The shape of `XeF_(3)^(+)` is :

Options

A. Trigonal planar
B. Pyramidal
C. Bent T-shpae
D. See-saw

Explanation

To determine the shape of the ion \( \text{XeF}_3^+ \), we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Central Atom and Its Valence Electrons**:
- The central atom in this molecule is xenon (Xe), which is a noble gas. Noble gases have a full outer shell of 8 electrons. However, since we have a positive charge (\(+\)), xenon will effectively have 7 valence electrons.

2. **Determine the Number of Bonds Formed**:
- Xenon forms three bonds with three fluorine (F) atoms. Each fluorine atom contributes one electron to the bond, resulting in three bonding pairs.

3. **Calculate the Number of Lone Pairs**:
- After forming three bonds, we subtract the number of bonding electrons from the total valence electrons.
- Initially, xenon has 7 electrons. Each bond with fluorine uses 1 electron, so:
\[ \text{Remaining electrons} = 7 - 3 = 4 \]
- These remaining 4 electrons will form 2 lone pairs.

4. **Count Bond Pairs and Lone Pairs**:
- We now have:
- Bond pairs: 3 (from the three Xe-F bonds)
- Lone pairs: 2 (remaining electrons)

5. **Determine Hybridization**:
- Hybridization can be determined using the formula:
\[ \text{Hybridization} = \text{Number of bond pairs} + \text{Number of lone pairs} = 3 + 2 = 5 \]
- The hybridization of 5 corresponds to \( \text{sp}^3\text{d} \).

6. **Predict the Molecular Geometry**:
- For a molecule with \( \text{sp}^3\text{d} \) hybridization and 3 bond pairs and 2 lone pairs, the molecular geometry is T-shaped. This is because the lone pairs will occupy equatorial positions to minimize repulsion, leaving the bond pairs to form a T-shape.

7. **Conclusion**:
- Therefore, the shape of \( \text{XeF}_3^+ \) is T-shaped.

### Final Answer:
The shape of \( \text{XeF}_3^+ \) is T-shaped.