The oxidation number of Fe in brown ring `[Fe(H_(2)O_(3))_(5)NO]^(2+)` is

Options

A. 0
B. `+1`
C. `+2`
D. `+3`

Explanation

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

### Step 1: Identify the components of the complex
The complex consists of:
- Iron (Fe)
- Five water molecules \((H_2O)\)
- One nitrosonium ion \((NO)\)

### Step 2: Assign oxidation numbers to known components
- The oxidation number of water \((H_2O)\) is 0 because it is a neutral molecule.
- The nitrosonium ion \((NO)\) has an oxidation number of +1.

### Step 3: Set up the equation
Let the oxidation number of iron be \(X\). The overall charge of the complex is +2. Therefore, we can set up the equation based on the sum of the oxidation numbers:

\[ X + (5 \times 0) + (+1) = +2 \]

### Step 4: Simplify the equation
This simplifies to:
\[ X + 0 + 1 = 2 \]
\[ X + 1 = 2 \]

### Step 5: Solve for \(X\)
Now, solve for \(X\):
\[ X = 2 - 1 \]
\[ X = +1 \]

### Conclusion
The oxidation number of iron (Fe) in the complex \([Fe(H_2O)_5NO]^{2+}\) is +1.

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