Atoms bond with each other through various types of chemical bonds. The three most common types of chemical bonds are:
Ionic Bonds: Ionic bonds form when there is a transfer of electrons from one atom to another. This occurs between atoms with significantly different electronegativity values. In an ionic bond, one atom gains electrons to become negatively charged (an anion), while the other atom loses electrons to become positively charged (a cation). The opposite charges attract each other, resulting in a bond.
Covalent Bonds: Covalent bonds form when atoms share electrons to achieve a more stable electron configuration. Covalent bonding occurs between nonmetal atoms. In a covalent bond, the shared electrons are attracted to the nuclei of both atoms, holding them together. There are two types of covalent bonds: nonpolar covalent bonds, where electrons are shared equally, and polar covalent bonds, where electrons are shared unequally due to differences in electronegativity.
Metallic Bonds: Metallic bonds occur in metals and involve the sharing of a sea of delocalized electrons among a lattice of metal cations. In a metallic bond, the positive metal ions are surrounded by a "sea" of valence electrons, which are free to move throughout the metal structure. This creates a strong bond between the metal ions and allows for the characteristic properties of metals, such as high electrical and thermal conductivity and malleability.
These bonding types can also interact in more complex situations. For instance, there can be bonds with partial ionic and partial covalent character (polar covalent bonds), or combinations of covalent and metallic bonding in certain compounds.
Overall, atoms bond with each other to achieve a more stable and lower-energy state by either gaining, losing, or sharing electrons. The specific type of bond formed depends on the types of atoms involved, their electronegativity, and the conditions under which they interact.