Oxidation Lab Different Metals Undergo Oxidation and Reduction.
Oxidation Lab
Part 1:
Purpose: 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. 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
Part 1:
Purpose: 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. 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