The dipole moment of `AX_(3), BX_(3)and CX_(3)` are 1.5 D, 0.5 D and 0 D respectively. The possible shapes of molecules may be (consider C has no Lone pair) (A, B and C are more electronegative than X)

Options

A. Pyramidal, T- shape, Trigonal planar respectively.
B. T - shape, Pyramidal, Square planar respectively.
C. T-shape, Pyramidal, Trigonal planar respectively.
D. Pyramidal, T- shape, Square planar respectively

Answer

To determine the possible shapes of the molecules AX₃, BX₃, and CX₃ based on their dipole moments (1.5 D, 0.5 D, and 0 D respectively), we will analyze the molecular geometry and hybridization of each molecule.

### Step 1: Analyze the dipole moments
- **AX₃** has a dipole moment of **1.5 D**. This indicates that the molecule has a net dipole moment, suggesting that it is likely to have an asymmetrical shape, which can be due to the presence of a lone pair of electrons.
- **BX₃** has a dipole moment of **0.5 D**. This suggests that the molecule is less polar than AX₃, indicating that it may have a slightly asymmetrical shape or a geometry that allows for some cancellation of dipole moments.
- **CX₃** has a dipole moment of **0 D**. This indicates that the molecule is symmetrical, meaning that the dipole moments cancel out completely.

### Step 2: Determine the hybridization and geometry
- For **AX₃**:
- Given that A is more electronegative than X and assuming A has one lone pair, the hybridization would be **sp³** (3 bond pairs and 1 lone pair). This leads to a **trigonal pyramidal** shape.

- For **BX₃**:
- If B has no lone pairs and is still more electronegative than X, it would have **sp²** hybridization (3 bond pairs). This would result in a **trigonal planar** shape. The slight dipole moment indicates that the molecule is not perfectly symmetrical, possibly due to slight differences in bond angles or bond lengths.

- For **CX₃**:
- Since C has no lone pairs and is more electronegative than X, it would also have **sp²** hybridization (3 bond pairs). The symmetry of this arrangement leads to a **trigonal planar** shape, resulting in a dipole moment of **0 D**.

### Conclusion:
- **AX₃**: Trigonal pyramidal shape (1.5 D dipole moment)
- **BX₃**: Trigonal planar shape (0.5 D dipole moment)
- **CX₃**: Trigonal planar shape (0 D dipole moment)

### Summary of Shapes:
- AX₃: Trigonal pyramidal
- BX₃: Trigonal planar
- CX₃: Trigonal planar