During this project we made our own battery. We used copper, zinc, and a couple pieces of cardboard cut in the shape of the penny and let it soaked in vinegar. After letting the pieces soak for a little, we stacked all of them together. Each cell we stacked added onto to the overall charge of the battery. When these things are in contact all together, with the electrolyte solution, Each metal forms positive ions. However zinc loses electrons more easily causing them to travel to the copper ions. Therefore the electrons transfer from the zinc to the copper.
Looking Back:
At first, our experiment didn't work. We asked another table if they could figure out why it wasn't working and what we did wrong. Turns out we had everything stacked in the wrong order. After we rearranged everything, it eventually worked out very well. We were able to construct a functional battery that gives powers to an LED light. First we had to sand down one side of a penny to expose the zinc and leave the other side of the penny alone because we needed it to have copper. We then put the copper side down, the zinc side up and the soaked cardboard that was in vinegar and placed it on top of the copper and repeated the stacking process seven more times. Then we tested the battery by trying to light up an LED light and it worked! This is because electrons flow from the zinc through the soaked cardboard to the copper.The reason why we repeatedly stacked the materials was so that the overall charge of the battery could increase which strengthens the battery.
Looking Beyond:
In order to make the battery and make sure it works, there needs to be zinc, copper, and a source of electrolytes. This is because when an atom that can lose electrons easier than an atom from a different element make contact, the electrons transfer. Just like how in the experiment, when in contact with the electrolyte solution (vinegar), the zinc loses its electrons easier so they transfer to the copperions. This illustrates the concept of oxidation and reduction. Oxidation is the loss of electrons while reduction is the gaining of electrons. In this case, the zinc goes through oxidation while the copper goes through reduction.
Looking Inward:
I believe my group got the desirable results that we had planned because we had great teamwork and good understanding of what we had to do. I worked with Morgan, Ivy, and Daisy. We all knew what to do and communicated very well. I believe I did well in this project and contributed a good amount to the success in the group as well as the others.
Looking Forward:
If I were to do this project again, I would probably use the concrete instead of sand paper to sand the penny because it's a lot faster. When we were inside to try to sand the pennies, it was slow and not as effective as when we went outside and sanded the pennies for a couple minutes. Other than that I wouldn't change anything.
Take Away:
This experiment taught me more about utilizing metals. I never new you could make a battery out of pennies and cardboard! It was interesting to make a battery without any wires besides the LED light. I also didn't know that under a pennies shiny coating was a metallic like substance, I always thought that pennies were just pure copper.
Looking Back:
At first, our experiment didn't work. We asked another table if they could figure out why it wasn't working and what we did wrong. Turns out we had everything stacked in the wrong order. After we rearranged everything, it eventually worked out very well. We were able to construct a functional battery that gives powers to an LED light. First we had to sand down one side of a penny to expose the zinc and leave the other side of the penny alone because we needed it to have copper. We then put the copper side down, the zinc side up and the soaked cardboard that was in vinegar and placed it on top of the copper and repeated the stacking process seven more times. Then we tested the battery by trying to light up an LED light and it worked! This is because electrons flow from the zinc through the soaked cardboard to the copper.The reason why we repeatedly stacked the materials was so that the overall charge of the battery could increase which strengthens the battery.
Looking Beyond:
In order to make the battery and make sure it works, there needs to be zinc, copper, and a source of electrolytes. This is because when an atom that can lose electrons easier than an atom from a different element make contact, the electrons transfer. Just like how in the experiment, when in contact with the electrolyte solution (vinegar), the zinc loses its electrons easier so they transfer to the copperions. This illustrates the concept of oxidation and reduction. Oxidation is the loss of electrons while reduction is the gaining of electrons. In this case, the zinc goes through oxidation while the copper goes through reduction.
Looking Inward:
I believe my group got the desirable results that we had planned because we had great teamwork and good understanding of what we had to do. I worked with Morgan, Ivy, and Daisy. We all knew what to do and communicated very well. I believe I did well in this project and contributed a good amount to the success in the group as well as the others.
Looking Forward:
If I were to do this project again, I would probably use the concrete instead of sand paper to sand the penny because it's a lot faster. When we were inside to try to sand the pennies, it was slow and not as effective as when we went outside and sanded the pennies for a couple minutes. Other than that I wouldn't change anything.
Take Away:
This experiment taught me more about utilizing metals. I never new you could make a battery out of pennies and cardboard! It was interesting to make a battery without any wires besides the LED light. I also didn't know that under a pennies shiny coating was a metallic like substance, I always thought that pennies were just pure copper.