Molecular shape of `ClF_(3) , l_(3)^(-)` and `XeO_(3)` respectively are

Options

A. T-shape , Linear , Pyramidal
B. Planar , Linear , Tetrahedral
C. T-shape , Planar , Pyramidal
D. Trigonal bipyramidal , Linear , Tetrahedral

Answer

To determine the molecular shapes of ClF3, I3^(-), and XeO3, we will follow a systematic approach that involves calculating the hybridization of each molecule and then deducing the shapes based on the number of bond pairs and lone pairs.

### Step 1: Determine the Hybridization of ClF3
1. **Identify the central atom**: In ClF3, chlorine (Cl) is the central atom.
2. **Count the valence electrons of Cl**: Chlorine has 7 valence electrons.
3. **Count the number of monovalent atoms**: There are 3 fluorine (F) atoms, each contributing 1 electron.
4. **Consider the charge**: There is no charge on ClF3.
5. **Use the hybridization formula**:
\[ \text{Hybridization} = \frac{1}{2} \left( \text{Valence electrons of central atom} + \text{Number of monovalent atoms} + \text{Charge} \right) \]
\[ = \frac{1}{2} (7 + 3 + 0) = \frac{10}{2} = 5 \]
This indicates sp3d hybridization.

6. **Determine bond pairs and lone pairs**: ClF3 has 3 bond pairs (from Cl-F bonds) and 2 lone pairs.
7. **Determine the molecular shape**: With 3 bond pairs and 2 lone pairs, the shape is T-shaped.

### Step 2: Determine the Hybridization of I3^(-)
1. **Identify the central atom**: In I3^(-), iodine (I) is the central atom.
2. **Count the valence electrons of I**: Iodine has 7 valence electrons.
3. **Count the number of monovalent atoms**: There are 2 iodine atoms bonded to the central iodine.
4. **Consider the charge**: The ion has a -1 charge.
5. **Use the hybridization formula**:
\[ \text{Hybridization} = \frac{1}{2} (7 + 2 + 1) = \frac{10}{2} = 5 \]
This also indicates sp3d hybridization.

6. **Determine bond pairs and lone pairs**: I3^- has 2 bond pairs (from I-I bonds) and 3 lone pairs.
7. **Determine the molecular shape**: With 2 bond pairs and 3 lone pairs, the shape is linear.

### Step 3: Determine the Hybridization of XeO3
1. **Identify the central atom**: In XeO3, xenon (Xe) is the central atom.
2. **Count the valence electrons of Xe**: Xenon has 8 valence electrons.
3. **Count the number of monovalent atoms**: There are no monovalent atoms.
4. **Consider the charge**: There is no charge on XeO3.
5. **Use the hybridization formula**:
\[ \text{Hybridization} = \frac{1}{2} (8 + 0 + 0) = \frac{8}{2} = 4 \]
This indicates sp3 hybridization.

6. **Determine bond pairs and lone pairs**: XeO3 has 3 bond pairs (from Xe-O bonds) and 1 lone pair.
7. **Determine the molecular shape**: With 3 bond pairs and 1 lone pair, the shape is pyramidal.

### Final Summary of Molecular Shapes
- ClF3: T-shaped
- I3^(-): Linear
- XeO3: Pyramidal

### Answer
The molecular shapes of ClF3, I3^(-), and XeO3 are T-shaped, linear, and pyramidal, respectively.