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He told that electrons give off light and “jump” between orbits in a nucleus. Many physicists believed this to be madness because they couldn’t visualize these electrons “jumping” orbits within an atom. They needed something that would actually back up the idea. Erwin Schrodinger decided something was not right with this model either. Schrodinger showed that electrons weren’t particles moving in an orbit at all and they certainly weren’t skipping orbits. He felt this model explained a hydrogen atoms’ spectrum, but the model needed more to understand about more difficult atoms. He believed no one was sure whether you could pinpoint an electron, but you could guess where it was. He stated that an electrons' location could be described as a cloud as they would be likely found in that

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H^ represents Hamiltonian operator that states all the energy within the system. ψ is what’s known as the wave function and E is all the energy binded together within the electron. The wave functions from each specific atom are called atomic orbitals. “Chemists define an atomic orbital as the region within an atom that encloses where the electron is likely to be 90% of the time” (Khan 8). This equation was used to calculate the energy in electrons. Even though this means the atomic orbitals aren’t right every time, Schrodinger’s equation was still used to calculate where they might lie. Schrodinger called his atomic model the Electron Cloud Model. It represents the nucleus surrounding a cloud. “The cloud” is essentially where any electron could lie within the atom. Using mathematical equations, it showed anyone one could predict where an electron was because the theory was that electrons come and go. They aren’t evenly spread out, or just stuck in one place. Nor do they orbit like