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. Understand the molecular geometry of OCl2. OCl2 is similar to water (H2O) in terms of its molecular shape, which is bent due to the presence of lone pairs on the oxygen atom.
2. Recall that the ideal bond angle for a tetrahedral geometry is 109.5°, but the presence of lone pairs can alter this angle. Lone pairs repel more strongly than bonded pairs, causing the bond angle to decrease.
3. Consider the electron pair geometry around the oxygen atom in OCl2. Oxygen has two lone pairs and two bonding pairs, leading to a bent shape similar to H2O.
4. Recognize that the bond angle in a bent molecule like OCl2 is typically less than the ideal tetrahedral angle of 109.5° due to the repulsion caused by lone pairs.
5. Conclude that the Cl–O–Cl bond angle in OCl2 is less than 120° but greater than 109.5°, as the lone pairs push the chlorine atoms closer together, reducing the bond angle from the ideal tetrahedral angle.