The stability order of oxide, peroxide and superoxide of alkalimetal is

Options

A. Normal oxide `gt` super oxide `gt` per oxide
B. Normal oxide `gt` per oxide `gt` super oxide
C. super oxide `gt` per oxide `gt` normal oxide
D. per oxide `gt` normal oxide `gt` super oxide

Answer

To determine the stability order of oxides, peroxides, and superoxides of alkali metals, we can follow these steps:

### Step 1: Understand the Types of Oxides
Alkali metals can form three types of oxides:
- **Oxides (O²⁻)**: These are simple oxides where oxygen has a -2 oxidation state.
- **Peroxides (O₂²⁻)**: These contain the peroxide ion where oxygen has a -1 oxidation state.
- **Superoxides (O₂⁻)**: These contain the superoxide ion where oxygen has a -1/2 oxidation state.

### Step 2: Analyze the Stability of Each Type
The stability of these compounds generally decreases as we move from oxides to peroxides to superoxides. This can be attributed to the size of the alkali metal cation and the charge density:
- **Oxides** are the most stable because they have a simple ionic structure with a strong electrostatic attraction between the cation and the oxide ion.
- **Peroxides** are less stable than oxides due to the presence of the O₂²⁻ ion, which introduces additional repulsion between the oxygen atoms.
- **Superoxides** are the least stable because the O₂⁻ ion has a larger size and lower charge density, making it less stable compared to the other two.

### Step 3: Establish the Stability Order
Based on the analysis, we can establish the stability order as follows:
- **Oxides (most stable) > Peroxides > Superoxides (least stable)**

### Final Answer
The stability order of oxides, peroxides, and superoxides of alkali metals is:
**Oxides > Peroxides > Superoxides**