The universe is built on a foundation of tiny building blocks – atoms. But these individual atoms rarely exist alone. They are driven by a fundamental force – chemical bonding – to join hands and form the vast array of molecules that make up our world. Understanding chemical bonding and its influence on molecular structure is akin to deciphering the language of matter, revealing the secrets behind the physical and chemical properties of everything from water to DNA. At the heart of chemical bonding lies the pursuit of stability. Atoms strive to achieve a configuration with a full outer shell of electrons, mirroring the inert nature of noble gases. This yearning for stability manifests in two primary forms of bonding: ionic and covalent. In ionic bonding, a dramatic transfer of electrons occurs between atoms. Metals, with their tendency to lose electrons, readily donate them to non-metals, resulting in oppositely charged ions. These ions, bound by powerful electrostatic attraction, form ionic compounds like table salt (NaCl). Covalent bonding, on the other hand, involves a more democratic approach. Here, atoms share electrons, forming a communal "sea" of electrons that holds the molecule together. This type of bonding gives rise to a vast array of molecules, from the simple structure of methane (CH₄) to the complex chains of proteins. The Lewis structure notation, with its dots representing valence electrons, serves as a valuable tool for depicting the electron sharing in covalent molecules.