Final answer:
Covalent bonds involve the sharing of electron pairs between atoms to achieve a stable electron configuration, while different from ionic and metallic bonding. Group 6A elements form two such bonds to complete their octet. Representation of such bonds can be visually illustrated using Lewis electron dot diagrams.
Step-by-step explanation:
Covalent bonds are a type of chemical bond where two atoms share one or more pairs of valence electrons. This sharing allows each atom to attain the electron configuration of a noble gas, achieving a more stable state. In the context of group 6A elements, these atoms require two additional electrons to fill their valence shell, leading to the formation of two covalent bonds to complete their octet.
Covalent bonding is distinct from ionic bonding, where electrons are completely transferred from one atom to another, creating ions that are held together by electrostatic forces. Unlike metallic bonding, where electrons are delocalized and shared among a lattice of metal cations, covalent bonds involve definite pairs of electrons shared between specific atoms.
Lewis electron dot diagrams are frequently used to represent covalent bond formations, indicating shared electron pairs and thereby providing a visual illustration of the molecule's structure. While single covalent bonds involve the sharing of one pair of electrons, some molecules require double or triple bonds to fully satisfy the valence requirements of the bonded atoms.