Metallic bonds examples
The following are the examples of metallic bond:
1. Sodium (Na)
A sodium atom’s valence shell has one electron. When more than one sodium atom is organised in a crystal lattice (bcc), molecular orbitals are created when the electrons in the outermost shell share space with another sodium atom. The valence electrons that are found in the atom’s outermost shell are dispersed across the metal’s space lattice. This is a case of a metallic bond.
Metallic bonds are created when negatively charged electrons and positively charged sodium metal ions join forces.
2. Aluminium (Al)
The valence shell of the aluminium atom contains three electrons. When aluminium atoms are organised in a crystal lattice (fcc), molecular orbitals are created when electrons in the outermost shell share interstitial space with other aluminium atoms. In the space lattice, these electrons are delocalized. More free electrons become available as the number of valence electrons rises. This is a case of a metallic bond. produced when positively charged aluminium metal ions and electrons came together.
3. Magnesium (Mg)
Two valence electrons make up the magnesium atom. Molecular orbitals are created when magnesium atoms are organised in a crystal lattice (hcp), which allows electrons in the valence shell to share space with other magnesium atoms. In the crystal, the electrons that are part of the valence shell are free to move around. between positively charged magnesium metal ions (2+) and electrons, forming a metallic connection. This is an illustration of a metallic connection.
4. Copper (Cu)
The copper atom’s outermost shell has one electron. The formation of molecular orbitals occurs when more than one copper atom is placed in a crystal lattice (fcc), where the electrons in the outermost shell share interstitial space with another copper atom. In the interstitial region of the metal lattice, the electrons in the valence shell are dispersed. They can move about freely. This is a case of a metallic bond. As the metallic link between the electrons and copper ions formed.
5. Iron (Fe)
Eight electrons make up the iron atom’s electron shell. The formation of molecular orbitals occurs when iron atoms are organised in a crystal lattice (bcc and fcc), where the electrons in the outermost shell share interstitial space with other iron atoms. These electrons’ delocalization occurs in the interstitial area. As the number of valence electrons rises, more electrons become available that aren’t attached to atoms. This is a case of a metallic bond. between positively charged iron metal ions and electrons, a metallic connection was created.
