The energy of a Photon is equal to the difference in the energy level of the Atom that it came from.
It decreases, following the law of conservation of energy. It will be a discrete value of energy (quanta) released; due to the specific energy levels of the atoms which would be released at a certain frequency.
As described by the Bohr model, the energy levels in an atom have discrete and characteristic energies. Transitions from one energy level to another correspond to emission or absorption of a photon with a characteristic energy that is exactly equal to the difference in atomic energy levels. Since the energy of a photon is defined by it’s frequency, the emitted or absorbed photons have characteristic frequencies corresponding to the difference in energy between the atomic energy levels.
It will absorb or emit energy, according to the difference in the corresponding energy levels.
When electrons in an atom give up energy by dropping from a higher energy state to a lower energy state, that energy is emitted as photons of light whose frequencies are the lost energy/ Placvk's constant.As the atom can have several levels of energy, a spectrum of several lines is produced.
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The energy difference, between two energy levels, is emitted as a photon, when the electron "falls down" to a lower energy level.
As excited electrons drop back to lower energy levels in the atom, photons having the energy of the difference between the two electron energy levels are emitted from the atom.
The difference in energy between the energy levels determines color of light emitted when an electron moves from one energy level to another.
a photon is emitted or absorbed
The more energy levels the electron jumps the more energy the emitted light will have. The more energy you have the shorter wavelength there is.
It has to do with the energy level accessible to the electron in a particular type of bond or orbital. The difference between the two energy levels determines the energy of the quantum step and consequently the frequency of the light absorbed or emitted.
The quantum theory of energy levels within atoms was aided by the emission spectrum. When excited with light, different elements emitted photons of different frequencies. The frequencies were different because the energy difference from excited to low energy state was different depending on the element.
That because only certain photons are emitted, we know that only certain energy changes are occurring.
They are smaller in magnitude than those between lower energy levels.
These colors are generated by excited electrons relaxing back to lower energy levels. Each element has unique energy levels permitted to electrons by quantum mechanics. As an electron drops to a lower level a photon is emitted, carrying away the difference in energy and the higher the energy the shorter its wavelength.
Energy is emitted when an electron moves from a higher energy level to a lower energy level.
They are smaller in magnitude than those between lower energy levels.