Which of the following molecule is non-polar & planar ?

Options

A. `XeF_(4)`
B. `NH_(2)^(-)`
C. `PF_(3)Cl_(2)`
D. `PCl_(3)F_(2)`

Explanation

To determine which of the given molecules is non-polar and planar, we can analyze each option based on their molecular geometry and polarity.

### Step-by-Step Solution:

1. **Identify the Molecules**: The question provides several molecules to analyze. Let's consider them: XeF4, NH2-, PF3Cl2, and PCl3F2.

2. **Analyze XeF4 (Xenon Tetrafluoride)**:
- **Molecular Geometry**: XeF4 has a square planar geometry due to the presence of four fluorine atoms around the central xenon atom and two lone pairs of electrons.
- **Polarity**: The symmetry of the molecule means that the dipole moments of the four Xe-F bonds cancel each other out, resulting in a non-polar molecule.
- **Conclusion**: XeF4 is non-polar and planar.

3. **Analyze NH2- (Amide Ion)**:
- **Molecular Geometry**: NH2- has a pyramidal shape due to the presence of a lone pair on nitrogen.
- **Polarity**: The presence of a negative charge on nitrogen creates a dipole moment, making it a polar molecule.
- **Conclusion**: NH2- is polar and not planar.

4. **Analyze PF3Cl2 (Phosphorus Trifluoride Dichloride)**:
- **Molecular Geometry**: PF3Cl2 has a trigonal bipyramidal shape, which is not planar.
- **Polarity**: The difference in electronegativity between fluorine and chlorine leads to a net dipole moment, making it a polar molecule.
- **Conclusion**: PF3Cl2 is polar and non-planar.

5. **Analyze PCl3F2 (Phosphorus Trichloride Difluoride)**:
- **Molecular Geometry**: PCl3F2 also has a trigonal bipyramidal shape, which is not planar.
- **Polarity**: Similar to PF3Cl2, the differences in electronegativity create a net dipole moment, making it a polar molecule.
- **Conclusion**: PCl3F2 is polar and non-planar.

6. **Final Conclusion**: Based on the analysis, the only molecule that is both non-polar and planar is **XeF4**.