Why do metals conduct electricity well?
Have you ever heard of the concept electronic sea? It seems like a term straight out of poetry, but it’s actually scientifically accurate. This is a concept that relates to the microscopic depths of matter, where studying the movement of electrons can help us understand the macroscopic world that surrounds us, for example, what is electrical conductivity actually? In fact, understanding the existence of this electron sea is critical to figuring out why elements like metals have higher electrical conductivity values than others like wood.
ELECTRONIC STRUCTURE
To understand the concept of the electron sea, it is absolutely necessary to delve into the structure of electrons. atoms. They have a core filled with protons and neutrons and an outer shell in which electrons spin randomly. Now, looking at this from a quantum point of view, this definition changes somewhat, since it is observed that in reality the electrons orbit in different layers And jumping between energy levels which are located at different distances from the core. Each of the layers is represented by so-called core numbers, so as this core number increases, so will electron energy what moves in it, as well as its distance from the core.
5 points for understanding quantum physics
Thus it is known by the name electronic configuration to the distribution followed by electrons in an atom between different energy levels. Each element will have a different distribution, which will be responsible for all its properties, including the conductivity they possess, thermal excitation or energy absorption capacity.
FORMATION OF AN ELECTRON MORAL
However, this seemingly general distribution for all elements is very different when we focus on metals. And, unlike other isolated atoms, in which electrons fill certain levels and shells, metals have a completely different form of interaction and distribution: they represent Crystal structure. Thus, while non-metal atoms join together to form matter by exchanging electrons and creating a bond, metals are arranged according to the arrangement much more organized And repetitivewhich allows electrons in the outer shells of each atom to interact with neighboring atoms.
In particular, the true actors are the electrons in the outer shell. They are known as valence electrons, are less tied to the core and have greater freedom of movement. Thus, the presence of several valence electrons in each atom and the ease of their movement is what contributes to the formation of that very characteristic “sea of electrons”. In fact, when metals bond together to form a solid, the valence electrons become increasingly delocalized, meaning that They do not belong to a specific atom and move throughout the crystal structure.. It is this dynamic sea in which electrons flow that gives the metal its characteristic electrical conductivity in addition to other unique properties such as ductility or thermal conductivity.
Metal connection diagram. The blue dots represent delocalized electrons that are free to move between atoms, making current flow favorable.
ELECTRICAL CONDUCTIVITY
For good electrical conductivity, electrons must have the ability get. In ordinary bonds, the exchange of electrons between two atoms greatly limits this possibility since they remain attached to the atoms to which they belong, which is why the mobility provided by a sea of electrons is so significant in metals. When an external electric field is applied, they can respond quickly by moving and orienting themselves, creating an electric current that current through all the material.
On the other side, temperature It also plays a decisive role in the conductive properties. Moreover, at higher temperatures this usually decreases, and at lower temperatures it increases. Seems counterproductive, doesn’t it? Shouldn’t they move faster at higher temperatures due to thermal excitation? Well, it is true that at high temperatures they increase their speed and vibration, but since they flow through the sea along with other electrons, this situation becomes easier collisions between them, which significantly reduces conductivity. In fact, at extremely low temperatures, some metals can experience superconductivitywhere resistivity and collisions are reduced to zero and electric current can flow without any loss.