Question

question 3 (2 points)
consider sulfur dioxide, so₂. the lewis structure has one single bond and one double bond.
the number of reds is 1.
the bond angles are 2° and the shape is 3.
so₂ 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 k. planar trigonal m. bent
n. pyramidal o. tetrahedral p. symmetrical q. asymmetrical

Explanation:

Step1: Determine the number of REDs (Region of Electron Density)

Sulfur has 6 valence electrons. In \(SO_2\), sulfur forms one single bond and one double bond with oxygen atoms and has one lone pair. The formula for REDs is number of bonds (single + double + triple) + number of lone pairs. Here, number of bonds \(= 2\) (one single and one double, counted as two regions) and lone pairs \(= 1\). So REDs \(=2 + 1=3\).

Step2: Determine the bond angle

For a molecule with 3 REDs (trigonal - planar electron - pair geometry) and one lone pair, the bond angle is approximately \(120^{\circ}\) (due to the repulsion from the lone pair).

Step3: Determine the molecular shape

With 3 REDs (trigonal - planar electron - pair geometry) and one lone pair, the molecular shape is bent.

Step4: Determine symmetry

\(SO_2\) has a bent shape. The oxygen atoms are not arranged symmetrically around the sulfur atom (because of the lone pair on sulfur). So it is an asymmetrical molecule.

Answer:

1. D. 3
2. H. 120
3. M. bent
4. Q. asymmetrical