Chemical Bonding: Types, Models, and Forces

Definition and purpose of chemical bonds

A chemical bond is the association of atoms or ions that holds them together to form molecules, crystals, and other structures. It arises from electrostatic attraction between oppositely charged species (as in ionic bonding), from the sharing of electrons (as in covalent bonding), or from a combination of these effects. Quantum mechanics explains how electron behavior stabilizes bonded systems, including how electron distribution and wavefunction effects lower the system’s energy and maintain an equilibrium bond distance where attractions and repulsions balance. Chemical bonds determine the structure and properties of matter, including bond strength, directionality, and polarity. Bonds are often grouped into strong (primary/intramolecular) bonds—such as covalent, ionic, and metallic bonds—and weak (secondary/intermolecular) bonds—such as hydrogen bonds, dipole–dipole interactions, and London dispersion forces. In practice, chemists use simplified rules and theories (e.g., electronegativity, the octet rule, VSEPR, valence bond theory, and molecular orbital theory) to predict how bonds form and how strongly atoms will interact.

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Strong versus weak chemical bonds

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