Arrange these compounds: $\ce{CO2}$, $\ce{CH3OH}$, $\ce{RbF}$, $\ce{CH3Br}$ in order of increasing boiling points.
I think I should consider the forces between them, that is:
- $\ce{CO2}$: dispersion forces
- $\ce{RbF}$: dispersion and ionic forces
- $\ce{CH3OH}$: Dipole-dipole interactions, Hydrogen bonding and dispersion forces
- $\ce{CH3Br}$: Dipole-dipole interactions and dispersion forces
It is obvious that $\ce{CO2}$ is the smallest one and because $\ce{CH3OH}$ stronger than $\ce{CH3Br}$ it will have higher boiling point
But how to arrange the rest? Or how to compare ionic forces with Dipole?