Dipolemoment is not zero for

Options

A. `PCl_5`
B. `ClF_3`
C. `XeF_4`
D. `C_2H_5C -=C C_2H_5`

Explanation

To determine which molecule has a dipole moment that is not zero, we will analyze each option provided in the question. Let's go through the analysis step by step:

### Step 1: Analyze PCl5
- **Hybridization**: PCl5 has a hybridization of sp³d.
- **Geometry**: The molecular geometry is trigonal bipyramidal.
- **Symmetry**: In this structure, the chlorine atoms are arranged in a symmetrical manner with 120-degree angles in the equatorial plane and 90-degree angles in the axial plane.
- **Dipole Moment**: Due to the symmetry of the molecule, the dipole moments of the bonds cancel each other out, resulting in a net dipole moment of zero.

**Hint**: Check the geometry and symmetry of the molecule to determine if the dipole moments cancel out.

### Step 2: Analyze ClF3
- **Hybridization**: ClF3 has a hybridization of sp³d.
- **Geometry**: The molecular geometry is T-shaped due to the presence of two lone pairs on the chlorine atom.
- **Symmetry**: The presence of lone pairs causes the molecule to be unsymmetrical. The bond dipoles do not cancel out completely because of the lone pairs.
- **Dipole Moment**: The dipole moments from the fluorine atoms do not cancel out, leading to a net dipole moment that is not zero.

**Hint**: Look for lone pairs and molecular geometry to determine if the molecule is symmetrical or not.

### Step 3: Analyze XeF4
- **Hybridization**: XeF4 has a hybridization of sp³d².
- **Geometry**: The molecular geometry is square planar.
- **Symmetry**: The four fluorine atoms are arranged symmetrically around the xenon atom, with lone pairs positioned above and below the plane of the fluorine atoms.
- **Dipole Moment**: The symmetry of the molecule means that the dipole moments cancel each other out, resulting in a net dipole moment of zero.

**Hint**: Assess the arrangement of atoms and lone pairs to evaluate symmetry.

### Step 4: Analyze C2H5-C2H5
- **Hybridization**: The molecule is primarily sp³ hybridized due to the presence of single bonds.
- **Geometry**: The molecule is symmetrical with respect to the central carbon-carbon bond.
- **Symmetry**: The identical ethyl groups on both sides create a symmetrical structure.
- **Dipole Moment**: The dipole moments from the bonds cancel out due to symmetry, resulting in a net dipole moment of zero.

**Hint**: Identify if the molecule has identical groups on both sides to determine symmetry.

### Conclusion
After analyzing all the options, we conclude that the dipole moment is not zero for **ClF3** due to its unsymmetrical shape caused by lone pairs. Therefore, the answer is:

**The dipole moment is not zero for ClF3.**