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jailbait
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When a photon has a wavelength close to the energy needed for an electron jump in an atom, the atom will absorb the photon. How close must the wavelength be to the energy required for the atom to still absorb it?
jailbait said:When a photon has a wavelength close to the energy needed for an electron jump in an atom, the atom will absorb the photon. How close must the wavelength be to the energy required for the atom to still absorb it?
The wavelength of a photon is directly related to an atom's ability to absorb it. This is because atoms have specific energy levels, and a photon with a wavelength that matches the energy difference between two levels can be absorbed by the atom.
The minimum wavelength of a photon that an atom can absorb depends on the energy levels of the atom. Each atom has a unique set of energy levels, so the minimum wavelength will vary from atom to atom.
No, an atom cannot absorb a photon with a longer wavelength than its energy levels. This is because the energy of a photon is directly proportional to its wavelength. If the energy of the photon is greater than the energy difference between the atom's levels, the excess energy will not be absorbed.
If the wavelength of a photon is too far from an atom's energy levels, the photon will not be absorbed by the atom. It may be scattered or transmitted through the material, but it will not interact with the atom in a way that causes absorption.
There is no specific maximum wavelength of a photon that an atom can absorb. However, as the wavelength of a photon increases, its energy decreases. Eventually, the energy of the photon will be too low to cause an electron transition in the atom, and it will not be absorbed.