How do solid solution alloys generally compare to pure metals in terms of conductivity?

Solid solution alloys typically exhibit poorer electrical and thermal conductivity compared to pure metals. This reduction in conductivity can be attributed to the presence of different elements in the alloy, which disrupts the orderly arrangement of atoms found in the pure metal. The variations in atomic size and structure within the alloy lead to increased scattering of charge carriers (electrons for electrical conductivity and phonons for thermal conductivity), resulting in a decrease in their overall conductivity.

Conductivity in metals is largely dependent on the availability of free electrons and their ability to move easily through the material. In pure metals, the atomic structure allows for a relatively uninterrupted pathway for these electrons. However, in solid solution alloys, the added solute atoms create a lattice distortion, which can hinder the flow of electrons and phonons.

Therefore, while pure metals typically have high conductivity values, solid solution alloys are generally less conductive due to the complexities introduced into their microstructure.