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 about identifying the group of molecules having identical shapes, we will analyze the given options step by step.

### Step 1: Analyze Option A
- **Molecules**: SF4 and XeF4
- **SF4 (Sulfur Tetrafluoride)**:
- Valence electrons: Sulfur has 6 valence electrons.
- Structure: 4 fluorine atoms bonded to sulfur, with 1 lone pair on sulfur.
- Shape: Seesaw (due to 4 bond pairs and 1 lone pair).
- Hybridization: sp³d.

- **XeF4 (Xenon Tetrafluoride)**:
- Valence electrons: Xenon has 8 valence electrons.
- Structure: 4 fluorine atoms in the plane and 2 lone pairs on xenon.
- Shape: Square planar (due to 4 bond pairs and 2 lone pairs).
- Hybridization: sp³d².

**Conclusion for Option A**: The shapes are different (seesaw vs. square planar), so this option is not correct.

### Step 2: Analyze Option B
- **Molecules**: ClF3, XeOF2, and XeF3+
- **ClF3 (Chlorine Trifluoride)**:
- Valence electrons: Chlorine has 7 valence electrons.
- Structure: 3 fluorine atoms bonded to chlorine, with 2 lone pairs on chlorine.
- Shape: T-shaped (due to 3 bond pairs and 2 lone pairs).
- Hybridization: sp³d.

- **XeOF2 (Xenon Oxyfluoride)**:
- Valence electrons: Xenon has 8 valence electrons, and oxygen contributes 2.
- Structure: 2 fluorine atoms bonded to xenon, with 2 lone pairs on xenon.
- Shape: T-shaped (due to 3 bond pairs and 2 lone pairs).
- Hybridization: sp³d.

- **XeF3+ (Xenon Trifluoride cation)**:
- Valence electrons: Xenon has 8 electrons, minus 1 for the positive charge gives 7.
- Structure: 3 fluorine atoms bonded to xenon, with 2 lone pairs on xenon.
- Shape: T-shaped (due to 3 bond pairs and 2 lone pairs).
- Hybridization: sp³d.

**Conclusion for Option B**: All three molecules (ClF3, XeOF2, and XeF3+) have the same shape (T-shaped), so this option is correct.

### Step 3: Analyze Option C
- **Molecules**: BF3 and PCl3
- **BF3 (Boron Trifluoride)**:
- Valence electrons: Boron has 3 valence electrons.
- Structure: 3 fluorine atoms bonded to boron, no lone pairs.
- Shape: Trigonal planar (due to 3 bond pairs).
- Hybridization: sp².

- **PCl3 (Phosphorus Trichloride)**:
- Valence electrons: Phosphorus has 5 valence electrons.
- Structure: 3 chlorine atoms bonded to phosphorus, with 1 lone pair on phosphorus.
- Shape: Trigonal pyramidal (due to 3 bond pairs and 1 lone pair).
- Hybridization: sp³.

**Conclusion for Option C**: The shapes are different (trigonal planar vs. trigonal pyramidal), so this option is not correct.

### Step 4: Analyze Option D
- **Molecules**: PCl5 and IF5
- **PCl5 (Phosphorus Pentachloride)**:
- Valence electrons: Phosphorus has 5 valence electrons.
- Structure: 5 chlorine atoms bonded to phosphorus, no lone pairs.
- Shape: Trigonal bipyramidal (due to 5 bond pairs).
- Hybridization: sp³d.

- **IF5 (Iodine Pentafluoride)**:
- Valence electrons: Iodine has 7 valence electrons.
- Structure: 5 fluorine atoms bonded to iodine, with 1 lone pair on iodine.
- Shape: Square pyramidal (due to 5 bond pairs and 1 lone pair).
- Hybridization: sp³d².

**Conclusion for Option D**: The shapes are different (trigonal bipyramidal vs. square pyramidal), so this option is not correct.

### Final Answer:
The correct group of molecules having identical shape is **Option B: ClF3, XeOF2, and XeF3+**.