Which of the following compound has non-zero dipole moment

Options

A. `XeF_(4)`
B. `B_(2)H_(6)`
C. `PF_(3)Cl_(2)`
D. `PCl_(3)F_(2)`

Answer

To determine which compound has a non-zero dipole moment, we will analyze the dipole moments of each given compound step by step.

### Step 1: Analyze XeF4
1. **Identify the structure**: Xenon tetrafluoride (XeF4) has a central xenon atom surrounded by four fluorine atoms.
2. **Hybridization and electron count**: Xenon has 8 valence electrons, and each fluorine has 7. The total is 8 + (4 x 7) = 36 electrons. Dividing by 8 gives 4 bond pairs and 2 lone pairs.
3. **Shape**: The shape is square planar due to the presence of 2 lone pairs opposite each other.
4. **Dipole moment**: The dipole moments of the four Xe-F bonds cancel each other out because of symmetry, resulting in a net dipole moment of zero.

**Conclusion for XeF4**: Zero dipole moment.

### Step 2: Analyze B2H6
1. **Identify the structure**: Diborane (B2H6) has a unique structure with "banana bonds" between boron and hydrogen.
2. **Electron count**: Each boron has 3 valence electrons and each hydrogen has 1. Total = (2 x 3) + (6 x 1) = 12 electrons.
3. **Bonding**: Boron can form 3 bonds with hydrogen, and due to the dimerization, there is no significant difference in electronegativity.
4. **Dipole moment**: The bonds are symmetrical and there is no net dipole moment.

**Conclusion for B2H6**: Zero dipole moment.

### Step 3: Analyze PF3Cl2
1. **Identify the structure**: Phosphorus trifluoride dichloride (PF3Cl2) has phosphorus as the central atom with three fluorine and two chlorine atoms.
2. **Shape**: The molecule adopts a trigonal bipyramidal geometry, with the fluorine atoms in the equatorial positions and chlorine in the axial positions.
3. **Dipole moment**: The electronegativity difference between fluorine and chlorine leads to a net dipole moment since the axial positions do not cancel out the dipole moments of the equatorial fluorine bonds.

**Conclusion for PF3Cl2**: Non-zero dipole moment.

### Step 4: Analyze PCl3F2
1. **Identify the structure**: Phosphorus trichloride difluoride (PCl3F2) has phosphorus as the central atom with three chlorine and two fluorine atoms.
2. **Shape**: This molecule also adopts a trigonal bipyramidal geometry, with chlorine atoms occupying the equatorial positions and fluorine in the axial positions.
3. **Dipole moment**: Similar to PF3Cl2, the electronegativity difference results in a net dipole moment due to the arrangement of the bonds.

**Conclusion for PCl3F2**: Non-zero dipole moment.

### Final Conclusion
Among the compounds analyzed, **PF3Cl2** and **PCl3F2** exhibit non-zero dipole moments due to their asymmetrical arrangements and differences in electronegativity.

### Answer:
**PF3Cl2** and **PCl3F2** have non-zero dipole moments.