What is the molecular geometry of ozone (O_3)?

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

Answer: (C)

Verified step by step guidance

1. Step 1: Draw the Lewis structure of ozone (O_3). Count the total valence electrons: each oxygen atom has 6 valence electrons, so for 3 oxygens, total electrons = 3 \times 6 = 18.
2. Step 2: Arrange the atoms with one oxygen in the center and the other two oxygens bonded to it. Connect the atoms with single bonds initially, then distribute the remaining electrons to satisfy the octet rule for each atom.
3. Step 3: Identify the presence of any lone pairs on the central oxygen atom. In ozone, the central oxygen has one lone pair of electrons after forming bonds with the two outer oxygens.
4. Step 4: Use the VSEPR (Valence Shell Electron Pair Repulsion) theory to determine the molecular geometry. The central atom has three regions of electron density (two bonding pairs and one lone pair), which corresponds to a trigonal planar electron geometry but results in a bent molecular shape due to the lone pair repulsion.
5. Step 5: Conclude that the molecular geometry of ozone is bent because the lone pair on the central oxygen atom pushes the bonded atoms closer together, creating an angle less than 120°.