Question:
Statement I: \( \mathrm{ClO_4^-} \), \( \mathrm{ICl_4^-} \), \( \mathrm{IBr_2^-} \) are tetrahedral, square planar and linear respectively.
Statement II: \( \left[\mathrm{Fe(CN)_6}\right]^{4-} \) is \( \mathrm{d^2sp^3} \) hybridized.
Statement I: \( \mathrm{ClO_4^-} \), \( \mathrm{ICl_4^-} \), \( \mathrm{IBr_2^-} \) are tetrahedral, square planar and linear respectively.
Statement II: \( \left[\mathrm{Fe(CN)_6}\right]^{4-} \) is \( \mathrm{d^2sp^3} \) hybridized.
Statement II: \( \left[\mathrm{Fe(CN)_6}\right]^{4-} \) is \( \mathrm{d^2sp^3} \) hybridized.
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In coordination chemistry, the geometry of a complex can be predicted based on the number of ligands and their arrangement around the central metal atom. The hybridization of the central atom is determined by the geometry of the complex.
Updated On: Apr 7, 2026
- Both Statement I and Statement II are correct
- Statement I is correct but Statement II is incorrect
- Statement I is incorrect but Statement II is correct
- Both Statement I and Statement II are incorrect
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The Correct Option is A
Solution and Explanation
Step 1: Analyze Statement I.
- \( \mathrm{ClO_4^-} \) has a tetrahedral structure. This is because the central chlorine atom is surrounded by four oxygen atoms with bond angles of approximately 109.5°, which is characteristic of a tetrahedral geometry.
- \( \mathrm{ICl_4^-} \) has a square planar structure. The iodine atom in this complex is surrounded by four chlorine atoms with 90° bond angles, which results in a square planar geometry.
- \( \mathrm{IBr_2^-} \) has a linear structure. This is due to the two bromine atoms bonded to the iodine atom, with bond angles of 180°, leading to a linear geometry.
Thus, Statement I is correct.
Step 2: Analyze Statement II.
\( \left[\mathrm{Fe(CN)_6}\right]^{4-} \) is a coordination complex with iron in the +2 oxidation state. The iron ion \( \mathrm{Fe^{2+}} \) has a \( \mathrm{d^6} \) electron configuration. In the presence of six cyanide ligands, the complex undergoes hybridization to form six bonds, resulting in an \( \mathrm{d^2sp^3} \) hybridization. This is because the iron ion uses two \( d \)-orbitals, one \( s \)-orbital, and three \( p \)-orbitals to form six bonds in an octahedral geometry. Therefore, Statement II is also correct.
Step 3: Conclusion.
Since both Statement I and Statement II are correct, the correct answer is option (A).
Final Answer: Both Statement I and Statement II are correct.
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