In the reaction `2FeC1_(2) + SnC1_(2) to 2FeC1_(2) + SnC1_(4)`

Options

A. `Fe^(+1)` reduced to `Fe^(+2)`
B. `Sn^(+2)` is reduced to `Sn^(+1)`
C. `Sn^(+2)` oxidized to `Sn`
D. `Fe^(+1)` gains two electrons

Explanation

To analyze the given chemical reaction and determine the correct statements regarding oxidation and reduction, we can follow these steps:

### Step 1: Write the reaction
The reaction given is:
\[ 2 \text{FeCl}_2 + \text{SnCl}_2 \rightarrow 2 \text{FeCl}_3 + \text{SnCl}_4 \]

### Step 2: Identify the oxidation states
- In \(\text{FeCl}_2\), iron (Fe) has an oxidation state of +2.
- In \(\text{FeCl}_3\), iron (Fe) has an oxidation state of +3.
- In \(\text{SnCl}_2\), tin (Sn) has an oxidation state of +2.
- In \(\text{SnCl}_4\), tin (Sn) has an oxidation state of +4.

### Step 3: Determine changes in oxidation states
- For iron (Fe):
- Changes from +2 (in \(\text{FeCl}_2\)) to +3 (in \(\text{FeCl}_3\)).
- This indicates that iron is losing an electron, which means it is being oxidized.

- For tin (Sn):
- Changes from +2 (in \(\text{SnCl}_2\)) to +4 (in \(\text{SnCl}_4\)).
- This indicates that tin is also losing two electrons, which means it is being oxidized as well.

### Step 4: Identify reduction
- Since oxidation is the loss of electrons, reduction is the gain of electrons.
- In this reaction, there is no species that is being reduced, as both iron and tin are being oxidized.

### Step 5: Conclusion
Based on the analysis, we can conclude:
- Iron (Fe) is oxidized from +2 to +3.
- Tin (Sn) is oxidized from +2 to +4.
- There is no reduction occurring in this reaction.

### Step 6: Correct statement
The correct statement regarding the reaction is that both iron and tin are being oxidized.