Which of the following statements is wrong for the solution of alkali metals in liquids ammonia`

Options

A. They are deep blue coloured solutions.
B. They are highly conducting in nature.
C. They are diamagnetic in nature.
D. Ammoniated cation and solvated electron are formed in the solution.

Explanation

To determine which statement is wrong regarding the solution of alkali metals in liquid ammonia, we can analyze the properties of these solutions step by step.

### Step-by-Step Solution:

1. **Understanding the Solubility of Alkali Metals in Liquid Ammonia:**
- Alkali metals (like sodium, potassium, etc.) are soluble in liquid ammonia. When an alkali metal (M) is added to liquid ammonia, it dissolves.

**Hint:** Remember that alkali metals react with ammonia to form solutions.

2. **Formation of Ammoniated Cations and Solvated Electrons:**
- In the solution, alkali metals form ammoniated cations, represented as \( M^+ \cdot nNH_3 \) (where \( n \) is the number of ammonia molecules coordinated to the cation). Along with this, solvated electrons are also produced.

**Hint:** Focus on the types of particles formed when alkali metals dissolve in ammonia.

3. **Color of the Solution:**
- The solution of alkali metals in liquid ammonia appears deep blue due to the presence of solvated electrons. These electrons absorb light in the red region of the spectrum and emit light in the blue region.

**Hint:** Consider how the color of a solution can indicate the presence of certain particles.

4. **Electrical Conductivity:**
- The presence of solvated electrons makes the solution a good conductor of electricity. This is because the free electrons can move and carry charge.

**Hint:** Think about how the movement of charged particles relates to conductivity.

5. **Magnetic Properties:**
- The presence of unpaired electrons in the solvated electrons makes the solution paramagnetic. Therefore, the statement claiming that the solution is diamagnetic is incorrect.

**Hint:** Recall the relationship between unpaired electrons and magnetic properties.

6. **Evaluating the Statements:**
- Based on the above analysis:
- Statement A: "They are deep blue color solutions" - True
- Statement B: "They are highly conducting in nature" - True
- Statement C: "They are diamagnetic in nature" - False (this is the wrong statement)
- Statement D: "Ammoniated cation and solvated electrons are formed in the solution" - True

### Conclusion:
The wrong statement regarding the solution of alkali metals in liquid ammonia is **C: "They are diamagnetic in nature."**