Development of Quantum Mechanics Bohr’s Contribution

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Presentation transcript:

Development of Quantum Mechanics Bohr’s Contribution AP Chemistry by Diane Paskowski

Questions to Consider Why do the different chemicals give us different colors? Why do we get colors at all? 7.1

Atomic Spectrum of Hydrogen Continuous spectrum – contains all the wavelengths of visible light Line spectrum – each line corresponds to a discrete wavelength: Hydrogen emission spectrum 7.3

Significance? Only certain energies are allowed for the electron in the hydrogen atom. Energy of the electron in the hydrogen atom is quantized. 7.3

Bohr Model Electron in a hydrogen atom moves around the nucleus only in certain allowed circular orbits. ΔE = -2.178×10-18J[(1/nfinal2)-(1/ninitial2)] Where n is the energy level (principal quantum number) 7.4

Electronic Transitions in the Bohr Model for the Hydrogen Atom 7.4

Figure 7.7 A Change Between Two Discrete Energy Levels Emits a Photon of Light

Line Spectrum Of Hydrogen http://www.mhhe.com/physsci/chemistry/essentialchemis try/flash/linesp16.swf

Bohr Model Bohr’s model is fundamentally incorrect. This model only works for hydrogen. Electrons do not move around the nucleus in circular orbits. 7.4