Why do atoms form ionic or covalent bonds?

Atoms form ionic or covalent bonds primarily to stabilize their energy levels. Atoms are driven by the desire to achieve a more stable electronic configuration, often resembling the nearest noble gas configuration. This stability is typically obtained through the interaction of electrons.

In ionic bonding, one atom donates an electron to another, resulting in the formation of positively and negatively charged ions. The electrostatic attraction between these oppositely charged ions leads to a stable ionic compound.

In covalent bonding, atoms share electrons to fill their outer electron shells. This sharing creates a bond that allows each atom to attain a more stable and lower energy state.

Stabilizing energy levels minimizes the potential energy of the system, making the resulting compound more stable and less reactive. Thus, the primary reason atoms form bonds is to achieve greater stability in their electron configurations.