Question:
Define the coordination number and oxidation state of the central metal ion in \([Co(NH_3)_6]Cl_3\).
Define the coordination number and oxidation state of the central metal ion in \([Co(NH_3)_6]Cl_3\).
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Neutral ligands such as \(NH_3\), \(H_2O\), and \(CO\) contribute zero charge when calculating oxidation states in coordination compounds.
Updated On: Apr 16, 2026
- Coordination number = 4, Oxidation state = +2
- Coordination number = 6, Oxidation state = +3
- Coordination number = 6, Oxidation state = +2
- Coordination number = 3, Oxidation state = +3
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The Correct Option is B
Solution and Explanation
Concept:
• Coordination number is the number of ligand donor atoms directly bonded to the central metal ion.
• Oxidation state of the central metal ion is calculated using the overall charge of the complex and the charges of the ligands.
Step 1: Determine the coordination number. In the complex ion: \[ [Co(NH_3)_6]^{3+} \] There are six \(NH_3\) ligands attached to the cobalt atom. Since each \(NH_3\) acts as a monodentate ligand, the coordination number is \[ \boxed{6} \]
Step 2: Determine the oxidation state of cobalt. Ammonia \((NH_3)\) is a neutral ligand, so it contributes 0 charge. Let the oxidation state of cobalt be \(x\). \[ x + 6(0) = +3 \] \[ x = +3 \] Thus, the oxidation state of cobalt is \[ \boxed{+3} \]
• Coordination number is the number of ligand donor atoms directly bonded to the central metal ion.
• Oxidation state of the central metal ion is calculated using the overall charge of the complex and the charges of the ligands.
Step 1: Determine the coordination number. In the complex ion: \[ [Co(NH_3)_6]^{3+} \] There are six \(NH_3\) ligands attached to the cobalt atom. Since each \(NH_3\) acts as a monodentate ligand, the coordination number is \[ \boxed{6} \]
Step 2: Determine the oxidation state of cobalt. Ammonia \((NH_3)\) is a neutral ligand, so it contributes 0 charge. Let the oxidation state of cobalt be \(x\). \[ x + 6(0) = +3 \] \[ x = +3 \] Thus, the oxidation state of cobalt is \[ \boxed{+3} \]
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