Given the correct order of initials T or F for following statements. Use T if statements is true and F it it is false:
(I)`(CH_(3))_(2)P(CF_(3))_(3)` is non-palar and `(CH_(3))_(3)P(CF_(3))_(2)` is polar molecule
(II)`CH_(3)hat(P)CH_(3)` bond angle are equal in `(CH_(3))_(3)P(CF_(3))_(2)` molecule
(III) `PF_(3)` will be more soluble in polar solvent than `SiF_(4)`

Options

A. TTF
B. FFT
C. FFF
D. FTT

Explanation

To solve the question, we will evaluate each of the three statements provided and determine whether they are true (T) or false (F).

### Statement I:
**(CH₃)₂P(CF₃)₃ is non-polar and (CH₃)₃P(CF₃)₂ is a polar molecule.**

1. **Determine the molecular geometry of (CH₃)₂P(CF₃)₃:**
- Phosphorus (P) is the central atom.
- The steric number of phosphorus is calculated as follows: 5 (from valence electrons) + 5 (from 5 monovalent atoms) = 10 / 2 = 5.
- This indicates an sp³d hybridization, leading to a trigonal bipyramidal geometry.
- In this structure, CF₃ groups will occupy the axial positions due to their higher electronegativity compared to CH₃ groups, which will occupy the equatorial positions.

2. **Evaluate the polarity:**
- The dipole moments from the CF₃ groups will cancel each other out due to symmetry, resulting in a net dipole moment of zero. Therefore, (CH₃)₂P(CF₃)₃ is non-polar.

3. **Determine the molecular geometry of (CH₃)₃P(CF₃)₂:**
- The steric number is calculated similarly, leading to the same trigonal bipyramidal geometry.
- In this case, the three CH₃ groups occupy equatorial positions, while the two CF₃ groups occupy axial positions.

4. **Evaluate the polarity:**
- The dipole moments from the CF₃ groups do not cancel out due to the presence of the three CH₃ groups, resulting in a net dipole moment. Therefore, (CH₃)₃P(CF₃)₂ is polar.

**Conclusion for Statement I:**
- (CH₃)₂P(CF₃)₃ is non-polar (True) and (CH₃)₃P(CF₃)₂ is polar (True).
- Therefore, the statement is **False (F)**.

### Statement II:
**(CH₃)₂P(CH₃) bond angles are equal in (CH₃)₂P(CF₃)₂ molecule.**

1. **Examine the bond angles:**
- In the (CH₃)₂P(CF₃)₂ molecule, the CH₃ groups are in equatorial positions and the CF₃ groups are in axial positions.
- The bond angles between the equatorial CH₃ groups will be 120 degrees due to the trigonal bipyramidal geometry.

**Conclusion for Statement II:**
- The bond angles between the CH₃ groups are equal (120 degrees).
- Therefore, the statement is **True (T)**.

### Statement III:
**PF₃ will be more soluble in polar solvent than SiF₄.**

1. **Evaluate the polarity of PF₃:**
- PF₃ has a trigonal pyramidal shape due to the presence of a lone pair on phosphorus.
- The dipole moments do not cancel out, making PF₃ a polar molecule.

2. **Evaluate the polarity of SiF₄:**
- SiF₄ has a tetrahedral shape, and the dipole moments from the four Si-F bonds cancel out, resulting in a non-polar molecule.

3. **Solubility in polar solvents:**
- Polar molecules are generally more soluble in polar solvents due to the principle "like dissolves like."
- Since PF₃ is polar and SiF₄ is non-polar, PF₃ will be more soluble in polar solvents.

**Conclusion for Statement III:**
- PF₃ is indeed more soluble in polar solvents than SiF₄.
- Therefore, the statement is **True (T)**.

### Final Answers:
- Statement I: F
- Statement II: T
- Statement III: T