To determine which of the given compounds has a pyramidal shape, we will analyze each of the options provided: XeF4, XeO3, XeF2, and XeF6.
### Step 1: Analyze XeF4
- **Valence Electrons**: Xenon (Xe) has 8 valence electrons. In XeF4, it forms 4 bonds with fluorine atoms.
- **Lone Pairs**: After forming 4 bonds, there are 2 lone pairs remaining on the xenon atom.
- **Hybridization**: The hybridization for XeF4 is sp³d².
- **Shape**: With 4 bond pairs and 2 lone pairs, the molecular geometry is square planar, not pyramidal.
### Step 2: Analyze XeO3
- **Valence Electrons**: Xenon has 8 valence electrons. In XeO3, it forms 3 bonds with oxygen atoms.
- **Lone Pairs**: After forming 3 bonds, there is 1 lone pair remaining on the xenon atom.
- **Hybridization**: The hybridization for XeO3 is sp³.
- **Shape**: With 3 bond pairs and 1 lone pair, the molecular geometry is trigonal pyramidal. This indicates that XeO3 has a pyramidal shape.
### Step 3: Analyze XeF2
- **Valence Electrons**: Xenon has 8 valence electrons. In XeF2, it forms 2 bonds with fluorine atoms.
- **Lone Pairs**: After forming 2 bonds, there are 3 lone pairs remaining on the xenon atom.
- **Hybridization**: The hybridization for XeF2 is sp³d.
- **Shape**: With 2 bond pairs and 3 lone pairs, the molecular geometry is linear, not pyramidal.
### Step 4: Analyze XeF6
- **Valence Electrons**: Xenon has 8 valence electrons. In XeF6, it forms 6 bonds with fluorine atoms.
- **Lone Pairs**: After forming 6 bonds, there are no lone pairs remaining on the xenon atom.
- **Hybridization**: The hybridization for XeF6 is sp³d³.
- **Shape**: With 6 bond pairs and no lone pairs, the molecular geometry is octahedral, not pyramidal.
### Conclusion
After analyzing all four compounds, we find that **XeO3 (xenon trioxide)** is the only compound with a pyramidal shape.
### Final Answer
The compound that has a pyramidal shape is **XeO3**.
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