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What kind of spectrum is produced when the electron jumps form a high energy state to a lower energy state?
Wiki User
∙ 10y ago
When an electron moves to a lower energy level, the difference in energy appears in the form of a photon, which the electron emits.
Wiki User
∙ 11y ago
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An electron jumps to a new energy level when?
the atom gains or loses energy
When an electron jumps from a higher to lower quantum what happens?
Energy excess is released. Lower levels have lower energy
Why electron jumps from ground state to exicted state?
Because they absorb energy.
How was Niel bohr model of an atom different from that of Rutherford model of an atom?
According to rutherford an electron jumps from one orbit to other by continueous discharge of energy ( classical thought about energy) while bohr said that electron jumps at once by discharging quanta of energy( quantum view of energy)
What happened to the energyof an electron as it goes farther from the nucleus?
if an electron gains enough energy it jumps to a higher energy level. when this happens the atom is in an "excited" state.
An electron jumps to a new energy level when?
the atom gains or loses energy
What is the physical process responsible for an emission nebula producing emission spectrum from the nebula?
This physical process is the same as any and all of those that produce Photons. These Photons are produced when any Electron Jumps from any Higher Energy level to any Lower Energy level [within the Atomic Valence Shell Rules].
Is an electron radiation?
Electrons are negative energy. When an electron jumps orbitals, it can either absorb or radiate energy in the form of photons.
Describe what happens to the outermost electron in a sodium atom when the atom is heated and made to give off a line spectrum?
the atom jumps up the the higher energy level and as it returns to the lower energy level it releases energy which turns into light
What did bohrs discover about the atom?
Bohr did not discover protons, neutrons, or electrons. Bohr used the energy changes in line emission spectra to develop a model that accounted for discrete energy changes. He used the signature spectra of hydrogen to design a model of a Hydrogen atom that showed the possible jumps that an electron could make after absorbing and then releasing energy. Some of the jumps create the visible bands we see by breaking down the light of glowing Hydrogen, while other jumps, non-visible, would still be created in the Electromagnetic Spectrum according to the energy changes of an electron jumping from outer electron rings to inner electron rings.
When an electron jumps from a higher to lower quantum what happens?
Energy excess is released. Lower levels have lower energy
Why electron jumps from ground state to exicted state?
Because they absorb energy.
How was Niel bohr model of an atom different from that of Rutherford model of an atom?
According to rutherford an electron jumps from one orbit to other by continueous discharge of energy ( classical thought about energy) while bohr said that electron jumps at once by discharging quanta of energy( quantum view of energy)
What happens when an electron in an atom absorbs energy?
When an electron in an atom absorbs a specific "Quantum" of energy, it will jump to the next specific energy level in the atom. It'll then jump back down, and in so doing releasing light and giving off a signature light spectrum for an element.
What happened to the energyof an electron as it goes farther from the nucleus?
if an electron gains enough energy it jumps to a higher energy level. when this happens the atom is in an "excited" state.
Why there are discontinous spaces between spectrum of hydrogen?
There are spaces in the atomic spectrum of hydrogen because there are discrete energy levels that the electron in the hydrogen atom can be located in. Generally speaking the further away from the nucleus, the higher the potential energy of the electron. When hydrogen gas is excited, the electron can jump up to higher energy levels. When that electron falls back down to a lower energy level, a photon is emitted with an energy equal to the energy difference between the atomic orbital it jumped from and the one it jumped to. Since excited electrons can make a number of different jumps (ex. 4->3, 4->2, 5->3, 5->2, etc) there are a series of photons given off with discrete energies. Each one of these photons has a distinct wavelength (given by the equation E=hf, where E is the energy of the photon, h is planck's constant and f is the frequency of the photon). Each line you see on the spectrum is a photon produced from a different energy jump, with a different wavelength. We are only able to see the photons that emit a wavelength in the visible spectrum (roughly 400-700 nm).
What happens to electrons when pigments in photo-systems 2 absorb light?
Light or photons are little packets of energy. When this energy is absorbed by an electron it boots the electrons energy and the electron jumps to a higher orbital shell position (which must be vacant of its electron). The electron can only do this when the energy needed for the jump and the energy in the incoming photon match. Thus specific colours of light are absorbed depending on the element present.
