Which of the following best describes the molecular geometry of ozone (O3)?

• A. Bent
• B. Linear
• C. Trigonal planar
• D. Tetrahedral

Answer: (A)

Verified step by step guidance

1. Step 1: Draw the Lewis structure of ozone (O\_3). Ozone has a total of 18 valence electrons (6 from each oxygen atom). Arrange the atoms with one oxygen in the center and the other two on the sides, then distribute electrons to satisfy the octet rule as much as possible.
2. Step 2: Determine the number of electron domains around the central oxygen atom. Count both bonding pairs (single or double bonds) and lone pairs of electrons on the central atom.
3. Step 3: Use the VSEPR (Valence Shell Electron Pair Repulsion) theory to predict the molecular geometry. The shape depends on the number of bonding pairs and lone pairs around the central atom, as electron pairs repel each other to minimize repulsion.
4. Step 4: Identify that the central oxygen in ozone has two bonding pairs and one lone pair, which corresponds to three electron domains. According to VSEPR, three electron domains with one lone pair result in a bent molecular geometry.
5. Step 5: Conclude that the molecular geometry of ozone is bent, not linear, trigonal planar, or tetrahedral, because the lone pair on the central oxygen atom causes a deviation from a straight line.