Metals are believed to possess a special type of bonding known as Metallic Bond. There are only few valence electrons or outermost electrons are very loosely bound to the nucleus.This develops the ability in metals to conduct electricity and heat. In the metallic bond, most metals crystallize in close- packet structures. There is a strong electron interaction among 8 to 12 nearest neighbour atoms. Also called as coordination number. Metallic crystals have considerably weak strength.So, the forces like van der Waal forces can not seem to exist between the metals.
What is Metallic Bond
This concept is based on the idea that high electrical and thermal conductivities of metals are due to the presence of free electrons (or mobile electrons). To understand this model of the metallic bond, the following characteristic properties of individual atoms of the metals must be remembered:
- The ionization energies of the atoms of the metallic elements are quite low.
- The number of valence electrons in metallic atoms is less than the number of vacant (empty) valence orbitals.
|Metals||Empty Valence orbitals.|
|Li (lithium: 1s2,2s2,2p0)||Three orbitals are vacant.|
|Na (Sodium: 1s2,2s2,2p6,3s1,3p0,3d0)||Three 3p and Five 3d Orbitals empty.|
Thus, the metals atom has only a few electrons in their valence orbitals (<1 or 2 in most of the cases). On account of the low ionization energies of metals have their valence electrons are loosely bound to the Kernels.
Kernels: Nucleus and all other bounded electrons except those in the valence shell.
Consequently, some of the atoms lose one or more of the valence electrons and change into positive ions (cations). When these electrons move. This movement of mobile electrons within the metal is similar to the movement of molecules in gases. Due to this reason, this concept is known as electron gas model.
Metallic Bond Definition
|The simultaneous attractive interaction between the mobile electrons and cores constitute a weak bond which is known as Metallic Bond.|
Electron Sea model
Metals have the ability to conduct electricity and heat. If metals ends are connected to the external source of electric current. Free electrons start moving from one end and cross through metal. The rate of conductivity of electrons will be the same. These electrons move freely and randomly throughout the metal which may be regarded as a collection of positive ions (cores or kernels) immersed in a sea of mobile electrons. In Lithium, the ions would be Li+ and one electron per atom would contribute to sea. These free electrons account for the characteristic metal properties.
Band Theory of Metals
According to the band theory, When energy is supplied to electrons. They jump from the valence band to conduction band. The conduction band allows electrons to move freely.This cause the flow of current. The electrical conductivity of metal decreases as temperature increases. The increase in temperature causes thermal agitation of metal ions.This impends the flow of electrons when an electric field is applied.
- Crystalline nonmetals, such as diamond and phosphorus are insulators. They do not conduct electricity. It is due to the fact that there is highest energy electrons occupy filled bands of molecular orbitals that are separated from the lowest empty band (conduction band) by the energy difference called the band gap.In insulators, this band is in energy different that is too large for him to jump to get the conduction band.
- Elements that are semiconductors have filled bands that are only slightly below.They do not overlap with the empty band. They do not allow electricity to pass at low temperature. A small increase in temperature sufficient to excite some of the electrons. The electrons jump into the highest energy band conduction band.
Metallic Bonding Diagram
The diagram shows the movement of electrons in a metal. The movement is non-directional. The strength of metallic bond decreases with:
- The Increase of valence electrons.
- The decrease in the size of the atom.
Properties of Metallic Bonds
The different Properties of Metals can be explained with the help of electron sea model.These are discussed as follow:
The high electrical conductivity of metals is because of the presence of mobile valence electrons which are ordinarily flowing probably equally in all directions. When a potential difference is applied across a metal, the electrons start moving towards the positive end. Consequently, the electric current flows throughout the metal. The electrical conductivity decreases with the rise in temperature.
The high thermal conductivity of metals is also due to the presence of mobile electrons. On heating one end of a metal, the kinetic energy of the electrons of that end increases. Consequently, the electrons start moving rapidly to another end i.e. cooler end of the metal and transfer some of their energy to this end. As a result, this end also acquires higher temperature so that the heat gets conducted throughout the metal.
When a beam of light falls on the surface of a metal, the surface electrons absorb photons of light and are set into to and fro oscillations. These oscillating electrons, being charged, immediately emit the absorbed energy in the form of visible light. As such, the light falling on the surface of metal appears to be reflected giving rise to shining appearance known as metallic luster. In all metals, except copper and gold, the electrons absorb light of all wavelengths in the spectrum.
Malleability and Ductility
Metals can be hammered into thin sheets (malleability) and drawn into wires (ductility) because of the non-directional nature of the metallic bond. When an external stress is applied, the layers of metal ions slide over one another but the basic structure remains the same because mobile electrons adjust rapidly to the new situation. Thus the shape of the metallic crystal can be changed or deformed without breaking.
Metals have a high tensile strength, i.e., they can resist stretching without breaking. Thus a large weight can be supported even by a wire of small cross section. The high tensile strength is due to the strong electrostatic attraction between the positively charged metal ions and the sea of mobile electrons.
Example of Metallic Bond
This picture of positive ions immersed in a sea of electrons is independent of directional limitations i.e., the metallic bond is not directional. By hammering the internal structure remain unchanged as a sea of electrons rapidly adjust to the new situation. Metallic Bond does not include the bond formation of elements which participate in covalent bonding.
Examples of metallic bond include all metals such as Copper(Cu), aluminum(Al), silver(Ag), gold(Au). Whereas the d block elements comprised the metallic bonding as well as Covalent Bonding. The reason behind of two types of bonding is involvement of 3d orbitals electrons.
Ionic Covalent and Metallic bonds
Mobile View: Full Table
|Constituent Particles||Poistive and Negative Ions||Positive ions in a sea of electrons||Atoms|
|Binding Force||Electrostatic Attraction Between Ions||Electrostatic Attraction Between cations and sea of electrons||Strong Covalent Bond|
|Hardness||Very Hard||Variable||Hard Except for graphite|
|Melting Point||Very High||Modetate||High|
|Conductivity||Conduct in Molten State||Good Conductors||Bad Conductors Except for Graphite|
|Solubilty||Soluble in Polar and Non-Polar||Insoluble in Polar and Non-Polar||Insoluble in Polar and Soluble in Non-Polar Solvent|
|Examples||NaCl, ZnS, CaO, KNO3 etc.||Metals and Alloys||Diamond Graphite, Sulphur, SiC etc.|
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