Choose the CORRECT statements :-

Options

A. `d_(P-F)("Axial")gt d_(P-F)"(equatorial) in " PF_(3)Cl_(2)`
B. `d_(P-F) gt d_(P-Cl) ` in `PF_(2)Cl_(3)`
C. `d_(P-Cl)(PF_(2)Cl_(3))gt d_(P-Cl)(PF_(3)Cl_(2))`
D. All `d_(P-Cl)` (in `PF_(2)Cl_(3)`) are identical while all `d_(P-F) ` (in `PF_(3)Cl_(2)`) are not identical

Answer

To solve the question, we need to analyze the statements regarding the two mixed halides: PF3Cl2 and PF2Cl3. We will evaluate each statement based on the properties of the compounds and the structure of phosphorus halides.

### Step-by-Step Solution:

1. **Understanding the Structures**:
- Both PF3Cl2 and PF2Cl3 have a trigonal bipyramidal structure with phosphorus as the central atom.
- In a trigonal bipyramidal geometry, there are five positions: two axial and three equatorial.

2. **Analyzing PF3Cl2**:
- In PF3Cl2, there are three fluorine atoms and two chlorine atoms.
- The more electronegative fluorine atoms will occupy the axial positions to minimize repulsion, while the chlorine atoms will occupy the equatorial positions.
- Therefore, the structure can be represented as:
- Axial: F, F
- Equatorial: Cl, Cl, F

3. **Analyzing PF2Cl3**:
- In PF2Cl3, there are two fluorine atoms and three chlorine atoms.
- Similarly, the fluorine atoms will occupy the axial positions, and the chlorine atoms will occupy the equatorial positions.
- The structure can be represented as:
- Axial: F, F
- Equatorial: Cl, Cl, Cl

4. **Evaluating the Statements**:
- **Statement A**: "The axial bond length will be greater than the equatorial bond length."
- This is correct because axial bonds are weaker and have longer bond lengths compared to equatorial bonds.
- **Statement B**: "The bond length of PF is greater than PCl in PF2Cl3."
- This is also correct because the PF bonds occupy axial positions (longer bond lengths) while PCl bonds occupy equatorial positions (shorter bond lengths).
- **Statement C**: "The phosphorus-chlorine bond length will be greater in PF2Cl3 as compared to PF3Cl2."
- This is incorrect because the PCl bond lengths in both compounds are equal as both occupy equatorial positions.
- **Statement D**: "All PCl bonds in PF2Cl3 are identical."
- This is correct because all chlorine atoms occupy the equatorial positions, leading to identical bond lengths.

5. **Conclusion**:
- The correct statements are A, B, and D. The only incorrect statement is C.

### Final Answer:
The correct statements are A, B, and D.

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