CHEM 1210 Lecture Notes - Lecture 7: Bohr Model, Planck Mass, Emission Spectrum
Document Summary
The idea that electrons are found in quantized energy levels, which are described by quantum numbers, does produce an emission spectrum similar to experimental data as photons of energy (e=hv) are absorbed or emitted. Bohr never explained why the ground state is stable. An electron is never found between energy levels. If light can be both a wave and a particle, perhaps matter can be both a particle and a wave. The de broglie model treats the electron as a wave. Standing waves in a circle - only certain wavelengths result in a standing wave. Other particles of matter, not just electrons, have wavelength too! Lambda (wavelength) = h /mv (planck/ mass x velocity (momentum)); the wavelength is tiny for other matter. waves are diffracted if the wavelength is comparable to the slit spacing. In classical physics, we can describe a particle"s position in terms of its speed and direction with great accuracy.
