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Thus the key requirement for quantative understanding of the action of biological molecules is the ability to correlate electrostatic interactions with structural information. To appreciate this point it is useful to compare the electrostatic energy of a charged amino acid in a polar solvent to the corresponding van der Waals energy. The electrostatic free energy, \u0394<jats:italic>G<\/jats:italic><jats:sub>el<\/jats:sub>, can be approximated (as will be shown in Section II) by the Born formula (\u0394<jats:italic>G<\/jats:italic><jats:sub>el<\/jats:sub>= \u2013(166Q<jats:sup>2<\/jats:sup>\/\u0101) (I \u2013 I\/<jats:italic>E<\/jats:italic>)). Where \u0394<jats:italic>G<\/jats:italic><jats:sub>el<\/jats:sub>is given in kcal\/mol,<jats:italic>Q<\/jats:italic>is the charge of the given group, in units of electron charge,<jats:italic>\u0101<\/jats:italic>is the effective radius of the group, and<jats:italic>E<\/jats:italic>is the dielectric constant of the solvent. With an effective radius of charged amino acids of approximately 2 \u00c5, Born's formula gives about \u2013 80 kcal\/mol for their energy in polar solvents where<jats:italic>E<\/jats:italic>is larger than 10. 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