Instead of allowing for continuous values for the angular momentum, energy, and orbit radius, Bohr assumed that only discrete values for these could occur (actually, quantizing any one of these would imply that the other two are also quantized). Calculate the energy, the frequency, and the wavelength of the photon emitted when the electron moves from the outer to the inner of these two orbits. The popular theory of atomic structure at the time of Rutherford’s experiment was the plum pudding model.

This atomic model is the modification of Rutherford’s atomic model (the nucleus is positively charged and is surrounded by electrons (negatively charged particles). Figure1 The gold foil experiment was conducted under the supervision of Ernest Rutherford at the University of Manchester in 1909 by Hans Geiger and Ernest Marsden. The popular theory of atomic structure at the time of Rutherford’s experiment was the plum pudding model. In 1913, Danish physicist Neil Bohr proposed the Bohr atomic model based on Planck’s quantum theory of radiation.

The absolute value of the energy difference is used, since frequencies and wavelengths are always positive. In July of 1913, Danish physicist Niels Bohr published the first of a series of three papers introducing this model of the atom, which became known simply as the Bohr atom. According to Bohr’s theory two of the allowed orbits in the hydrogen atom have radii of 52.918 and 211.67 pm. The gold foil experiment was conducted under the supervision of Ernest Rutherford at the University of Manchester in 1909 by Hans Geiger and Ernest Marsden. In this equation, h is Planck’s constant and E i and E f are the initial and final orbital energies, respectively.

Bohrs atom model