A molecule possessing dipole moment is

Options

A. `CH_(4)`
B. `H_(2)O`
C. `BF_(3)`
D. `CO_(2)`

Answer

To determine which molecule possesses a dipole moment, we will analyze each of the given options: CH4, H2O, BF3, and CO2.

### Step 1: Analyze CH4 (Methane)
- **Hybridization**: CH4 is sp³ hybridized.
- **Molecular Geometry**: It has a tetrahedral structure.
- **Dipole Moment**: The individual C-H bonds have dipole moments, but due to the symmetrical tetrahedral shape, these dipole moments cancel each other out.
- **Net Dipole Moment**: The net dipole moment is zero.

### Step 2: Analyze H2O (Water)
- **Hybridization**: H2O is also sp³ hybridized.
- **Molecular Geometry**: It has a bent or V-shaped structure due to the presence of two lone pairs on the oxygen atom.
- **Dipole Moment**: The O-H bonds are polar due to the difference in electronegativity between oxygen and hydrogen. The lone pairs also contribute to the dipole moment.
- **Net Dipole Moment**: The dipole moments do not cancel out, resulting in a net dipole moment. Therefore, H2O is a polar molecule.

### Step 3: Analyze BF3 (Boron Trifluoride)
- **Hybridization**: BF3 is sp² hybridized.
- **Molecular Geometry**: It has a trigonal planar structure.
- **Dipole Moment**: The B-F bonds are polar, but due to the symmetrical trigonal planar shape, the dipole moments cancel each other out.
- **Net Dipole Moment**: The net dipole moment is zero.

### Step 4: Analyze CO2 (Carbon Dioxide)
- **Hybridization**: CO2 is sp hybridized.
- **Molecular Geometry**: It has a linear structure.
- **Dipole Moment**: The C=O bonds are polar, but the linear shape causes the dipole moments to cancel each other out.
- **Net Dipole Moment**: The net dipole moment is zero.

### Conclusion
Among the given options, only **H2O** possesses a dipole moment.

### Final Answer
The molecule possessing a dipole moment is **H2O**.

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