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Because they absorb energy.
Hydrogen atom = 1 proton 1 electron Hydrogen's 1 electron occupies the lowest energy level, 1s orbital. The atom is therefore in its "ground state". When a photon of correct frequency "collides" with a electron in hydrogen's 1s orbital the energy contained in the photon is transferred to the electron. The electron then gets added energy, so it is at a higher energy state. When it reaches this higher energy state the electron jumps to the next energy level and there it starts its new orbit. Hydrogen atom is now "excited" For any other atoms it is the same thing because all atoms can undergo excitation. The only difference between hydrogen's 1 electron and other atom's many electrons is WHICH ELECTRON will be "excited"
jumps to the a higher orbital. This is only possible if the energy it absorbed is large enough to let it jump the gap. If the energy is not large enough for the electron to jump that gap, the electron is forbidden to absorb any of that energy.
When an electron moves to a lower energy level, the difference in energy appears in the form of a photon, which the electron emits.
no
Because they absorb energy.
Hydrogen atom = 1 proton 1 electron Hydrogen's 1 electron occupies the lowest energy level, 1s orbital. The atom is therefore in its "ground state". When a photon of correct frequency "collides" with a electron in hydrogen's 1s orbital the energy contained in the photon is transferred to the electron. The electron then gets added energy, so it is at a higher energy state. When it reaches this higher energy state the electron jumps to the next energy level and there it starts its new orbit. Hydrogen atom is now "excited" For any other atoms it is the same thing because all atoms can undergo excitation. The only difference between hydrogen's 1 electron and other atom's many electrons is WHICH ELECTRON will be "excited"
Depends on the isotope can be 0 or 1 hydrogen is a highly unstable element that the electron Jumps betweent the two energy levels
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.
The electron emits a photon of light which we can see in a spectrograph as color. Four colors are normally seen in a hydrogen atom subjected to energy.
jumps to the a higher orbital. This is only possible if the energy it absorbed is large enough to let it jump the gap. If the energy is not large enough for the electron to jump that gap, the electron is forbidden to absorb any of that energy.
When an electron moves to a lower energy level, the difference in energy appears in the form of a photon, which the electron emits.
when an electron moves from excited state to ground state it emits photons of wavelength equal to the difference between the two energy levels. Consider a hydrogen atom. If the electron is at the second energy level in the atom (the energy of this level is -3.4 eV )it can stay there for about only 10^-8 s and then after that it just to the level below .If it jumps from second to ground state (energy of ground state is -13.6 eV) it emits aphoton of energy = 13.6-3.4 =10.2 eV. .............................Gho$t
It jumps from one electron to the other.
Electrons are negative energy. When an electron jumps orbitals, it can either absorb or radiate energy in the form of photons.
the atom gains or loses energy