Bohr model - Electron energy levels in hydrogen

In atomic physics, the Bohr model depicts the atom as a small, positively charged nucleus surrounded by electrons in orbit - similar in structure to the solar system, but with electrostatic forces providing attraction, rather than gravity. Its key success was in explaining the Rydberg formula for the spectral emission lines of atomic hydrogen; while the Rydberg formula had been known experimentally, it did not gain a theoretical underpinning until the Bohr model was introduced. The Bohr model is not a complete model of the atom, and f ...

Including:

• Bohr model - History
• Bohr model - Refinements
• Bohr model - Electron energy levels in hydrogen
• Bohr model - Energy in terms of other constants
• Bohr model - Rydberg Formula
• Bohr model - Shortcomings

Read more here: » Bohr model: Encyclopedia - Bohr model

The Bohr model is accurate only for one-electron systems such as the hydrogen atom or singly-ionized helium. This section uses the Bohr model to derive the energy levels of hydrogen. The derivation starts with three simple assumptions: 1) All particles are wavelike, and an electron's wavelength λ, is related to its velocity v by: where h is Planck's Constant, and me is the mass of the ...

See also:

Bohr model, Bohr model - History, Bohr model - Refinements, Bohr model - Electron energy levels in hydrogen, Bohr model - Energy in terms of other constants, Bohr model - Rydberg Formula, Bohr model - Shortcomings

Read more here: » Bohr model: Encyclopedia II - Bohr model - Electron energy levels in hydrogen

In the early part of the 20th century, experiments by Ernest Rutherford and others had established that atoms consisted of a diffuse cloud of negatively charged electrons surrounding a small, dense, positively charged nucleus. Given this experimental data, it is quite natural to consider a planetary model for the atom, with electrons orbiting a sun-like nucleus. However, a naive planetary model has several difficulties, the most serious of which is the loss of energy by synchrotron radiation. That is, a moving electric charge emits electroma ...

See also:

Bohr model, Bohr model - History, Bohr model - Refinements, Bohr model - Electron energy levels in hydrogen, Bohr model - Energy in terms of other constants, Bohr model - Rydberg Formula, Bohr model - Shortcomings

Read more here: » Bohr model: Encyclopedia II - Bohr model - History

Several enhancements to the Bohr model were proposed; most notably the Sommerfeld model or Bohr-Sommerfeld model, which attempted to add support for elliptical orbits to the Bohr model's circular orbits. This model supplemented condition (4) with an additional radial quantization condition, the Sommerfeld-Wilson quantization condition where p is the generalized momentum conjugate to t ...

See also:

Bohr model, Bohr model - History, Bohr model - Refinements, Bohr model - Electron energy levels in hydrogen, Bohr model - Energy in terms of other constants, Bohr model - Rydberg Formula, Bohr model - Shortcomings

Read more here: » Bohr model: Encyclopedia II - Bohr model - Refinements

The Rydberg formula describes the transitions or quantum jumps between one energy level and another. When the electron moves from one energy level to another, a photon is given off. Using the derived formula for the different 'energy' levels of hydrogen one may determine the 'wavelengths' of light that a hydrogen atom can give off. The energy of photons that a hydrogen atom can give off are given by the difference of two hydrogen energy levels: where nf< ...

See also:

Bohr model, Bohr model - History, Bohr model - Refinements, Bohr model - Electron energy levels in hydrogen, Bohr model - Energy in terms of other constants, Bohr model - Rydberg Formula, Bohr model - Shortcomings

Read more here: » Bohr model: Encyclopedia II - Bohr model - Rydberg Formula

The Bohr model gives an incorrect value for the ground state orbital angular momentum. The angular momentum in the true ground state is known to be zero. The Bohr model also has difficulty with or fails to explain: The spectra of larger atoms. At best, it can make some approximate predictions about the emission spectra for atoms with a single outer-shell electron (atoms in the lithium group.) The relative intensities of spectral lines; although in some simple cases, it was able to provide reasonable estimates (f ...

See also:

Bohr model, Bohr model - History, Bohr model - Refinements, Bohr model - Electron energy levels in hydrogen, Bohr model - Energy in terms of other constants, Bohr model - Rydberg Formula, Bohr model - Shortcomings

Read more here: » Bohr model: Encyclopedia II - Bohr model - Shortcomings