There is an academic myth that believes that chemical theory researchers perfectly know what binds atoms in a molecule. The amount of heated open discussions about the nature of bonds in the literature disproves this myth. Another fantasy shared by students and teachers alike is that when advancing from introductory to advanced courses the student will slowly improve the basic and primitive models of the bond (starting from the covalent and ionic bonds from a Lewis sharedelectrons perspective), will completely fill the missing concepts, and in the end, everything will be accurately explained and understood. If not even specialists know all the facets of the bond, this myth also cannot be true, and students should know it. This article was written following an advanced undergraduate course on the chemical Bond. Being a quantum chemistry class, approaches the bonds by broad conceptual description of many types of interactions (covalent, non-covalent, ionic, dative, H-bond, halogen and other hole interactions, hyperconjugation, coordinative, metallic, van der Waals in all its forms, etc.), as well as brief explanations of techniques to compute them (Hückel, Hartree Fock, configuration of interactions, and DFT) and other topics connected with the bond (potential energy surface, reactivity, orbitals, etc.).