Which of the oxides is strong oxidizing agent ?

Options

A. `SiO_2`
B. `GeO_2`
C. `SnO_2`
D. `PbO_2`

Answer

To determine which oxide is a strong oxidizing agent among the group of oxides from Group 14 (the carbon group), we can follow these steps:

### Step 1: Identify the Oxides
The oxides we are considering from Group 14 include:
- Silicon dioxide (SiO2)
- Germanium dioxide (GeO2)
- Tin dioxide (SnO2)
- Lead dioxide (PbO2)

### Step 2: Understand Oxidation States
In Group 14, the elements can exhibit oxidation states of +2 and +4. The +4 oxidation state is generally more stable for lighter elements (Si, Ge), while the +2 oxidation state becomes more stable for heavier elements (Sn, Pb) due to the inert pair effect.

### Step 3: Analyze the Stability of Oxidation States
- **Silicon (Si)**: +4 is stable.
- **Germanium (Ge)**: +4 is stable.
- **Tin (Sn)**: +4 is stable, but +2 is also significant.
- **Lead (Pb)**: +4 is less stable than +2 due to the inert pair effect.

### Step 4: Determine the Reducing Potential
To be a strong oxidizing agent, an oxide must be able to undergo reduction easily. This means it should readily convert from a higher oxidation state to a lower one:
- For SiO2 and GeO2, the +4 state is stable and does not easily reduce to +2.
- For SnO2, while +4 is stable, it can reduce to +2 but not as readily as PbO2.
- For PbO2, the +4 state is less stable and can easily reduce to +2.

### Step 5: Conclusion
Since PbO2 can easily reduce to PbO (where lead is in the +2 oxidation state), it acts as a strong oxidizing agent compared to the other oxides. Therefore, the answer is:

**Lead dioxide (PbO2) is the strongest oxidizing agent among the given oxides.**

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