answersLogoWhite

0

Neils Bohr made the ASSUMPTION that electrons could only exist in discrete energy levels when the electrostatic field of a nucleus -- he made no attempt to show WHY this was so.

Louis de Broglie postulated that electron movement could be described as a wave, with the wavelength being equal to Planck's Constant divided by the electron's momentum. Starting with this postulate, one can derive that the only permitted radial orbits of an electron are those with a circumference equal to a multiple of these wavelengths.

Erwin Schrodinger devised a mathematical formula for which one could derive these energy levels -- and a lot more. As such, Schrodinger's Equation was more fundamental to our understanding of sub-atomic reality. Schrondinger viewed his wave function (more precisely, the product of the wave function) as the charge density of a smeared-out electron.

Although you didn't ask, it was Max Born who showed that the wave-function product was, instead, the probability of finding a point-like electron at a specific place and time.

User Avatar

Wiki User

12y ago

What else can I help you with?