In solution, the complex, `[Pt(NH_3)_6]Cl_4` gives

Options

A. 4 ions
B. 3 ions
C. 2 ions
D. 5 ions

Answer

To solve the question regarding the complex `[Pt(NH₃)₆]Cl₄`, we need to determine what ions this complex gives in solution.

### Step-by-Step Solution:

1. **Identify the Complex**: The complex is `[Pt(NH₃)₆]Cl₄`. This indicates that we have a platinum ion coordinated with six ammonia ligands and four chloride ions.

2. **Determine the Coordination Number**: The coordination number of platinum in this complex is 6, which is the number of ligands (NH₃) attached to the platinum ion.

3. **Determine the Oxidation State of Platinum**:
- Ammonia (NH₃) is a neutral ligand, contributing 0 to the overall charge.
- The chloride ions (Cl⁻) are negatively charged.
- The overall charge of the complex can be calculated as follows:
- Let the oxidation state of platinum be x.
- The contribution from 6 NH₃ ligands is 0.
- The contribution from 4 Cl⁻ ions is -4.
- Therefore, the equation becomes:
\[ x + 0 - 4 = 0 \]
Simplifying this gives:
\[ x - 4 = 0 \implies x = +4 \]
- Thus, the oxidation state of platinum in this complex is +4.

4. **Determine the Ions Produced in Solution**:
- When `[Pt(NH₃)₆]Cl₄` dissolves in solution, it dissociates into its constituent ions.
- The complex ion `[Pt(NH₃)₆]^{4+}` remains intact, while the chloride ions dissociate.
- Therefore, the dissociation can be represented as:
\[ [Pt(NH₃)₆]Cl₄ \rightarrow [Pt(NH₃)₆]^{4+} + 4Cl^{-} \]
- This means that one complex ion and four chloride ions are produced.

5. **Conclusion**: The complex `[Pt(NH₃)₆]Cl₄` gives a total of 5 ions in solution: one complex ion and four chloride ions.

### Final Answer:
The complex `[Pt(NH₃)₆]Cl₄` gives 5 ions in solution: one `[Pt(NH₃)₆]^{4+}` ion and four `Cl⁻` ions.