![]() Then the development of the quantum theory and the Schrodinger equation refined the picture of the energy levels of atomic electrons. The Bohr model of the atom started the progress toward a modern theory of the atom with its postulate that angular momentum is quantized, giving only specific allowed energies. No classical model could be found which would yield stable electron orbits. It was expected that orbits of electrons about positive nuclei would be unstable because they would radiate energy and therefore spiral into the nucleus. Bohr's model suggests that the atomic spectra of atoms is produced by electrons gaining energy from some source, jumping up to a higher energy level, then immediately dropping. ![]() This presented a considerable problem for classical physics, because accelerated charges were known to radiate electromagnetic energy. Bohr's model suggests each atom has a set of unchangeable energy levels, and electrons in the electron cloud of that atom must be in one of those energy levels. These spectral "lines" formed regular series and came to be interpreted as transitions between atomic energy levels. In the years before the beginning of the 20th century, the light emitted from luminous gases was found to consist not of a continuous range of wavelengths, but of discrete colors which were different for different gases. The numbers apply to the hydrogen orbits. The electron waves for the first three Bohr orbits are visualized here, depicting the waves as meeting a kind of resonance condition so that the continuing waves interfere constructively with each under these conditions. For orbit n, there are n wavelengths of the electron wave, and these wavelengths are n x the wavelength of orbit n=1. Instead, he incorporated into the classical mechanics. ![]() In 1913, Niels Bohr attempted to resolve the atomic paradox by ignoring classical electromagnetism’s prediction that the orbiting electron in hydrogen would continuously emit light. It is a standing wave phenomenon and has to do with resonanceĮlectron Wavelengths and Bohr Orbit RadiiThe Bohr orbit radius goes up with the square of the principal quantum number n. 1: An introduction to the Bohr Model of the Atom. Wave nature of electron Electron Waves and OrbitsAsking why electrons can exist only in some states and not in others is similar to asking how your guitar string knows what pitch to produce when you pluck it.
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