Bonding in Metals: The Electron Sea Model
Metallic bonding may be described as the sharing of free electrons among a lattice of positively charged metal ions.
Describe the electron sea model of metallic bonding.
- Many of the unique properties of metals can be explained by metallic bonds.
- Metallic bonds can occur between different elements to form an alloy.
- In contrast to electrons that participate in both ionic and covalent bonds, electrons that participate in metallic bonds delocalize, forming a sea of electrons around the positive nuclei of metals. The availability of “free” electrons contributes to metals being excellent conductors.
- metallic bond: A chemical bond in which mobile electrons are shared over many nuclei; this leads to electrical conduction.
- electron sea: The body of delocalized electrons that surrounds positive metal ions in metallic bonds.
Metallic bonding may be described as the sharing of free electrons among a lattice of positively charged metal ions. The structure of metallic bonds is very different from that of covalent and ionic bonds. While ionic bonds join metals to nonmetals, and covalent bonds join nonmetals to nonmetals, metallic bonds are responsible for the bonding between metal atoms.
In metallic bonds, the valence electrons from the s and p orbitals of the interacting metal atoms delocalize. That is to say, instead of orbiting their respective metal atoms, they form a “sea” of electrons that surrounds the positively charged atomic nuclei of the interacting metal ions. The electrons then move freely throughout the space between the atomic nuclei.
The characteristics of metallic bonds explain a number of the unique properties of metals:
- Metals are good conductors of electricity because the electrons in the electron sea are free to flow and carry electric current.
- Metals are ductile and malleable because local bonds can be easily broken and reformed.
- Metals are shiny. Light cannot penetrate their surface; the photons simply reflect off the metal surface. However, there is an upper limit to the frequency of light at which the photons are reflected.
Metallic bonds can occur between different elements, forming an alloy. Aluminum foil and copper wire are examples of metallic bonding in action.
Metallic bonds are mediated by strong attractive forces. This property contributes to the low volatility, high melting and boiling points, and high density of most metals. The group-XII metals zinc, cadmium, and mercury are exceptions to this rule.
Doping: Connectivity of Semiconductors
The process of adding substances to a pure semiconductor for the purposes of modulating its electrical properties is known as doping.
Examine the method of doping a pure semiconductor in order to increase its electrical conductivity.
- Semiconductors are doped to generate either a surplus or a deficiency in valence electrons.
- Doping allows researchers to exploit the properties of sets of elements, referred to as dopants, in order to modulate the conductivity of a semiconductor.
- There are two types of dopants, n-type dopants and p-type dopants; n-type dopants act as electron donors, and p-type dopants act as electron acceptors.
- Combining n-type and p-type semiconductors creates systems which have useful applications in modern electronics.
- doping: The addition of small quantities of an element (an impurity) to a pure semiconductor to change its electrical conductivity characteristics.
- p-type semiconductor: A doped semiconductor in which conduction is due to the movement of positively-charged holes.
- n-type semiconductor: A doped semiconductor in which conduction is due to the movement of additional electrons.
Electrical Conduction in Solids
There are two general categories of semiconductors: intrinsic semiconductors, which are composed of only one material, and extrinsic semiconductors, which have had other substances added to them to alter their properties. In semiconductor production, the process of creating extrinsic semiconductors by adding substances to a pure semiconductor for the purposes of modulating its electrical properties is known as doping. Semiconductors are doped to generate either a surplus or a deficiency in valence electrons.
Energy Bands in Solids
Electrons in free atoms have discrete energy values. In contrast, the energy states available to the free electrons in a metal sample form a continuum of “energy bands.” In the atomic lattice of a substance, there is a set of filled atomic energy “bands” with a full complement of electrons, and a set of higher energy unfilled “bands” which have no electrons. The highest energy band contains valence electrons available for chemical reactions. 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. In order for a substance to conduct electricity, its valence electrons must cross the band gap, which is the energy gap between the valence band and conduction band.
If the gap between the valence and conduction bands is large, then the substance does not conduct electricity easily (it is an insulator). On the other hand, these bands overlap in metallic samples, which make these samples excellent conductors of electricity. In the case of semiconductors, the gap is small enough for electrons to jump to the conduction band due to thermal or some other excitation.
Because the band gap is so small for semiconductors, doping with small amounts of impurities can dramatically increase the conductivity of the material. Doping, therefore, allows scientists to exploit the properties of sets of elements referred to as “dopants” in order to modulate the conductivity of a semiconductor.
There are two types of dopants, n-type (“n” for negative), and p-type (“p” for positive) dopants. n-type dopants act as electron donors and have extra valence electrons with energies very close to the conduction band. When incorporated into the atomic lattice of a semiconductor, the valence electrons of n-type dopants can be easily excited to the conduction band. p-type dopants assist in conduction by accepting electrons. When a p-type dopant is incorporated into the atomic lattice of a semiconductor, it is able to host electrons from the conduction band, allowing the easy formation of positive holes.
Generating an n-Type Semiconductor
When doping a semiconductor, such as the group IV element silicon (Si), with arsenic (As), a pentavalent n-type dopant from group V in the periodic table (which has one more valence electron than the semiconductor), the dopant behaves as an electron donor. When this occurs, an atom of dopant replaces an atom of silicon in the lattice, and therefore an extra valence electron is introduced into the structure. The fifth valence electron of As creates a surplus of electrons. When just a few atoms of the dopant replace silicon atoms in the lattice, an n-type semiconductor is created. The newly created semiconductor is better able to conduct current than the pure semiconductor.
Generating a p-Type Semiconductor
When a group IV semiconductor is doped with a p-type trivalent group III dopant (such as boron, B), which has one less valence electron than the semiconductor, the dopant acts as an electron acceptor. When a few atoms of trivalent dopant replace silicon atoms in the lattice, a vacant state (or electron “hole”) is created and can act as electron carrier through the structure, which creates a p-type semiconductor. p-type semiconductors are characterized by a deficit of electrons and positive holes, which have the same effect as a surplus of positive charge. These positive holes accept electrons, rendering the semiconductor more effective at conducting current.
The p-n Junction
When we place p-type and n-type semiconductors in contact with one another, a p-n junction is formed. p-n junctions are basic components of most common electrical devices. While semiconductors doped with either n-type dopants or p-type dopants are better conductors than intrinsic semiconductors, interesting properties emerge when p- and n-type semiconductors are combined to form a p-n junction.
If no electricity is being passed through the system, then no current passes through the junction between n- and p-type semiconductors. In this scenario, the surplus of electrons from the n-type semiconductor and the deficiency in electrons from the p-type semiconductor combine to create a depletion region. In this state, the system is said to be at equilibrium. However, if the cathode of a battery is connected to the p-type semiconductor, and the anode is connected to the n-type semiconductor, the system is said to be “forward biased.” In this scenario, electrons flow from the anode toward the cathode pole and charge flows across the junction. If the connectivity is reversed, with the battery anode connected to the p-type semiconductor and the cathode connected to the n-type semiconductor, the system is said to be “reverse biased” and negligible charge flows across the junction. Combining n-type and p-type semiconductors creates a system which has useful applications in modern electronics.
Electronic devices and instruments, such as digital alarm clocks, mp3 players, computer processors, and the electronics in cell phones, all take advantage of semiconductor technology. Doping provides a way to modulate the properties of semiconductors that have broad applications in daily life.