The lowest O-O bond length in the following molecule is :

Options

A. `O_(2)F_(2)`
B. `O_(2)`
C. `H_(2)O_(2)`
D. `O_(3)`

Answer

To determine the lowest O-O bond length among the given molecules, we need to analyze the types of bonds present in each molecule. Here’s a step-by-step solution:

### Step 1: Identify the Molecules
We need to consider the following molecules:
1. O2 (dioxygen)
2. O2F2 (oxygen difluoride)
3. H2O2 (hydrogen peroxide)
4. O3 (ozone)

### Step 2: Analyze the Bond Types
- **O2**: The bond between the two oxygen atoms is a double bond (O=O).
- **O2F2**: Each oxygen is bonded to a fluorine atom and has a single bond between the two oxygen atoms (O-O).
- **H2O2**: The bond between the two oxygen atoms is a single bond (O-O).
- **O3**: The ozone molecule has resonance structures, which means the bond between the oxygen atoms can be considered as a partial double bond due to resonance (O-O with partial double bond character).

### Step 3: Compare Bond Lengths
- **Double Bonds** (like in O2) are shorter than single bonds.
- **Single Bonds** (like in O2F2 and H2O2) are longer than double bonds.
- **Partial Double Bonds** (like in O3) are generally shorter than single bonds but longer than double bonds.

### Step 4: Conclusion
From the analysis:
- O2 has a double bond (shortest bond length).
- O2F2 has a single bond.
- H2O2 has a single bond.
- O3 has a partial double bond.

The lowest O-O bond length is found in O2 due to the presence of a double bond.

### Final Answer
The lowest O-O bond length is in O2 (dioxygen).

---