`[Cr(CN)_(6)][Co(NH_(3))_(6)]` contains

Options

A. Cationic complex
B. Anionic complex
C. Neutral ligands
D. Anionic ligands

Answer

To analyze the coordination compound \([Cr(CN)_{6}][Co(NH_{3})_{6}]\), we will break it down step by step.

### Step 1: Identify the components of the complex
The given complex is made up of two parts: \([Cr(CN)_{6}]\) and \([Co(NH_{3})_{6}]\).

### Step 2: Determine the charge of each complex
1. **For \([Cr(CN)_{6}]\)**:
- The cyanide ion (CN) has a charge of -1.
- Since there are 6 cyanide ions, the total negative charge contributed by CN is \(6 \times (-1) = -6\).
- To balance this charge, chromium must have an oxidation state of +3 (since -6 + 3 = -3, which is the overall charge of the complex).
- Therefore, \([Cr(CN)_{6}]\) has a charge of -3.

2. **For \([Co(NH_{3})_{6}]\)**:
- Ammonia (NH3) is a neutral ligand, contributing no charge.
- Therefore, cobalt must have an oxidation state of +3 to balance the overall charge of the complex.
- Hence, \([Co(NH_{3})_{6}]\) has a charge of +3.

### Step 3: Identify the overall charge of the coordination compound
The overall coordination compound is neutral because it consists of a cationic complex \([Co(NH_{3})_{6}]^{3+}\) and an anionic complex \([Cr(CN)_{6}]^{3-}\).

### Step 4: Classify the ligands
- **Cyanide (CN)**: This is an anionic ligand because it carries a negative charge.
- **Ammonia (NH3)**: This is a neutral ligand because it carries no charge.

### Conclusion
Based on the analysis:
- The complex contains both cationic and anionic components.
- It has both neutral ligands (NH3) and anionic ligands (CN).

### Final Answer
The coordination compound \([Cr(CN)_{6}][Co(NH_{3})_{6}]\) contains:
- Cationic complex: Yes
- Anionic complex: Yes
- Neutral ligands: Yes
- Anionic ligands: Yes