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L05 - SUMMARY FROM LAST CLASS Quantized atom Bohrs model of...

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Dr. P. Lucas U of A MSE 110 Quantized atom SUMMARY FROM LAST CLASS Bohr’s model of the hydrogen atom was rationalized by de Broglie’s principle: since the electrons behave as waves, only the orbits which satisfy n λ = 2 π r are stable. There must be an integral number of wavelength around the orbit otherwise the wave interfere destructively and disappear. The electron forms a standing wave on the stable orbits. The standing wave is a general concept that also applied to the waves of a string of length L between two pegs, In this case The wave nature of particles is the source of quantization. Schrodinger used established wave equation and applied it to electron using de Broglie’s principle to obtain his famous equation. , 3 , 2 , 1 2 = = n n L λ 0 ) ( 8 2 2 2 2 = + ψ π ψ V E h m x Ψ is a wave function corresponding to each stable state of the electron around the nucleus. The Schrodinger equation allow us to calculate Ψ and E for each stable state (orbit) of the electron, and Ψ 2 the region of space of orbits. These states correspond to the familiar orbitals of the atoms.
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Dr. P. Lucas U of A MSE 110 Bohr’s Model ATOMIC STRUCTURE Bohr’s model is powerful in its simplicity to describe the quantized character of atoms, which rationalize observation such as atomic spectra. Provides a rational to the concept of stable orbits, or electronic states. Illustrate the link between wave nature of electrons in atoms and quantization through de Broglie’s principle. However, that model is too simplistic and can not explain all properties of atoms. There are actually additional stable states for the electron that Bohr can not explain but which are well describe using Scrodinger equation
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Dr. P. Lucas U of A MSE 110 Bohr vs Schrödinger ATOMIC STRUCTURE
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