Find the total number of polar molecules
`SF_(4),PCl_(5),PCl_(3)F_(2),SF_(6),XeF_(2),NO_(2)^(+),BF_(2)Cl,BF_(3),PF_(3)Cl_(2)`

Explanation

To determine the total number of polar molecules from the given list, we will analyze each molecule based on its molecular geometry and the presence of polar bonds.

### Step-by-Step Solution:

1. **Identify the Molecules:**
The molecules given are:
- SF₄
- PCl₅
- PCl₃F₂
- SF₆
- XeF₂
- NO₂⁺
- BF₂Cl
- BF₃
- PF₃Cl₂

2. **Analyze Each Molecule:**
- **SF₄:**
- Sulfur has 6 valence electrons, forms 4 bonds with fluorine, and has 1 lone pair.
- Geometry: Seesaw (trigonal bipyramidal).
- The dipole moments do not cancel out due to the lone pair, making SF₄ polar.

- **PCl₅:**
- Phosphorus has 5 valence electrons, forms 5 bonds with chlorine, and has no lone pairs.
- Geometry: Trigonal bipyramidal.
- The dipole moments cancel out, making PCl₅ non-polar.

- **PCl₃F₂:**
- Phosphorus has 5 valence electrons, forms 3 bonds with chlorine and 2 bonds with fluorine, and has no lone pairs.
- Geometry: Trigonal bipyramidal.
- The dipole moments do not cancel out due to the presence of more electronegative fluorine, making PCl₃F₂ polar.

- **SF₆:**
- Sulfur has 6 valence electrons, forms 6 bonds with fluorine, and has no lone pairs.
- Geometry: Octahedral.
- The dipole moments cancel out, making SF₆ non-polar.

- **XeF₂:**
- Xenon has 8 valence electrons, forms 2 bonds with fluorine, and has 3 lone pairs.
- Geometry: Linear.
- The dipole moments cancel out, making XeF₂ non-polar.

- **NO₂⁺:**
- Nitrogen has 5 valence electrons, forms 2 bonds with oxygen, and has no lone pairs.
- Geometry: Linear.
- The dipole moments do not cancel out, making NO₂⁺ polar.

- **BF₂Cl:**
- Boron has 3 valence electrons, forms 2 bonds with fluorine and 1 bond with chlorine, and has no lone pairs.
- Geometry: Trigonal planar.
- The dipole moments do not cancel out, making BF₂Cl polar.

- **BF₃:**
- Boron has 3 valence electrons, forms 3 bonds with fluorine, and has no lone pairs.
- Geometry: Trigonal planar.
- The dipole moments cancel out, making BF₃ non-polar.

- **PF₃Cl₂:**
- Phosphorus has 5 valence electrons, forms 3 bonds with fluorine and 2 bonds with chlorine, and has no lone pairs.
- Geometry: Trigonal bipyramidal.
- The dipole moments do not cancel out, making PF₃Cl₂ polar.

3. **Count the Polar Molecules:**
From the analysis:
- Polar: SF₄, PCl₃F₂, NO₂⁺, BF₂Cl, PF₃Cl₂
- Non-polar: PCl₅, SF₆, XeF₂, BF₃

**Total Polar Molecules = 5**

### Final Answer:
The total number of polar molecules is **5**.