4. Now let's look at what happens when we move to the second shelf, n2 = 2. What is the wavelength of light emitted whenmoving from the 3rd| 2ndenergy levels.and486 nm95 nm1875 nm656 nm Spectroscopy, or the study of how light interacts with matter, is an extremely powerful tool scientists use to identify unknownsubstances. One branch of spectroscopy is the measurement of the interactions between gases and visible light.Sending a very high voltage through a gas adds energy to the system causing some of the electrons to enter a more unstable, orexcited, state. To return to the stable state, the electron emits scme of that energy in the form of light.Using the fact that electrons can only exist in certain energy "shelves," we can predict what wavelengths of light, or colors, are emittedwhen we add energy to the system. The following equation shows the energy levels for a hydrogen atom with only one electron (whendealing with multiple electrons and protons the math becomes far more complex and is outside the scope of this activity).= R#)Where:A is the wavelength of light|RH is the Rydberg Constant for a Hydrogen atom, 1.0974 · 10’ /mn2 is the final energy levelnj is the starting energy level(n1 and n2 are always integers: 1, 2, 3, ...)

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Answered: 2. What is the wavelength of light…

2. What is the wavelength of light emitted when 4. Now let's look at what happens when we move to the second shelf, n2 = moving from the 3rd and 2nd energy levels. 486 nm 95 nm 1875 nm 656 nm

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter6: Electronic Structure And The Periodic Table

Section: Chapter Questions

Problem 80QAP: In the photoelectric effect, electrons are ejected from a metal surface when light strikes it. A...

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Question

4. Now let's look at what happens when we move to the second shelf, n2 = 2. What is the wavelength of light emitted when
moving from the 3rd
| 2nd
energy levels.
and
486 nm
95 nm
1875 nm
656 nm

Spectroscopy, or the study of how light interacts with matter, is an extremely powerful tool scientists use to identify unknown
substances. One branch of spectroscopy is the measurement of the interactions between gases and visible light.
Sending a very high voltage through a gas adds energy to the system causing some of the electrons to enter a more unstable, or
excited, state. To return to the stable state, the electron emits scme of that energy in the form of light.
Using the fact that electrons can only exist in certain energy "shelves," we can predict what wavelengths of light, or colors, are emitted
when we add energy to the system. The following equation shows the energy levels for a hydrogen atom with only one electron (when
dealing with multiple electrons and protons the math becomes far more complex and is outside the scope of this activity).
= R#)
Where:
A is the wavelength of light|
RH is the Rydberg Constant for a Hydrogen atom, 1.0974 · 10’ /m
n2 is the final energy level
nj is the starting energy level
(n1 and n2 are always integers: 1, 2, 3, ...)

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