CHEM 1000 Lecture Notes - Lecture 6: Azimuthal Quantum Number, Magnetic Quantum Number, Bohr Radius
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20 Jan 2017
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Atomic spectra- the spectra of excited atoms could not be explained by 19th century models of the atom. Spectra were ultimately explained by the quantum theory. Energy has a limited number of discrete values. The energy between two energy values is a quantum of energy. The fundamental principles of the bohr model of the atom are: The electron moves in circular orbits around the nucleus. The electron has constant energy and no energy is emitted. An electron can only go from one allowed orbit to another. Cannot explain emission spectra from multi- electron atoms. Cannot explain the effect of magnetic fields on spectra. No reason for the fixed, quantized orbits. The most important is that of wave- particle duality. The photoelectric effect required that although light was a wave it has particle like properties. De broglie formulated the reverse, the wave particle duality. When the wave length is comparable to the dimensions. When the wavelength is like spacing between atoms.
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