conductive

Examples of conductive in the following topics:

• Doping: Connectivity of Semiconductors

  • The conduction band is the band above the valence band.
  • Electrons in the conduction band are free to move about in the lattice and can conduct current.
  • If the gap between the valence and conduction bands is large, then the substance does not conduct electricity easily (it is an insulator).
  • The overlap or size of the gap between the valence and conduction bands determines the electrical conductivity of a substance.
  • The gap between the valence and conduction bands determines whether a substance will conduct electricity.

• Electrolyte and Nonelectrolyte Solutions

  • Unlike nonelectrolytes, electrolytes contain dissolved ions that enable them to easily conduct electricity.
  • The resulting solution will conduct electricity because it contains ions.
  • As mentioned above, when an ionizable solute dissociates, the resulting solution can conduct electricity.
  • As a result, solutions containing nonelectrolytes will not conduct electricity.
  • In the human body, electrolytes have many uses, including helping neurons conduct electrical impulses.

• General Properties of Metals

  • Those ions are surrounded by de-localized electrons, which are responsible for the conductivity.
  • Metals in general are conductive, with high electrical conductivity and high thermal conductivity.
  • The electrical and thermal conductivities of metals originate from the fact that their outer electrons are delocalized.
  • This is very instrumental in the conductivity of the metal.
  • As a result, they retain their shiny appearance and good conductivity for many decades (like aluminium, magnesium, some steels, and titanium).

• Metallic Crystals

  • These ions are surrounded by delocalized electrons, which are responsible for conductivity.
  • In a quantum-mechanical view, the conducting electrons spread their density equally over all atoms that function as neutral (non-charged) entities.
  • Metals in general have high electrical conductivity, high thermal conductivity, and high density.
  • In metals, the charge carriers are the electrons, and because they move freely through the lattice, metals are highly conductive.
  • Electrical conductivity, as well as the electrons' contribution to the heat capacity and heat conductivity of metals, can be calculated from the free electron model, which does not take the detailed structure of the ion lattice into account.

• Conductors

  • A conductor is a material that is able to conduct electricity with minimal impedance to the electrical flow.
  • Insulators are non-conducting materials with few mobile charges; they carry only insignificant electric currents.
  • In describing conductors using the concept of band theory, it is best to focus on conductors that conduct electricity using mobile electrons.
  • There are even conductive polymers.
  • Thermal and electrical conductivity often go together.

• Silver

  • Silver has the highest electrical conductivity of any element and the highest thermal conductivity of any metal.
  • It has the highest electrical conductivity of any element and the highest thermal conductivity of any metal.
  • Recognize the propensity of silver halides to precipitate out of solution when formed, as well as silver's electrical and thermal conductivity properties

• Semiconductors

  • In semiconductors, only a few electrons exist in the conduction band just above the valence band, and an insulator has almost no free electrons.
  • In semiconductors, the band gap is small, allowing electrons to populate the conduction band.
  • In insulators, it is large, making it difficult for electrons to flow through the conduction band.
  • N-type semiconductors are a type of extrinsic semiconductor in which the dopant atoms are capable of providing extra conduction electrons to the host material (e.g. phosphorus in silicon).
  • As the energy in the system increases, electrons leave the valence band and enter the conduction band.

• Voltaic Cells

  • These scientists conducted several experiments on chemical reactions and electric current during the late 18th century.
  • Electrochemical cells have two conductive electrodes, called the anode and the cathode.
  • Electrodes can be made from any sufficiently conductive materials, such as metals, semiconductors, graphite, and even conductive polymers.
  • When an electrically conducting device connects the electrodes, the electrochemical reaction is:

• Comparison between Covalent and Ionic Compounds

  • Although solid ionic compounds do not conduct electricity because there are no free mobile ions or electrons, ionic compounds dissolved in water make an electrically conductive solution.
  • In contrast, covalent compounds do not exhibit any electrical conductivity, either in pure form or when dissolved in water.

• Ionic Bonding and Electron Transfer

  • Most of these solids are soluble in H2O and conduct electricity when dissolved.
  • The ability to conduct electricity in solution is why these substances are called electrolytes.