Detailed Breakdown: Chemical Bonding
The Nature of Chemical Bonding: All bonding is the result of electrostatic attractions between oppositely charged species. In ionic bonds, electrons are transferred from a metal to a non-metal, creating a lattice of ions. In covalent bonds, electrons are shared between non-metals to achieve stability.
Molecular Geometry and VSEPR Theory: The Valence Shell Electron Pair Repulsion theory states that electron domains around a central atom position themselves as far apart as possible. This predicts the 3D shape (e.g. tetrahedral, trigonal planar) and bond angles (e.g. $109.5^\circ, 120^\circ$) of molecules.
Intermolecular Forces (IMFs): The physical properties of covalent substances (melting point, solubility) are governed by London dispersion forces, dipole-dipole interactions, and Hydrogen bonding. Hydrogen bonding, the strongest IMF, occurs when $H$ is bonded to $N, O, \text{ or } F$.