The correct structure of `PCl_3F_2` is

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Explanation

To determine the correct structure of \( PCl_3F_2 \), we can follow these steps:

### Step 1: Determine the Valence Electrons
First, we need to calculate the total number of valence electrons in \( PCl_3F_2 \).
- Phosphorus (P) has 5 valence electrons.
- Each chlorine (Cl) has 7 valence electrons, and there are 3 chlorine atoms: \( 3 \times 7 = 21 \) electrons.
- Each fluorine (F) also has 7 valence electrons, and there are 2 fluorine atoms: \( 2 \times 7 = 14 \) electrons.

Adding these together:
\[ 5 + 21 + 14 = 40 \text{ valence electrons} \]

### Step 2: Identify the Central Atom
In \( PCl_3F_2 \), phosphorus (P) is the central atom because it can form more bonds than chlorine and fluorine.

### Step 3: Determine the Hybridization
Phosphorus will form 5 bonds (3 with Cl and 2 with F). Therefore, the hybridization of phosphorus is \( sp^3d \).

### Step 4: Determine the Molecular Geometry
With \( sp^3d \) hybridization, the molecular geometry is trigonal bipyramidal. In this geometry:
- The equatorial positions can accommodate 3 atoms, and the axial positions can accommodate 2 atoms.

### Step 5: Position the Atoms
To minimize electron pair repulsion, the more electronegative atoms (fluorine) should occupy the axial positions. Thus:
- Place the 2 fluorine atoms in the axial positions.
- Place the 3 chlorine atoms in the equatorial positions.

### Step 6: Draw the Structure
The structure can be represented as follows:
- One Cl atom is on a wedge (indicating it is coming out of the plane).
- Another Cl atom is on a dash (indicating it is going behind the plane).
- The third Cl atom is in the plane of the paper.

### Final Structure
The final structure of \( PCl_3F_2 \) shows:
- 2 fluorine atoms in the axial positions.
- 3 chlorine atoms in the equatorial positions.

This gives us the correct representation of the molecule.

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