Question

question 2 (2 points)
consider sulfur trioxide, so3. the lewis structure has 2 single bonds and one double bond.
the number of reds is 1.
the bond angles are 2 ° and the shape is 3.
so3 is a 4 symmetrical/asymmetrical molecule.
a. 0 b. 1 c. 2 d. 3 e. 4 f. 180 g. 90 h. 120
i. 109.5 j. diatomic k. linear l. planar trigonal m. bent
n. pyramidal o. tetrahedral p. symmetrical q. asymmetrical

Explanation:

• Number of REDs (Region of Electron Density): In \(SO_3\), using the formula for REDs (bonds + lone pairs). Sulfur has 3 bonds (2 single + 1 double, but in VSEPR, double/triple bonds count as one region) and 0 lone pairs. So, \(3 + 0=3\).
• Bond Angles: For a molecule with 3 REDs and no lone pairs (trigonal planar geometry), the bond angle is \(120^{\circ}\) (based on VSEPR theory).
• Shape: With 3 REDs and no lone pairs, the shape is planar trigonal (VSEPR - trigonal planar geometry).
• Symmetry: \(SO_3\) has a planar trigonal shape. The dipoles (if any, but \(S - O\) bonds have some polarity) cancel out due to the symmetrical planar trigonal arrangement. So, it is a symmetrical molecule.

Answer:

1. D. 3
2. H. 120
3. L. planar trigonal
4. P. symmetrical