Calculate the frequency (in Hertz) and wavelength (in nanometers) of a photon emitted by a hydrogen atom when its electron drops from n = 4 state to n = 2 state.The first line of the Balmer series occurs at a wavelength of 656.3 nm. What is the energy difference between the two energy levels involved in the emission that results in this spectral line? An electron in the hydrogen atom makes a transition from an energy state of principal quantum numbers ni to the n = 2 state. If the photon emitted has a wavelength of 434 nm, what is the value of ni? 1. Calculate the frequency (in Hertz) and wavelength (in nanometers) of a photon emitted by a hydrogenatom when its electron drops from n = 4 state to n = 2 state.(Answers = 6.17 x 1014/s; 486 nm)2. The first line of the Balmer series occurs at a wavelength of 656.3 nm. What is the energy differencebetween the two energy levels involved in the emission that results in this spectral line? (Answer3.027 x 10 -19 J)3. An electron in the hydrogen atom makes a transition from an energy state of principal quantumnumbers n; to the n = 2 state. If the photon emitted has a wavelength of 434 nm, what is the value ofn;? (Answer = 5)

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Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter5: Electron Configurations And The Periodic Table

Section: Chapter Questions

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Calculate the frequency (in Hertz) and wavelength (in nanometers) of a photon emitted by a hydrogen atom when its electron drops from n = 4 state to n = 2 state.
The first line of the Balmer series occurs at a wavelength of 656.3 nm. What is the energy difference between the two energy levels involved in the emission that results in this spectral line?
An electron in the hydrogen atom makes a transition from an energy state of principal quantum numbers n_i to the n = 2 state. If the photon emitted has a wavelength of 434 nm, what is the value of n_i?

1. Calculate the frequency (in Hertz) and wavelength (in nanometers) of a photon emitted by a hydrogen
atom when its electron drops from n = 4 state to n = 2 state.
(Answers = 6.17 x 1014/s; 486 nm)
2. The first line of the Balmer series occurs at a wavelength of 656.3 nm. What is the energy difference
between the two energy levels involved in the emission that results in this spectral line? (Answer
3.027 x 10 -19 J)
3. An electron in the hydrogen atom makes a transition from an energy state of principal quantum
numbers n; to the n = 2 state. If the photon emitted has a wavelength of 434 nm, what is the value of
n;? (Answer = 5)

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