`SbF_5` reacts with `XeF_4` and `XeF_6` to form ionic compounds `[XeF_3^+][SbF_6]^-` and `[XeF_5^+][SbF_6^-]`.
The geometry of `XeF_3^+` ion and` XeF_5^+` ion, respectively, is :-

Options

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

Answer

To determine the geometry of the ions \( [XeF_3^+] \) and \( [XeF_5^+] \), we will analyze the valence electrons and the bonding arrangements for each ion.

### Step 1: Analyze \( [XeF_3^+] \)

1. **Count the Valence Electrons**:
- Xenon (Xe) has 8 valence electrons.
- Each fluorine (F) contributes 1 electron, and there are 3 fluorine atoms, contributing a total of 3 electrons.
- Therefore, the total number of valence electrons is \( 8 + 3 = 11 \).
- Since it has a positive charge (+1), we lose 1 electron, resulting in \( 11 - 1 = 10 \) electrons.

2. **Determine the Bonding and Lone Pairs**:
- Out of the 10 electrons, 3 are used for bonding with the 3 fluorine atoms.
- This leaves us with \( 10 - 6 = 4 \) electrons remaining.
- These 4 electrons will form 2 lone pairs.

3. **Calculate the Steric Number**:
- The steric number is the sum of the number of bonding pairs and lone pairs.
- Here, we have 3 bonding pairs (from the 3 F atoms) and 2 lone pairs.
- Thus, the steric number is \( 3 + 2 = 5 \).

4. **Determine the Geometry**:
- With a steric number of 5 and 2 lone pairs, the molecular geometry is based on the arrangement of the bonding pairs.
- The ideal arrangement for a steric number of 5 is trigonal bipyramidal, but with 2 lone pairs, the shape is altered to T-shaped.

### Step 2: Analyze \( [XeF_5^+] \)

1. **Count the Valence Electrons**:
- Again, Xenon has 8 valence electrons.
- Each of the 5 fluorine atoms contributes 1 electron, giving a total of 5 electrons.
- Therefore, the total number of valence electrons is \( 8 + 5 = 13 \).
- With a positive charge (+1), we lose 1 electron, resulting in \( 13 - 1 = 12 \) electrons.

2. **Determine the Bonding and Lone Pairs**:
- Out of the 12 electrons, 5 are used for bonding with the 5 fluorine atoms.
- This leaves us with \( 12 - 10 = 2 \) electrons remaining.
- These 2 electrons will form 1 lone pair.

3. **Calculate the Steric Number**:
- The steric number is the sum of the number of bonding pairs and lone pairs.
- Here, we have 5 bonding pairs (from the 5 F atoms) and 1 lone pair.
- Thus, the steric number is \( 5 + 1 = 6 \).

4. **Determine the Geometry**:
- With a steric number of 6 and 1 lone pair, the molecular geometry is based on the arrangement of the bonding pairs.
- The ideal arrangement for a steric number of 6 is octahedral, but with 1 lone pair, the shape is altered to square pyramidal.

### Final Answer:
- The geometry of \( [XeF_3^+] \) is T-shaped.
- The geometry of \( [XeF_5^+] \) is square pyramidal.