Why atoms form chemical bonds?

Atoms form chemical bonds in order to achieve a more stable and energetically favorable state. Atoms have a natural tendency to attain a stable configuration of electrons in their outermost energy level, which is also known as their valence shell. When the valence shell is complete, the atom is said to be in a more stable state.

Chemical bonds are formed when two or more atoms interact with each other, and their electrons are shared or transferred between them. By doing so, the atoms can achieve a more stable configuration of electrons in their outermost energy level, resulting in a lower potential energy and greater stability.

There are three main types of chemical bonds: covalent bonds, ionic bonds, and metallic bonds. In covalent bonds, two atoms share one or more pairs of electrons, while in ionic bonds; one or more electrons are transferred from one atom to another. In metallic bonds, a group of atoms share their valence electrons in a sea of electrons.

So, the formation of chemical bonds is a natural process driven by the desire of atoms to attain a more stable and energetically favorable configuration of electrons in their outermost energy level.