If `XeOF_(4)` how many angles are of `90^(@)`?

Answer

To determine how many angles in the molecule XeOF₄ are 90 degrees, we will follow these steps:

### Step 1: Determine the Valence Electrons
- Xenon (Xe) has 8 valence electrons.
- Oxygen (O) contributes 6 valence electrons.
- Each Fluorine (F) contributes 7 valence electrons, and there are 4 fluorine atoms.

**Calculation:**
- Total valence electrons = 8 (Xe) + 6 (O) + 4 * 7 (F) = 8 + 6 + 28 = 42 valence electrons.

### Step 2: Determine the Number of Bond Pairs and Lone Pairs
- In XeOF₄, we have 4 fluorine atoms and 1 oxygen atom bonded to xenon.
- This gives us 5 bond pairs (4 F and 1 O).
- There is 1 lone pair on xenon.

### Step 3: Calculate the Steric Number
- The steric number is the sum of bond pairs and lone pairs.
- Steric number = 5 (bond pairs) + 1 (lone pair) = 6.

### Step 4: Determine the Hybridization
- With a steric number of 6, the hybridization is sp³d².

### Step 5: Determine the Geometry
- The geometry corresponding to sp³d² hybridization is octahedral.

### Step 6: Determine the Molecular Shape
- With 5 bond pairs and 1 lone pair, the shape becomes square pyramidal.

### Step 7: Analyze the Bond Angles
- In a perfect octahedral arrangement, the bond angles between the bonds are 90 degrees.
- However, the presence of the lone pair causes repulsion, which distorts the angles.

### Step 8: Conclusion
- Due to the lone pair's repulsion, the angles that would ideally be 90 degrees are affected and become less than 90 degrees.
- Therefore, there are **0 angles of 90 degrees** in XeOF₄.

### Final Answer:
**0 angles of 90 degrees.**

---