Metallic bond and Bond dipole

Metallic bond

In explaining the metallic bond in need of a thorough description of the electron's energy levels through quantum mechanics. Intuitively and easy to understand, Drude loorentz at the beginning of the 20th century proposed a model. With these models one can explain many things about the nature of nature, and can also explain the metallic bond as the first approach. This model explains that some outer electrons away from atoms form a cloud of electrons scattered throughout the crystal.

A metal can be said as a material composed of cations submerged in a cloud of electrons, and the attractive forces between the cation and the electron cloud is a bond of cohesion. In a metal crystal there is no limiting factor, for example, the amount and direction of covalent bonds in the crystal bonding and electrical neutrality in the crystal ions. Many metals have a crystalline arrangement of two kinds of arrangement of meetings, where the atoms are arranged at the meeting. This gives an explanation why the metals have high densities and have the properties of clay as well as easy on the wrought. Electrical conductivity and good heat on metals can be understood from the easy movement of electrons.

Bond dipole

Ties are much weaker than the other three types of bonding (ionic, metallic and covalent) is the bond dipole, which is the bond that caused the electrostatic attractive forces of molecular dipoles or group of atoms. Molecule formed by covalent bonds often form a permanent dipole because the electrons are in the middle between bonded atoms, and a positive charge and negative charge is not evenly distributed. Molecules attract each other electro statically between the positive and negative ends resulting in a bond. Bond dipole of the hydrogen atom as a positive end-called hydrogen bonds are quite strong bond because the small radius of the hydrogen ion. Association also has a permanent dipole nature of lead.

There is also a bond is called bond dipoles that do not have a fluctuating nature of lead. This happens because at any moment there are more electrons on one side of the nucleus than in the other. This bond on the bond called van der Walls, a weaker binding one level of the hydrogen bonding.