Which of the following molecule is theoretically not possible ?

Options

A. `SF_(4)`
B. `OF_(2)`
C. `OF_(4)`
D. `O_(2)F_(2)`

Answer

To determine which of the following molecules is theoretically not possible, we will analyze the given options one by one based on their hybridization and electronic configurations.

### Step-by-Step Solution:

1. **Analyze SF4:**
- Sulfur (S) has an electronic configuration of 3s² 3p⁴.
- In SF4, sulfur can undergo hybridization to form sp³d hybrid orbitals.
- The structure of SF4 is based on a seesaw shape due to the presence of one lone pair and four bonding pairs.
- Since sulfur has d-orbitals available (being in the third period), it can expand its octet and accommodate four fluorine atoms.
- **Conclusion:** SF4 exists.

2. **Analyze OF2:**
- Oxygen (O) has an electronic configuration of 2s² 2p⁴.
- In OF2, oxygen forms two sigma bonds with fluorine atoms and has two lone pairs.
- The hybridization of oxygen in OF2 is sp³, as it involves four orbitals (2 bonding + 2 lone pairs).
- **Conclusion:** OF2 exists.

3. **Analyze OF4:**
- Oxygen, as previously mentioned, has an electronic configuration of 2s² 2p⁴ and does not have d-orbitals available for hybridization.
- To form OF4, oxygen would need to accommodate four fluorine atoms, which would require it to expand its octet.
- However, since oxygen lacks d-orbitals, it cannot undergo the necessary hybridization to form OF4.
- **Conclusion:** OF4 does not exist.

4. **Analyze O2F2:**
- O2F2 has a structure similar to H2O2, where each oxygen atom is bonded to one fluorine atom and has two lone pairs.
- The hybridization of each oxygen in O2F2 is sp³, which is feasible as it involves four orbitals (2 bonding + 2 lone pairs).
- **Conclusion:** O2F2 exists.

### Final Answer:
Based on the analysis, the molecule that is theoretically not possible is **OF4**.