Which of the following molecule is planar as well as polar :

Options

A. `PCl_(3)`
B. `SF_(4)`
C. `ClF_(3)`
D. None of these

Answer

To determine which of the following molecules is both planar and polar, we will analyze each molecule's hybridization, shape, and dipole moment.

### Step-by-Step Solution:

1. **Identify the Molecules**: We need to analyze the given molecules one by one. Let's assume the molecules are phosphorus trichloride (PCl3), sulfur tetrafluoride (SF4), and chlorine trifluoride (ClF3).

2. **Calculate Hybridization and Shape for PCl3**:
- **Valence Electrons**: Phosphorus (P) has 5 valence electrons, and there are 3 chlorine (Cl) atoms, each contributing 1 electron.
- **Total**: 5 (P) + 3 (Cl) = 8 electrons.
- **Hybridization**: The number of hybrid orbitals (x) = 5 (valence electrons) - 0 (no charge) + 3 (monovalent atoms) = 4.
- **Shape**: With 3 bond pairs and 1 lone pair, the shape is trigonal pyramidal, which is non-planar.

3. **Calculate Hybridization and Shape for SF4**:
- **Valence Electrons**: Sulfur (S) has 6 valence electrons, and there are 4 fluorine (F) atoms.
- **Total**: 6 (S) + 4 (F) = 10 electrons.
- **Hybridization**: The number of hybrid orbitals (x) = 6 (valence electrons) - 0 (no charge) + 4 (monovalent atoms) = 5.
- **Shape**: With 4 bond pairs and 1 lone pair, the shape is seesaw, which is also non-planar.

4. **Calculate Hybridization and Shape for ClF3**:
- **Valence Electrons**: Chlorine (Cl) has 7 valence electrons, and there are 3 fluorine (F) atoms.
- **Total**: 7 (Cl) + 3 (F) = 10 electrons.
- **Hybridization**: The number of hybrid orbitals (x) = 7 (valence electrons) - 0 (no charge) + 3 (monovalent atoms) = 10.
- **Shape**: With 3 bond pairs and 2 lone pairs, the shape is T-shaped, which is planar.

5. **Determine Polarity**:
- For PCl3, the dipole moment is directed towards Cl, but due to its pyramidal shape, it is non-planar and thus non-polar.
- For SF4, the seesaw shape leads to cancellation of some dipole moments, resulting in a net dipole moment, but it is non-planar.
- For ClF3, the T-shaped structure has a net dipole moment directed towards the more electronegative fluorine atoms, making it polar.

### Conclusion:
The molecule that is both planar and polar is **ClF3**.

### Final Answer:
**ClF3** is the correct answer.

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