Determine the Cl–O–Cl bond angle for the OCl₂ molecule.

• A. >109.5°
• B. <109.5°
• C. >120°
• D. <120°

Answer: (B)

Verified step by step guidance

1. First, recognize that OCl2 is a molecule with a central oxygen atom bonded to two chlorine atoms. This is similar to the structure of water (H2O), where the central atom is also oxygen.
2. Understand that the electron geometry around the central oxygen atom is tetrahedral due to the presence of two bonding pairs (O-Cl bonds) and two lone pairs of electrons.
3. Recall that the ideal bond angle for a tetrahedral electron geometry is 109.5°. However, lone pairs occupy more space than bonding pairs, causing the bond angle to be less than 109.5°.
4. Consider the effect of the lone pairs on the bond angle. The repulsion between the lone pairs is greater than the repulsion between the bonding pairs, which compresses the Cl–O–Cl bond angle.
5. Conclude that the Cl–O–Cl bond angle in OCl2 is less than 109.5° due to the repulsion caused by the lone pairs on the oxygen atom.