Which of the following statement is true?

Options

A. `SbF_(4)^(-) and SF_(4)` are isostructural
B. In `IOF_(5)` the hybridization of central atom is `sp^(3)d^(2)`
C. Double bond(s) in `SOF_(4) and XeO_(3)F_(2)`, is/are occupying equatorial position(s) of their
D. All of these

Answer

To solve the question, we need to analyze the statements provided and determine which one is true based on the hybridization and molecular geometry of the given compounds. Let's break down the solution step by step.

### Step 1: Analyze the first statement (SBF4 and SF4)
- **Hybridization of SBF4**:
- **Valence electrons of Sb**: 5 (from group 15)
- **Monovalent atoms**: 4 (F)
- **Charge**: -1
- **Hybridization formula**: \( \text{Hybridization} = \frac{(5 + 4 + 1)}{2} = 5 \)
- **Result**: \( \text{Hybridization} = sp^3d \)

- **Hybridization of SF4**:
- **Valence electrons of S**: 6 (from group 16)
- **Monovalent atoms**: 4 (F)
- **Charge**: 0
- **Hybridization formula**: \( \text{Hybridization} = \frac{(6 + 4)}{2} = 5 \)
- **Result**: \( \text{Hybridization} = sp^3d \)

- **Geometry**: Both have the same hybridization (sp³d), indicating a similar structure.

### Step 2: Analyze the second statement (IOF5)
- **Hybridization of IOF5**:
- **Valence electrons of I**: 7 (from group 17)
- **Monovalent atoms**: 5 (F)
- **Charge**: 0
- **Hybridization formula**: \( \text{Hybridization} = \frac{(7 + 5)}{2} = 6 \)
- **Result**: \( \text{Hybridization} = sp^3d^2 \)

### Step 3: Analyze the third statement (SOF4 and XCO3F2)
- **Hybridization of SOF4**:
- **Valence electrons of S**: 6 (from group 16)
- **Monovalent atoms**: 4 (F)
- **Charge**: 0
- **Hybridization formula**: \( \text{Hybridization} = \frac{(6 + 4)}{2} = 5 \)
- **Result**: \( \text{Hybridization} = sp^3d \)

- **Hybridization of XCO3F2** (assuming X is a noble gas):
- **Valence electrons of X**: 8 (from group 18)
- **Monovalent atoms**: 2 (F)
- **Charge**: 0
- **Hybridization formula**: \( \text{Hybridization} = \frac{(8 + 2)}{2} = 5 \)
- **Result**: \( \text{Hybridization} = sp^3d \)

### Step 4: Determine the positions of atoms
- In SOF4, the oxygen is in an equatorial position due to the presence of lone pairs.
- In XCO3F2, the fluorine atoms occupy the axial positions.

### Conclusion
All three statements are true based on the analysis of hybridization and molecular geometry.

### Final Answer
The correct option is: **All of the above statements are true.**

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