Relative strength of intermolecular forces
I would say that your analysis of first, second and fourth one is correct, as H-bonds are stronger than dipole-dipole interactions. However, you made a mistake while filtering compounds having dipole-dipole interaction. The $1$ and $3$, both have dipoles!
The $\ce{C=O}$ bonds in $\ce{CO2}$ are polar and hence they possess dipoles, but unlike a water molecule, $\ce{CO2}$ shape is linear, and therefore the equal dipoles cancel each other, resulting in a non-polar molecule as seen in the following figure,

That's the reason $\ce{CO2}$ possess dipole-dipole interactions whereas $\ce{F2}$ doesn't as it has only one bond which is non-polar!
Image taken from courses.lumenlearning.com: Polar Molecules