identify the atoms that are being oxidized and reduced..
2FeCl3 + 2KI --> 2FeCl2 + 2KCl + I2
Isn't Fe going from +3 to +2, and gained an electron to do that?
Isn't I going from -1 to zero, losing an electron in the process?
Yes. It is.
To identify the atoms that are being oxidized and reduced, we need to determine the changes in oxidation states of each element in the reaction:
2FeCl3 + 2KI --> 2FeCl2 + 2KCl + I2
In FeCl3, iron (Fe) has an oxidation state of +3, and in FeCl2, it has an oxidation state of +2. This indicates that iron is being reduced from an oxidation state of +3 to +2.
In KI, iodine (I) has an oxidation state of -1, and in I2, it has an oxidation state of 0. This implies that iodine is being oxidized from an oxidation state of -1 to 0.
Therefore, iron is being reduced, and iodine is being oxidized in this reaction.
To identify the atoms being oxidized and reduced in a chemical reaction, you need to determine the changes in oxidation numbers.
Here's how you can figure out which atoms are being oxidized and reduced in the given reaction:
1. Write down the oxidation numbers for each atom in the reaction.
Fe: +3 in FeCl3, +2 in FeCl2 (reduced)
Cl: -1 in FeCl3, -1 in FeCl2 (no change)
I: -1 in KI, 0 in I2 (oxidized)
K: +1 in KI, +1 in KCl (no change)
2. Compare the initial oxidation numbers to the final oxidation numbers.
The element that has a decrease in its oxidation number is being reduced, and the element that has an increase in its oxidation number is being oxidized.
Therefore, in the given reaction:
- Iron (Fe) is being reduced from +3 in FeCl3 to +2 in FeCl2.
- Iodine (I) is being oxidized from -1 in KI to 0 in I2.
In summary:
- The iron atoms are being reduced.
- The iodine atoms are being oxidized.