The three types of chemical bonds that valence electrons participate in are:
Ionic Bonds: Ionic bonds occur when there is a transfer of electrons between atoms. One atom donates electrons to another atom, resulting in the formation of ions. The oppositely charged ions are then attracted to each other, forming an ionic bond. An example is the bond between sodium (Na) and chlorine (Cl) to form sodium chloride (NaCl).
Covalent Bonds: Covalent bonds occur when atoms share electrons to achieve a stable electron configuration. In this type of bond, the participating atoms have similar electronegativity, resulting in a shared electron pair between them. An example is the bond between two hydrogen (H) atoms in a hydrogen molecule (H2).
Metallic Bonds: Metallic bonds occur in metallic elements, where valence electrons are delocalized and move freely among the metal atoms. These shared electrons create a bond that holds the metal atoms together in a lattice structure. An example is the bonding in a piece of solid copper (Cu), where the valence electrons are shared among the copper atoms.
It's important to note that there are also other types of chemical bonds, such as polar covalent bonds and hydrogen bonds, which involve varying degrees of electron sharing or attraction. However, the three types mentioned above are the fundamental categories based on the nature of valence electron participation.