Which of the following is non-conducting?

Options

A. `CoCl_(3).6NH_(3)`
B. `CoCl_(3).5NH_(3)`
C. `CoCl_(3).4NH_(3)`
D. `CoCl_(3).3NH_(3)`

Answer

To determine which of the given coordination complexes is non-conducting, we need to analyze the complexes based on their composition and the presence of ions. Here’s a step-by-step solution:

### Step 1: Identify the Coordination Complexes
The coordination complexes provided are:
1. \( \text{Co(NH}_3\text{)}_6\text{Cl}_3 \)
2. \( \text{Co(NH}_3\text{)}_5\text{Cl}_2 \)
3. \( \text{Co(NH}_3\text{)}_4\text{Cl} \)
4. \( \text{Co(NH}_3\text{)}_3\text{Cl}_3 \)

### Step 2: Understand the Structure
In coordination complexes:
- The central metal atom (in this case, cobalt) is surrounded by ligands (NH3 and Cl).
- The ligands can be neutral (like NH3) or negatively charged (like Cl).
- The counter ions (Cl) are outside the coordination sphere.

### Step 3: Determine the Ionization
When these complexes dissolve in solution, they can dissociate into ions:
1. \( \text{Co(NH}_3\text{)}_6\text{Cl}_3 \) → \( \text{Co(NH}_3\text{)}_6^{3+} + 3\text{Cl}^- \) (produces ions)
2. \( \text{Co(NH}_3\text{)}_5\text{Cl}_2 \) → \( \text{Co(NH}_3\text{)}_5^{2+} + 2\text{Cl}^- \) (produces ions)
3. \( \text{Co(NH}_3\text{)}_4\text{Cl} \) → \( \text{Co(NH}_3\text{)}_4^{+} + \text{Cl}^- \) (produces ions)
4. \( \text{Co(NH}_3\text{)}_3\text{Cl}_3 \) → \( \text{Co(NH}_3\text{)}_3^{3+} + 3\text{Cl}^- \) (produces ions)

### Step 4: Identify Non-Conducting Complex
A non-conducting complex is one that does not produce ions when dissolved in solution. This means it does not dissociate into charged particles.

From the analysis:
- The first three complexes produce ions when they dissociate.
- The fourth complex, \( \text{Co(NH}_3\text{)}_3\text{Cl}_3 \), has no ionization sphere, meaning it does not dissociate into ions.

### Conclusion
Thus, the non-conducting coordination complex is:
**\( \text{Co(NH}_3\text{)}_3\text{Cl}_3 \)**