Which of the following will have the molecular shape of a trigonal bipyramid?

Options

A. `PF_(3)Cl_(2)`
B. `IF_(5)`
C. `BrF_(5)`
D. `SbF_(5)^(2-)`

Explanation

To determine which of the given compounds has a molecular shape of trigonal bipyramidal, we need to analyze the number of bond pairs and lone pairs around the central atom in each compound. The trigonal bipyramidal shape occurs when there are five bond pairs and no lone pairs.

### Step-by-Step Solution:

1. **Understand the Trigonal Bipyramidal Shape**:
- A trigonal bipyramidal molecular shape has a central atom bonded to five other atoms, with bond angles of 120° in the equatorial plane and 90° between the axial and equatorial positions.

2. **Identify the Compounds**:
- The options given are PF3Cl2, IF5, BrF5, and SbF5-2.

3. **Analyze Each Compound**:
- **Option A: PF3Cl2**:
- Phosphorus (P) has 5 valence electrons. It forms 5 bonds (3 with F and 2 with Cl) and has 0 lone pairs.
- Bond pairs = 5, Lone pairs = 0.
- This fits the criteria for a trigonal bipyramidal shape.

- **Option B: IF5**:
- Iodine (I) has 7 valence electrons. It forms 5 bonds with F and has 1 lone pair.
- Bond pairs = 5, Lone pairs = 1.
- This results in a square pyramidal shape, not trigonal bipyramidal.

- **Option C: BrF5**:
- Bromine (Br) also has 7 valence electrons. It forms 5 bonds with F and has 1 lone pair.
- Bond pairs = 5, Lone pairs = 1.
- This also results in a square pyramidal shape, not trigonal bipyramidal.

- **Option D: SbF5-2**:
- Antimony (Sb) has 5 valence electrons. With a -2 charge, it effectively has 7 electrons. It forms 5 bonds with F and has 2 lone pairs.
- Bond pairs = 5, Lone pairs = 2.
- This leads to a different geometry, not trigonal bipyramidal.

4. **Conclusion**:
- The only compound that has a trigonal bipyramidal shape is **PF3Cl2**.

### Final Answer:
**PF3Cl2** has a molecular shape of trigonal bipyramidal.