WHERE DOES METAL ION BONDING OCCUR FREE

The delocalized electrons can conduct both electricity and heat from one end of the metal to another with low resistance. The electron sea model accounts for several metallic properties, including high thermal and electrical conductivity, metallic luster, ductility, and malleability. This electron sea model accounts for most physical properties of metals such as conductance to heat and electricity, high melting and boiling points, malleability, and ductility. Such an attractive force between the negatively charged electrons and metal cations is called metallic bonds, holding the atoms together. These electrons can be shared by multiple neighboring metal-cations through a strong, attractive force between these negatively and positively charged species.

WHERE DOES METAL ION BONDING OCCUR FREE

The atom forms a positively charged metal ion, while the free outer electrons exist as negatively charged delocalized electron clouds. The ionization energy of metal atoms (energy required to remove an electron from the atom) is low, facilitating the easy removal of valence electrons from the parent atom.

However, the valence electrons in metal atoms are loosely held due to their low electronegativity or attraction with the nucleus. Most metal atoms do not possess enough valence electrons to enter into an ionic or covalent bonding. A simplified model to describe metallic bonding has been developed by Paul Drüde called the “Electron Sea Model”. Metallic bonds are formed between two metal atoms. Electrons then flow into the new shape to accommodate the deformity. Since there are no localized bonds in metals, the metal atoms can slide past each other allowing easy deformity. Metals can easily be pounded into sheets due to their malleability or into wires due to the ductility property. According to the electron sea model, when heat is applied to one end of the metal, the electrons move freely and quickly disperse the heat throughout the metal. Metals are also excellent thermal conductors. However, when dissolved in water, the cations and anions dissociate and can move when subjected to a potential difference, creating an electric current. This is because, in a crystalline ionic bond, electrons are transferred from the metal to the nonmetal, but remain localized to one ion. In contrast, ionic compounds are nonconductors of electricity in their solid form but can conduct electricity when dissolved in water. This is why most metals are excellent conductors of electricity. For example, when a voltage difference is applied to a metal wire, like copper wire, the negatively charged electrons move freely towards the wire’s positive end, generating an electric current.

The electron sea model accounts for several important characteristics of metals. These electrons are not confined to any single ion but are evenly distributed and relatively free to move within the metal. These potassium cations are held together in close-packing because of their attraction to the negatively charged sea of electrons.

Due to the low ionization energy, each potassium atom can easily lose its valence electron to become a cation. Metallic bonds and most of their properties can be explained using the simple electron sea model. This gives the metallic bond distinct properties in contrast to ionic and covalent bonds. Compared to nonmetals, metals have low ionization energies, allowing them to lose valence electrons easily. A metallic bond is a bond between two metal atoms.

Where does metal ion bonding occur