use figure 1a in chapter 10 to answer the following questions. if a molecule is symmetrical it cannot be a polar molecule because all of the dipoles will oppose each other and cancel out, as in co₂. if a molecule is asymmetrical it might be a polar molecule - it has to have one or more dipoles (polar covalent bonds). if the molecule is an ion, it is extremely polar even if it doesnt have polar covalent bonds because it itself is a dipole. diatomic molecules like o₂ with no reds are __1__ symmetrical/asymmetrical and __2__ nonpolar/polar diatomic molecules like fcl with no reds are __3__ symmetrical/asymmetrical and __4__ nonpolar/polar linear molecules like co₂ with __5__ reds are __6__ symmetrical/asymmetrical and __7__ nonpolar/polar linear molecules like cos with __8__ reds are __9__ symmetrical/asymmetrical and __10__ nonpolar/polar a. symmetrical b. asymmetrical c. nonpolar d. polar e. 0 f. 1 g. 2 h. 3 i. 4

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# Brief Explanations:
- For $O_2$: It is a diatomic molecule with identical atoms. The electron distribution is uniform, so it is symmetrical ($A$). Since there is no dipole (as the atoms are the same), it is non - polar ($C$).
- For $FCl$: It is a diatomic molecule with different atoms. The electron distribution is not uniform (because of the difference in electronegativity between $F$ and $Cl$), so it is asymmetrical ($B$). And it has a dipole (polar covalent bond), so it is polar ($D$).
- For $CO_2$: The formula for the number of regions of electron density ($REDs$) around the central $C$ atom in $CO_2$ (using the formula $n=\frac{V + M - C+A}{2}$, where $V$ is the valence electrons of the central atom ($C:4$), $M$ is the number of monovalent atoms ( $O$ is not monovalent, so $M = 0$), $C$ is the charge of cation ( $0$), $A$ is the charge of anion ($0$)). The Lewis structure of $CO_2$ is $O = C=O$. The central $C$ atom has $2$ regions of electron density ($G$). The molecule is linear and symmetrical ($A$). The dipoles cancel out, so it is non - polar ($C$).
- For $COS$: The central $C$ atom. The Lewis structure is $O = C=S$. It has $2$ regions of electron density ($G$). The molecule is linear but asymmetrical ($B$) because $O$ and $S$ have different electronegativities. The dipoles do not cancel out, so it is polar ($D$).

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

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