Jj. Dannenberg et al., Are hydrogen bonds covalent or electrostatic? A molecular orbital comparison of molecules in electric fields and H-bonding environments, J PHYS CH A, 103(35), 1999, pp. 7083-7086
The extent to which hydrogen-bonding can be considered to be a covalent or
resonance effect, rather than an electrostatic or electrostatic plus polari
zation effect, is modeled by ab initio molecular orbital calculations in gr
aded uniform electric fields of molecules that form chains of H-bonds. The
stabilization energy, dipole moments, and relaxed geometrical structural pa
rameters of these molecules are tabulated as a function of applied field. T
he H-bonding interactions of a molecule are judged to be due to electrostat
ic and polarization effects if all of the tabulated parameters agree with t
hose calculated for an infinite chain of H-bonding molecules at the same va
lue of the applied electric field. If these parameters individually agree w
ith those of the infinite chain of H-bonding dimers at substantially differ
ent values of the applied field, effects other than electrostatic and polar
ization, such as covalent or resonance effects, must be important. Of the t
wo molecules studied, urea appears to be reasonably well-described by elect
rostatic plus polarization effects, whereas the other molecule, the enol of
1,3-cyclohexanedione, clearly is not.