The group of molecules having identical shape is:

Options

A. `SF_(4), XeF_(4), C Cl_(4)`
B. `ClF_(3), XeOF_(2), XeF_(3)^(+)`
C. `BF_(3), PCl_(3), XeO_(3)`
D. `PCl_(5), IF_(5), XeO_(2)F_(2)`

Explanation

To solve the question regarding the group of molecules having identical shape, we will analyze the hybridization and geometry of the given molecules in each option.

### Step-by-Step Solution:

1. **Identify the molecules in each option:**
- Option 1: SF4, XeF4, CCl4
- Option 2: ClF3, XeF2, XeF3+
- Option 3: NH3, H2O, CH4
- Option 4: BF3, AlCl3, SO3

2. **Analyze Option 1: SF4, XeF4, CCl4**
- **SF4:**
- Valence electrons: S (6) + 4 * F (7) = 6 + 28 = 34
- Total electron pairs = (34/2) = 17 pairs (not used here, just for understanding)
- Hybridization: sp3d (5 electron pairs: 4 bond pairs + 1 lone pair)
- Shape: Seesaw (due to lone pair)
- **XeF4:**
- Valence electrons: Xe (8) + 4 * F (7) = 8 + 28 = 36
- Total electron pairs = (36/2) = 18 pairs
- Hybridization: sp3d2 (6 electron pairs: 4 bond pairs + 2 lone pairs)
- Shape: Square planar (due to lone pairs)
- **CCl4:**
- Valence electrons: C (4) + 4 * Cl (7) = 4 + 28 = 32
- Total electron pairs = (32/2) = 16 pairs
- Hybridization: sp3 (4 bond pairs)
- Shape: Tetrahedral
- **Conclusion for Option 1:** Different shapes (Seesaw, Square planar, Tetrahedral) → Incorrect.

3. **Analyze Option 2: ClF3, XeF2, XeF3+**
- **ClF3:**
- Valence electrons: Cl (7) + 3 * F (7) = 7 + 21 = 28
- Total electron pairs = (28/2) = 14 pairs
- Hybridization: sp3d (5 electron pairs: 3 bond pairs + 2 lone pairs)
- Shape: T-shaped (due to lone pairs)
- **XeF2:**
- Valence electrons: Xe (8) + 2 * F (7) = 8 + 14 = 22
- Total electron pairs = (22/2) = 11 pairs
- Hybridization: sp3d3 (5 electron pairs: 2 bond pairs + 3 lone pairs)
- Shape: Linear (due to lone pairs)
- **XeF3+:**
- Valence electrons: Xe (8) + 3 * F (7) - 1 (for positive charge) = 8 + 21 - 1 = 28
- Total electron pairs = (28/2) = 14 pairs
- Hybridization: sp3d2 (5 electron pairs: 3 bond pairs + 2 lone pairs)
- Shape: T-shaped (due to lone pairs)
- **Conclusion for Option 2:** Different shapes (T-shaped, Linear, T-shaped) → Incorrect.

4. **Analyze Option 3: NH3, H2O, CH4**
- **NH3:**
- Valence electrons: N (5) + 3 * H (1) = 5 + 3 = 8
- Total electron pairs = (8/2) = 4 pairs
- Hybridization: sp3 (3 bond pairs + 1 lone pair)
- Shape: Trigonal pyramidal
- **H2O:**
- Valence electrons: O (6) + 2 * H (1) = 6 + 2 = 8
- Total electron pairs = (8/2) = 4 pairs
- Hybridization: sp3 (2 bond pairs + 2 lone pairs)
- Shape: Bent
- **CH4:**
- Valence electrons: C (4) + 4 * H (1) = 4 + 4 = 8
- Total electron pairs = (8/2) = 4 pairs
- Hybridization: sp3 (4 bond pairs)
- Shape: Tetrahedral
- **Conclusion for Option 3:** Different shapes (Trigonal pyramidal, Bent, Tetrahedral) → Incorrect.

5. **Analyze Option 4: BF3, AlCl3, SO3**
- **BF3:**
- Valence electrons: B (3) + 3 * F (7) = 3 + 21 = 24
- Total electron pairs = (24/2) = 12 pairs
- Hybridization: sp2 (3 bond pairs)
- Shape: Trigonal planar
- **AlCl3:**
- Valence electrons: Al (3) + 3 * Cl (7) = 3 + 21 = 24
- Total electron pairs = (24/2) = 12 pairs
- Hybridization: sp2 (3 bond pairs)
- Shape: Trigonal planar
- **SO3:**
- Valence electrons: S (6) + 3 * O (6) = 6 + 18 = 24
- Total electron pairs = (24/2) = 12 pairs
- Hybridization: sp2 (3 bond pairs)
- Shape: Trigonal planar
- **Conclusion for Option 4:** All shapes are Trigonal planar → Correct.

### Final Answer:
The group of molecules having identical shape is **Option 4: BF3, AlCl3, SO3**.