The oxidation number of iron in `Fe_3O_4` is

Options

A. ` +2 `
B. `+3`
C. `8/3`
D. `2/3`

Explanation

To determine the oxidation number of iron in the compound \( Fe_3O_4 \), we can follow these steps:

### Step 1: Identify the oxidation states of the known elements
In \( Fe_3O_4 \), we have iron (Fe) and oxygen (O). The oxidation state of oxygen is typically \(-2\).

### Step 2: Set up the equation for the total oxidation state
Since there are 4 oxygen atoms in \( Fe_3O_4 \), the total contribution of oxygen to the oxidation state is:
\[ 4 \times (-2) = -8 \]

### Step 3: Let the oxidation state of iron be \( x \)
Since there are 3 iron atoms in the compound, the total contribution from iron will be:
\[ 3x \]

### Step 4: Write the equation for the overall charge
The overall charge of the compound \( Fe_3O_4 \) is neutral (0). Therefore, we can set up the equation:
\[ 3x + (-8) = 0 \]

### Step 5: Solve for \( x \)
Rearranging the equation gives:
\[ 3x = 8 \]
Now, dividing both sides by 3:
\[ x = \frac{8}{3} \]

### Step 6: Conclusion
The oxidation number of iron in \( Fe_3O_4 \) is \( \frac{8}{3} \).

### Final Answer:
The oxidation number of iron in \( Fe_3O_4 \) is \( \frac{8}{3} \).

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