Ethane, $\text{CH}_3\text{CH}_3$, and fluoromethane, $\text{CH}_3\text{F}$, contain the same total number of electrons in their molecules. Their boiling points are listed as follows: $\text{CH}_3\text{CH}_3$ = $184.5\,\text{K}$, $\text{CH}_3\text{F}$ = $194.7\,\text{K}$. What causes this difference in boiling points?
- A$\text{CH}_3\text{F}$ has a larger $M_r$ than $\text{CH}_3\text{CH}_3$.
- B$\text{CH}_3\text{F}$ has a permanent dipole, $\text{CH}_3\text{CH}_3$ does not.
- C$\text{CH}_3\text{F}$ has a strong C-F bond, $\text{CH}_3\text{CH}_3$ does not.
- DHydrogen bonding occurs in $\text{CH}_3\text{F}$, but not in $\text{CH}_3\text{CH}_3$.