Find the number of compounds having zero dipole moment :
`BF_(3),"CCl"_(4),XeF_(6),SF_(6),PCl_(2)F_(3),PClF_(4),CHCl_(3),HF,SO_(3),SO_(2)`

Explanation

To determine the number of compounds having zero dipole moment from the given list, we will analyze each compound based on its molecular geometry and symmetry. A compound will have a zero dipole moment if the dipole moments of its bonds cancel each other out due to symmetry.

### Step-by-Step Solution:

1. **BF₃ (Boron Trifluoride)**:
- **Valence Electrons**: Boron has 3 valence electrons and forms 3 bonds with fluorine.
- **Geometry**: Trigonal planar (3 bond pairs, 0 lone pairs).
- **Dipole Moment**: The dipoles from each B-F bond cancel out due to symmetry.
- **Result**: Zero dipole moment.

2. **CCl₄ (Carbon Tetrachloride)**:
- **Valence Electrons**: Carbon has 4 valence electrons and forms 4 bonds with chlorine.
- **Geometry**: Tetrahedral (4 bond pairs, 0 lone pairs).
- **Dipole Moment**: The dipoles from each C-Cl bond cancel out due to symmetry.
- **Result**: Zero dipole moment.

3. **XeF₆ (Xenon Hexafluoride)**:
- **Valence Electrons**: Xenon has 8 valence electrons and forms 6 bonds with fluorine.
- **Geometry**: Distorted octahedral (5 bond pairs, 1 lone pair).
- **Dipole Moment**: The dipoles do not cancel out due to the presence of a lone pair.
- **Result**: Non-zero dipole moment.

4. **SF₆ (Sulfur Hexafluoride)**:
- **Valence Electrons**: Sulfur has 6 valence electrons and forms 6 bonds with fluorine.
- **Geometry**: Octahedral (6 bond pairs, 0 lone pairs).
- **Dipole Moment**: The dipoles from each S-F bond cancel out due to symmetry.
- **Result**: Zero dipole moment.

5. **PCl₂F₃ (Phosphorus Dichloride Trifluoride)**:
- **Valence Electrons**: Phosphorus has 5 valence electrons and forms 5 bonds (2 with Cl and 3 with F).
- **Geometry**: Trigonal bipyramidal (5 bond pairs, 0 lone pairs).
- **Dipole Moment**: The dipoles do not cancel out due to the different electronegativities and positions of Cl and F.
- **Result**: Non-zero dipole moment.

6. **PClF₄ (Phosphorus Chloride Tetrafluoride)**:
- **Valence Electrons**: Phosphorus has 5 valence electrons and forms 5 bonds (1 with Cl and 4 with F).
- **Geometry**: Seesaw (5 bond pairs, 0 lone pairs).
- **Dipole Moment**: The dipoles do not cancel out due to the different electronegativities and positions of Cl and F.
- **Result**: Non-zero dipole moment.

7. **CHCl₃ (Chloroform)**:
- **Valence Electrons**: Carbon has 4 valence electrons and forms 4 bonds (1 with H and 3 with Cl).
- **Geometry**: Tetrahedral (4 bond pairs, 0 lone pairs).
- **Dipole Moment**: The dipoles do not cancel out due to the presence of Cl and H.
- **Result**: Non-zero dipole moment.

8. **HF (Hydrogen Fluoride)**:
- **Valence Electrons**: Hydrogen has 1 valence electron and fluorine has 7 valence electrons.
- **Geometry**: Linear (1 bond pair).
- **Dipole Moment**: The dipole moment is directed from H to F.
- **Result**: Non-zero dipole moment.

9. **SO₃ (Sulfur Trioxide)**:
- **Valence Electrons**: Sulfur has 6 valence electrons and forms 3 bonds with oxygen.
- **Geometry**: Trigonal planar (3 bond pairs, 0 lone pairs).
- **Dipole Moment**: The dipoles from each S=O bond cancel out due to symmetry.
- **Result**: Zero dipole moment.

10. **SO₂ (Sulfur Dioxide)**:
- **Valence Electrons**: Sulfur has 6 valence electrons and forms 2 bonds with oxygen.
- **Geometry**: Bent (2 bond pairs, 1 lone pair).
- **Dipole Moment**: The dipoles do not cancel out due to the bent shape.
- **Result**: Non-zero dipole moment.

### Summary of Results:
- Compounds with zero dipole moment: **BF₃, CCl₄, SF₆, SO₃**
- Total number of compounds with zero dipole moment: **4**

### Final Answer:
The number of compounds having zero dipole moment is **4**.