Interaction of L11 stationary phase (Phenyl, Biphenyl)

Types of interactions   Origin of force Feature
van der Waals force
Orientation force
Induced force
London dispersion force
Permanent Dipole-Permanent Dipole
Charged-Induced dipole
Induced dipole-induced dipole
Attenuates at -6th power of
distance and makes an
important contribution only at
short distances.
Dispersion is dominant in nonpolar molecules.
Charge transfer interaction   Electron donor-Electron acceptor Coloring by charge transfer
Hydrogen bond   Functional groups such as
OH and NH
Strong specificity and
Hydrophobic interaction   Non-polar groups in polar
Entropy domination

As shown in the figure above, benzene has the highest electron density in the center, and the phenyl and biphenyl
groups of the L11 stationary phase have a dipole-dipole interaction, which is the orientation force of the van der
Waals force. It then exhibits characteristic selectivity by the π-π and CH-π interactions that are treated as part of

★π-π stacking and T-type stacking are known as benzene arrangement states as π-π interactions. It is presumed that
T-type stacking is close to the CH-π interaction, which is the interaction between the central part of benzene and
hydrogen of CH.