It is shown that for most crystalline materials, the reason for melting is overloading of their crystal lat tices with point defects with increasing temperature, rather than an excess of the energy of thermal vibra tions of the lattice sites over the value of their binding energy. The latter occurs only in simple (single ele ment) substances or in certain complex substances with a small number of defects.There is no generally accepted theory of melting. It is often thought that the melting point T m of solids, i.e., crystalline substances, is the temperature at which the oscillation energy of particles in the lattice sites reaches the energy of their bonds in the lattice, namely, the level of melting heat Q (or the crystalliza tion heat).If this were so, then the ratio Q/RТ m (R = 8.314 kJ/mol K) would be practically constant for all substances (at a pressure of 0.1 MPa). For simple (sin gle element) substances, this ratio ranges from 0.25 to 5 (Fig. 1). Only for metals and a number of light sub stances (Н 2 , D 2 , T 2 , Be, B, N 2 , O 2 , and F 2 ) is this ratio close to unity. There are a few exceptions, such as helium, white phosphorus, sulfur, and plutonium. In the case of nonmetals, this value is always greater than 1.5.For a huge number of complex (multielement) sub stances, including crystals of organic substances, the results are even more significant. Here, this value var ies generally from 1.5 to tens of units. However, for approximately 5-10% of complex substances (those