

When finished staple to your lab and turn in.

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

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) + 2 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

Double Replacement

Double Replacement

Combination

Single Replacement

Oxidation-Reduction (redox)

Precipitation

Oxidation-Reduction (redox)

Precipitation

Oxidation-Reduction (redox)

Batteries – An example of oxidation reduction

Aluminum is more reactive than Zinc

Extra Practice

• Page 2 of your pink Writing Single and Double Replacements worksheet

• Label the appropriate reactions as Redox (Oxidation-Reduction)

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!

Exit Task

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. Explain using Claim, Evidence, Reasoning (ClEvR!)

Next Class Is Review Day!

• Claim: 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, 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).