The number of peroxide bonds in perxenate ion `[XeO_(6)]^(4-)` is

Options

A. `0`
B. `2`
C. `3`
D. `1`

Explanation

To determine the number of peroxide bonds in the perxenate ion \([XeO_6]^{4-}\), we can follow these steps:

### Step 1: Understand the Peroxide Bond
A peroxide bond is characterized by an oxygen-oxygen single bond (O-O). This is different from the typical double bonds between oxygen and other elements.

### Step 2: Analyze the Structure of Perxenate Ion
The perxenate ion \([XeO_6]^{4-}\) consists of one xenon atom (Xe) and six oxygen atoms (O). To understand how these atoms are bonded, we need to consider the oxidation states and bonding characteristics.

### Step 3: Determine the Oxidation State of Xenon
In the perxenate ion, xenon (Xe) typically has an oxidation state of +6. Each oxygen atom in the ion can either be in the -2 oxidation state (as in typical oxides) or in a -1 oxidation state when involved in a peroxide bond.

### Step 4: Draw the Lewis Structure
To visualize the bonding:
- Xenon can form double bonds with some of the oxygen atoms.
- The remaining oxygen atoms can be bonded as negatively charged oxides.

The structure can be represented as:
- \(Xe\) with double bonds to four oxygen atoms and single bonds to two other oxygen atoms, which are negatively charged.

### Step 5: Count the Peroxide Bonds
In the structure of \([XeO_6]^{4-}\):
- There are no O-O single bonds present.
- All the bonds involving oxygen are either double bonds or single bonds to negatively charged oxygen atoms.

### Conclusion
Since there are no O-O single bonds in the perxenate ion, the number of peroxide bonds in \([XeO_6]^{4-}\) is **0**.

### Final Answer
The number of peroxide bonds in the perxenate ion \([XeO_6]^{4-}\) is **0**.

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