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What happend when an electron in a hydrogen atom moves to a higher level?
Wiki User
∙ 11y ago
It immediately falls back to the ground state and emits a photon of light.
Wiki User
∙ 11y ago
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What is the number for electrons on hydrogen's first energy level?
Hydrogen's electron configuration is 1s1. It has only one electron. It is located in the first energy level.
What is the hydrogen main e level?
Hydrogen has only one electron.
What is the difference between excited hydrogen atom and any other atom?
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"
What is the ground level of hydrogen?
The ground state electron configuration of hydrogen is 1s1.
When the electron emits lights does the electron move up to a higher energy level or down to a lower energy level?
In the Bohr model of the atom, an electron emits a photon when it moves from a higher energy level to a lower energy level.
What do Each of the colored lines in hydrogen's emission spectrum corresponds with?
transition of an electron from a higher energy level to a lower energy level.
The outer electron levels of hydrogen?
Hydrogen has only 1 electron and has only 1 energy level.
When an electron in an atom of hydrogen moves from the second to the first principal energy level the result is the emission of?
one photonAn electron moves from a higher orbit to a lower orbit
What is the number for electrons on hydrogen's first energy level?
Hydrogen's electron configuration is 1s1. It has only one electron. It is located in the first energy level.
What is the hydrogen main e level?
Hydrogen has only one electron.
What color would be given off by an electron shifting from level 6 to level 2 in hydrogen?
Hydrogen has only one electron on one shell.
According to Bohr's model of the hydrogen atom how is hydrogen's emission spectrum produced?
it is produced when an electron from a higher energy orbit drops down to a lower level of energy orbit.
What is the difference between excited hydrogen atom and any other atom?
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"
What is the ground level of hydrogen?
The ground state electron configuration of hydrogen is 1s1.
Electron X can change to a higher energy level or a lower energy level Which statement is true of electron X?
Electron X absorbs energy when it changes to a higher energy level. Electron X absorbs energy when it changes to a higher energy level. It takes energy to do that.
According to Bohr model of hydrogen atom how is hydrogen's emission spectrum produced?
It's produced when an electron from a higher energy orbit drops down to a lower level energy orbit
How do you explain the diagram that shows 4 energy levels of hydrogen - 1 at the bottom 4 at the top - the values are n4-0.85eV n3-1.51eV n2-3.4eV n1-13.6eV?
The diagram shows the ionization energies of hydrogen. The ionization energy for a ground-state electron in hydrogen is 13.6eV. Let's jump. An electron orbits an atom of hydrogen in as low an energy level as possible. That's the ground state of hydrogen. To tear that electron away, it takes some amount of energy. In this case, it takes 13.6eV to strip off that electron. But what if the electron is in the next higher allowable energy level because the gas it hot? In that case, it takes less energy to tear that electron away because you've got a "head start" owing to the fact that the electron is in a higher orbital than the ground state. And what if it's in the next higher allowable energy level? Or the next? Less and less energy is required to strip off the electron as it moves to higher energy levels. These are the ionization energies of hydrogen. These energy levels are specific to hydrogen. Each other element will have a different set if ionization energies associated with it. And with atoms with many electrons and complex electron structures, the problem can quickly become very complex.
