Hydrogen bonding occurs where HYDROGEN is bound to a strongly electronegative element, i.e. hydrogen is bound to fluorine, nitrogen, or oxygen. In $"fluoroform"$, the hydrogen is bound to carbon not fluorine. The molecule is polar but does NOT display hydrogen bonding. And the best indicator for intermolecular forces is given by boiling point:
$"Normal boiling point,"$ $HF=19.5$ $""^@C$
$"Normal boiling point,"$ $HCF_3=-82.1$ $""^@C$
$"Normal boiling point,"$ $CF_4=-127.8$ $""^@C$
Can you account for the volatilites in terms of intermolecular force?