Alkali metals oxide are obtained by combustion of the metals.Although Na normally gives `Na_2O_2`,it will take up further oxygen at elevated pressure and temperature to form `NaO_2`.The per and superoxides of the heavier alkalies can also be prepared by passing stoichiometric amounts of oxygen into their solution in liquid ammonia.
The different alkali metal oxides can be distinguished by reaction with water.The superoxides reacts with `CO_2` and give oxygen gas.The stability of per and superoxides is based upon that larger cation can stablise larger anion, due to larger lattice energy.
Alkali metals dissolve in liquid ammonia.Dilute solutions are dark blue in colour but as the concentration increases above 3M, the colour changes to copper bronze and the solution acquires the metallic lusture due to the formation of metal ions clusters.The solutions of alkali metals in liquid ammonia are good conductors of electricity due to the presence of ammoniated cations and ammoniated electrons.However, the conductivity decreases as the concentrations increases, since ammoniated electrons and ammoniated cation associate.
Solution of sodium metals in liquid ammonia is strongly reducing
due to the presence of :

Options

A. Sodium hydride
B. Sodium atoms
C. Sodium amide
D. Solvated electrons

Explanation

To solve the question regarding why the solution of sodium metal in liquid ammonia is strongly reducing, we can break down the information provided in the paragraph and the video transcript into a step-by-step analysis.

### Step-by-Step Solution:

1. **Understanding the Context**:
- Alkali metals, when burned, form oxides. Sodium typically forms sodium peroxide (Na₂O₂) and can further react to form sodium superoxide (NaO₂) under specific conditions.
- The stability of peroxides and superoxides is attributed to the ability of larger cations to stabilize larger anions due to lattice energy considerations.

**Hint**: Remember that the stability of compounds often relates to the size and charge of the ions involved.

2. **Properties of Alkali Metals in Liquid Ammonia**:
- Alkali metals dissolve in liquid ammonia, forming solutions that are initially dark blue. As the concentration increases, the color changes to copper bronze, indicating the formation of metal ion clusters.
- These solutions are good conductors of electricity due to the presence of ammoniated cations and ammoniated electrons.

**Hint**: Focus on the role of ammoniated ions and how they contribute to the conductivity of the solution.

3. **Conductivity and Reducing Nature**:
- The conductivity decreases with increasing concentration because ammoniated electrons and cations tend to associate, reducing the number of free charge carriers.
- The presence of ammoniated electrons is crucial as they are responsible for the strong reducing nature of the sodium solution.

**Hint**: Consider how the presence of free electrons contributes to the reducing behavior of a solution.

4. **Identifying the Reducing Agent**:
- The question specifically asks why the sodium solution in liquid ammonia is strongly reducing. The answer lies in the presence of solvated electrons.
- Solvated electrons are free electrons that are surrounded by solvent molecules (in this case, ammonia), which enhances their ability to donate electrons in redox reactions.

**Hint**: Recall that reducing agents are substances that can donate electrons to other species.

5. **Conclusion**:
- Therefore, the solution of sodium metal in liquid ammonia is strongly reducing due to the presence of **solvated electrons**.

### Final Answer:
The solution of sodium metal in liquid ammonia is strongly reducing due to the presence of **solvated electrons**.

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