Molecular shape of `XeF_(2), BeF_(2) and CF_(2)` are :

Options

A. the same, with 3, 0 and 0 lone pair of electrons respectively
B. the same, with 3, 1 and 0 lone pair of electrons respectively
C. different, with 0, 1 and 2 lone pair of electrons respectively
D. different, with 3, 0 and 1 lone pair of electrons respectively

Explanation

To determine the molecular shapes of `XeF2`, `BeF2`, and `CF2`, we will analyze the number of valence electrons, bond pairs, and lone pairs for each molecule. Here’s a step-by-step solution:

### Step 1: Determine the Valence Electrons
- **XeF2 (Xenon Difluoride)**:
- Xenon (Xe) has 8 valence electrons.
- Each Fluorine (F) has 7 valence electrons, and there are 2 fluorine atoms: 2 × 7 = 14.
- Total valence electrons = 8 + 14 = 22.

- **BeF2 (Beryllium Difluoride)**:
- Beryllium (Be) has 2 valence electrons.
- Each Fluorine (F) has 7 valence electrons, and there are 2 fluorine atoms: 2 × 7 = 14.
- Total valence electrons = 2 + 14 = 16.

- **CF2 (Carbon Difluoride)**:
- Carbon (C) has 4 valence electrons.
- Each Fluorine (F) has 7 valence electrons, and there are 2 fluorine atoms: 2 × 7 = 14.
- Total valence electrons = 4 + 14 = 18.

### Step 2: Determine Bond Pairs and Lone Pairs
- **XeF2**:
- Xenon forms 2 bonds with fluorine atoms.
- Total bond pairs = 2.
- Total lone pairs = (Total valence electrons - Bonding electrons) / 2 = (22 - 4) / 2 = 9 lone pairs.
- However, in the VSEPR theory, we consider only the lone pairs that affect the shape, which are 3 lone pairs.

- **BeF2**:
- Beryllium forms 2 bonds with fluorine atoms.
- Total bond pairs = 2.
- Total lone pairs = (Total valence electrons - Bonding electrons) / 2 = (16 - 4) / 2 = 6 lone pairs.
- However, in this case, Be does not have any lone pairs that affect the shape, so it has 0 lone pairs.

- **CF2**:
- Carbon forms 2 bonds with fluorine atoms.
- Total bond pairs = 2.
- Total lone pairs = (Total valence electrons - Bonding electrons) / 2 = (18 - 4) / 2 = 7 lone pairs.
- However, carbon has 1 lone pair that affects the shape.

### Step 3: Determine Molecular Shapes
- **XeF2**:
- With 2 bond pairs and 3 lone pairs, the shape is linear (due to the arrangement of lone pairs in the equatorial position).

- **BeF2**:
- With 2 bond pairs and 0 lone pairs, the shape is linear.

- **CF2**:
- With 2 bond pairs and 1 lone pair, the shape is bent.

### Summary of Shapes
- **XeF2**: Linear
- **BeF2**: Linear
- **CF2**: Bent

### Final Answer
- The molecular shapes of `XeF2`, `BeF2`, and `CF2` are linear, linear, and bent, respectively.