Which one of the following molecule is polar?

Options

A. `XeF_4`
B. `IF_5`
C. `SbF_5`
D. `CF_4`

Answer

To determine which molecule among the given options is polar, we need to analyze the molecular geometry and the presence of dipole moments in each molecule. A polar molecule has an uneven distribution of electron density, leading to a dipole moment that is not equal to zero. Here’s a step-by-step solution:

### Step 1: Identify the Molecular Structures
We need to examine the molecular structures of the given molecules to determine their symmetry and polarity.

### Step 2: Analyze the First Molecule (XeF4)
- **Structure**: Square planar
- **Symmetry**: This molecule is symmetrical.
- **Dipole Moment**: Since it is symmetrical, the dipole moment is zero.
- **Conclusion**: XeF4 is a non-polar molecule.

### Step 3: Analyze the Second Molecule (IF5)
- **Structure**: Square pyramidal
- **Symmetry**: This molecule has a lone pair, making it asymmetrical.
- **Dipole Moment**: The dipole moment is not equal to zero due to the asymmetrical shape.
- **Conclusion**: IF5 is a polar molecule.

### Step 4: Analyze the Third Molecule (SbF5)
- **Structure**: Trigonal bipyramidal
- **Symmetry**: This molecule is symmetrical.
- **Dipole Moment**: The dipole moment is zero.
- **Conclusion**: SbF5 is a non-polar molecule.

### Step 5: Analyze the Fourth Molecule (CF4)
- **Structure**: Tetrahedral
- **Symmetry**: This molecule is symmetrical.
- **Dipole Moment**: The dipole moment is zero.
- **Conclusion**: CF4 is a non-polar molecule.

### Final Conclusion
Among the analyzed molecules, **IF5** is the only polar molecule.