The answer to each of the following is a non-negative integer
Find the number of d-orbitals used for bonding of `XeOF_4`

Answer

To find the number of d-orbitals used for bonding in \( \text{XeOF}_4 \), we can follow these steps:

### Step 1: Determine the Valence Electrons of Xenon
Xenon (Xe) is a noble gas and has 8 valence electrons.

### Step 2: Identify the Bonds and Lone Pairs
In \( \text{XeOF}_4 \):
- Xenon forms one bond with oxygen (O).
- Xenon forms four bonds with fluorine (F).
- Therefore, there are a total of 5 bonds (1 with O and 4 with F).

### Step 3: Calculate the Number of Lone Pairs
To find the number of lone pairs on xenon:
- Total valence electrons = 8
- Electrons used in bonding = 5 bonds × 2 electrons/bond = 10 electrons
- Since xenon has only 8 valence electrons, it cannot form 5 bonds without using its d-orbitals.

### Step 4: Determine Hybridization
The hybridization can be determined using the formula:
\[ \text{Hybridization Index} = \text{Number of Sigma Bonds} + \text{Number of Lone Pairs} \]
- Number of sigma bonds = 5 (1 from O and 4 from F)
- Number of lone pairs = 1 (since 8 - 10 = -2, which indicates that 2 d-orbitals are used)

Thus, the total is:
\[ \text{Hybridization Index} = 5 + 1 = 6 \]
This indicates \( \text{sp}^3\text{d}^2 \) hybridization.

### Step 5: Identify the d-Orbitals Used
In \( \text{sp}^3\text{d}^2 \) hybridization, 2 d-orbitals are used for bonding.

### Final Answer
The number of d-orbitals used for bonding in \( \text{XeOF}_4 \) is **2**.

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