`SbF_(3)` reacts with `XeF_(4) and XeF_(6)` to form ionic compounds `[XeF_(3)^(+)][SbF_(6)^(+)] and [XeF_(5)^(+)][SbF_(6)^(-)]` then molecular shape of `[XeF_(3)^(+)]` ion and `[XeF_(5)^(+)]` ion respectively

Options

A. square pyramidal, T - shaped
B. Bent - T - shape, square pyramidal
C. See - saw, square pyramidal
D. Square pyramidal, See - saw

Answer

To determine the molecular shapes of the ions \([XeF_3^+]\) and \([XeF_5^+]\), we can follow these steps:

### Step 1: Determine the Valence Electrons for Xenon in Each Ion
- **For \([XeF_3^+]\)**:
- Xenon (Xe) has 8 valence electrons.
- Since it is a cation (\(+\)), we subtract 1 electron: \(8 - 1 = 7\) valence electrons.

- **For \([XeF_5^+]\)**:
- Again, starting with 8 valence electrons for xenon, we subtract 1: \(8 - 1 = 7\) valence electrons.

### Step 2: Count the Bonding Pairs
- **For \([XeF_3^+]\)**:
- There are 3 fluorine atoms bonded to xenon, which means there are 3 bonding pairs.

- **For \([XeF_5^+]\)**:
- There are 5 fluorine atoms bonded to xenon, resulting in 5 bonding pairs.

### Step 3: Calculate the Number of Lone Pairs
- **For \([XeF_3^+]\)**:
- Total electrons available = 7
- Electrons used in bonding = \(3 \text{ (bonding pairs)} \times 2 = 6\)
- Remaining electrons = \(7 - 6 = 1\)
- This means there are 1 lone pair.

- **For \([XeF_5^+]\)**:
- Total electrons available = 7
- Electrons used in bonding = \(5 \text{ (bonding pairs)} \times 2 = 10\)
- Since we only have 7 electrons, we cannot have lone pairs in this case. Thus, there are 0 lone pairs.

### Step 4: Determine the Hybridization
- **For \([XeF_3^+]\)**:
- Total pairs = 3 (bonding pairs) + 1 (lone pair) = 4 pairs.
- Hybridization = \(sp^3\).

- **For \([XeF_5^+]\)**:
- Total pairs = 5 (bonding pairs) + 0 (lone pairs) = 5 pairs.
- Hybridization = \(sp^3d\).

### Step 5: Determine the Molecular Shapes
- **For \([XeF_3^+]\)**:
- With 3 bonding pairs and 1 lone pair, the molecular shape is **T-shaped**.

- **For \([XeF_5^+]\)**:
- With 5 bonding pairs and 0 lone pairs, the molecular shape is **square pyramidal**.

### Conclusion
- The molecular shape of \([XeF_3^+]\) is **T-shaped**.
- The molecular shape of \([XeF_5^+]\) is **square pyramidal**.

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