According to the data above, it is evident that not all metals share the same amount of reactivity. Some metals are reluctant to give up their electrons while others go out of there way to part ways with the negative particles. This causes metals to fall in different levels on the reduction and oxidation spectrum of the reactivity chart. The chart below shows the levels of reactivity of metals and non-metals to go through reduction highest to lowest, lowest to highest shows oxidation.
This lab contained both single and redox reactions for every single reaction that took place. Single replacement is when a single cation replaces another cation. Ex:
Redox equations are simply reactions that transfer electrons from one substance to another. Single Replacement reactions can also be redox reactions, as electrons can be transferred when the replacement of cations happens.
Of the metals tested These were the most theoretically :
- Magnesium (reduction potential: -2.37)
- Zinc (reduction potential: -0.76)
- Iron (reduction potential: -0.44)
- Copper (reduction potential: 0.15)
- Silver (reduction potential: 0.80)
The correlation between the rankings and their reduction potentials are appropriate. This is because all reactions these metals were included in they were being oxidized, meaning they lost electrons. So the metals with the negative reduction potential are more likely to react in a oxidation reaction than the numbers with the positive reduction potentials. The metals with the higher reduction potentials are more likely to react in a reduction reaction while the lower numbers less likely.