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How the concept of ionization energy of H-atom can be justify from bohr model of atom?
In the Bohr model of the hydrogen atom, the electron is assumed to orbit the nucleus in discrete energy levels. The ionization energy of the hydrogen atom corresponds to the energy required to completely remove the electron from its orbit, moving it from its lowest energy level to an unbound state. This energy depends on the specific energy level the electron is in, as each energy level has a corresponding ionization energy.
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"
How much energy is needed to completely remove an electron from n2 in a hydrogen atom?
How much energy is required to move the electron of the hydrogen atom from the 1s to the 2s orbital
What quantum number of the hydrogen atom comes closest to giving a 31--diameter electron orbit?
The quantum number that determines the size of an electron's orbit in a hydrogen atom is the principal quantum number, denoted by "n." For an electron orbit with a 31 Å diameter, the closest principal quantum number would be n = 4, because the average radius of the electron for an orbit corresponding to n is approximately given by n^2 Å in hydrogen atom.
How does the electron's energy change as the orbit of the electron increases?
As the orbit of the electron increases, the electron's energy also increases. Electrons in higher energy orbits are farther from the nucleus and have more potential energy. Conversely, electrons in lower energy orbits are closer to the nucleus and have less energy.
What is the energy of electron in first orbit?
The energy of an electron in the first orbit of a hydrogen atom is -13.6 electron volts (eV). This energy value represents the lowest energy level in the atom and is known as the ground state energy.
How the concept of ionization energy of H-atom can be justify from bohr model of atom?
In the Bohr model of the hydrogen atom, the electron is assumed to orbit the nucleus in discrete energy levels. The ionization energy of the hydrogen atom corresponds to the energy required to completely remove the electron from its orbit, moving it from its lowest energy level to an unbound state. This energy depends on the specific energy level the electron is in, as each energy level has a corresponding ionization energy.
What happens to excess energy when the electron jumps from a higher energy orbit to a lower energy orbit in the hydrogen atom?
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.
When an electron in an atom of hydrogen moves from the second to the first principal energy level the result is the emission of?
When an electron in a hydrogen atom moves from the second to the first energy level, it emits a photon of light with a specific energy corresponding to the difference in energy levels. This process is known as electronic transition or photon emission.
According to Bohr's model of the hydrogen atom how is hydrogen's emission spectrum produced?
In Bohr's model of the hydrogen atom, hydrogen's emission spectrum is produced when electrons jump between different energy levels within the atom. When an electron moves from a higher energy level to a lower one, it releases energy in the form of light, which is observed as distinct spectral lines in the emission spectrum. The energy of the emitted light corresponds to the energy difference between the initial and final energy levels of the electron.
What is the process to calculate the ionization energy of a hydrogen atom?
To calculate the ionization energy of a hydrogen atom, you can use the formula E -13.6/n2 electron volts, where n is the energy level of the electron being removed. The ionization energy is the amount of energy required to remove an electron from the hydrogen atom.
How much energy is required to ionize a hydrogen atom containing an electron in the n4 level?
The energy required to ionize a hydrogen atom with an electron in the n4 level is 0.85 electron volts.
In the Bohr model of the atom an electron in an orbit has a fixed .?
energy
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"
How much energy is needed to completely remove an electron from n2 in a hydrogen atom?
How much energy is required to move the electron of the hydrogen atom from the 1s to the 2s orbital
Why are electron in the electron cloud?
electron cloud refers to orbit present in the atom and electron can can be revolved by the orbit only as it is an imaginary path made of energy
What quantum number of the hydrogen atom comes closest to giving a 31--diameter electron orbit?
The quantum number that determines the size of an electron's orbit in a hydrogen atom is the principal quantum number, denoted by "n." For an electron orbit with a 31 Å diameter, the closest principal quantum number would be n = 4, because the average radius of the electron for an orbit corresponding to n is approximately given by n^2 Å in hydrogen atom.
