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

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) 

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)

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

Learning targets

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 

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)

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!

Chemical reactions practice questions

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

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

The Basics What is the name of ClO-3 chlorate

The Basics What is formula for sodium carbonate? Na2CO3

Now for some good stuff!

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.

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

3. Balance the Following Equations C2H2 + O2  CO2 + H2O Mg(OH)2 + H3PO4  Mg3(PO4)2 + H2O AlF3 + CaSO4  Al2(SO4)3 + CaF2 2 C2H2 + 5 O2  4 CO2 + 2 H2O  3 Mg(OH)2 + 2 H3PO4  Mg3(PO4)2 + 6 H2O 2 AlF3 + 3 CaSO4  Al2(SO4)3 + 3 CaF2

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

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)

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)

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

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

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

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

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+

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).

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!