Metallic properties of chemical elements

At the moment, science knows one hundred and five chemical elements, systematized in the form of a periodic table. The overwhelming majority of them are considered to be metals, which implies that these elements have special qualities. This is the so-called metallic properties. These characteristics, in the first place, include plasticity, increased thermal and electrical conductivity, the ability to form alloys, a low value of the ionization potential.

The metallic properties of an element are due to the ability of its atoms when interacting with the atomic structures of other elements to shift electron clouds in their direction or to "give" their free electrons to them. The most active metals are those that have a low ionization energy and electronegativity. Also, pronounced metallic properties are characteristic for elements having the largest radius of an atom and an 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, respectively, decreases. In this connection, the 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 nonmetallic properties increase. And, on the contrary, when the atomic radius increases, the metal properties are noted to increase. Therefore, the characteristic common feature of all metals are, so-called, restorative qualities - the same ability of an atom to give free electrons.

Most clearly, the metal properties of the elements are manifested in the substances of the first, second groups of main subgroups of the periodic table, as well as in alkaline and alkaline-earth metals. But the strongest restorative qualities are observed in France, and in the water environment - in lithium due to a higher indicator of hydration energy.

The number of elements exhibiting metallic properties within the period increases with the number of the period. In the periodic table, metals from nonmetals are separated by a diagonal line that extends from boron to astatine. On this dividing line there are elements in which both qualities are manifested equally. Such substances include silicon, arsenic, boron, germanium, astatum, 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 the elements with dual qualities are located. Consequently, the transition from a clearly expressed metal to a typical non-metal is carried out gradually, which is reflected in the periodic table.

The general properties of metallic elements (high electrical conductivity, thermal conductivity, ductility, characteristic luster, plasticity, etc.) are due to the similarity of their internal structure, or more precisely - the presence of a crystal lattice. However, there are many qualities (density, hardness, melting point), which give all metals a purely individual physico-chemical properties. These characteristics depend on the structure of the crystal lattice of each particular element.