![]() ![]() So, putting electrons into higher energy states within an atom. Photon absorption provides the energy for electrons to 'climb' the set of energy levels for that element. Consequently an emission spectra is a series of specific, single color lines (against a black background) for each of the emitted frequencies. The emissions correspond with electrons descending 'down' their energy levels, with the energy differences being carried away by photons with the appropriate frequency. ![]() ![]() The lowest energy (or ground state) corresponds to orbit closest to the nucleus and photons with specific amounts of electromagnetic radiation are absorbed or emitted when an electron moves from one orbit to another (absorbed to move further up the permitted levels and away from the nucleus)Īn atomic line spectrum is the whole range of specific photon radiation frequencies that an element can emit or absorb as it's electrons move between the energy levels allowed in those atoms. Only orbits with a very specific set of energy values are permitted (which all atoms of a given element have in common and are unique to that element). The electrons cannot occupy just any orbital radius. The electrons are held in orbit by the Coulomb (electrical) force between the positively-charged nucleus and the negatively-charged electrons. The Bohr model resembles a planetary system in which the negatively-charged electrons orbit a small and very dense, positively-charged nucleus at the atom's center. Radiation is absorbed or emitted when an electron moves from one orbit to another. The lowest energy is found in the smallest orbit. The energy of the orbit is related to its size. Therefore, electrons orbit the nucleus in orbits that have a set size and energy. When electrons return to a lower energy level, they emit energy in the form of light. Orbits further from the nucleus exist at higher energy levels. Moreover, the Bohr model postulates that electrons orbit the nucleus at fixed energy levels. The Bohr model or Rutherford–Bohr model, presented by Niels Bohr and Ernest Rutherford in 1913, is a system consisting of a small, dense nucleus surrounded by orbiting electrons-similar to the structure of the Solar System, but with attraction provided by electrostatic forces in place of gravity. The main difference between emission and absorption spectra is that an emission spectrum has different colored lines in the spectrum, whereas an absorption spectrum has dark-colored lines in the spectrum.Īccording to Bohr's model, an electron would absorb energy in the form of photons to get excited to a higher energy level as long as the photon's energy was equal to the energy difference between the initial and final energy levels. ![]()
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