In the complex ion `[Fe(H_(2)O)_(5)NO]^(2+)`

Options

A. Fe is in the `=2` oxidation state and NO coordinates as `NO^(+)`
B. Fe is in the `+3` oxidation state and NO coordinates as `NO^(-)`
C. Fe is in the `+2` oxidation state and NO coordinates as neutral NO (nitrosyl) radical
D. Fe is in the `+1` oxidation state and NO coordinates as `NO^(+)` (nitrosonium ion)

Explanation

To determine the oxidation states of iron and nitric oxide in the complex ion \([Fe(H_2O)_5NO]^{2+}\), we can follow these steps:

### Step 1: Identify the components of the complex
The complex ion consists of:
- Iron (Fe)
- Five water molecules (H2O)
- One nitric oxide molecule (NO)

### Step 2: Determine the oxidation state of water
Water (H2O) is a neutral ligand, meaning it does not contribute to the overall charge of the complex. Therefore, the oxidation state of each water molecule is 0.

### Step 3: Determine the oxidation state of nitric oxide
Nitric oxide (NO) is also a neutral ligand in this context. It does not contribute to the overall charge of the complex either. Therefore, the oxidation state of NO is also 0.

### Step 4: Write the equation for the overall charge
The overall charge of the complex ion is +2. We can express this mathematically:
\[ \text{Charge of Fe} + \text{Charge from 5 H2O} + \text{Charge from NO} = +2 \]
Since both H2O and NO are neutral, we have:
\[ \text{Charge of Fe} + 0 + 0 = +2 \]

### Step 5: Solve for the oxidation state of iron
From the equation above, we can deduce:
\[ \text{Charge of Fe} = +2 \]
Thus, the oxidation state of iron in this complex is +2, which is referred to as ferrous (Fe²⁺).

### Step 6: Conclusion
The oxidation states are:
- Iron (Fe) = +2 (ferrous)
- Nitric oxide (NO) = 0 (as a neutral ligand)

### Final Answer
The oxidation state of iron in \([Fe(H_2O)_5NO]^{2+}\) is +2, and the oxidation state of nitric oxide is 0.

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