Among the following, total no. of planar species is :
(i) `SF_(4) " " (ii) BrF_(3) " " (iii) XeF_(2) " " (iv) IF_(5)`
(v)` SbF_(4)^(-) " " (vi) SF_(5)^(-) " " (vii) SeF_(3)^(+) " " (viii) CH_(3)^(+)`
(ix) `PCl_(4)^(+)`

Answer

To determine the total number of planar species among the given compounds, we will analyze each compound one by one based on their molecular geometry and shape.

### Step-by-Step Solution:

1. **Analyze SF₄:**
- Sulfur (S) has 6 valence electrons.
- It forms 4 bonds with fluorine (F), leaving 2 electrons as lone pairs.
- The steric number is 5 (4 bond pairs + 1 lone pair).
- Geometry: Trigonal bipyramidal.
- Shape: Seesaw (due to one lone pair).
- **Conclusion:** SF₄ is **non-planar**.

2. **Analyze BrF₃:**
- Bromine (Br) has 7 valence electrons.
- It forms 3 bonds with fluorine, leaving 4 electrons as lone pairs.
- The steric number is 5 (3 bond pairs + 2 lone pairs).
- Geometry: Trigonal bipyramidal.
- Shape: T-shaped (due to two lone pairs).
- **Conclusion:** BrF₃ is **planar**.

3. **Analyze XeF₂:**
- Xenon (Xe) has 8 valence electrons.
- It forms 2 bonds with fluorine, leaving 6 electrons as lone pairs.
- The steric number is 5 (2 bond pairs + 3 lone pairs).
- Geometry: Trigonal bipyramidal.
- Shape: Linear (due to three lone pairs).
- **Conclusion:** XeF₂ is **planar**.

4. **Analyze IF₅:**
- Iodine (I) has 7 valence electrons.
- It forms 5 bonds with fluorine, leaving 1 electron as a lone pair.
- The steric number is 6 (5 bond pairs + 1 lone pair).
- Geometry: Octahedral.
- Shape: Square pyramidal (due to one lone pair).
- **Conclusion:** IF₅ is **non-planar**.

5. **Analyze SbF₄⁻:**
- Antimony (Sb) has 5 valence electrons.
- It forms 4 bonds with fluorine, leaving 1 electron as a lone pair.
- The steric number is 5 (4 bond pairs + 1 lone pair).
- Geometry: Trigonal bipyramidal.
- Shape: Seesaw (due to one lone pair).
- **Conclusion:** SbF₄⁻ is **non-planar**.

6. **Analyze SF₅⁻:**
- Sulfur (S) has 6 valence electrons.
- It forms 5 bonds with fluorine, leaving 1 electron as a lone pair.
- The steric number is 6 (5 bond pairs + 1 lone pair).
- Geometry: Octahedral.
- Shape: Square pyramidal (due to one lone pair).
- **Conclusion:** SF₅⁻ is **non-planar**.

7. **Analyze SeF₃⁺:**
- Selenium (Se) has 6 valence electrons.
- It forms 3 bonds with fluorine, leaving 1 electron as a lone pair.
- The steric number is 4 (3 bond pairs + 1 lone pair).
- Geometry: Tetrahedral.
- Shape: Trigonal pyramidal (due to one lone pair).
- **Conclusion:** SeF₃⁺ is **non-planar**.

8. **Analyze CH₃⁺:**
- Carbon (C) has 4 valence electrons.
- It forms 3 bonds with hydrogen, leaving no lone pairs.
- The steric number is 4 (4 bond pairs).
- Geometry: Tetrahedral.
- Shape: Trigonal planar (due to no lone pairs).
- **Conclusion:** CH₃⁺ is **planar**.

9. **Analyze PCl₄⁺:**
- Phosphorus (P) has 5 valence electrons.
- It forms 4 bonds with chlorine, leaving no lone pairs.
- The steric number is 4 (4 bond pairs).
- Geometry: Tetrahedral.
- Shape: Tetrahedral (due to no lone pairs).
- **Conclusion:** PCl₄⁺ is **non-planar**.

### Summary of Planar Species:
- Planar species identified:
- BrF₃
- XeF₂
- CH₃⁺

**Total number of planar species = 3.**

### Final Answer:
The total number of planar species among the given compounds is **3**.