Redox Reaction Lab Report
Purpose
Determine which kinds of reactions involve electron transfer as the driving force.
Background
Redox (reduction-oxidation) reactions include all chemical reactions in which atoms have their oxidation state changed. So, when a metal and a nonmetal react, there is an ionic bond formed, which means one of them loses electrons while the other gains them. Since this reaction involves the exchange of electrons it is termed as a redox reaction. The oxidation states in a metal- nonmetal are simple to determine because they are given oxidation states similar to their charges. However, when two nonmetals react; the situation is a bit more complex. As all nonmetals have similarly high electronegativity values, it is unreasonable to assume that there will be a transfer of electrons between them in an oxidation-reduction reaction. In these instances the valence electrons are transferred moving closer to that atom which has the higher …show more content…
Observe what happens when magnesium metal is placed in 1.0 M HCl solution. 2. Observe what happens when zinc metal is placed in 1.0 M copper nitrate solution. 3. Observe what happens when copper metal is placed in zinc nitrate solution. 4. Observe whether 0.1 M iron (III) chloride solution or iron (II) sulfate decolorize when added to 0.1 M potassium permanganate. 5. Add drops of potassium permanganate to the solution that changed color in the previous step. Record how many drops were added until the purple color of the ion no longer changed. 6. Observe color changes when sodium iodide solution is reacted with chlorine water and bromine water (separately). 7. Observe color changes when sodium bromide solution is reacted with chlorine water and iodine solution (separately). 8. Observe what happens when 3M sulfuric acid and potassium permanganate are added to hydrogen peroxide antiseptic. Observe what happens when potassium permanganate is added to hydrogen peroxide
Determine which kinds of reactions involve electron transfer as the driving force.
Background
Redox (reduction-oxidation) reactions include all chemical reactions in which atoms have their oxidation state changed. So, when a metal and a nonmetal react, there is an ionic bond formed, which means one of them loses electrons while the other gains them. Since this reaction involves the exchange of electrons it is termed as a redox reaction. The oxidation states in a metal- nonmetal are simple to determine because they are given oxidation states similar to their charges. However, when two nonmetals react; the situation is a bit more complex. As all nonmetals have similarly high electronegativity values, it is unreasonable to assume that there will be a transfer of electrons between them in an oxidation-reduction reaction. In these instances the valence electrons are transferred moving closer to that atom which has the higher …show more content…
Observe what happens when magnesium metal is placed in 1.0 M HCl solution. 2. Observe what happens when zinc metal is placed in 1.0 M copper nitrate solution. 3. Observe what happens when copper metal is placed in zinc nitrate solution. 4. Observe whether 0.1 M iron (III) chloride solution or iron (II) sulfate decolorize when added to 0.1 M potassium permanganate. 5. Add drops of potassium permanganate to the solution that changed color in the previous step. Record how many drops were added until the purple color of the ion no longer changed. 6. Observe color changes when sodium iodide solution is reacted with chlorine water and bromine water (separately). 7. Observe color changes when sodium bromide solution is reacted with chlorine water and iodine solution (separately). 8. Observe what happens when 3M sulfuric acid and potassium permanganate are added to hydrogen peroxide antiseptic. Observe what happens when potassium permanganate is added to hydrogen peroxide