The shape of `XeF_3^+` is

Options

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

Answer

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

### Step 1: Identify the central atom and its valence electrons
- The central atom in \( \text{XeF}_3^+ \) is xenon (Xe).
- Xenon is in group 18 of the periodic table and has 8 valence electrons.

### Step 2: Determine the number of fluorine atoms and their contribution
- There are 3 fluorine (F) atoms, and each fluorine atom contributes 1 electron for bonding.
- Therefore, the total number of electrons contributed by the fluorine atoms is \( 3 \times 1 = 3 \) electrons.

### Step 3: Account for the positive charge
- The positive charge \( (+1) \) means we have one less electron to consider.
- Thus, the total number of electrons to consider for bonding is \( 8 \, (\text{from Xe}) + 3 \, (\text{from F}) - 1 \, (\text{positive charge}) = 10 \) electrons.

### Step 4: Determine the hybridization
- The number of electron pairs is calculated by dividing the total number of electrons by 2:
\[ \text{Number of electron pairs} = \frac{10}{2} = 5 \]
- This indicates that the hybridization of xenon in \( \text{XeF}_3^+ \) is \( \text{sp}^3\text{d} \).

### Step 5: Determine the molecular geometry
- In \( \text{sp}^3\text{d} \) hybridization, there are 5 hybrid orbitals.
- Since there are 3 bonding pairs (from the 3 fluorine atoms) and 2 lone pairs of electrons, the arrangement of the electron pairs is trigonal bipyramidal.
- However, the presence of 2 lone pairs will affect the shape. The lone pairs will occupy the equatorial positions to minimize repulsion, leaving the bonding pairs in a T-shaped configuration.

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

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

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