explain electrical conductivity in metallic solids and ionic solids
explain electrical conductivity in metallic solids and ionic solids
Electrical conductivity is metallic solids:
Metals have valence electrons which are free to move in lattice , these electrons are called free electrons. These mobile electrons are responsible for the electrical conductivity of metals. There are n number of atomic orbitals in an atom. A set of atomic orbitals of almost similar energy is called a band. There are two type of bands in a solid atom one with valence electrons is called valence band while the other of higher energy is called conduction band.
In case of metallic solids the conduction band overlaps with valence band and electrons of valence band are free to move into conduction band. In absence of electric field , equal number of electrons can move in all directions. In the presence of electric field i.e. when metal is connected to electrodes the movement of electrons becomes directional giving rise to the electrical conductance.
Metallic solids show increases in resistance with increase in temperature
Electrical conductivity is ionic solids:
An ionic solid does not conduct electricity in solid state but it do so in liquid state. In liquid state or solutions, the ionic solid dissociate into constituent ions. The movement of these ions under the influence of electric field is responsible for the electrical conductance.
Electrolytes i.e. ionic solids in solution, show decrease in resistance with increase in temperature.
Electrical conductivity is metallic solids:
Metals have valence electrons which are free to move in lattice , these electrons are called free electrons. These mobile electrons are responsible for the electrical conductivity of metals. There are n number of atomic orbitals in an atom. A set of atomic orbitals of almost similar energy is called a band. There are two type of bands in a solid atom one with valence electrons is called valence band while the other of higher energy is called conduction band.
In case of metallic solids the conduction band overlaps with valence band and electrons of valence band are free to move into conduction band. In absence of electric field , equal number of electrons can move in all directions. In the presence of electric field i.e. when metal is connected to electrodes the movement of electrons becomes directional giving rise to the electrical conductance.
Metallic solids show increases in resistance with increase in temperature
Electrical conductivity is ionic solids:
An ionic solid does not conduct electricity in solid state but it do so in liquid state. In liquid state or solutions, the ionic solid dissociate into constituent ions. The movement of these ions under the influence of electric field is responsible for the electrical conductance.
Electrolytes i.e. ionic solids in solution, show decrease in resistance with increase in temperature.
