To rationalize the driving factors in the competition of halogen bonding and hydrogen bonding, the complexes of the combined halogen-/hydrogen-bond donor difluoroiodomethane with the Lewis bases trimethylphosphine, dimethyl sulfide and chloromethane are studied. For all Lewis bases, ab initio calculations lead to halogen- and hydrogen-bonded complexes. Fourier transform-IR experiments involving solutions of mixtures of difluoroiodomethane with trimethylphosphine(-d(9)) or dimethyl sulfide(-d(6)) in liquid krypton confirm the coexistence of a halogen-bonded and hydrogen-bonded complex. Also for solutions containing chloromethane, evidence of the formation of binary associations is found, but no definitive assignment of the multiple complex bands could be made. Using van't Hoff plots, the experimental complexation enthalpies for the halogen- and hydrogen-bonded complex of difluoroiodomethane with trimethylphosphine are determined to be -15.4 (4) and -10.5 (3) kJ mol(-1), respectively, while for the halogen- and hydrogen-bonded complexes with dimethyl sulfide, the values are -11.3 (5) and -7.7 (6) kJ mol(-1), respectively. The experimental observation that for both trimethylphospine and dimethyl sulfide the halogen-bonded complex is more stable than the hydrogenbonded complex supports the finding that softer Lewis bases tend to favor iodine halogen bonding over hydrogen bonding.