Figure shows the results of the dipolar contribution for 139 electrolytes. In panel A we show the dipolar contribution to ln γ ± for four electrolytes with different ion-water interaction strength. The cross-over point x Dipole h marks a boundary: dipole-dipole interaction becomes unfavorable for higher concentrations and complex interactions become more important. The droplet size of the observation volume where this happens is determined by 1/x Dipole h . Panel B shows the depth of the dipolar contribution to ln γ ± versus its exponent for the different 1:1 to 3:2 electrolytes as well as ionic liquids. We display electrolytes with x Dipole h = 1 with open markers. The vertical line at λ Dipole = 0.5 refers to a value corresponding to the Debye-Hückel (DH) law. Electrolytes with large D Dipole show in general exponents close to the DH-value. A comparison to panels A and C shows that D Dipole is determined by both, the strength of the electrolyte and the limiting concentration where higher order terms become more important. A larger exponent indicates an increased importance of thermal averaging effects (Remember, that thermal averaging changes the 1/R 3 -interaction of close dipoles to a 1/R 6dependency, when the effective interaction strength is much smaller than kT ). This is especially prominent for ionic liquids which show the largest exponents among all electrolytes. Panel C supports this picture. Here, we observe that a) electrolytes with smaller 1/x Dipole ) -κ with D 0 = 2.81(8) and κ = 0.42 . The lines display the power law for 1:1 (blue) and 2:1 and 1:2 (yellow) electrolytes. A few electrolytes with exceptional properties are labeled separately.