Question:
Identify the most stable oxidation state of iron by following.
Identify the most stable oxidation state of iron by following.
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Fe(III) has the half-filled d5 configuration, which is especially stable.
Updated On: Nov 12, 2026
- \(+2\)
- \(+3\)
- \(+6\)
- \(+4\)
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The Correct Option is B
Solution and Explanation
Step 1: Understanding the Concept
Half-filled subshells have extra stability due to symmetry and exchange energy.
Step 2: Write the configurations
Iron: \([\text{Ar}]3d^{6}4s^{2}\)
\(\text{Fe}^{3+}\): \([\text{Ar}]3d^{5}\), a half-filled \(d\) subshell.
Step 3: Compare the options
\(\text{Fe}^{2+}\) is \(3d^{6}\), and \(+4\) and \(+6\) are rare and unstable.
So \(+3\) is most stable.
Final Answer:
The most stable oxidation state of iron is +3. \[ \boxed{\text{(B) }+3} \]
Half-filled subshells have extra stability due to symmetry and exchange energy.
Step 2: Write the configurations
Iron: \([\text{Ar}]3d^{6}4s^{2}\)
\(\text{Fe}^{3+}\): \([\text{Ar}]3d^{5}\), a half-filled \(d\) subshell.
Step 3: Compare the options
\(\text{Fe}^{2+}\) is \(3d^{6}\), and \(+4\) and \(+6\) are rare and unstable.
So \(+3\) is most stable.
Final Answer:
The most stable oxidation state of iron is +3. \[ \boxed{\text{(B) }+3} \]
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