`PCl_(5)` is an example of a molecule having `sp^(3)d`-hybridisation. Three out of the orbitals in `sp_(x)p_(y)`-hybridisation while remaining two have `p_(x)d_(x^(2))`-hybridisation. If P-atom is attached to substitutuents differ in electronegativity, as in `PCl_(x)F_(5-x)`, then it is has been experimently observed that the more electronegativity substituent occupies the axial position of t.b.p geometry.
Q. The incorrect statement regarding `PCl_(2)F_(2)^-` molecule will be:

Options

A. given compound is polar
B. both axial position occupied by F-atoms
C. both Cl atoms present in equatorial position
D. one Cl atom present at axial and other Cl atom is present at equatorial position of geometry

Answer

To solve the question regarding the incorrect statement about the molecule \( PCl_2F_2^- \), we will follow these steps:

### Step 1: Determine the Hybridization and Geometry
1. **Identify the steric number**: The steric number is calculated using the formula:
\[ \text{Steric Number} = \text{Number of valence electrons of central atom} + \text{Number of monovalent substituents} + \frac{\text{Charge}}{2} \]
For phosphorus (\( P \)), it has 5 valence electrons. In \( PCl_2F_2^- \):
- There are 4 monovalent substituents (2 Cl and 2 F).
- The charge is -1.
\[ \text{Steric Number} = 5 + 4 + \frac{-1}{2} = 5 \]

2. **Determine the hybridization**: A steric number of 5 corresponds to \( sp^3d \) hybridization.

3. **Identify the geometry**: The geometry of a molecule with \( sp^3d \) hybridization is trigonal bipyramidal (TBP).

### Step 2: Draw the Molecular Structure
1. **Place the more electronegative substituents**: Fluorine (F) is more electronegative than chlorine (Cl), so the two F atoms will occupy the axial positions in the TBP geometry, while the two Cl atoms will occupy the equatorial positions.

2. **Add the lone pair**: Since there is a negative charge, we can assume that there is a lone pair of electrons on phosphorus, which will also occupy an equatorial position.

### Step 3: Analyze the Statements
1. **Statement A**: The compound is polar.
- **Analysis**: The dipole moments of the two F atoms will partially cancel each other, but the dipole moments from the Cl atoms will not cancel out completely, making the molecule polar. This statement is correct.

2. **Statement B**: Both axial positions are occupied by F atoms.
- **Analysis**: This is true as per the structure drawn. This statement is correct.

3. **Statement C**: Both Cl atoms are present in equatorial positions.
- **Analysis**: This is also true as per the structure drawn. This statement is correct.

4. **Statement D**: One Cl atom is present in the axial position and the other Cl atom is present in the equatorial position.
- **Analysis**: This statement is incorrect because both Cl atoms are in the equatorial positions.

### Conclusion
The incorrect statement regarding \( PCl_2F_2^- \) is:
**D: One Cl atom present at axial position and other Cl atom present at equatorial position.**