ad 23 electrons then the atom would be enormous. Another problem with the orbital of an electron was that no energy could be observed by the electron orbit decay. Next, if the center of an atom was composed of protons (+) and the electrons (-) orbited this positive core why didn't the electrons crash into the protons, causing an ultra violet catastrophe. Also, if the core was composed of just positive protons and opposite charges repel then how did the protons stay together. And the final problem, the atom didn't weigh enough. When scientists added the weight of the electrons and the weight of the protons and subtracted that from the overall weight of the atom there was a remainder. Something had to be missing from the model of an atom to make up for the weight difference. The answers to these questions came from the next big contributors to this theory, Niles Bohr and Chadwick.Niles Bohr developed a theory known as the Bohr theory of the atom. He assumed that electrons are arranged in definite energy levels, or quantum levels, at a specific distance from the nucleus. The arrangement of these electrons is called the electron configuration. There are seven levels, which were derived from the seven colors he saw, each of which has a specific number of electrons that it has capacity for. The first level can only accommodate two electrons, the second can hold up to eight electrons, the third can hold up to eight-teen, and so on. If an atom had four electrons you wouldn't find two in the first, one in the second, and one in the sixth. Electrons always occupy the lowest energy levels first. Electrons in a "ground state" are in their regular energy level and give off no energy; however, if an electron is in an "excited state" it sends energy in quantum packets (photons) and light is observes. When excited electrons jump up a level they give off light energy: however, they can never go down a level, energy can never be lost only gained. Chadwi...
