If we use the example of hydrogen chloride, hydrogen’s outer shell has an s-orbital (1s1), whereas chlorine’s outer shell has a p-orbital ([Ne] 3s23p5)12. This means that the electron shared between them is required to have two different energy levels. In the Copenhagen Interpretation, the electron is required to have two energy levels simultaneously, which either requires hydrogen to change to a p- orbital, which defies the exothermic nature of making the bond, or requires that chlorine change to an s-orbital, which means that hydrogen chloride takes part in electron emission, which hasn’t been detected by the compound. In the theory I have presented, the electron is individually dependent on a single atom in the covalent bond, and the force of attraction exerted by the nucleus of an atom determines the energy level, an increase in the force of attraction causing an increase in energy levels. This allows for the exothermic nature of the making of hydrogen chloride, as well as the absence of electron emission in the compound.