question 2 (2 points)
planar trigonal molecules like so₃ with __1__ reds are __2__
symmetrical/asymmetrical and __3__ nonpolar/polar
planar trigonal molecules like so₂s with __4__ reds are __5__
symmetrical/asymmetrical and __6__ nonpolar/polar
bent molecules like so₂ with __7__ reds are __8__ symmetrical/asymmetrical and
__9__ nonpolar/polar
a. symmetrical b. asymmetrical c. nonpolar d. polar
e. 0 f. 1 g. 2 h. 3 i. 4

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Accepted Answer

# Brief Explanations:
- For $SO_3$:
    - The number of regions of electron - density (REDS) around the central $S$ atom is calculated. Using the formula $n=\frac{V + M - C + A}{2}$ (where $V$ is the valence electrons of the central atom, $M$ is the number of monovalent atoms, $C$ is the charge of cation, $A$ is the charge of anion). For $SO_3$, $V = 6$ (valence electrons of $S$), $M=0$, $C = 0$, $A = 0$. So $n=\frac{6 + 0-0 + 0}{2}=3$.
    - In $SO_3$, the three $S - O$ bonds are identical and the molecule has a trigonal - planar geometry. The bond dipoles cancel out each other (because of symmetry), so it is symmetrical and non - polar.
 - For $SO_2S$ (assuming it is a typo and you mean a molecule with a trigonal - planar geometry but different groups):
    - Let's assume a general trigonal - planar molecule with different substituents. The number of regions of electron - density around the central atom is still 3 (using the same electron - density formula as above). But due to different substituents, the bond dipoles do not cancel out. So it is asymmetrical and polar.
 - For $SO_2$:
    - Using the formula $n=\frac{V+M - C + A}{2}$, for $SO_2$, $V = 6$ (valence electrons of $S$), $M = 0$, $C=0$, $A = 0$. But there is a lone pair. The number of regions of electron - density $n = 3$ (two $S - O$ bonds and one lone pair). The molecule has a bent geometry. The bond dipoles do not cancel out (because of the asymmetrical distribution of electron density due to the lone pair), so it is asymmetrical and polar.

# Answer:
1. H. 3
2. A. symmetrical
3. C. nonpolar
4. H. 3
5. B. asymmetrical
6. D. polar
7. H. 3
8. B. asymmetrical
9. D. polar

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