All fluorine atoms are in same plane in

Options

A. `CHF_(3)`
B. `CIF_(3)`
C. `XeOF_(4)`
D. All of these

Explanation

To determine in which of the given compounds all fluorine atoms are in the same plane, we will analyze the molecular geometry of each compound provided in the options.

### Step-by-Step Solution:

1. **Analyzing CHF3 (Chloroform)**
- The central atom is carbon (C).
- Carbon is bonded to three fluorine (F) atoms and one hydrogen (H) atom.
- The molecular geometry around carbon is tetrahedral due to the four substituents.
- However, since hydrogen is less electronegative, it will be positioned above the plane formed by the three fluorine atoms.
- **Conclusion**: All three fluorine atoms are in the same plane.

2. **Analyzing CIF3 (Chlorine Trifluoride)**
- The central atom is chlorine (Cl).
- Chlorine is bonded to three fluorine (F) atoms and has one lone pair.
- The molecular geometry is also tetrahedral due to the four regions of electron density (three F atoms and one lone pair).
- The lone pair will occupy one position, and the three fluorine atoms will be arranged in a plane.
- **Conclusion**: All three fluorine atoms are in the same plane.

3. **Analyzing XeOF4 (Xenon Oxyfluoride)**
- The central atom is xenon (Xe).
- Xenon is bonded to one oxygen (O) atom (with a double bond) and four fluorine (F) atoms.
- The molecular geometry is square planar due to the arrangement of four fluorine atoms around xenon.
- In a square planar geometry, all four fluorine atoms lie in the same plane.
- **Conclusion**: All four fluorine atoms are in the same plane.

4. **Final Conclusion**
- Since all three compounds (CHF3, CIF3, and XeOF4) have their fluorine atoms in the same plane, the correct answer is:
- **Option D: All of the above.**