Fe show on oxidation state of +1 in:

Options

A. `Fe(CO)_(5)`
B. `[Fe(H_(2)O)_(5)NO]SO_(4)`
C. `Fe_(4)[Fe(CN)_(6)]_(3)`
D. `Fe_(4)Cl_(4)^(-)`

Answer

To determine in which compound iron (Fe) shows an oxidation state of +1, we can analyze various compounds of iron and calculate the oxidation state in each case.

### Step-by-Step Solution:

**Step 1: Analyze the compound FeCO5**
- In FeCO5, the oxidation state of the carbonyl group (CO) is 0.
- Let the oxidation state of iron be \( x \).
- The total oxidation state for the compound is \( x + 5(0) = x \).
- Since CO is neutral, the oxidation state of Fe in FeCO5 is 0.
- Therefore, Fe does not show +1 oxidation state in this compound.

**Step 2: Analyze the compound FeH2O5**
- In FeH2O5, we need to consider the oxidation states of water (H2O) and other components.
- The oxidation state of water is 0.
- Let the oxidation state of iron be \( x \).
- The total oxidation state for the compound is \( x + 5(0) = x \).
- Therefore, we cannot conclude the oxidation state of Fe in this compound directly.

**Step 3: Analyze the compound NO+**
- In NO+, the oxidation state of nitrogen (N) is +2.
- Let the oxidation state of iron be \( x \).
- The total oxidation state for the compound is \( x + 2 = +1 \).
- Rearranging gives \( x = +1 - 2 = -1 \).
- This indicates that Fe does not show +1 oxidation state in this compound.

**Step 4: Analyze the compound FeSO4**
- In FeSO4, the oxidation state of sulfate (SO4) is -2.
- Let the oxidation state of iron be \( x \).
- The total oxidation state for the compound is \( x + (-2) = 0 \).
- Rearranging gives \( x = +2 \).
- Therefore, Fe does not show +1 oxidation state in this compound either.

**Step 5: Conclusion**
- After analyzing the compounds FeCO5, FeH2O5, NO+, and FeSO4, we find that iron shows an oxidation state of +1 in the compound **FeH2O5**.

### Final Answer:
Iron (Fe) shows an oxidation state of +1 in the compound **FeH2O5**.