Question:
In the coordination complex, Potassium hexacyanoferrate(II), the central atom/ion acts as,
In the coordination complex, Potassium hexacyanoferrate(II), the central atom/ion acts as,
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The central metal accepts lone pairs from ligands.
Updated On: Oct 1, 2026
- Bronsted-Lowry acid
- Lewis base
- Lewis acid
- Bronsted-Lowry base
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The Correct Option is C
Solution and Explanation
Step 1: Understanding the Concept:
In a coordination complex, the central metal ion accepts electron pairs from ligands into its empty orbitals. A species that accepts an electron pair is a Lewis acid.
Step 2: Apply:
Potassium hexacyanoferrate(II) is \(K_4[Fe(CN)_6]\). The central ion is \(Fe^{2+}\), which has empty \(d\), \(s\) and \(p\) orbitals. Each \(CN^-\) ligand donates a lone pair to \(Fe^{2+}\).
Step 3: Conclusion:
So \(Fe^{2+}\) is the electron pair acceptor, a Lewis acid, option (C). The ligands are Lewis bases. Bronsted-Lowry acid or base would involve proton transfer, which does not happen here.
Final Answer:
The metal ion accepts electron pairs, so it is a Lewis acid. \[ \boxed{C:\ \text{Lewis acid}} \]
In a coordination complex, the central metal ion accepts electron pairs from ligands into its empty orbitals. A species that accepts an electron pair is a Lewis acid.
Step 2: Apply:
Potassium hexacyanoferrate(II) is \(K_4[Fe(CN)_6]\). The central ion is \(Fe^{2+}\), which has empty \(d\), \(s\) and \(p\) orbitals. Each \(CN^-\) ligand donates a lone pair to \(Fe^{2+}\).
Step 3: Conclusion:
So \(Fe^{2+}\) is the electron pair acceptor, a Lewis acid, option (C). The ligands are Lewis bases. Bronsted-Lowry acid or base would involve proton transfer, which does not happen here.
Final Answer:
The metal ion accepts electron pairs, so it is a Lewis acid. \[ \boxed{C:\ \text{Lewis acid}} \]
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