Hydrogen occurs for molecules in which hydrogen is bound to a STRONGLY electronegative atom such as fluorine, oxygen, or nitrogen. And so it occurs primarily in the element hydrides....$NH_3$, $HF$, $H_2O$... Now hydrogen-bonding acts as an intermolecular force that STRONGLY ELEVATES the boiling point...i.e. $stackrel(delta+)H-stackrel(delta^-)Fcdotsstackrel(delta+)H-stackrel(delta^-)FcdotsH-stackrel(delta^-)FcdotsH-Fcdots$..
And if we look at the normal boiling points...
$"ammonia"$ $-44$ $""^@C$
$"hydrogen fluoride"$ $+19$ $""^@C$
$"water"$ $+100$ $""^@C$
...all of these are high for such SMALL molecules. The boiling point of water is ASTONISHINGLY high...and this is to be attributed to the effectiveness and extent of hydrogen-bonding....
On the other hand, for $Cl_2$, while this is a bigger molecule, with more electrons to contribute to the dispersion force, dichlorine is NON-POLAR with NO dipole interaction to contribute to the intermolecular force, and hence a reduced normal boiling point of $-33.8$ $""^@C$...
