To determine what is getting oxidized in the reaction:
[tex]\[ Fe + Cu(NO_3)_2 \rightarrow Cu + Fe(NO_3)_2 \][/tex]
we need to examine the changes in the oxidation states of the elements involved.
1. Assign the initial oxidation states:
- For iron (Fe) in its solid form (left-hand side), the oxidation state is 0.
- For copper (Cu) in [tex]\( Cu(NO_3)_2 \)[/tex], the copper is in the [tex]\( Cu^{2+} \)[/tex] form, so its oxidation state is +2.
2. Assign the final oxidation states:
- For iron (Fe) in [tex]\( Fe(NO_3)_2 \)[/tex], iron is in the [tex]\( Fe^{2+} \)[/tex] form, so its oxidation state is +2.
- For copper (Cu) in its solid form (right-hand side), the oxidation state is 0.
3. Calculate the changes in oxidation states:
- For iron (Fe): The oxidation state changes from 0 to +2.
[tex]\[ \text{Change in oxidation state for } \text{Fe} = +2 - 0 = +2 \][/tex]
- For copper (Cu): The oxidation state changes from +2 to 0.
[tex]\[ \text{Change in oxidation state for } \text{Cu} = 0 - (+2) = -2 \][/tex]
4. Identify the species being oxidized:
- Oxidation involves an increase in oxidation state.
- For iron (Fe), the oxidation state increases from 0 to +2, which means iron is getting oxidized.
- For copper (Cu), the oxidation state decreases from +2 to 0, which means copper is getting reduced.
Therefore, iron (Fe) is the species that is getting oxidized in the reaction.
