Which of the following best describes the electron geometry around each oxygen atom in an O2 molecule?

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

Answer: (C)

Verified step by step guidance

1. Recall that the electron geometry around an atom is determined by the regions of electron density (bonding and lone pairs) around that atom.
2. Consider the Lewis structure of the O\_2 molecule: each oxygen atom is bonded to the other oxygen atom by a double bond, and each oxygen atom has two lone pairs of electrons.
3. Count the total regions of electron density around one oxygen atom: there is one bonding region (the double bond counts as one region) and two lone pairs, making a total of three regions.
4. According to VSEPR theory, three regions of electron density around an atom correspond to a trigonal planar electron geometry.
5. However, since the question asks specifically about the electron geometry around each oxygen atom in O\_2, and the molecule is diatomic with a double bond and lone pairs, the overall shape of the molecule is linear, but the electron geometry around each oxygen atom is trigonal planar due to the three regions of electron density.