Ionization energy is the minimum energy required to remove an electron from an atom. It is usually expressed in units of kJ/mol, that is, the energy in kilojoules required to remove one mole of electrons from one mole of atoms. (a) Calculate the ionization energy for the hydrogen atom. (b) Repeat the calculation, assuming in this second case that the electrons are removed from the n = 2 state.
(a)

Interpretation:
The ionization energy for the hydrogen atom and the ionization energy in which the electrons are removed from the
Concept Introduction:
The emission of radiation given by an energized hydrogen atom to the electron falling from a higher-energy orbit to a lower orbit give a quantum of energy in the form of light. Based on electrostatic interaction and law of motion, Bohr derived the following equation.
where
The electrons are excited thermally when the light is used by an object. As a result, an emission spectrum comes. Line spectra consist of light only at specific, discrete wavelengths. In emission, the electron returns to a lower energy state from
This transition results in the photon’s emission with frequency
When
To calculate: The ionization energy for the hydrogen atom
Answer to Problem 7.125QP
The ionization energy for the hydrogen atom is
Explanation of Solution
Ionization energy is the minimum energy required to remove an electron from an atom. It is usually expressed in units of
Therefore, the energy difference (
Therefore, the ionization energy for the hydrogen atom is
(b)

Interpretation:
The ionization energy for the hydrogen atom and the ionization energy in which the electrons are removed from the
Concept Introduction:
The emission of radiation given by an energized hydrogen atom to the electron falling from a higher-energy orbit to a lower orbit give a quantum of energy in the form of light. Based on electrostatic interaction and law of motion, Bohr derived the following equation.
where
The electrons are excited thermally when the light is used by an object. As a result, an emission spectrum comes. Line spectra consist of light only at specific, discrete wavelengths. In emission, the electron returns to a lower energy state from
This transition results in the photon’s emission with frequency
When
To calculate: The ionization energy in which the electrons are removed from the
Answer to Problem 7.125QP
The ionization energy in which the electrons are removed from the
Explanation of Solution
The energy difference (
Therefore, the energy difference (
Therefore, the ionization energy in which the electrons are removed from the
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