All alkali metals dissolve in anhydrous liquid ammonia to give blue colour solution. It is the ammoniated electron which is reponsible for the blue colour of the solution, and the electrical conductivity is due to the ammoniated cation, `[M(NH_(3))_(x)]^(+)` as well as the ammoniated electron,` [e(NH_(3))_(y)]^(-)`, value of x and y depend on the extent of solvation by `NH_(3)`. Dilute solutions are paramagnetic due to free ammoniated electrons.
Q. Which of the following statement about solution of alkali metals in liquid ammonia is correct?

Options

A. The solution have strong oxidizing properties
B. Both the dil. Solution as well as conc. Solution are equally paramagnetic in nature
C. Charge transfer is responsible for the colour of the solution
D. None of these

Explanation

To solve the question regarding the properties of alkali metals in liquid ammonia, we will analyze the information provided and evaluate the statements based on the properties of the solution.

### Step-by-Step Solution:

1. **Understanding the Reaction**:
- Alkali metals (like sodium, potassium, etc.) dissolve in anhydrous liquid ammonia. This process leads to the formation of an ammoniated cation, represented as `[M(NH₃)ₓ]⁺`, and an ammoniated electron, represented as `[e(NH₃)ᵧ]⁻`. The values of x and y depend on the extent of solvation by ammonia.

**Hint**: Recognize that the alkali metal interacts with ammonia to form a complex ion and an electron.

2. **Color of the Solution**:
- The blue color of the solution is attributed to the presence of the ammoniated electron. This electron is free and contributes to the color observed in the solution.

**Hint**: Remember that the color is linked to the presence of free electrons in the solution.

3. **Electrical Conductivity**:
- The electrical conductivity of the solution arises from both the ammoniated cation and the ammoniated electron. The ammoniated electron is responsible for the conductivity due to its mobility.

**Hint**: Consider how charged species contribute to conductivity in a solution.

4. **Paramagnetism**:
- Dilute solutions of alkali metals in liquid ammonia are paramagnetic due to the presence of free ammoniated electrons. This means they have unpaired electrons, which is a characteristic of paramagnetic substances.

**Hint**: Recall that paramagnetism is linked to unpaired electrons.

5. **Evaluating the Statements**:
- **Statement 1**: "Solutions have strong oxidizing properties."
- This is **false**. Alkali metals in ammonia exhibit reducing properties due to the presence of free electrons.

- **Statement 2**: "Dilute solution as well as concentrated solution are equally paramagnetic in nature."
- This is **false**. While dilute solutions are paramagnetic due to free electrons, concentrated solutions may behave differently due to interactions between ions.

- **Statement 3**: "Charge transfer is responsible for the color of the solution."
- This is **false**. The blue color is due to the presence of the ammoniated electron, not charge transfer.

6. **Conclusion**:
- Since all the statements provided are false, the correct answer to the question is "None of these."

### Final Answer:
None of the statements about the solution of alkali metals in liquid ammonia is correct.