1. Review day! NO NEW INFO! Take out… Lab notebook Metal Series Lab
Metal Activity Series Packet
Grab…
1 Review Sheet
HW SHEET!

2. warm-up
Predict if the following reactions will occur. If a reaction does occur predict stable products AND balance the equation:
Al(s) + ZnCl2(aq) 
Co(s) + NaCl(aq) 
Mg(s) + HCl(aq) 
Al(s) + Fe(NO3)2(aq) 
Ca(s) + Pb(NO3)2(aq) 

3. warm-up-Answers
Predict if the following reactions will occur. If a reaction does occur predict stable products AND balance the equation:
2Al(s) + 3ZnCl2(aq)  2AlCl3(aq) + 3Zn(s)
Co(s) + NaCl(aq)  NO REACTION
Mg(s) + 2HCl(aq)  MgCl2(aq) + H2(g)
2Al(s) + 3Fe(NO3)2(aq)  2Al(NO3)3(aq) + 3Fe(s)
Ca(s) + Pb(NO3)2(aq)  Ca(NO3)2(aq) + Pb(s)

4. 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
Elements at the bottom hold electrons tightly/ less likely to react

5. Learning targets

6. test!
On the test, you will have a periodic table, solubility chart, and metal activity series
Test = 25 multiple choice and 5 short answer (problem solving, 3-4 sentences, etc.)
Lab Books will be turned in at the beginning of class to grade
The test will probably take the whole period! Bring additional HW if you finish early 

7. What are we doing today? Turn in your lab
Check your answers to the packet
Log this on your HW sheet
Total Unit 4 Homework and HIGHLIGHT THIS
Complete the Test Review Assignment in your lab book and check answer key online
Check Skyward/HW Sheet for missing assignments
All missing Unit 4 assignments can be turned in the day of the test for credit- otherwise 75% credit
Do the practice questions from this PowerPoint in your lab book (HW along with Test Review)

8. Homework review!
Team captain is the person who has the longest finger nails
Keep the team on track!
STAY ON TASK! This review day is a gift. Don’t abuse it!
Log on HW sheet, give a UNIT 4 Total and highlight!
Finished?
Work on the Unit 4 Test Review!

9. Chemical reactions practice questions

10. The basics What is the correct name of CuCl2
Copper (II) chloride or cupric chloride

11. The Basics
How should I balance the equation… Mg + O2  MgO 2Mg + O2  2MgO

12. The Basics
What is the name of ClO-3 chlorate

13. The Basics
What is formula for sodium carbonate?
Na2CO3

14. Now for some good stuff!

15. 1. Consider this reaction
2AgCl(s) + Pb(NO3)2(aq) 2AgNO3(aq) + PbCl2(s) Let’s say you started with 10g of silver chloride and 10g of lead nitrate. After the reaction, you had 12 g of silver nitrate. a. How many grams of lead chloride do you have? b. Explain how you know this! A: 8 grams. The law of conservation of mass says that the mass of the reactants = mass of the products. This is why we balance equations.

16. 2. Name the 4 driving forces for a Reaction
Formation of a solid
Formation of a Water
Formation of a gas
Transfer of electrons

17. 3. Balance the Following Equations
C2H2 + O2  CO2 + H2O
Mg(OH)2 + H3PO4  Mg3(PO4)2 + H2O
AlF3 + CaSO4  Al2(SO4)3 + CaF2
2 C2H O2  4 CO H2O 
3 Mg(OH) H3PO4  Mg3(PO4)2 + 6 H2O
2 AlF3 + 3 CaSO4  Al2(SO4)3 + 3 CaF2

18. 4. Classify these reactions in as many ways as possible
NaN3 (s)  Na3N (s) + N2 (g) (2 ways)
2 AgNO3 (aq)+ CuCl2 (aq)Cu(NO3)2 (aq) +2 AgCl (s) (2 ways)
2 HCl (aq) + Mg (s)  H2 (g) + MgCl2 (aq) (2 ways)
Ca(OH)2 (aq) +2 HNO3 (aq) Ca(NO3)2 (aq) +H2O (l) (2 ways)
Decomposition and Oxidation Reduction
Double Replacement and Precipitation
Single Replacement and Oxidation Reduction
Double Replacement and Acid-Base

19. 5. Identify the solid that will form and finish/balance these equations
CuCl2(aq) + AgNO3(aq) 
KOH(aq) + MgS(aq) 
CuCl2(aq)+ 2 AgNO3(aq)  Cu(NO3)2(aq) + 2 AgCl(s)
2 KOH(aq) + MgS(aq)  K2S(aq) + Mg(OH)2(s)

20. 6. Writing Ionic Equations
Write the molecular, complete ionic and net ionic equations for the reaction of magnesium chloride with potassium carbonate.
Molecular:
MgCl2(aq) + K2CO3(aq)  2 KCl(aq) + MgCO3(s)
Complete Ionic:
Mg+2(aq) + 2Cl-1(aq) + 2K+1(aq) + CO3-2(aq)  2K+1(aq)+ 2Cl-1(aq) + MgCO3(s)
Net Ionic:
Mg+2(aq) + CO3-2(aq)  MgCO3(s)

21. 7. NaNO3(aq) + NH4Cl(aq)  NH4NO3(aq) + NaCl(aq)
Why doesn’t a solid form when sodium nitrate is reacted with ammonium chloride?
What will this look like at the microscopic level after the two are mixed?
NaNO3(aq) + NH4Cl(aq)  NH4NO3(aq) + NaCl(aq)
All of the ions are soluble in water and won’t form a solid
There would just be Na+, NO3-, NH4+, and Cl- ions “floating around” in one container

22. 8. Oxidation-Reduction In the following equation:
3 Mg(s) + 2 AlCl3(aq)  3 MgCl2(aq) + 2 Al(s)
How many total electrons are transferred in this reaction?
Is the Mg oxidized or reduced?
Which metal is the more active?
Mg: 0  +2(3) loss of 6 electrons
Al: +3(2)  0 gain of 6 electrons
Oxidized
Magnesium: It doesn’t hold on to its electrons and gives them to Al

23. 9. Lab Problem
From the following table determine 1B, 2B, and 3B. Your choices for B chemicals are Potassium Chloride, Sodium Phosphate, and Silver Nitrate. It has already been determined that 1A is Barium Nitrate, 2A is Potassium Carbonate, and 3A is Sodium Sulfate
Barium Nitrate
Potassium Carbonate
Sodium Sulfate 1B
Yes No 2B 3B 1B 2B 3B No
Yes

24. Lab Problem– Answers
Barium Nitrate
Potassium Carbonate
Sodium Sulfate 1B
Yes No 2B 3B 1B 2B 3B No
Yes
3B is AgNO3 because it forms a solid with the other two B chemicals
1B is Na3PO4 because it forms a solid with Barium Nitrate
2B is KCl because it does not form a solid with any of the A’s

25. 10. Redox Reactions
Give an example of a double replacement reaction Explain why double replacement reactions are NOT oxidation reduction reactions. Na2SO4(aq) + CaCl2(aq)  2NaCl(aq) + CaSO4(s) This is not a oxidation reduction reaction because no element gets oxidized or reduced. This is because charges or ions do not change in a double replacement. Na+1 is still Na+1 SO42- is still SO42- Cl-1 is still Cl-1 Ca2+ is still Ca2+

26. 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!) 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).

27. For the rest of the period
Unit 4 Test Review
Due the day of the test
Review old assignments
Review your notes
Highlight/annotate/summarize
Help out a struggling classmate
Make sure your notebook is all ready
Review complete
All entry tasks complete
Responsibility is shown by keeping yourself organized!