Broken Translational Invariance in
the Solid State
Simple Energetics of Solids
Why do solids form? The Hamiltonian of the electrons and ions is:
It is invariant under the symmetry, fi^ri+ a, Ra —► Ra + a. However, the energy can usually be minimized by forming a crystal. At low enough temperature, this will win out over any possible entropy gain in a competing state, so crystallization will occur. Why is the crystalline state energetically favorable? This depends on the type of crystal. Different types of crystals minimize different terms in the Hamiltonian. In molecular and ionic crystals, the potential energy is minimized. In a molecular crystal, such as solid nitrogen, there is a van der Waals attraction between molecules caused by polarization of one by the other. The van der Waals attraction is balanced by short-range repulsion, thereby leading to a crystalline ground state. In an ionic crystal, such as NaCl, the electrostatic energy of the ions is minimized (one must be careful to take into account charge neutrality, without which the electrostatic energy diverges). In covalent and metallic crystals, crystallization is driven by the minimization of the electronic kinetic energy. In a metal, such as sodium, the kinetic energy of the electrons is lowered by their ability to move throughout the metal. In a covalent solid, such as diamond, the same is true. The kinetic energy gain is high enough that such a bond can even occur between just two molecules (as in organic chemistry). The energetic gain of a solid is called the cohesive energy.