According to VSEPR model, molecules adopt geometries in which their valence electron pairs position themselves as far from each other as possible. The VSEPR model considers double and triple bonds to have slightly greater repulsive effects than single bonds because of the repulsive effect of `pi` -electrons. However the lone pair creates the maximum repulsive effect.
Which of the following statement is false ?

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 respective geometry
D. none of these

Explanation

To determine which statement is false according to the VSEPR model, we will analyze the given statements one by one based on the information provided in the video transcript.

### Step 1: Analyze the first statement about SbA4 and Sa4 being isostructural.
- **SbA4** (Antimony tetrafluoride) has a central atom of antimony (Sb) from group 15, which has 5 valence electrons. With 4 fluorine atoms (each contributing 1 electron) and one additional negative charge, the total number of electrons becomes 6.
- The structure can be drawn with 4 bond pairs and 1 lone pair, leading to a steric number of 5. This indicates sp³d hybridization and a trigonal bipyramidal geometry.
- **Sa4** (Sulfur tetrafluoride) has a central atom of sulfur (S) from group 16, which has 6 valence electrons. With 4 fluorine atoms, it also has 4 bond pairs and 1 lone pair, leading to a steric number of 5, sp³d hybridization, and trigonal bipyramidal geometry.
- Both species have the same geometry, hence they are isostructural. This statement is **true**.

### Step 2: Analyze the second statement about hybridization in IUF5.
- **IUF5** (Iodine pentafluoride) has iodine (I) as the central atom from group 17, which has 7 valence electrons. With 5 fluorine atoms and 1 oxygen, the total number of electrons is 6 bond pairs and 0 lone pairs.
- The steric number is 6, leading to sp³d² hybridization. This statement is also **true**.

### Step 3: Analyze the third statement regarding double bonds in SOF4 and XeO3F2.
- **SOF4** (Sulfur oxyfluoride) has sulfur as the central atom from group 16, with 6 valence electrons. It has 4 bond pairs and 1 lone pair, leading to a steric number of 5 and sp³d hybridization.
- **XeO3F2** (Xenon trifluoride) has xenon as the central atom from group 18, with 8 valence electrons. It has 3 oxygen atoms and 2 fluorine atoms, leading to a steric number of 5 and sp³d hybridization.
- The statement claims that double bonds in SOF4 and XeO3F2 occupy equatorial positions. However, SOF4 does not have double bonds; it has single bonds with one lone pair. Therefore, this statement is **false**.

### Conclusion
The false statement is about the double bonds in SOF4 and XeO3F2 occupying equatorial positions, as SOF4 does not contain double bonds.