Since this species is nonpolar, all we have is the dispersion force to overcome.
From the Lewis structure, we see that this species would have both dispersion forces and hydrogen bonding.
From the Lewis structure (draw it!), we see that this species has a bent molecular geometry and two lone pairs; it is therefore polar. We would have to overcome disperion forces and dipole-dipole forces to boil this substance (but there would be no H-bonding present - why not?)
Doug Chapman firstname.lastname@example.org 6/30/08