Which one of the following species is planar and non-polar with two lone pairs of electrons on the central atom ?

Options

A. `CIF_3`
B. `XeF_5^(-)`
C. `PCl_5`
D. `BrF_5`

Explanation

To solve the question, "Which one of the following species is planar and non-polar with two lone pairs of electrons on the central atom?", we will analyze the given species step by step.

### Step 1: Identify the species
We need to examine the given species: ClF3, XeF5^-, PCl5, and BrF3.

### Step 2: Draw the Lewis structures
- **ClF3**: Chlorine (Cl) is the central atom. It has 7 valence electrons and forms 3 bonds with fluorine (F), leaving 2 lone pairs. The molecular geometry is T-shaped due to the presence of lone pairs, and it is polar.

- **XeF5^-**: Xenon (Xe) is the central atom. It has 8 valence electrons and forms 5 bonds with fluorine, leaving 2 lone pairs. The molecular geometry is square pyramidal, and the shape is planar. The dipoles cancel out, making it non-polar.

- **PCl5**: Phosphorus (P) is the central atom. It has 5 valence electrons and forms 5 bonds with chlorine (Cl), leaving no lone pairs. The geometry is trigonal bipyramidal, and it is non-polar but not planar.

- **BrF3**: Bromine (Br) is the central atom. It has 7 valence electrons and forms 3 bonds with fluorine, leaving 2 lone pairs. The molecular geometry is T-shaped, and it is polar.

### Step 3: Analyze the polarity and geometry
From the analysis:
- ClF3: Polar, T-shaped
- XeF5^-: Non-polar, planar
- PCl5: Non-polar, non-planar
- BrF3: Polar, T-shaped

### Conclusion
The only species that is planar and non-polar with two lone pairs of electrons on the central atom is **XeF5^-**.

### Final Answer
**XeF5^-**