Definition and Properties of Metal Bonds
Do you know what is meant by metal bonding ??? Because on this occasion we will discuss about the understanding of metal bonds, the characteristics of metal bonds, the nature of metal bonds, the process of forming metal bonds, and the complete example. Therefore, let us consider the review below.
Metal Bonds
Understanding Metal Bonds
Metal bonds are chemical bonds formed by the sharing of valence electron electrons between metal tomatoes. Example: ferrous metal, zinc, and silver. Metal bonds are not ionic or covalent bonds. One theory put forward to explain metal bonds is the theory of a sea of electrons. Examples of metal bonding. The place of valence electron position of an iron atom (Fe) can overlap with the place of position of the valence electron of other Fe atoms.
This overlap between valence electrons allows the valence electrons of each Fe atom to move freely in the space between Fe + ions to form a sea of electrons. Because the charges are opposite (Fe2 + and 2 e–), there is a pull between the Fe + ions and these free electrons. As a result, bonds are called metal bonds.
Characteristics of Metal Bonds
Metal atoms can be likened to ping-pong balls that are packed tightly together.
Metal atoms have very few valence electrons, so it is very easy to be released and form positive ions.
Therefore the outer shell of a metal atom is relatively loose (there are many empty spots) so that electrons can move from 1 atom to another atom.
The mobility of electrons in the metal is so free, that the metal valence electrons undergo a delocalisation, a state in which the valence electrons are not fixed on 1 atom, but always move from 1 atom to another.
The valence electrons blend into a cloud of electrons which surrounds the positive metal ions.
The presence of metal bonds causes metals to be:
Metals are solid at standard temperatures and pressures, with the exception of the element mercury and gallium which are both liquid. As a reminder, the properties of metals are as follows:
High thermal and electrical conductivity.
Sparkling and reflecting light.
Can be forged.
Have variations in mechanical strength.
Keep in mind that metal bonding is a major force that holds metal atoms together. Metal bonding is the result of the attraction of a positive charge from the metal and the negative charge of the electrons that move freely.
Metal properties cannot be included in bonding criteria such as covalent bonds or ionic bonds. Ionic compounds cannot conduct electricity in the solid phase, and ionic compounds are fragile (as opposed to metal properties). and; Atoms of metal compounds contain only one to three valence electrons. Thus the atom cannot form covalent bonds. Covalent compounds are poor conductors of electricity and are generally liquid (with the opposite properties of metal formation). Thus, the metal forms a different bonding model.
Metal Bond Formation Process
In the metal bonding process there is mutual lending of electrons, only the number of atoms together lend their valence electrons (electrons in the outer shell) not only between two but several atoms but in an unlimited number. Each atom surrenders valence electrons to be used together, thus there will be bonds of attraction between atoms that are close together.
The distance between these atoms will remain the same, meaning that if there are atoms moving away the attractive force will pull it back to its original position and if it moves too close there will be a repulsive force because the nuclei are too close when the electric charge is the same so that the position atom relative to other atoms will remain.
In metal bonds, the nuclei of a particular atom are spaced apart and arranged irregularly while electrons are lent to one another as if forming an electron mist. In metals, the outer atomic orbitals filled with electrons fuse into a delocalized system which is the basis for the formation of metal bonds. Delocalisation is a state in which the valence electrons do not remain in one atom's position, but always move from one atom to another.
Metal atoms can be joined together to connect in all directions to become a very large molecule. One atom will bind to several other atoms around it. As a result these atoms are strongly bonded and become solid (except Hg) metals and are generally hard.