From that excitation state, the electron can then drop back down, releasing a photon with a fixed amount of energy based on the energy lost by the electron when it fell to the lower orbital. The electron can absorb one quantum of energy and jump up to the excitation state. In the case of one ground state plus one excitation state, there is only one possible state change. The number of movements an electron can make depends on the number of excitation states available. When the electron returns to the ground state, it can no longer release energy but can absorb quanta of energy and move up to excitation states (higher orbitals). The energy contained in that photon corresponds to the difference between the two states the electron moves between. When it does, the electron releases a photon of electromagnetic energy. An electron in an excited state can release energy and 'fall' to a lower state. When an electron absorbs energy, it jumps to a higher orbital. The higher the excitation state, the more energy the electron contains. Higher orbitals represent higher excitation states. The lowest energy level an electron can occupy is called the ground state. Electrons can move between orbits by releasing or absorbing energy.

As long as an electron remains in the same orbital, the energy content of that electron remains constant.Electrons in each orbital contain a set quantity of energy.Each orbital is at a different distances from the nucleus.Electrons can exist only in a finite number of orbitals.Electrons travel in circular paths around the nucleus of an atom.

Instead, electrons maintain discrete positions around the nucleus. However, the Bohr atom remains a popular teaching tool because it illustrates the relationship between energy, electron position, and the emission of electromagnetic energy.ĭevelopment of the Bohr model of the atom helped establish a framework for understanding how electrons absorb and release discrete amounts (quanta) of energy by indicating that electrons associated with an atom do not have free range to be anywhere around that atom. The planetary model is not consistent with our current knowledge of the structure of the atom.

It is essential to understand that the planet-like imagery is just a representation. Change the number of excitation states the electron has with the slider at the lower left and click on the hidden, visible and comment buttons to toggle information about the atom on and off. Click on the grey rings to move the electron from orbital to orbital. The Bohr model represented an advancement in the understanding of atomic structure and contributed to the development of quantum mechanics.Ībove is a Bohr Atom. The model assumed an atom's structure resembles the solar system with the atomic nucleus at the center and electrons moving in circular orbits similar planet orbiting the Sun.

The Bohr model of the atom, developed in the early twentieth century, was an attempt to explain patterns in way atoms and electrons absorb, retain, and release energy.

Bohr model of atom