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What is the oxidation number of iron in ...

What is the oxidation number of iron in the brown ring complex compound ?

A

0

B

1

C

`+2`

D

`+3`

Text Solution

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The correct Answer is:
To determine the oxidation number of iron (Fe) in the brown ring complex compound, we can follow these steps: ### Step-by-Step Solution: 1. **Identify the Complex**: The brown ring complex is represented as [Fe(H2O)5(NO)]²⁺. 2. **Assign Oxidation States**: - The oxidation state of the nitrosyl (NO) ligand in this complex is +1. - The oxidation state of water (H2O) is 0 (neutral). 3. **Set Up the Equation**: - Let the oxidation number of iron (Fe) be represented as \( X \). - The overall charge of the complex is +2. 4. **Write the Algebraic Expression**: - The equation can be set up as follows: \[ X + (1 \text{ for NO}) + (5 \times 0 \text{ for H2O}) = +2 \] - This simplifies to: \[ X + 1 = 2 \] 5. **Solve for X**: - Rearranging the equation gives: \[ X = 2 - 1 \] - Therefore: \[ X = +1 \] 6. **Conclusion**: - The oxidation number of iron (Fe) in the brown ring complex is +1.
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