Where ψ = ψ ( x, y, z ) ψ = ψ ( x, y, z ) is the three-dimensional wave function of the electron, m e m e is the mass of the electron, and E is the total energy of the electron. (This is analogous to the Earth-Sun system, where the Sun moves very little in response to the force exerted on it by Earth.) An explanation of this effect using Newton’s laws is given in Photons and Matter Waves. The proton is approximately 1800 times more massive than the electron, so the proton moves very little in response to the force on the proton by the electron. In Bohr’s model, the electron is pulled around the proton in a perfectly circular orbit by an attractive Coulomb force. The hydrogen atom consists of a single negatively charged electron that moves about a positively charged proton ( Figure 8.2). The hydrogen atom is the simplest atom in nature and, therefore, a good starting point to study atoms and atomic structure.
Use quantum numbers to calculate important information about the hydrogen atom.Distinguish between the Bohr and Schrödinger models of the atom.Identify the physical significance of each of the quantum numbers ( n, l, m n, l, m) of the hydrogen atom.Describe the hydrogen atom in terms of wave function, probability density, total energy, and orbital angular momentum.By the end of this section, you will be able to:
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