Write the sum of lone pairs of electron on central atom of `SF_(4), CF_(4), XeF_(4), XeF_(2)` and `ClF_(3)`.

Explanation

To find the sum of lone pairs of electrons on the central atom of the molecules \( SF_4, CF_4, XeF_4, XeF_2, \) and \( ClF_3 \), we will analyze each molecule step by step.

### Step 1: Analyze \( SF_4 \)
1. **Valence Electrons**: Sulfur (S) has 6 valence electrons.
2. **Monovalent Atoms**: There are 4 fluorine (F) atoms surrounding sulfur.
3. **Formula**: Using the formula \( X = \frac{1}{2} \left( \text{Valence Electrons} + \text{Monovalent Atoms} - \text{Charge on Cation} + \text{Charge on Anion} \right) \):
\[ X = \frac{1}{2} (6 + 4) = 5 \]
4. **Hybridization**: \( SP^3D \) (5 regions of electron density).
5. **Lone Pairs**: The structure shows 4 bond pairs and 1 lone pair.
- **Lone Pairs in \( SF_4 \)**: 1

### Step 2: Analyze \( CF_4 \)
1. **Valence Electrons**: Carbon (C) has 4 valence electrons.
2. **Monovalent Atoms**: There are 4 fluorine atoms.
3. **Formula**:
\[ X = \frac{1}{2} (4 + 4) = 4 \]
4. **Hybridization**: \( SP^3 \) (4 regions of electron density).
5. **Lone Pairs**: The structure shows 4 bond pairs and 0 lone pairs.
- **Lone Pairs in \( CF_4 \)**: 0

### Step 3: Analyze \( XeF_4 \)
1. **Valence Electrons**: Xenon (Xe) has 8 valence electrons.
2. **Monovalent Atoms**: There are 4 fluorine atoms.
3. **Formula**:
\[ X = \frac{1}{2} (8 + 4) = 6 \]
4. **Hybridization**: \( SP^3D^2 \) (6 regions of electron density).
5. **Lone Pairs**: The structure shows 4 bond pairs and 2 lone pairs.
- **Lone Pairs in \( XeF_4 \)**: 2

### Step 4: Analyze \( XeF_2 \)
1. **Valence Electrons**: Xenon (Xe) has 8 valence electrons.
2. **Monovalent Atoms**: There are 2 fluorine atoms.
3. **Formula**:
\[ X = \frac{1}{2} (8 + 2) = 5 \]
4. **Hybridization**: \( SP^3D \) (5 regions of electron density).
5. **Lone Pairs**: The structure shows 2 bond pairs and 3 lone pairs.
- **Lone Pairs in \( XeF_2 \)**: 3

### Step 5: Analyze \( ClF_3 \)
1. **Valence Electrons**: Chlorine (Cl) has 7 valence electrons.
2. **Monovalent Atoms**: There are 3 fluorine atoms.
3. **Formula**:
\[ X = \frac{1}{2} (7 + 3) = 5 \]
4. **Hybridization**: \( SP^3D \) (5 regions of electron density).
5. **Lone Pairs**: The structure shows 3 bond pairs and 2 lone pairs.
- **Lone Pairs in \( ClF_3 \)**: 2

### Final Calculation
Now, we will sum the lone pairs from each molecule:
\[ \text{Total Lone Pairs} = 1 (SF_4) + 0 (CF_4) + 2 (XeF_4) + 3 (XeF_2) + 2 (ClF_3) = 8 \]

### Conclusion
The sum of lone pairs of electrons on the central atom of \( SF_4, CF_4, XeF_4, XeF_2, \) and \( ClF_3 \) is **8**.

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