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In the given unbalanced reaction Fe^(+2)...

In the given unbalanced reaction
`Fe^(+2)+Cr_2O_7rarrFe^(+3)+Cr^(+3)` which atoms /groups is /are oxidised?

A

Fe

B

`Cr_2O_7`

C

Cr

D

all of these

Text Solution

AI Generated Solution

The correct Answer is:
To determine which atoms or groups are oxidized in the reaction \( \text{Fe}^{+2} + \text{Cr}_2\text{O}_7^{2-} \rightarrow \text{Fe}^{+3} + \text{Cr}^{+3} \), we need to analyze the changes in oxidation states of the elements involved. ### Step 1: Identify the oxidation states of each element in the reactants and products. - In the reactants: - \( \text{Fe}^{+2} \) has an oxidation state of +2. - In \( \text{Cr}_2\text{O}_7^{2-} \), each chromium (Cr) has an oxidation state of +6 (since the overall charge is -2 and there are 7 oxygen atoms each with an oxidation state of -2). - In the products: - \( \text{Fe}^{+3} \) has an oxidation state of +3. - \( \text{Cr}^{+3} \) has an oxidation state of +3. ### Step 2: Determine the changes in oxidation states. - For iron (Fe): - It changes from +2 to +3, indicating that it has lost one electron. This loss of electrons signifies that iron is being oxidized. - For chromium (Cr): - It changes from +6 in \( \text{Cr}_2\text{O}_7^{2-} \) to +3 in \( \text{Cr}^{+3} \), indicating that it has gained electrons. This gain of electrons signifies that chromium is being reduced. ### Step 3: Conclusion on oxidation. From the analysis, we conclude that: - The atom that is oxidized in this reaction is **iron (Fe)**, as it goes from an oxidation state of +2 to +3, losing electrons in the process. ### Final Answer: **Iron (Fe) is the atom that is oxidized.** ---
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