Nitrogen, $\text{N}_2$, and carbon monoxide, $\text{CO}$, each have $M_r = 28$. The boiling point of $\text{N}_2$ is $77\,\text{K}$, whereas the boiling point of $\text{CO}$ is $82\,\text{K}$. What might account for this difference in boiling points?
- A$\text{CO}$ molecules have a permanent dipole; the $\text{N}_2$ molecules are not polar.
- B$\text{N}_2$ has $\sigma$ and $\pi$ bonding; $\text{CO}$ has $\sigma$ bonding only.
- C$\text{N}_2$ has a strong $\text{N}\equiv\text{N}$ bond; $\text{CO}$ has a $\text{C}=\text{O}$ bond.
- DThe $\text{CO}$ molecule has more electrons than the $\text{N}_2$ molecule.