The bond angle of `Cl_(2)O` is:

Options

A. Smaller than that of `F_(2)O`
B. Greater than that of `H_(2)O`
C. Smaller than that of `H_(2)O`
D. Same as the of `F_(2)O`

Explanation

To determine the bond angle of Cl₂O (dichlorine monoxide), we can follow these steps:

### Step 1: Determine the molecular structure of Cl₂O
- Cl₂O consists of two chlorine (Cl) atoms and one oxygen (O) atom.
- The oxygen atom is the central atom, with the two chlorine atoms bonded to it.

### Step 2: Draw the Lewis structure
- Oxygen has six valence electrons, and each chlorine has seven valence electrons.
- In total, Cl₂O has 20 valence electrons (6 from O + 7*2 from Cl).
- The Lewis structure shows the oxygen atom bonded to two chlorine atoms with lone pairs on the oxygen atom.

### Step 3: Identify the shape of the molecule
- The molecular geometry can be determined using the VSEPR (Valence Shell Electron Pair Repulsion) theory.
- The oxygen atom has two bonding pairs (from Cl) and two lone pairs, resulting in a bent shape.

### Step 4: Calculate the bond angle
- The bond angle in Cl₂O is approximately 110.9 degrees. This is due to the repulsion between the lone pairs which pushes the bonding pairs closer together.

### Step 5: Compare with other molecules
- For comparison, the bond angles of F₂O (approximately 103 degrees) and H₂O (approximately 104.5 degrees) can be noted.
- This shows that the bond angle in Cl₂O is greater than both F₂O and H₂O.

### Conclusion
- The bond angle of Cl₂O is approximately 110.9 degrees, which is greater than that of H₂O and F₂O.