Oxidation Lab Different Metals Undergo Oxidation and Reduction free essay sample

You are going to investigate the ease with which different metals undergo oxidation and reduction. Materials:| 4 samples of each of: lead, zinc, iron, copper | spot plates steel wool/sand paper | | | | Solutions of: | copper(II) sulfate Ferric nitrate Silver nitrate Lead (II) nitrate | | Procedure: 1. Obtain 4 samples of each metal and clean with steel wool or sand paper. Wash your hands after cleaning the metals so you are not exposed to lead dust). 2. Fill four bubbles on a spot plate with one of the solutions. Place one metal in each of the bubbles. Observe and record the before and after appearance. 3. Fill four new bubbles with a second solution. Place one sample of each metal in each of the bubbles. Observe and record the before and after appearance. 4. Repeat the above until all four solutions have been tested. Hypothesis: Write the reaction equation for each metal in copper (II) sulfate. Reaction equation| How will you ID the product? | Zn(s) + CuSO4 (aq) ZnSO4(aq) + Cu(s)Zn0(s) Zn2+(aq) +2e-Cu+2(aq)+2e- Cu0(s)| You will Id the products by the chemical reaction that will occur. We will write a custom essay sample on Oxidation Lab Different Metals Undergo Oxidation and Reduction or any similar topic specifically for you Do Not WasteYour Time HIRE WRITER Only 13.90 / page Zinc be the element under going oxidation as it looses electrons and copper will be the reduction as it gains electrons. | Pb(s)+CuSO4 (aq) Cu SO4 (aq) + Pb(s)| No reaction. There will be no gaining or loosing electrons| Fe(s)+CuSO4 (aq) + FeSO4 (aq) +Cu(s)Fe0(s) Fe+3(aq) +3e-Cu+2(s) + +-e Cu0(s)| Oxidation will occur because iron has high oxidation number then copper. | Cu(s)+CuSO4 (aq) CuSO4 (aq) + Cu(s)| No reaction. There will be no gaining or loosing electrons| Write the reaction equation for each metal in Ferric nitrate Reaction equation| How will you ID the product? | Zn(s) + Fe(NO3)3(aq) Fe(NO3)3(aq) + Z (s)| No reaction. There will be no gaining or loosing electrons| Pb(s) + Fe(NO3)3(aq) Pb (NO3)3(aq) +Fe(s)Pb0(s) Pb+2(aq)+2e-Fe+3(aq) + + 3e- Fe0(s)| Lead will be oxidized. Iron will be reduced| Fe(s) + Fe(NO3)3(aq) Fe(s) + Fe(NO3)3(aq)| No reaction. There will be no gaining or loosing electrons| Cu(s) + Fe(NO3)3(aq) Cu (NO3)3(aq) +Fe(s)Cu0(s) Cu+2(aq) + 2e-Fe+3(aq) + + 3e- Fe0(s)| Copper will be oxidized and iron will be reduced. | Write the reaction equation for each metal in Lead (II) nitrate Reaction equation| How will you ID the product? Zn(s) + Pb(NO3)2 Zn(NO3)2(aq)+Pb(s)Zn0(s) Zn2+(aq) +2e-Pb+4(aq) + +4e- Pb0(s)| Zinc will be oxidized and lead will be reduced. | Pb(s) + Pb(NO3)2 Pb(s) + Pb(NO3)2 | No reaction| Fe(s) + Pb(NO3)2 Fe(NO3)2(aq)+Pb(s)| No reaction. There will be no gaining or loosing electrons| Cu(s) + Pb(NO3)2 Cu(NO3)2(aq)+Pb(s)| No reaction. There will be no gaining or loosing electrons| Write the reaction equation for each me tal in silver nitrate Reaction equation| How will you ID the product? | Zn(s) + AgNO3(aq) ZnNO3(aq) +Ag(s)Zn0(s) Zn2+(aq) +2e-Ag+1(aq) + +1e- Ag0(s)| Zinc will be oxidized and silver will be reduced| Pb(s) + AgNO3(aq) PbNO3(aq) +Ag(s)Pb0(s) Pb+2(aq) +2e-Ag+1(aq) + +1e- Ag0(s)| Lead will be oxidized and silver will be reduced| Fe(s) + AgNO3(aq) FeNO3(aq) +Ag(s)Fe0(s) Fe+3(aq) +3e-Ag+1(aq) + +1e- Ag0(s)| Iron will be oxidized and silver will be reduced| Cu(s) + AgNO3(aq) CuNO3(aq) +Ag(s)Cu0(s) Cu+2(aq) + 2e-Ag+1(aq) + +1e- Ag0(s)| Copper will be oxidized and silver will be reduced| Part II: Once you have submitted your hypothesis, view the lab results here, create an observations table, and complete the discussion questions. Discussion Questions: Write the oxidation half-reaction, reduction half-reaction and the redox equation for each reaction you observed. Zinc + Copper (II) Sulfate * Zn0(s) Zn2+(aq) +2e- Oxidation half- reaction * Cu+2(aq)+2e- Cu0(s) Reduction half reaction * Zn0(s) + Cu+2(aq) Zn2+(aq) + Cu0(s) Balanced redox Iron and Copper (II) Sulfate * Fe0(s) Fe+3(aq) +3e- Oxidation half- reaction Cu+2(aq) + +-e Cu0(s) Reduction half reaction * Fe0(s) + Cu+2(aq) Fe+3(aq) + Cu0(s) Balanced redox Ferric Nitrate and Lead * Pb0(s) Pb+2(aq)+2e- Oxidation half- reaction * Fe+3(aq) + + 3e- Fe0(s) Reduction half reaction * Pb0(s) + Fe+3(aq) Pb+2(aq) + Fe0(s) Balanced redox Copper and Ferric Nitrate * Cu0(s) Cu+2(aq) + 2e- Oxidation half- reaction * Fe+3(aq) + + 3e- Fe0(s) Reduction half reaction * Cu0(s) + Fe+3(aq) Cu+2(aq) + Fe0(s) Balanced redox Zinc and Lead (II) Nitrate Zn0(s) Zn2+(aq) +2e- Oxidation half- reaction * Pb+4(aq) + +4e- Pb0(s) Reduction half reaction * Zn0(s) + Pb+4(aq) Zn2+(aq) + Pb0(s) Balanced redox Zinc and Silver Nitrate * Zn0(s) Zn2+(aq) +2e- Oxidation half- reaction * Ag+1(aq) + +1e- Ag0(s) Reduction half reaction * Zn0(s) + Ag+1(aq) Zn2+(aq) + Ag0(s) Balanced redox Iron and Silver Nitrate * Fe0(s) Fe+3(aq) +3e- Oxidation half- reaction * Ag+1(aq) + +1e- Ag0(s) Reduction half reaction * Fe0(s) + Ag+1(aq) Fe+3(aq) + Ag0(s) Balanced redox Copper and Silver Nitrate Cu0(s) Cu+2(aq) + 2e- Oxidation half- reaction * Ag+1(aq) + +1e- Ag0(s) Reduction half reaction * Cu0(s) + Ag+1(aq) Cu+2(aq) + Ag0(s) Balanced redox Lead and Silver Nitrate * Pb0(s) Pb+2(aq) +2e- Oxidation Half reaction * Ag+1(aq) + +1e- Ag0(s) Reduction half reaction * Pb0(s) + Ag+1(aq) Pb+2(aq) + Ag0(s) Balanced redox Which metal underwent the most reactions? Zinc underwent the most reactions during this experiment. Zinc reacted with 3 out of 4 solutions, the only solution it did not react with was zinc iron. Which cation underwent the most reactions? Silver underwent the most reactions as it reacted with all four metal samples. Which metal underwent the most oxidations? Zinc underwent the most oxidation in this experiment. Which metal underwent the most reductions? Silver Nitrate underwent the most reductions and it was reduced by all four metal samples. Compare the metal that was most easily oxidized with the metal that was most easily reduced with their positions on the reactivity series. Is there any trend present? Silver(Ag),was most easily reduced and was lowest on the reactivity series in comparison with the other solutions. Zinc (Zn) had the highest reactivity out of all the metal samples it was compared against. If your dog accidentally swallowed a sentimental keepsake, with which of the above metals would you hope it was made? Why? If my dog swallowed something that held meaning to me, I would hope that it would have been copper because copper does not react with acids. There is stomach acid in a dog and copper would have most likely stood up to the stomach contents. Other metals could react with the contents of the dogs stomach, such as water, steam from the dogs breath on the way down and the acid in the dogs stomach. How did your results compare to your hypothesis? Did you get what you expected? My hypothesis was correct with the reactions of the metals and solutions. I did expect silver nitrate to react with all the metals as the cation is lower on the reactivity series. I also expected zinc to react with all the solutions except the ferric solution because ferric has a higher oxidation number that the zinc.