Which of the following complex has higher `Delta_(0)` VALUE?

Options

A. `[Fe(H_(2)O)_(6)]^(2+)`
B. `[FeCl_(6)]^(3-)`
C. `[Fe(H_(2)O)_(6)]^(3+)`
D. All have equal

Answer

To determine which complex has a higher Δ₀ (Delta zero) value, we need to analyze the ligands and the overall charge of the complexes involved. Here’s a step-by-step solution:

### Step 1: Identify the Ligands
- The ligands in the complexes are H₂O (water) and Cl⁻ (chloride).
- According to crystal field theory, ligands can be classified as strong or weak. H₂O is considered a stronger ligand compared to Cl⁻.

**Hint:** Remember that stronger ligands typically lead to larger Δ₀ values.

### Step 2: Compare the Ligands
- Since H₂O is a stronger ligand than Cl⁻, the Δ₀ value for complexes containing H₂O will be greater than those containing Cl⁻.

**Hint:** Stronger ligands increase the splitting of d-orbitals, resulting in a higher Δ₀ value.

### Step 3: Analyze the Complexes
- Consider the complexes: Fe(H₂O)₆³⁺ and FeCl₃.
- The complex Fe(H₂O)₆³⁺ has H₂O as the ligand, while FeCl₃ has Cl⁻ as the ligand.

**Hint:** Look at the ligands present in each complex to assess their strength.

### Step 4: Consider the Charge of the Complexes
- The charge on the complex also affects the Δ₀ value. A higher charge on the metal ion can lead to a greater Δ₀ value due to increased electrostatic interactions.
- Fe(H₂O)₆³⁺ has a +3 charge, while FeCl₃ typically has a +3 charge as well, but the ligands differ in strength.

**Hint:** Higher charges on the central metal ion can enhance the Δ₀ value.

### Step 5: Conclusion
- Since Fe(H₂O)₆³⁺ contains the stronger ligand H₂O, it will have a higher Δ₀ value compared to FeCl₃, which contains the weaker ligand Cl⁻.
- Therefore, the complex with the higher Δ₀ value is **Fe(H₂O)₆³⁺**.

**Final Answer:** Fe(H₂O)₆³⁺ has the higher Δ₀ value.