According to VSEPR theory, the geometry of the molecule `OF_2` would be

Options

A. Linear
B. Square planer
C. Tetrahedral
D. Octahedral

Explanation

To determine the geometry of the molecule OF₂ (oxygen difluoride) according to VSEPR theory, we can follow these steps:

### Step 1: Identify the central atom
The central atom in OF₂ is oxygen (O).

### Step 2: Determine the number of valence electrons
Oxygen has 6 valence electrons. Each fluorine (F) atom has 7 valence electrons. Since there are two fluorine atoms, the total number of valence electrons contributed by fluorine is 2 × 7 = 14. Therefore, the total number of valence electrons in OF₂ is:
\[ 6 \, (\text{from O}) + 14 \, (\text{from 2 F}) = 20 \, \text{valence electrons} \]

### Step 3: Draw the Lewis structure
In the Lewis structure of OF₂, oxygen will form two single bonds with the two fluorine atoms. After forming these bonds, oxygen will have 2 of its 6 valence electrons used up, leaving it with 4 electrons. These remaining 4 electrons will be represented as 2 lone pairs on the oxygen atom.

### Step 4: Calculate the steric number
The steric number is calculated as the sum of the number of sigma bonds and the number of lone pairs on the central atom. In OF₂:
- There are 2 sigma bonds (one with each fluorine).
- There are 2 lone pairs on oxygen.

Thus, the steric number is:
\[ \text{Steric number} = \text{Number of sigma bonds} + \text{Number of lone pairs} = 2 + 2 = 4 \]

### Step 5: Determine hybridization
With a steric number of 4, the hybridization of the central atom (oxygen) is sp³.

### Step 6: Determine the molecular geometry
The sp³ hybridization corresponds to a tetrahedral arrangement of electron pairs. However, because there are 2 lone pairs, the actual shape of the molecule will be bent or V-shaped.

### Conclusion
Thus, according to VSEPR theory, the geometry of the molecule OF₂ is tetrahedral, but the shape is bent.

### Final Answer
The geometry of the molecule OF₂ is tetrahedral.

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