At present, science knows one hundred and five chemical elements, systematized in the form of a periodic table. The vast majority of them are classified as metals, which implies the presence of these elements with special qualities. These are the so-called metallic properties. Such characteristics, first of all, include plasticity, increased heat and electrical conductivity, the ability to form alloys, and low ionization potential.
The metallic properties of this or that element are caused by the ability of its atoms to interact with the atomic structures of other elements to shift electron clouds in their direction or "give" their free electrons to them. The most active metals are those that have low ionization energy and electronegativity. Also pronounced metallic properties are characteristic of elements having the largest possible radius of the atom and the extremely small number of external (valence) electrons.
As the valence orbit is filled, the number of electrons in the outer layer of the atomic structure increases, and the radius, accordingly, decreases. In this regard, atoms begin to strive for the attachment of free electrons, and not for their recoil. The metallic properties of such elements tend to decrease, and their non-metallic properties increase. And, conversely, with an increase in the atomic radius, an increase in the metallic properties is noted. Therefore, a characteristic common feature of all metals is the so-called reducing qualities - the very ability of an atom to donate free electrons.
The metallic properties of the elements are most pronounced in the substances of the first and second groups of the main subgroups of the periodic table, as well as in alkali and alkaline earth metals. But the strongest reducing qualities are observed in France, and in the aquatic environment - in lithium due to a higher rate of hydration energy.
The number of elements that exhibit metallic properties within a period increases with increasing period number. In the periodic table, metals from non-metals are separated by a diagonal line that runs from boron to astatine. According to this dividing line, there are elements in which those and other qualities are equally manifested. Such substances include silicon, arsenic, boron, germanium, astatine, antimony and tellurium. This group of elements is called metalloids.
Each period is characterized by the presence of a kind of "border zone" in which elements with dual qualities are located. Consequently, the transition from a pronounced metal to a typical non-metal is carried out gradually, which is reflected in the periodic table.
The general properties of metal elements (high electrical conductivity, thermal conductivity, ductility, characteristic luster, ductility, etc.) are due to the similarity of their internal structure, or rather, the presence of a crystal lattice. However, there are many qualities (density, hardness, melting point) that give all metals purely individual physicochemical properties. These characteristics depend on the structure of the crystal lattice of each particular element.